All Questions
Tagged with solutions aqueous-solution
29
questions
30
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3
answers
30k
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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 ...
- 3,479
13
votes
2
answers
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Should bromine water be called a solution?
Bromine water is a reagent which is used to test for unsaturation in organic compound. It is $2.8~\%$ bromine in water. In many places, it is refer to as bromine solution.
But it is observed that ...
- 26.3k
19
votes
3
answers
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Why there is no change in water level when salt is added?
Let us say we have one glass of water and after that when we add one or two spoon of salt then we notice that salt dissolves in it but when we measure the water level we found that there is no ...
- 1,491
9
votes
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 ...
- 153
7
votes
1
answer
2k
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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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5
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3
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Can there be more solvent in a solute?
Something I know that leads to this question:
Water dissolved in ethanol.
It might sounds weird to say water as a solute. Textbooks always says that solvent is the one present in larger quantity. ...
- 2,688
28
votes
5
answers
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Why is water "the universal" solvent?
This is an old question that our textbook tried to answer but worsened the situation.
Many things are soluble in water. So many, that studying solutions will always require studying aqueous ones. It ...
- 10.7k
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 ...
- 371
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
8
votes
2
answers
2k
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Is there a soluble salt, or compound that when dissolved in water results in a solution with density less than pure water?
Generally water soluble salts tend to 'fit between' the molecules of water such that the volume of the resulting solution does not increase much relative to the volume and added mass of the salt. So ...
- 2,773
2
votes
3
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2k
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Saturated vs Supersaturated
The way I was told is that a saturated solution contains the maximum amount of solute and a supersaturated solution contains more solute than a solution can hold at a particular temperature. But I was ...
- 95
1
vote
2
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448
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Does adding solutes to water alter its triple point? [closed]
Does adding solutes to water alter its triple point? If yes, how do we find the new temperature and pressure of this point?
- 153
12
votes
3
answers
38k
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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 ...
- 223
11
votes
1
answer
20k
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Why do some substances ionize instead of dissolving in water?
My question can also be understood as
what make something electrolyte or nonelectrolyte?
I think this question stems mainly from my confusion with the definitions of ionizing and dissolving.
...
- 2,688
10
votes
2
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Are all solutions of weak acid/bases buffers?
I am having a difficult time understanding what makes a buffer a buffer.
Buffers in my textbook are defined as a solution of a weak acid or base and their conjugate acid/base. So if I were to just ...
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