All Questions
Tagged with aqueous-solution acid-base
43
questions
10
votes
3
answers
12k
views
How to set up equation for buffer reaction?
For buffer equations, how can you tell what to react with water?
For example, if I have a 1 M acetic acid solution and 1 M sodium acetate solution (a conjugate acid-base pair) mixed together and am ...
- 109
9
votes
4
answers
4k
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Why does the inverse relationship between the strengths of an acid and its conjugate base appear to be violated in the case of chloric(I) acid?
Hypochlorous acid is a weak acid with $\mathrm{p}K_\mathrm{a}(\ce{HClO}) = 7.53$. Then why is its conjugate base, $\ce{ClO-}$, a weak base in water? Shouldn't the strength of the base be inversely ...
- 205
13
votes
2
answers
10k
views
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
7
votes
3
answers
50k
views
Is magnesium sulfate basic, neutral or acidic?
A question in my college test was whether $\ce{MgSO4}$ is neutral, acidic or basic. I was told to solve this kind of problem by hydrolyzing any ions that do not "come from" a strong acid or a strong ...
8
votes
2
answers
8k
views
Is there a difference in the reactions of a dilute acid and a concentrated acid?
All of the exams that I've sat so far, and the homework questions I've had, always ask for the reaction between a substance and a dilute acid. Is there a difference in the reaction between a dilute ...
- 389
4
votes
1
answer
1k
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How do I quantify the carbonate system and its pH speciation?
I did Environmental Water Chemistry as part of my undergraduate course where we quantified pH-speciation for the full carbonate system and I got it right according to my tutor. My speciation profile ...
- 500
2
votes
2
answers
10k
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Why is potassium phosphate KH2PO4 in this reaction?
This is a continuation of this question because the first thing that came in my mind is that why potassium phosphate in this reaction is $\ce{KH2PO4}$ and not $\ce{K3PO4}$?
In the wikipedia article ...
- 26.3k
26
votes
4
answers
3k
views
What software can calculate aqueous solution equilibria?
What software is available out there to calculate the equilibrium in a set of reactions in aqueous solution? In particular, I'm interested in software general enough to simulate things like titration ...
- 23.8k
23
votes
3
answers
3k
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Is "Sulfuric acid... makes a poor electrolyte... very little of it will dissociate into ions" really true? What does that actually mean?
While researching chromate conversion coating for edits to this answer in Space Exploration SE, I came upon the following passage in Corrosion Resistance of Stainless Steel to Sulfuric Acid
Sulfuric ...
- 5,900
18
votes
4
answers
54k
views
How much can the pH change through dilution?
Consider an acidic solution with Hydrogen ion concentration, $\ce{[H+]}$ of $10^{-5}\:\mathrm{M}$. Since $\:\mathrm{pH} = -\log \ce{[H+]}$ the $\:\mathrm{pH}$ of solution is $5$. Suppose we dilute ...
- 299
10
votes
1
answer
635
views
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 ...
- 247
7
votes
1
answer
4k
views
Aspirin Hydrolysis at pH 2
Conducting an experiment, I found that very little salicylic acid was evolved performing hydrolysis at $\mathrm{pH \ 2}$ and at $\pu{45 ^\circ C}$. In fact, far more salicylic acid was evolved at $\...
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5
votes
2
answers
3k
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Calculating approximate pH of polyprotic acids
When I took up ionic equilibria and titrations after a long break, I found it hard to solve the questions regarding pH calculations of polyprotic acds. Consider these two questions as examples:-
...
- 6,795
4
votes
1
answer
9k
views
Is there a difference between ‘ammonium hydroxide’ and ‘aqueous ammonia’?
Water ($\ce{H2O}$) can be added to ammonia ($\ce{NH3}$) in order to form ammonium hydroxide ($\ce{NH4OH}$):
$$\ce{NH3 + H2O -> NH4OH}$$
But we know that ammonia is gaseous at STP so writing $\ce{...
- 636
4
votes
1
answer
1k
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Can acid-base reactions occur in a non-aqueous medium?
To better illustrate my question, allow me to refer to the case of ammonium chloride, formed through a classic acid-base reaction.
The reaction between ammonia and hydrogen chloride to give ammonium ...
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