All Questions
Tagged with aqueous-solution solubility
28
questions
30
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Why do salts such as NaCl dissolve?
If we look at solubility of salts in water, we are told that they disassociate, because the positive $\ce{Na}$ ion is attracted to the partially negative oxygen in water and the negative $\ce{Cl}$ is ...
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9
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1
answer
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Vapor pressure of immiscible liquids
I have read that vapour pressure of a mixture of two immiscible liquids is
$$P=P^0_A + P^0_B$$ where A and B are immiscible liquids.
If they are immiscible, they would form separate layers. Thus ...
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29
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1
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Are all NO3- salts soluble in water? If so, why?
All the examples of $\ce{NO3-}$ salts are soluble in water (all that I know about).
Is it always so or there is some salt which doesn't dissolve in water?
If so what is the reason behind it?
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28
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7
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Why is silver chloride less soluble than silver nitrate?
Related: Reaction between silver nitrate and aluminum chloride
Experimentally, $\ce{AgCl}$ is insoluble in water, but $\ce{AgNO3}$ is soluble. They're pretty common in a lab (well, $\ce{AgCl}$ is a ...
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Why do some solid chemicals dissolve better in colder water?
I just discovered that some solid chemicals, such as $\ce{Na2SO4}$, dissolve better in cold water than hot water from here and would like to know if there is any particular reason as to why. Is it ...
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2
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Why does solubility of solids sometimes decrease with temperature increase?
Recently I was researching $\ce{Ca(OH)_2}$, and I found this on Wikipedia:
\begin{array}{|c|l|}\hline
{\rm \color{blue}{Solubility~in~water}}
& {\mathrm{0.189\,g/100\,mL}\ (0\,^\circ\mathrm{...
- 4,197
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votes
1
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Formation of MnO2 vs [Mn(H2O)6]4+ in aqueous solution
I am looking for reasons why $\ce{Mn(IV)}$ wouldn't be stable as a hydrate. I know that from standard reduction potentials it exists as a ppt of $\ce{MnO2}$, but what is stopping it from being a ...
- 1,120
5
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1
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How can an insoluble compound be a strong electrolyte
Here's a quote from Petrruci General Chemistry (pg. 160):
Silver chloride, $\ce{AgCl}$ is an insoluble ionic compound. When $\ce{AgCl}$ dissolved in water, it is 100% dissociated into $\ce{Ag}^+\text{...
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24
votes
4
answers
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Can other substances be dissolved in a saturated solution?
If I have a liter of water fully saturated with sucrose would it be possible to dissolve something like salt or any other substance in the water? Or when the solution is saturated, is it impossible to ...
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10
votes
1
answer
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How to derive the conductivity titration curve which accounts for salt formation
I derived an equation that gave me the volume of base required to get a certain $\mathrm{pH}$:
In a titration between a weak acid $\ce{HA}$ and weak base $\ce{B}$ (adding base into acid solution) the ...
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9
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3
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Why is there a decrease in the total volume when NaOH dissolves in water?
When a solute is added to a solvent, the volume of the solution should be equal to the sum of the individual volume of the solute and solvent (i.e total volume), right? But why is there a decrease in ...
- 299
2
votes
2
answers
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Do strong acids actually dissociate completely?
Do strong acids actually dissociate completely (every single molecule dissociates), or are they just assumed to do so for the sake of simplicity? That seems odd, considering weak acids, many of which ...
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12
votes
3
answers
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Differentiation between zinc, aluminium, and magnesium ions in solution
If I have three aqueous ionic solutions in which I know that the cation is $\ce{Al^3+}$, $\ce{Mg^2+}$, or $\ce{Zn^2+}$, how do I find out which is which?
I was thinking to add $\ce{OH-}$ in the form ...
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Why aren't the copper(II) ions in CuSO4 precipitated by hydroxide ions from water?
From my own experience and literature, I know that $\ce{CuSO4}$ is well soluble in water and dissociates into $\ce{Cu^2+}$ and $\ce{SO4^2-}$. $\ce{Cu(OH)2}$, however, is not: $K_\mathrm{sp} = 2 \cdot ...
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Will this reaction form magnesium carbonate?
I have magnesium oxide pills I take. I know if I dissolve them they'll form magnesium hydroxide, and I'm trying to make pure magnesium from my pills. I've come up with a double replacement reaction, ...
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