All Questions
75
questions
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Trichloroacetic acid aqueous solution
I have bought some anhydride of trichloroacetic acid (TCA) and would like to prepare an acidic solution. My problem is, that I don't know how much "powder" to mix with how much water to produce an x% ...
- 197
-1
votes
1
answer
3k
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Calculate pH at equivalence point [closed]
Calculate the pH at the equivalence point of a titration of 62 mL of 0.1 M $\ce{CH_3NH_2}$ with 0.20 M HCl. The $\ce{K_b}=4.4\cdot10^{-4}$.
At the equivalence point, the moles of CH3NH2 equals the ...
0
votes
0
answers
1k
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Will hydrogen chloride dissolved in ethanol react with magnesium?
Magnesium will react with aqueous HCl to form magnesium chloride and hydrogen gas. Simple. But I've just read in my textbook that HCl in a solution of ethanol no reaction will take place. There is no ...
- 165
4
votes
4
answers
4k
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Why does the degree of dissociation change when we dilute a weak acid even though the equilibrium constant is constant?
$K$ represents the ratio of concentrations of molecules in a solution at equilibrium, which means that $Q_\mathrm{r}$ (that ratio at any given point) looks to be identical to $K$. In other words, the ...
-1
votes
2
answers
174
views
Wouldn't adding a proton acceptor still make a solution just as acidic?
Say if you add NH3 to a solution, and it accepts a proton, it still becomes NH4+ in a solution, which is also acidic. A base should decrease the hydrogen ion concentration in a solution, but how does ...
-1
votes
2
answers
1k
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Calculate pH of a mixture of a strong base and acid. Knowing only the pH, wt/v%, and volume of both solution. [closed]
Title explains all. I have been stuck on this for an hour and for some reason cannot understand it. I have tried to do an ICE table but get stuck halfway as I do not know whether I would use the w/v ...
1
vote
2
answers
6k
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Buffer Solution with Strong Acid?
I was thinking: Could we could make a strong acid-strong base buffer solution? Take, for instance, a mixture of 1 L $\ce{HCl}$ (0.1 M) and 1 L of aqueous salt, $\ce{Na_2SO_4}$ (also 0.1 M), note that $...
- 482
5
votes
1
answer
643
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Why do my equilibrium calculations on this HF/NH4OH buffer system not match those in literature?
I've been trying to reproduce Figure 2 from this research paper (full text available).
The Problem
However I can't seem to get the same values as in the paper. I did the math both by hand and with ...
- 161
-1
votes
1
answer
99
views
Titrations in three equibilums
You have three solutions:
0.1 M solution of a weak monovalent acid
0.1 M solution of a strong monovalent acid
0.1 M solution of a weak divalent acid
Each solution is titrated with 0.15 M NaOH. What ...
- 91
-1
votes
3
answers
2k
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How to make a pH 6.8 Tris buffer?
To preface this, I am a biologist.
I need to make a $\mathrm{pH}=6.8$, $\pu{1 M}$ Tris buffer. We have access to Tris base and Tris Hydrochloride. (Unfortunately, none of the fancy Tris compounds ...
user62143
-6
votes
1
answer
645
views
what is the final concentration of the mixture [closed]
In a bizarre twist of chemical fate, an accident results in you results in you mixing 2L of a 3.00M solution of NaCl with 4L of a 1.50M solution of NaCl. what is the final concentration of the mixture?...
3
votes
2
answers
5k
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Why doesn't a buffer solution change ph(Appreciably?)
Consider a buffer solution containing weak acid $\ce{CH3COOH}$ and its salt $\ce{CH3COONa}$:
\begin{align}
\ce{CH3COOH &<=> CH3COO- + H+} \tag{1}\\
\ce{CH3COONa &-> CH3COO- + Na+} \...
- 4,197
1
vote
1
answer
555
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Acid-Base buffer question
Calculate the change in pH of a buffer made by combining $\pu{500 ml}$ of $\pu{0.1 M}$ $\ce{CH_3CH_2COOH}$ and $\pu{500 ml}$ of $\ce{CH_3CH_2COONa}$, when $0.04$ moles of $\ce{NaOH}$ is added to the ...
-3
votes
2
answers
1k
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Is it possible to prepare a solution of hydrogen sulfate in a lab? What is the procedure to do so?
I don't want a buffer solution with it, I want to know if its possible to have a solution with only $\ce{HSO4^{-}}$ ions in it.
- 1
-2
votes
2
answers
87
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What do we call ions without basic and acidic properties
According to Brønsted theory,
Acids are substances (molecules and ions) donating $\ce{H+}$
Bases are substances (molecules and ions) receiving $\ce{H+}$
I've been trying to find a complete Brønsted-...
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