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].
831
questions
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ʟ-Glutamine solubility in hot water
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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0answers
23 views
chemically extract sodium from a food for health purposes [closed]
Spirulina is a consumable algae with some benefits and only one downside I have noticed. according to my research 2,300 mg of sodium a day is way too much. 10 OZ. of spirulina contains just under 3,...
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5answers
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Why is the melting point of p-dichlorobenzene higher than those of o-dichlorobenzene and m-dichlorobenzene?
I was going through alkyl and aryl halides and noted the following statement in my textbook:
p-dichlorobenzene has higher melting point and solubility than those of o-dichlorobenzene and m-...
1
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0answers
39 views
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 ...
1
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1answer
108 views
How does a mostly non-polar molecule prevent a polar head from being pulled off by other polar molecules?
Linear-shaped molecules of a solute with a large non-polar section and a small polar head are not soluble in a polar solvent. Why is this? Why don't the attractive forces between a molecule of polar ...
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1answer
33 views
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 ...
1
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1answer
74 views
Are Hansen solubility parameters available for inorganic salts or ionic molecules?
Are Hansen solubility parameters available for inorganic salts or ionic molecules (e.g. potassium oleate, potassium stearate, sodium dioctyl sulfosuccinate (AOT), sodium dodecyl benzol sulfonate (SDBS)...
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1answer
242 views
Trends in solubility of group 2 nitrates
In my lab report, we are required to explain the trends in solubility of group 2 salts, going down the group. I had explained all of the trends except one, group 2 nitrates. The following is the data ...
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7answers
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The solubility of haloalkanes in water
Haloalkanes aren't very soluble in water because they can't form hydrogen bonds, and the energy required to break hydrogen bonds in water etc is higher than the energy released when new bonds between ...
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0answers
23 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.
1
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2answers
81 views
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 ...
0
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1answer
152 views
Solubility in wrong temperature?
I have a question on my chemistry homework that asks for the solubility of zinc oxide (ZnO) in water at 20 degrees celsius
I found the solubility, but in 30 degrees instead of 20
0.16 mg/100 mL
...
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0answers
39 views
Out of pyrrole and pyrrolidine,which is more soluble in benzene [closed]
Question:-
Out of pyrrole and pyrrolidine,which is more soluble in benzene.
Dipole moment values suggests that pyrrole has more polarity than pyrrolidine.So pyrrolidine should be more soluble in ...
10
votes
1answer
1k views
What substance has the lowest solubility product?
What substance has the lowest $K_\mathrm{sp}$ and what is its value? The lowest I could find is $2.6\cdot 10^{-124}$ for cobalt(III) sulfide $\ce{Co2S3}$.
5
votes
2answers
303 views
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 ...
3
votes
1answer
54 views
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 ...
5
votes
0answers
44 views
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 ...
3
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1answer
58 views
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 ...
0
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1answer
63 views
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 ...
5
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0answers
539 views
Why isn't orthoboric acid soluble in cold water even though it has polar B-OH bonds?
This is the information I found regarding orthoboric acid's solubility:
Textbook (NCERT India): Sparingly soluble in water (didn't say what temperature - presumably cold) and highly soluble in hot ...
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2answers
103 views
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 ...
0
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1answer
81 views
How to predict which complex is formed and which are soluble?
How does one come to know (in this table) which metal cations form ammonia complexes and which ones form hydroxy complexes on reaction with $\ce{NH4OH}$
Reference:
J.D Lee - Concise Inorganic ...
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1answer
45 views
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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1answer
56 views
Why are alkali metal compounds like sodium hydride or sodium amide strong bases but weak nucleophiles?
I understand why compounds such as $\ce{NaH}$ or $\ce{NaNH2}$ are weak nucleophiles: as they aren't very soluble in organic solvents, they react only on the clusters' surface. But why are they strong ...
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0answers
2k views
What is the difference between dissolution and absorption?
Let us first look at the definitions from Gold Book:
Absorption:
The process of one material (absorbate) being retained by another (absorbent); this may be the physical solution of a gas, liquid, ...
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0answers
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Purification of Glycine
I have a few Kg of Glycine with ~ 10ppm Heavy Metals, I'm wondering how I could conveniently purify all of it down to say < 1ppm Heavy Metals.
What would be the most efficient and convenient way to ...
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0answers
13 views
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 ...
2
votes
1answer
456 views
Predicting Ka/Kb values using values for solubility in water
Given that $K_\mathrm{a}$ values are determined by the position of equilibrium for a species such as $\ce{HCl}$ where $K_\mathrm{a} = \ce{\frac{{[H^{+}]}{[Cl^{-}]}}{[HCl]}}$, I was wondering whether ...
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1answer
56 views
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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4answers
2k views
Insoluble Group I/ammonium salts
Most solubility references (e.g. this one) say that there are "few" insoluble salts of alkali metals.
Are there any exceptions?
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3answers
6k views
Why is sodium carbonate less soluble in water than sodium bicarbonate?
Why is sodium carbonate less soluble in water than sodium bicarbonate? If you think about their structures, the only thing that is different is that sodium carbonate has two sodium atoms, while sodium ...
2
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2answers
71 views
Does K2CO3 react in minute amounts with glassware at higher temperatures?
At a temperature of $\pu{750 ^\circ C}$, $\ce{K2CO3}$ and $\ce{SiO2}$ react with each other in substantial proportions, forming $\ce{K2SiO3}$ and $\ce{CO2}$ in the process$\ce{^{[1]}}$.
We all know as ...
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1answer
76 views
Why does barium sulphate not dissolve in HCl while barium sulphite does?
Intuition tells me that the ionic bond in the sulphate must be stronger than that in the sulphite.
Is this true?
If it is then why? The charge on the barium ion is 2+ in both cases and the charge on ...
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1answer
82 views
Why does p-nitrophenol give sodium bicarbonate test, but o-nitrophenol does not?
Both ortho- and para-nitrophenol are less acidic than carbonic acid. But still paranitrophenol reacts with sodium bicarbonate to give carbonic acid and sodium paranitrophenoxide.
However, this is not ...
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0answers
34 views
What limits supersaturation in the absence of nucleation sites? [closed]
Imagine a scenario where we have a chamber with air that is supersaturated with water vapour. In this ideal scenario there are no nucleation sites (e.g no suspended particles or nucleation on the ...
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0answers
60 views
The most convenient process to purify Oxalic Acid up to a high level of purity
I am set out to purify a batch of commercial oxalic acid with the aim in mind to end up with a highly pure product (starting from $\pu{4,000 ppm}$ total impurities and doing so with basic lab ...
8
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1answer
111 views
Why is the water solubility of CO worse than that of CO2?
I tried my best to ask SciFinder, Google, and Google Scholar the wrong questions ...
I found many paper on the fitting of the solubility to some equations to be able to calculate the amount of $\ce{CO}...
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2answers
1k views
Why is dichloromethane immiscible in water?
We know that like dissolves like. And dichloromethane is a polar solvent and water is also a polar solvent. Also there ought to be a strong hydrogen bonding between the chlorine and hydrogen atoms. So ...
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2answers
62 views
Solubility of Organic Compound confusion
My teacher wrote the following on the board today:
A solute will only dissolve if the energy required to break the bonds
in the solute and solvent is less than the energy released from the
...
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0answers
830 views
Solubility of Aluminium Halides by Fajans rule
According to Fajan's rule polarizability of anion is directly related to the size and hence the covalent character would be more.
Now going by this definition aluminium chloride having greater ...
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1answer
54 views
Using solubility product to determine the mass of the precipitate of a reaction
I mix together $\pu{100 mL}$ of an aqueous $\ce{NaCl}$ solution at $\pu{0.5 M}$ and $\pu{100 mL}$ of an aqueous $\ce{AgNO3}$ solution at $\pu{0.3 M}$. Assuming that the solubility of $\ce{NaCl}$ in ...
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0answers
31 views
Why does solubility of Carbonate salts of Alkali metals in water increase down the group?
Carbonate salts have a very large anion so hydration energy should dominate over lattice energy. Since hydration energy is inversely proportional to radius of ion, I would expect Lithium to release ...
4
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1answer
167 views
Can ionic compounds dissolved in organic solvent conduct electricity?
Ionic compounds dissolved in water, as an aqueous solution, can conduct electricity.
Can they conduct electricity if they are dissolved in organic solvent?
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1answer
133 views
Does CO2 dissolve in water?
First of all not a homework question, but one day it suddenly popped into my head while opening a bottle of soda and accidentally leaving a glass out for a while.
I get that $\ce{CO2}$ in water is not ...
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3answers
1k views
Understanding the solubility of Ca(HCO3)2
According to wikipedia $\ce{Ca(HCO3)2}$ has the following solubility values:
$\pu{16.1 g/100 mL} \,(\pu{0^\circ C)}$
$\pu{16.6 g/100 mL} \,(\pu{20^\circ C)}$
$\pu{18.4 g/100 mL} \,(\pu{100^\circ C)}...
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3answers
2k views
Solubility Product and Buffers
The ionization constant of benzoic acid is $6.46 \times 10^{-5}$ and solubility product for silver benzoate is $2.5 \times 10^{-13}$. How many times silver benzoate is more soluble in a buffer of $\...
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0answers
29 views
Chemical that will dissolve the oils left over from broken down coffee grounds?
When coffee grounds breakdown in pipes there is a black sludge residue as a result. Is there a chemical that would dissolve this residue?
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2answers
70 views
How to calculate mass of calcium fluoride that will dissolve in sodium fluoride solution?
The solubility product of calcium fluoride, $\ce{CaF2},$ is $\pu{1.46E-10 mol^3 dm^{-9}.}$
What mass of calcium fluoride will dissolve in $\pu{500 cm^3}$ of $\pu{0.10 mol dm^{-3}}$ sodium fluoride ...
1
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1answer
11k views
What is the reason for the different solubility of silver halides in ammonia?
According to my knowledge, I know that $\ce{AgCl}$ dissolves in dilute ammonia, $\ce{AgBr}$ dissolves in concentrated ammonia and $\ce{AgI}$ does not dissolve even with concentrated ammonia.
What is ...
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1answer
67 views
Qualitative Analysis- Distinguishing between two ions or two salts [duplicate]
I know my question is going to be quite below the level of this site but I am 1st grade in university and I can't understand anything.
I am going to give an example from the book: distinguish ...
