Questions tagged [solubility]

For questions related to the solubility of compounds in various solvents, especially in water. Do not confuse with [solutions] or [aqueous-solution].

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A problem regarding solubility and concentration

A solution is $\pu{0.10 M}$ $\ce{Ba(NO3)2}$ and $\pu{0.10 M}$ $\ce{Sr(NO3)2}$. If solid $\ce{Na2CrO4}$ is added to the solution, what is the $\ce{[Ba+]}$ when $\ce{SrCrO4}$ begins to precipitate? $\...
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Are aqueous solutions soluble in water?

Are already existing aqueous solutions (eg. NaCl in water) soluble in water? Since the solute is already broken up into ions, it shouldn't be, right?
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Solubility of d -block metal salts

Which d-block salts are usually insoluble in water at room temperature? I know that generlly sulphides , hydroxides and oxides of d -block metals are insoluble but I want to know more acidic radicals ...
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Dissolving Polystyrene with D-Limonene

I have a product, which according to the MSDS is mostly D-Limonene. I don't have the means to chemically test it, but I did try dissolving polystyrene with it. Before I come check it again, should I ...
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Deposition of saturated solution and affect of evaporated water

20g of water is evaporated from 200g of saturated solution of KNO3(aq) at 60°C by heating and the solution was cooled to 20°C. How many grams of KNO3 were deposited? The solubility of KNO3 in 100g of ...
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Effect of water vaporation on saturated solution

At a high temperature, water is evaporated from the saturated solution by heating. What is the solution losing exactly by the fact that the water left the saturated solution? Does it affect its ...
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Deciding whether a precipitate would be soluble in water or not by calculation (problem solving) [closed]

This question is purely mathematical, I just could not understand how to approach it. (For reference the question mentions that compounds with solubility higher than 1 mol/L are soluble and insoluble ...
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Weak acids, aluminum and silver

I'm curious what weak acids will form soluble salts with aluminum, but not silver. From a solubility chart, $\ce{HCl, HBr}$ and $\ce{HI}$ will form soluble aluminum salts, but not with silver; however,...
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Solubility of potassium silicate in water

It is somewhat surprising to me that there is almost no data about solubility of potassium silicate in water under normal conditions. The only thing I was able to find is the following: <0.336 g/L ...
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57 views

Are all mixtures linear?

I'm writing a computer program to help a factory produce bottles of mixtures. A mixture is usually alcohol, water and some other stuff, like menthol. But could also be water and NaOH and some oils (...
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Does #4 LDPE Plastic Bottle Leach into Water?

I understand that Water Bottles expire due only to the fact that the plastic can degrade over time and leach into the water making the water's taste not as desirable as the manufacturer might intend. ...
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Is it possible to make a solution of zinc oxide in a high school chemistry lab?

As part of my IB Chemistry curriculum, we are required to conduct our own experiment researching our own question. I'm in the preliminary research phase and wanted to conduct an experiment looking at ...
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Student Question regarding molecular van der Waals volume and Polarizability

I would like to request a crosscheck of my understandings regarding molecular van der Waals volume and polarizability. Please have a look through my statements about these 2 concepts below and point ...
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51 views

How does chromium behave in a carbonate solution? [closed]

I'm wondering how chromium (as a metal or as a salt) behaves in a concentrated carbonate solution. Will it form any, one or several carbonate specie(s)? Will the metal solubilize? How does it affect ...
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Why does increasing charge density matter more for the hydration enthalpy compared to the lattice energy?

For the solvation of ionic salts, if we look down a group, say Group II, and we keep the anion constant, we find that the solubility decreases going down the group. This is because the hydration ...
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I need help finding several immiscible liquids [closed]

I am trying to fill a vial with as many immiscible liquids as possible so that they form many separate layers. I want to do this as a way to visualise how liquids with different refractive indexes ...
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33 views

NaHCO3 decomposition dynamics and extent vs Temperature

I'm wondering approximately how fast and to which extent $\ce{NaHCO3}$ will decompose (to $\ce{CO2}$ and $\ce{H2O}$) at $50$, $60$, $70$, $80$, $90$, $100$, $110$, $120$, and $\pu{130 ^\circ C}$. It ...
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76 views

Are all gases equal in their ability to carry with them lower volatility matter at a given temperature? [closed]

As we all know water is a great solvent in it's liquid form relative to other substances. I wonder however how it performs as a gas relative to other stuff. Does anyone know how well steam carries ...
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How does a shock, such as the snap of the disk in a reusable hand warmer, trigger the re-crystalization of a supersaturated solution?

Reusable handwarmers are made of something dissolved nearly to its saturation point in hot water (Sodium Acetate in the case of HotSnapz) at a high temperature, and then cooled to a temperature at ...
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How can I solubilize fragrance oil into polyvinyl acetate/clear glue?

I'm a highschool student who makes slime for fun, using PVA glue and Borax as my main ingredients. Earlier, I had the idea of adding fragrance oils to clear glue. However, because they aren't soluble, ...
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Solubility Product, and it's relation to solubility

In order to remove temporary hardness of water, it is boiled. On boiling, while Ca(HCO3)2 gives CaCo3(ppt.) , Mg(HCO3)2 gives Mg(OH)2(ppt.). According to my book precipitation of Mg(OH)2 occurs due to ...
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47 views

Is an aqueous solution of potassium bicarbonate acidic or basic in nature?

The following is the definition of an acid salt according to my textbook: The salts formed by the partial replacement of the replaceable hydrogen atoms (H+ ions) of an acid molecule by a metallic or ...
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How long will it takes two miscible liquids to fully mix (homogenize) through diffusion?

This question occurred to me while I was pouring milk into my coffee and was too lazy to stir. Assume you have some volume $V_a$ of liquid A directly on top of another volume $V_b$ of liquid B. The ...
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Comparison of the solubility of lead(II) iodide in water and in lead(II) nitrate solution [closed]

Solubility of $\ce{PbI2}$: Is $\ce{PbI2}$ more soluble in $\ce{H2O}$ or in an aqueous solution of Lead(II) nitrate? $K_\mathrm{sp} (\ce{PbI_{2}})=8.7\times 10^{-9}$ I'm not very good in Chemistry, I ...
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Zinc salt with a very high relative aqueous solubility?

Zinc bromide, iodide, and chloride are highly soluble in water, both in absolute terms, and relative to other metals. I think however that there is a zinc compound with even higher relative aqueous ...
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Hydrogen bonding in sugar acids

I recently learnt that the reason for low solubility of mucic acid as compared to glucaric acid was more hydrogen bonding in the crystal state of mucic acid as compared to glucaric acid. I would ...
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Comparing the solubility of glucaric acid and mucic acid

Why is glucaric acid soluble in water but not mucic acid? The chemical formulae seem to be the same so why is it that one is more soluble than the other?
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Effect of pressure on gas solubility in liquids

By Henry's Law ($K=\frac{x}{p}$), we know that increasing the partial pressure of a gas also increases its solubility on liquids. Now a lot of sources (this, for instance) illustrate this by ...
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77 views

Why are amino acids least soluble at isoelectric point?

At isoelectric point amino acids exist as zwitterions. As a molecule it is electrically neutral, but still has a positive and a negative charge. Then why are amino acids still least soluble at ...
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48 views

Do solid insoluble ions react with soluble ions in aqueous solution? [closed]

Do solid and insoluble ions (like aluminium phosphate) react with soluble ions in aqueous solution (like potassium sulfate)? When would a solid ion react with an ion in aqueous solution in general?
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Adding a base and a salt to a hydrated complex

The question goes like this: $\ce{Fe(NO3)3}$ V= $\pu{1 liter}$ and $\ce{[Fe(NO3)3]} =\pu{0.1 moles/liter}$. Calculate the $\mathrm{pH}$ of this solution using the values of $K$ given. We add a solid ...
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Controlled burn with colored flames (Gender Reveal) [closed]

Is there a single solvent that can dissolve chemicals/elements that when burned, will produce the color of its respective chemical/element? If so, what chemical/element can be dissolved in this ...
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How likely is it for monocalcium phosphate to spontaneously convert to dicalcium phosphate?

I'm trying to make liquid fertilizer by dissolving triple superphosphate (TSP) into water. TSP is supposed to be $\ce{Ca(H2PO4)2·H2O}$, which is quite soluble in water ($\pu{2g/100mL}$). The ...
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How does the solubility of hydrated ions differ from unhydrated ions?

So the hydrated compound I am thinking about specifically is pentahydrate copper sulphate. I know when you put ionic compounds in water, the ions because hydrated by the water molecules. However, what ...
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Creating 100mg/L aspirin solution

I plan on creating 100 mL of 100mg/L aspirin solution by dissolving 10 mg of pure aspirin powder in 100 mL of buffer solution (of different pHs). Problematically, aspirin doesn’t tend towards ...
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Is there a way of finding solubility/solvent from basic information? [closed]

Let's say I have a compound and I want to find a solvent for it. Looking on some where like Wikipedia, it is quite easy to find solubility, in various solvents for common compounds. However it can be ...
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ʟ-Glutamine solubility in hot water [closed]

What happens when you try to dissolve ʟ-glutamine in hot water (above 80 °C)? Does the heat destroy the ʟ-glutamine?
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Why does the solubility of haloalkanes in water decreases as the length of the carbon chain increases?

Due to the polar halogen-carbon bond in haloalkanes, they are more soluble than hydrocarbon in water. But the solubility is still very low because the overall influence of the dipole-dipole ...
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Effects of evaporating the solvent of a supersaturated solution

What happens to the solute if you heat up a supersaturated solution? Since a supersaturated solution is already more than saturated with solute and unstable, my theory is that as you heat the ...
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1answer
46 views

Water solubility comparison of stereoisomers of bicyclo [4.4.0] decane-3,4-diol

I think, (I) must be more soluble in water. It is due to trans configuration and thus, forming more effectively inter-molecular hydrogen bonds with water molecules.
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What is the physical explanation driving current flow in a concentration cell?

In a galvanic cell, current is driven because the species at the cathode is reduced by grabbing some electrons from the cathode. The cathode now lacks electrons so it pulls them from the anode. Now ...
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Solubility of ortho- and para-nitrophenol in benzene

Which one between o-nitrophenol and p-nitrophenol is more soluble in benzene? And what is the reason? If the solvent had been polar, hydrogen bonding would have provided a lot of explanation, but what ...
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Alkoxide metathesis

I am attempting a synthesis for acetylacetone. The preparation I wish to carry out is described on orgsynth by condensation of acetone and ethyl acetate with a base catalyst. The problem for me is ...
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What acids, solvents is lithium-6 fluoride soluble in (other than HF)?

$\ce{LiF}$ is quite insoluble in water, and I'm trying to use some water-soluble acid or solvent to dissolve $\ce{^6LiF}$ (95% enriched) in. I'm not a chemistry person, I'm a radiation detection ...
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Amine vs Amide Solubility

I had a question regarding the solubility of amines and amides. I was looking into the solubility of butanamide and n-Butylamine, and it turns out that whilst butylamine is miscible in water, the ...
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Caustic and Toxicological Determination [closed]

I need to determine whether or not a product that I am importing is "toxic" and or "corrosive" as defined below. But I am a chemistry n00b — that is to say I have virtually zero ...
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How can magnesium hydroxide be a strong base and be sparingly soluble at the same time?

A strong base means it completely dissociates forming $ OH^- $ ions when added to aqueous solution. Sparingly soluble means it dissolves very little when added to aqueous solution. Yet magnesium ...
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1answer
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The Solubility of Tyrosine

I find very little data on the solubility of tyrosine, other than that it has a very low solubility at room temperature for an AA. (1) Does anyone know different ways to dissolve fair amounts of it in ...
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Free Energy vs. Common Ion Effect in Ultrapurification

I'm wondering which of the two phenomenae grows in importance and which one becomes irrelevant when the proportion of impurities in a product being purified become increasingly small: The common ion ...
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Why can’t I use solubility product for normally soluble compounds?

Solubility product only applies to sparing soluble ionic compounds (chemguide) I read this in a website. But I don’t see what this should be the case. Taking $\ce{NaCl}$ for example, there’s an ...

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