Salts - Science topic

Remediating NaCl? How would you expect this to occur? These are elements

The rate of dissolving is influenced by stirring, temperature, and size of solute particles. Stirring helps distribute solute particles, speeding up the rate of dissolving. Warm solvents dissolve solutes faster due to increased particle movement. Smaller solute particles dissolve faster due to increased surface area. Stirring affects the rate of dissolving because it spreads the solvent's molecules around the solute and increases the chance of them coming into contact with it. Because of this, stirring makes solvents dissolve faster. Other factors affecting a solvent's solubility include temperature and particle size. The stirring allows fresh solvent molecules to continually be in contact with the solute. If it is not stirred, then the water right at the surface of the solute becomes saturated with dissolved sugar molecules, meaning that it is more difficult for additional solute to dissolve. If we stir a solution in an effort to dissolve a solute in a solvent, as was done in the five beakers, we can increase the rate of dissolution by increasing the interactions between solute and solvent particles. Since solubility is the upper limit, it cannot be increased by stirring the solution or by adding more solute. Stirring the solution will simply increase the rate of dissolution, but not the maximum amount of solute that can be dissolved. With an increase in temperature, more solute can be dissolved in the solvent.Agitation and stirring will increase the rate at which salt dissolves in water and increased movement of water molecules allow sodium ions and chloride ions to be pulled apart as shells of hydration are formed. Agitation and stirring will increase the rate at which salt dissolves in water and increased movement of water molecules allow sodium ions and chloride ions to be pulled apart as shells of hydration are formed. Stirring a solute into a solvent speeds up the rate of dissolving because it helps distribute the solute particles throughout the solvent. As the temperature increases, the number of grams of sugar that dissolves in water increases significantly. As the temperature increases, the number of grams of salt that dissolves in water increases only slightly. The process of stirring or agitating makes the solvent molecules is in contact with the solute particles on a continuous basis. So, if the mixture of salt and water will be stirred continuously, then the process of dissolution will take place frequently.

The principle behind both of them is the same; however, Potassium is more prone to induce precipitations than Sodium, which may be problematic for some analytical techniques. If these consideration do not affect your analysis, you may use Sodium salt for easier handling.

The surface tension of water is increased when salt is added to it. Although the strong interactions between sodium cations and partial negative oxygen, and chloride anions and partial positive hydrogens disrupt some hydrogen bonding between water molecules, they actually strengthen the surface tension of water. The surface tension of the liquid increases after we add salt to the water and surface tension arises due to the cohesive nature of a liquid which resists an external force on the liquid surface. Water molecules pull the sodium and chloride ions apart, breaking the ionic bond that held them together. After the salt compounds are pulled apart, the sodium and chloride atoms are surrounded by water molecules, as this diagram shows. Once this happens, the salt is dissolved, resulting in a homogeneous solution. As temperature decreases, surface tension increases. Conversely, as surface tension decreases strong; as molecules become more active with an increase in temperature becoming zero at its boiling point and vanishing at critical temperature. However, the surface tension of water can be broken by adding certain substances such as detergents. Soaps and detergents are useful for cleaning because when they break water's surface tension, they are able to spread out onto dirty surfaces and soak into laundry, breaking up dirt and oil. As for the why, it's simple mass conservation. If all the water evaporates then you get 5g of salt as salt does not evaporate. When seawater evaporates, water is removed, salt remains, and relatively salty water is left behind. This relatively salty water can float at the surface; as, in the tropics it floats because is it so warm and buoyant. So if you allow water to evaporate inside a sealed container, the container with the water and the water vapor will have the same mass before, during, and after evaporation. This rule applies to any change of state in a closed system.When salt is added to water, the surface tension of the liquid rises. Although some hydrogen bonds between water molecules are broken by the strong interactions between sodium cations and partial negative oxygen and chloride anions and partial positive hydrogens, they actually increase the surface tension of water. The surface tension of water is increased when salt is added to it. Although the strong interactions between sodium cations and partial negative oxygen, and chloride anions and partial positive hydrogens disrupt some hydrogen bonding between water molecules, they actually strengthen the surface tension of water.

To increase the rate at which salt dissolves in water, you can take the following actions:

Water molecules pull the sodium and chloride ions apart, breaking the ionic bond that held them together. After the salt compounds are pulled apart, the sodium and chloride atoms are surrounded by water molecules, as this diagram shows. Once this happens, the salt is dissolved, resulting in a homogeneous solution. The reason that the sugar seems to disappear is that the sugar molecules are now more attracted to water molecules. When the water is stirred the sugar molecules mix with the water molecules. The water molecules insert themselves with the sugar molecules and begin to surround each individual molecule. Salt also contains ions. Water helps in separating these ions by decreasing the interionic forces allowing the salt to disperse throughout the water. So, the particles of salt occupy the spaces in between the particles of water and hence get dissolved. This happens because water molecules are not tightly packed and have space between them hence when we dissolve the salt in it the salt particles occupy the space between the molecules of the water and thus the water level doesn't rise up. Dissolving a solid in liquid, such as table salt in water, is a physical change because only the state of the matter has changed. Physical changes can often be reversed. Allowing the water to evaporate will return the salt to a solid state. Therefore, dissolving salt in water is a chemical change. The reactant (sodium chloride or NaCl) is different from the products (sodium cation and chlorine anion). Thus, any ionic compound that is soluble in water would experience a chemical change. Salt (sodium chloride) is made from positive sodium ions bonded to negative chloride ions. Water can dissolve salt because the positive part of water molecules attracts the negative chloride ions, and the negative part of water molecules attracts the positive sodium ions. When water is heated and cooled it goes through a series of reversible changes. Water in its solid state is called ice. When ice is heated, it melts and becomes liquid water. Further heating causes the liquid to change to a gas, water vapor. The NaCl compound (the main compound of table salt) is an ionically bound, crystalline compound. Water molecules dissolve the Na and Cl atoms, which are bound in crystal form before being dissolved. As a result, water is a solvent.

Dr Ameer K Ibraheem thank you for your contribution to the discussion

Dr John Duchek thank you for your contribution to the discussion

Adding salt to water makes the water denser. As the salt dissolves in the water, it adds mass (more weight to the water). This makes the water denser and allows more objects to float on the surface that would sink in fresh water. About 3.5 percent of the weight of seawater comes from the dissolved salts. When salt is dissolved in fresh water, the density of the water increases because the mass of the water increases. When salt is dissolved in fresh water, the density of the water increases because the mass of the water increases. As the volume available for the particle to dissolve increases, by switching from NPV to cell or vessel volume thedissolution rate is expected to increase due to bulk concentration reduction. Surface area is larger when a given amount of a solid is present as smaller particles. Hence, the total surface area of the crushed salt will be more than that of the uncrushed crystals, resulting in higher rate of dissolving of the crushed salt in water. Actually, sodium chloride added to water will decrease the volume of the solution, up to around 2% for a saturated solution. Even when fully saturated, that's not a big change, so you may not have been able to observe it without something with a narrow neck like a volumetric flask.Salt water is denser than pure water because the salt in it contributes to the mass of the entire solution. A given quantity of solute dissolves faster when it is ground into small particles than if it is in the form of a large chunk, because more surface area is exposed. The packet of granulated sugar exposes far more surface area to the solvent and dissolves more quickly than the sugar cube.The salt concentration in slightly saline water is 1,000 to 3,000 ppm (0.1–0.3%); in moderately saline water is 3,000 to 10,000 ppm (0.3–1%); and in highly saline water is 10,000 to 35,000 ppm (1–3.5%). Seawater has a salinity of roughly 35,000 ppm, equivalent to 35 grams of salt per one liter (or kilogram) of water. At a given temperature, the density of an aqueous solution of sodium chloride, sometimes called “saline,” is a function of concentration. As the concentration of NaCl increases, the density of the solution increases in a fairly linear manner.

The level of water does not change when salt is dissolved in water because the salt particles dissociate and occupy the intermolecular spaces between the water particles. Since only the empty spaces are occupied, the level of water does not increase. When salt is mixed with water, the salt dissolves because the covalent bonds of water are stronger than the ionic bonds in the salt molecules. This happens because water molecules are not tightly packed and have space between them hence when we dissolve the salt in it the salt particles occupy the space between the molecules of the water and thus the water level doesn't rise up. The antiparticle space between the water particles is more as compared to salt. Salt also contains ions. Water helps in separating these ions by decreasing the intrinsic forces allowing the salt to disperse throughout the water. The salt doesn't literally disappear but they converted into ions from solid crystals in the aqueous medium of water. Also you may know that the ions are stable only in an aqueous medium. The NaCl crystal molecules are formed by the strong Coulombian force of attraction between Na+ and Cl- ions. This is because, when we add salt to water and stirred to dissolve, the particles of salt separate out and enter the empty spaces between the particles. This means, particles of matter have empty spaces between them. When we add a solid substance to a liquid, the particles solid get into the spaces between the liquid particles so, since the solids occupy the spaces inside liquid atoms, the volume of the liquid doesn't increase. Example: Sugar dissolves in water completely at different levels. This is because, when we add salt to water and stirred to dissolve, the particles of salt separate out and enter the empty spaces between the particles. This means, particles of matter have empty spaces between them. When salt is dissolved in fresh water, the density of the water increases because the mass of the water increases. Also, the size of the sugar molecule is greater than that of the salt molecule. Thus a single sugar molecule can attract more water molecules than the table salt leading to its faster dissolution in water.You should have noticed sugar had the highest solubility of all your tested compounds (about 200 grams per 100 milliliters of water) followed by Epsom salts (about 115 grams/100 milliliters) table salt (about 35 grams/100 milliliters) and baking soda (almost 10 grams/100 milliliters). Sugar dissolves in water because energy is given off when the slightly polar sucrose molecules form intermolecular bonds with the polar water molecules. The weak bonds that form between the solute and the solvent compensate for the energy needed to disrupt the structure of both the pure solute and the solvent. The reason for this is salt is an ionic compound, while sugar is a covalent compound. Ionic compounds generally have much higher melting points than covalent compounds. This is because to melt an ionic compound you have to weaken the ionic bonds between the ions.

Dissolving a solid in liquid, such as table salt in water, is a physical change because only the state of the matter has changed. Physical changes can often be reversed. Allowing the water to evaporate will return the salt to a solid state. If you can get back the substances you started the reaction with, that's a reversible reaction. A reversible change might change how a material looks or feels, but it doesn't create new materials. As reversible reactions include dissolving, evaporation, melting and freezing. Mixing of salt in water is a change that can be reversed by heating and melting of salt. Mixing salt in water is a change that cannot be reversed. If we dissolve a salt in water, the salt will dissociate into its constituent ions which means that some new substance is being formed. It is an irreversible process and there will be either change in temperature, energy, evolution of gas or precipitate formation.No volume of water does not reduce when you add salt the salt molecules will be upholder by water molecules between their gaps so, volume of water is neither increases nor decreases when salt is added. Adding salt (NaCl) to water actually does increase the volume a little bit, although by less than the volume of the added salt. The Na+ and Cl- ions fit nicely in the water, not taking up much room. When sodium chloride dissolves in water to make a saturated solution there is a 2.5 per cent reduction in volume. Saturated salt solution has a density of 1.202 g/ml. Ask students why they think saltwater is denser than regular water. Saltwater has a higher mass because of the added salt but still occupies the same amount of space in a container that regular water would, and hence is denser.

Dr Likhon chandra Roy thank you for your contribution to the discussion

Dr Jurgen Weippert thank you for your contribution to the discussion

The level of water does not change when salt is dissolved in water because the salt particles dissociate and occupy the intermolecular spaces between the water particles. Since only the empty spaces are occupied, the level of water does not increase. When common salt is dissolved in water, what will be the change in volume and why? There will be no change in volume as the salt gets into the spaces present between the water molecules. Adding salt (NaCl) to water actually does increase the volume a little bit, although by less than the volume of the added salt. The Na+ and Cl- ions fit nicely in the water, not taking up much room. The sodium chloride molecules will break down into Na+ and Cl- ions and be constantly collided by the water molecules, forcing it to spread out into a low concentration state. This is called diffusion. The volume of water of increase by the volume of the salt, theoretically. When salt is dissolved in fresh water, the density of the water increases because the mass of the water increases. When sodium is added to water, the sodium melts to form a ball that moves around on the surface. It fizzes rapidly before it disappears. Compared to the volume of the solution, or to the solvent, the volume of your solute is so tiny; at the same time, the solute will dissolve in your solvent. So the solute will not account to the volume of a solution. Back to the point, when we dissolve table salt, an ionic compound, in water, the water molecules break away from the hydrogen bonds to solvate the ions. This enables the water molecules to exist closer to each other and greatly reduces the space between water molecules, reducing the overall volume of the solution. When we crush a solid there is a greater surface area of the solid solute, meaning there are more collisions between the solute and solvent particles. More collisions mean the rate of dissolving is faster. This means the greater the surface area of a solute is the faster it dissolves. Crushing a solute helps to increase the rate of dissolving by increasing the surface area of the solute. If more solvent can come in contact with a greater amount of solute, the rate of dissolving increases.

Solid substances with greater surface areas dissolve faster than solid substances with smaller surface areas. In general, solids dissolve faster with increased temperature. The solubility of gas depends on pressure and temperature. When it comes to solid solutes, increasing the temperature will increase the rate of dissolving. As heat is added, the solute particles move around more, getting closer to the solvent molecules. This makes helps the solid dissolve faster in a liquid. The rate of dissolving depends on the surface area temperature and amount of stirring. The disjoining pressure of small particles is greater than that of large particles, so small particles have a higher interfacial solubility. Due to their higher differential concentration, thinner diffusion layer and increased surface area, small particles dissolve faster. When the total surface area of the solute particles is increased, the solute dissolves more rapidly. Breaking a solute into smaller pieces increases its surface area and increases the speed of the dissolving process. Yes, salt and other ionic compounds like it will dissolve faster the hotter the water it is dissolved in. This is because hot temperatures make atoms move quicker and the quicker they move, the easier they come apart. Surface area is larger when a given amount of a solid is present as smaller particles. Hence, the total surface area of the crushed salt will be more than that of the uncrushed crystals, resulting in higher rate of dissolving of the crushed salt in water. Agitation and stirring will increase the rate at which salt dissolves in water and increased movement of water molecules allow sodium ions and chloride ions to be pulled apart as shells of hydration are formed. As the surface area increases, the solute dissolves faster. Crystals of fine table salt have a greater surface area for the same amount of mass than large crystals of coarse sea salt. Thus fine table salt dissolves faster than the larger crystals of sea salt.

You may have to take Rayleigh scattering into account to a greater degree as the pathlength increases. Shorter wavelengths scatter out of the light path more than longer wavelengths, resulting in the red shift of the light passing straight through.

Sakshi Thakur

During the sol-gel method, the reaction between a metal precursor (e.g. metal alkoxide) and carbamide (urea) involves hydrolysis and condensation reactions. The metal precursor reacts with water to form metal hydroxide, while carbamide acts as a complexing agent to control the reaction. This results in the formation of metal oxide nanoparticles. For example, in the case of titanium isopropoxide as the metal precursor, the reaction can be represented as: Ti(OC3H7)4 + 4H2NC(O)NH2 + 6H2O → Ti(OH)4 + 4H2NCONH2 + 4C3H7OH. The carbamide helps in stabilizing and controlling the nanoparticle growth during the sol-gel process.

I think that is Drosophila melanogaster larvae.

Thanks to everyone who responded. i solved this problem It is true that all polyelectrolytes become swelling, but in my case, the problem was that I put in an excessive amount of initiator because I did not consider the strong intensity of my UV lamp. Therefore, this problem occurred because the correct cross-linked network was not formed within a fast reaction time and had a short chain.

These salts cost very little, and I would simply throw them out and buy new ones. If the issue goes away, great, If not, then you have narrowed down the options very quickly with little cost. You could also buy a bottle of sterile water to rule out some issue with your production system (I think you can have contaminants that do not affect the resistivity).

Have you tried to freeze-dried samples before extract DNA? Sometimes may help to extract DNA in tough samples. Phenol-chloroform extraction with a bead beating step is usually effective, although not recommended because of the toxicity of this chemicals.

Best

Carlo

Roy Cohen Thank you so much!

Zbigniew Jońca

I also wonder why it didn't use volumetric flasks in this procedure.

This procedure simply presented methods for weights.

Samsul Islam thank you for sharing the procedure.

My main concern is the acidic nature of the final solution that may affect the metal surface I will use for immobilizing my oligos.

Its 1,10- phenanthroline and 2-amino-5-methyl-1,3,4-thiadiazole ligand.

Due to the effect of diffusion layer on its salt form

Dear Dr. 圭圭 Li ,

I suggest you to have a look at the following, interesting document:

Corrosion of Copper Alloys in Consumer Electronics Environments

Anand V. Samant And Fritz C. Grensing

NACE INTERNATIONAL: VOL. 54, NO. 12

Available at: https://materion.com/-/media/files/alloy/article-reprints/materials-performance-dec15_pp-64-67.pdf

where Standard ASTM Methods were used and cited in Bibliography.

My best regards, Pierluigi Traverso.

Hi Genesis Marrero

Interesting observation! Based on your description, it seems like the crystals could indeed be salt precipitates. There could be several reasons for this, here are a few possible explanations. Media evaporation: If your cultures are not fully sealed or the incubator is not properly humidified, evaporation could cause the salts in the culture medium to become more concentrated over time. This might lead to precipitation, especially near cells which could act as nucleation points for crystal formation. Interaction with the disc material: Calcium phosphate could be reacting with components of the culture medium, leading to formation of insoluble salts. I hope these ideas help you in understanding and investigating this phenomenon further!

Dear Lorenzo,

I am VERY much wondering why HSQC is a problem.

Doing so you can estimate how many more scans it will take to have a signal substantially higher than noise.

All this is of course ONLY true for small molecules where relaxation can be neglected.

In our experience matching and tuning is NOT highly affected on 13C by high salt....

Goog luck

Alfred

Zhiling Luo

You, apparently, know the division of electrolytes into salting in and salting out. Salting agents are weakly hydrated, salting out agents are highly hydrated. The gel on the electrolyte acts similarly. The decrease in the solubility of the salt corresponds to the salting out of the electrolyte under the action of the gel and vice versa.

To measure Dissolved Organic Carbon (DOC) in saltwater, a commonly used and widely accepted methodology is the high-temperature combustion method using a Total Organic Carbon (TOC) analyzer. This method involves the following steps:

In continuation of Dr. Michael J. Benedik's suggestion, based on a similar experience I had, I recommend that if you do not have a clone, increase the incubation time (for example, instead of 18 hours t, 24 hours).

some times for some cases, it works.

@Joshua Depiver

Thank you for your kind answers!!

Could you give some more details about how you prepare the sample and do the calculation?

Because total soluble solids are increasing and increasing diffusion copolymerizatin step so that increasing refractive index g/dl(g/100ml).

There isn't a universally "standard" condition for hot corrosion tests as the parameters depend on various factors such as the materials tested, the specific experimental setup, the nature of the coatings, the specific research questions or industrial conditions being simulated, and the protocols followed by different research groups or industrial bodies. Hence, the variance in test conditions you observed in the literature.

However, the parameters you provided: salt deposit in the range of 0.3mg to 0.8mg/cm^2, temperatures of 920C or 970C, and duration between 250h to 300h, appear to be within common ranges for testing the hot corrosion resistance of thermal barrier coatings (TBCs).

Generally, the salt deposit simulates the salts encountered in actual service conditions (such as sea salt or impurities in fuel for aero engines), the temperature corresponds to the typical operating temperatures of gas turbines, and the duration is selected to provide a balance between accelerated testing and mimicking long-term service exposure.

Regarding the choice of best parameters, it depends on the specifics of your case:

Therefore, it would be best to consult your research advisor or a materials scientist with experience in TBCs and hot corrosion testing to determine the optimal test parameters for your specific situation. You should also thoroughly review the relevant literature and potentially conduct preliminary experiments to optimize your test conditions.

Hi Rehana

It would depende wich salt are you talking about and what are the conditions. For example, carbonate ion has been reported that enhance the degradation of methylene blue under LED light.

I am the exact opposite of you, I loss more proteins at low salt concentration.

1. Yes, There are several resources that can be used to determine whether a halophyte excludes or accumulates salt in its parts. These include:

eHALOPH: This is a database of salt-tolerant plants, including halophytes. It provides records of plant species that are tolerant of salt.

Scientific articles: Scientific articles can provide information on the mechanisms of salt tolerance in halophytes, including whether they exclude or accumulate salt in their parts.

Wikipedia: The Wikipedia page on halophytes provides information on the anatomy, physiology, and biochemistry of halophytes, as well as examples of halophytes and their salt tolerance levels

Overall, eHALOPH and scientific articles are likely to be the most useful resources for determining whether a halophyte excludes or accumulates salt in its parts.

3. Check in

www.intechopen.com With Zaffar Malik

You could enzymatically pretreat your agar to convert any sulphate into volatile H₂S which would be driven off during autoclaving.

Also are you using ultrapure agar (like the sort used for gel electrophoresis)?

Maybe you should use some sort of surface active compound like tween or triton for micelle formation. Because the substances you use are hydrophobic and in an aqueous solution, they will probably be well transferred with the help of micelles.

You could make it by mixing boric acid solution with NaOH until the desired pH is reached, assuming the desired pH is higher than the pH of the boric acid solution.

Here is a calculator for preparation of borate buffer at pH 8.5:

Water and mineral salts first enter through the cell wall and cell membrane of the root hair cell by osmosis. The root hairs small diameter and greater length makes sure that they have a large surface area over which to absorb water and mineral salts. Water fills the vacuole of the root hair cell. Epidermal cells secrete a waxy substance called cuticle, which coats, waterproofs, and protects the above-ground parts of plants. Cuticle helps prevent water loss, abrasions, infections, and damage from toxins.

Of course, all programs that are used to display crystal structures (like Jmol, Vest, Atoms, Diamond etc etc) will have a tool to measure the distance between a pair of atoms. Just look at the manual of the program you use.

Microstrip moisture sensor can be used to detect dissolved salt and sugar in liquid.

Ref: Wireless Personal Communications 122 (2022) 593-601

Yes!

pH is the negative logarithm of the concentration of H⁺: H⁺ = 10^-pH pH 2.75 = 0.001778279M

This is a good summary from OpenAI. Hope it helps!

"Removing salts from well water typically involves a process known as desalination. There are several methods you can consider, depending on the specific salt content and your requirements. Here are a few common approaches:

Reverse Osmosis (RO): Reverse osmosis is a widely used desalination method. It involves passing water through a semipermeable membrane that allows water molecules to pass through while blocking the majority of salt and other impurities. RO systems are effective in removing a wide range of salts and are commonly used for residential and commercial water treatment.

Distillation: Distillation involves heating the water to create steam, which is then condensed back into liquid form, leaving behind most of the salts and impurities. Distillation can be effective in removing salts, but it tends to be more energy-intensive compared to other methods.

Electrodialysis: Electrodialysis uses an electric current and a series of ion-exchange membranes to remove salts from water. The process involves separating the water into two streams, one with a higher salt concentration and the other with a lower concentration. Electrodialysis is commonly used in industrial applications.

Ion Exchange: Ion exchange involves exchanging undesirable ions, such as sodium or calcium, with more desirable ions, such as hydrogen or potassium. This method uses a resin bed that attracts and retains the unwanted ions, effectively reducing the salt content of the water. Ion exchange systems are commonly used for water softening but may not be as effective for high levels of salt removal.

It's worth noting that the choice of method depends on various factors, including the specific salts present, the volume of water, and your budget. Consulting with a water treatment professional or an environmental engineer would be beneficial to assess your situation and determine the most suitable approach for your well water."

Atmospheric circulation transports heat over the surface of the Earth that affects the water cycle, including the formation of clouds and precipitation events. The movement of air masses brings us our daily weather, and long-term patterns in circulation determine regional climate and ecosystems. Most of the world's deserts are located near 30 degrees north latitude and 30 degrees south latitude, where the heated equatorial air begins to descend. The descending air is dense and begins to warm again, evaporating large amounts of water from the land surface. The resulting climate is very dry. 30 degrees N & S Latitudes air sinks causing a drying effect and many deserts in this region and the Horse Latitudes because lack of wind caused sailors to become becalmed. 90 degrees N & S Latitudes: air sinks over the poles and moves equator ward. As the air leaves the equator, it rains away more moisture, becoming denser and slightly cooler, until finally dry, it sinks, creating the arid bands where many of the world's famous deserts lie. Salt crystallisation occurs in semi-arid environments, where the evaporation of water from rock surfaces leads to the crystallisation of salts. Crystallisation leads to a dramatic increase in volume which exerts pressure on the surrounding rock, and can eventually fracture the rock. Salt also works to weather rock in a process called haloclasty. Saltwater sometimes gets into the cracks and pores of rock. If the saltwater evaporates, salt crystals are left behind. As the crystals grow, they put pressure on the rock, slowly breaking it apart. Physical forces in the desert that break down rocks include the daily heating and cooling of rocks on the surface, expansion of plant root in cracks, the freezing and melting of ice in cracks, and exposure to wind and precipitation. While water is still the dominant agent of erosion in most desert environments, wind is a notable agent of weathering and erosion in many deserts. This includes suspended sediment traveling in haboobs, or dust storms, that frequent deserts.

Dear Dr. Aimal Khan These terminologies could be differentiated based on the outcomes of the process. Calcination is the decomposition of a substance at high temp (below melting point) releasing volatile components under limited or no air conditions. While thermal decomposition is the thermal breakdown of particular materials into different products (like oxidation).

I cannot think of any DNA measurement technique that would not be sensitive to protein and/or salt contamination. Cant you purify a few ul of your sample and measure DNA from that?

the different salts help precipitate the RNA but excess salts or other salts could inhibit downstream reactions.

this chapter explains it well

Definitely no. I suggest you follow the M+H adduct for SRM acquisition and not select the Na adduct for precursor selection. Na may reduce the MH signal intensity as per your observation. To clarify the NaCl adverse effects on your molecule ionization, additional experiments must be performed. I recommended several approaches above to find out the why ion quenching effect was experienced and during these experiments, I suggest preferring MH precursor if +ESI is in use and your molecule is convenient to form protonated pseudomolecular.

Sodium chloride, commonly known as salt , is an ionic compound with the chemical formula NaCl, representing a 1:1 ratio of sodium and chloride ions. With molar masses of 22.99 and 35.45 g/mol respectively, 100 g of NaCl contains 39.34 g Na and 60.66 g Cl. To make a 0.1M NaCl solution, you could weigh 5.844g of NaCl and dissolve it in 1 litre of water; OR 0.5844g of NaCl in 100mL of water OR make a 1:10 dilution of a 1M sample.Normal saline is 0.9% saline. This means that there is 0.9 G of salt (NaCl) per 100 ml of solution, or 9 G per liter. This solution has 154 mEq of Na per liter."Normal saline" is an aqueous solution of 0.9% NaCl. This means that normal saline can be prepared by measuring out 0.9 g of NaCl and diluting this amount of NaCl to a final volume of 100 ml's in water. This would be the same as diluting 9 g of NaCl to a final volume of 1 liter in water. They are parenteral solutions containing various concentrations of sodium chloride in water for injection intended for intravenous administration. For 0.45% Sodium Chloride Injection, USP, each 100 mL contains 450 mg sodium chloride in water for injection. Electrolytes per 1000 mL: sodium 77 mEq; chloride 77 mEq.

I reviewed clustering applied to the seawater intrusion problem around the world (10.1007/s12665-011-1299-y). I describe how this approach is used to support seawater intrusion identification. In the review, there was a case study in Tanzania, maybe you can check that article to look for similarities with respect to Mombasa. Also, this paper (https://doi.org/10.1016/j.jhydrol.2021.126844) is highly recommended for you.

You might be able to guess how much resin to use based on how much N(Bu)4 was left after you stirred it. Given the # of moles of resin you used and how much exchanged you could calculate a rough equilibrium constant for the exchange. From that you could figure how many exchanges were needed and size the column accordingly.

Thank you very much Bruce Neagle

In HPLC ligand exchange columns, the counter ion loss phenomenon occurs because the ligand on the column has a higher affinity for the analyte ions than for the counter ions in the mobile phase. As a result, the analyte ions can displace the counter ions on the column and bind to the ligand.

The mechanism of cation exchange in a ligand exchange column involves the competition between the counter ions in the mobile phase and the analyte cations for binding to the ligand on the column. When the analyte cations encounter the ligand on the column, they can replace the counter ions bound to the ligand through a process known as ion exchange. This process occurs because the analyte cations have a stronger affinity for the ligand than the counter ions.

It is important to note that cation exchange in ligand exchange columns can occur even with salt forms of the cations. This is because the salt form of a cation contains the cation itself and its corresponding counter ion. When the salt form of a cation is injected into the HPLC system, the cation can bind to the ligand on the column and displace the counter ions, even if the counter ion is the same as the one already on the column.

To prevent counter ion loss and subsequent column degradation, guard columns can be used to remove contaminants and protect the analytical column. Guard columns are typically packed with the same stationary phase material as the analytical column and are placed before the analytical column in the HPLC system. Guard columns can be replaced or cleaned more frequently than analytical columns, which can help extend the life of the analytical column.

Dear Sir you may try the protein separation with foam fractionation coloumn. it would suppose to help you

Elsewhere at this forum (*), I have presented a correlation for the density of NaCl aqueous solutions, with respect to both concentration and temperature dependency; and also another corrrelation for the molar saturating concentrations (C_sat) of those solutions (273 K ≤ T ≤ 373 K): Csat = 2.819686E-05·T2 - 1.530550E-02·T + 7.428573

(*) https://www.researchgate.net/post/How_can_I_dissolve_6_molar_sodium_chloride

Fateme Frootan if that didn't work with you then you can modify your chemical in defined media by using the model described in;

The effect of pH on decolorization of water treatment is positive, meaning that higher pH values lead to higher efficiency of color removal. However, this may depend on the type of dye and the treatment method used. The effect of dye concentration on decolorization is negative, meaning that lower concentrations of dye result in higher efficiency of color removal.

Hello Noor Ul Ain ,

Your copper nitrate trihydrate is a deliquescent salt, which means that it will absorb water from the atmosphere and eventually liquify. The only way to slow down this process is to store the bottle containing the salt in a sealed descicator backfilled with dry nitrogen gas. Every time you take out and open the bottle to use some of the salt, you should backfill the bottle with dry nitrigen gas before you screw the bottle lid back on and place the sealed bottle back in the descicator, which you refill with dry nitrogen gas.

Regards,

Tom Cuff

This is why a baiting medium is required. I have suggested for it based on my experience of isolating a variety of Bacillus organisms. Some plasticizers can be hydrolyzed by Bacillus organisms, especially thermophilic Bacillus species. Thermophilic Bacillus spp., are found in both. composts and from Landfill sites. In a broader sense, a landfill is similar to a composting site. Albeit, in a landfill the microenvironment is more anaerobic, again depending on the depth that is sampled.

Phosphate-buffered saline (PBS) buffer solutions are mixed Na/K monobasic and dibasic phosphate solutions with added Na/K chloride salts. The neutral salts (NaCl/KCl )do not contribute noticeably for the solution pH.

We can predict the pH of PBS buffer solutions after the following 'adapted' Henderson–Hasselbalch equation, within the effective buffer range pH = pK_a2 ± 1 (6.2―8.2):

pH = pK_a2 + log₁₀{(C_Na2HPO4 + C_K2HPO4)/(C_NaH2PO4 + C_KH2PO4)}

Here C refers to nominal (formal) concentrations of the salts in the mixed solution. K_a2 is the second dissociation constant of phosphoric acid.

You may want to check my post at this related query:

Calculating the nutrition solution volume for a hydroponic system depends on several factors, including the type of plants being grown, the stage of growth, and the size of the hydroponic system. Here are the general steps to calculate the nutrition solution volume for a hydroponic system:

It's important to note that these are general guidelines, and you may need to make adjustments based on your specific plants and system. Additionally, it's important to monitor the nutrient solution regularly to ensure that the plants are getting the nutrients they need and that the solution is not becoming too diluted or too concentrated.

I would think the easiest way would be to prepare it under an inert gas such as nitrogen. Perhaps prepare an initial solution at neutrality, bubble N2 through for a few minutes to de gas the solution. Provide a N2 cover and then add your excess ammonia.

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