All Questions
Tagged with ionic-compounds solubility
46
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How to determine the dynamic of progression of two simultaneous precipitation (double replacement) reactions? [duplicate]
We have a solution of mineral water with potassium chromate added to it, and want to titrate the chloride ions in the mineral water. We were told to use silver nitrate for this, which would produce ...
4
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1
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290
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What factors cause a few sodium salts to be water-insoluble?
We know that almost all salts with sodium as cation are water-soluble. But there are a few examples where the salt is water-insoluble; such as sodium bismuthate, sodium fluorosilicate, and much more.
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Solubility of SrF2 in aqueous solution of NaF
This might be really simple question but I have no idea how to proceed to solve such kind of question.
The solubility product of $\ce{SrF2}$ in water is $\pu{8E-10}$. Calculate its solubility in 0.1M ...
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Confusion related to exception in Fajan's rule (Regarding prediction in solubility of compounds in polar solvents)
My teacher taught us that higher the ionic character in a compound, higher is its solubility in polar solvents like water.
To illustrate this statement, he also gave us the following example-
LiOH< ...
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-1
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1
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Is lead iodide a strong electrolyte?
So, lead iodide is insoluble. I see conflicting answers online. Some say it's a weak electrolyte because it is insoluble, others say it is a strong electrolyte because it is an ionic compound and any ...
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2
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Why is the Conductivity trend same in fused and in dissolved or aqueous state of ionic compounds?
For an example if we take $\ce{KCl}$ and $\ce{NaCl}$ then I have understood the part where in aqueous state $\ce{Na+}$ becomes bigger than $\ce{K+}$ hence the conductivity reverses but in fused state ...
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1
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Isn't my book doing this problem about ionic product wrongly?
Problem:
After adding a $\pu{150 mL}$ $\pu{6.7\times10^{-5} M}$ $\ce{NaOH}$ solution to a $\pu{100 mL}$ $\pu{2.5\times10^{-5} M}$ $\ce{FeCl2}$ solution, green colored $\ce{Fe(OH)2}$ precipitate is ...
user60158
7
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Why is it advised to use neutral ferric chloride solution while performing confirmatory test for acetate ions? [duplicate]
The reaction of $\ce{FeCl3}$ with $\ce{CH3COO-}$ is
$$\ce{3Fe^{+3} +6CH3COO- +H2O<=> [Fe3(OH)2(CH3COO)6]^{+} +2H^{+}}$$
Recently I read that a solution of $\ce{FeCl3}$ hydrolyses very quickly to ...
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2
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Why are entries missing on a solubility data chart for ionic compounds? [closed]
There is a solubility chart in my college chemistry class text for "Solubility of Ionic compounds in water". I have copied and pasted image of chart below. I was surprised to find a dozen ...
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5
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Why does the dissolution of calcium hydroxide have a negative entropy?
We had an experiment on the dissolution of calcium hydroxide and we obtained the experimental entropy value $\pu{-203 J mol^-1 K^-1}$ with a percent error of $26.7\%.$ Doesn't dissolving a solid in a ...
2
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2
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Is ionisation an equilibrium process?
I read in a page that ionisation is an irreversible process. But, as equilibrium is always reversible would that mean equilibrium does not involve ionisation process.
And than dissociation is a ...
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5
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352
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Why does beryllium have an exceptionally high hydration energy?
You would expect solubility of Group $2$ fluorides to increase down the group, as lattice energy plummets much more sharply than hydration energy does. For the most part, this is true: $\ce{BaF2}$ is ...
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4
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Are Group 2 metal fluoride salts less soluble in organic solvents than Group 1 fluorides?
It is clear that Group 1 metal fluoride salts DO NOT readily form solutions in organic medium. The amount of solvation that can occur leading to the eventual release of a fluoride ion depends on many ...
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Dielectric constant for gases possessing van der Waals forces [closed]
I've learnt that water can dissolve ionic bonds because it possesses a high dielectric constant.
In the cases of covalent compounds (especially the non-polar covalent compounds), where the molecules ...
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2
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Order of solubility of sodium halides and potassium iodide
Order the following ionic compounds in decreasing order according to their ease to dissolve in water.
a) NaBr; b) KI; c) NaF; d) NaCl.
d > a > b > c
a > b > c > d
b > c > d &...
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