All Questions
12
questions
2
votes
1
answer
103
views
Equilibrium Solubility of CO2 in Aqueous Solution and its Dependence on H3O+ Concentration
The equilibrium solubility of $\ce{CO2}$ in an aqueous solution is given by three chemical reactions:
$$
\begin{align}
\ce{CO2(g) &<=> CO2(aq)}\label{rxn:R1}\tag{R1}\\
\ce{CO2(aq) + H2O &...
3
votes
2
answers
2k
views
Calculate the titer of a solution
I hope this is the right place to ask. We have this exercise without solution
One litre of diluted sodium hydroxide solution (c = 0.15mol/litre) is
to be prepared in the laboratory. The titer from ...
- 423
1
vote
1
answer
105
views
What is the maximum number of silver(Ⅰ) ions in one litre of a 0.003 M sodium sulfide solution?
What is the maximum number of silver(Ⅰ) ions that can be present dissolved in one litre of a $\pu{0.003 M}$ $\ce{Na2S}$ solution?
According to my book, silver(I) reacts with sulfide producing $\ce{...
- 423
1
vote
0
answers
101
views
Physical Chemistry: Specifically the Dissolution of Carbonates
Please note this question is different to the other that keeps being mentioned. That one is about the concentration of just $\ce{HCO3-}$ when no $\ce {pH}$ was given.
Whereas, in this one I am trying ...
- 51
0
votes
0
answers
550
views
Adding aluminum sulfate to neutralize an aqueous solution of sodium silicate with pH of 12.6
How much aluminum sulfate do I need to add to an aqueous solution of sodium silicate to neutralize the solution (pH from 12.6 to 7)?
For a water treatment school project, we remove sodium silicate ...
- 173
2
votes
1
answer
987
views
How to calculate molar concentration from equilibrium equations with no initial concentration given?
I have the equations:
\begin{align}
\ce{CO2(g) + H2O(l) &<=> H2CO3(aq)} &\quad K_1 &= 10^{-1.47} \tag{1}\\
\ce{H2CO3(aq) &<=> H+(aq) + HCO3-(aq)} &\quad K_2 &= 10^{-...
- 51
0
votes
0
answers
138
views
Problem in the calculation of ionic strength of a solution
Recently I've been trying to answer the question 10-13 (c) of 9th edition of Fundamentals of Analytical Chemistry of Skoog et al. Comparing my answers with the student manual , I realized that my ...
- 177
0
votes
1
answer
271
views
Why are some weak acid equilibrium approximations invalid in very dilute solutions?
Using two approximations for the dissociation of a weak acid, we can write
$$K_\mathrm{a}= \frac{[\ce{H+(aq)}]^2}{[\ce{HA(aq)}]}$$
One of these two approximations we use is that the concentration of ...
- 209
-1
votes
1
answer
512
views
An equilibrium question involving mixing equal volumes of HCl and H2SO4
Question: Calculate the concentrations of H3O(+) and SO4(2-) in a solution prepared by mixing equal volumes of 0.2M HCl and 0.6M H2SO4. (Ka1 for H2SO4 is very large, and Ka2 for H2SO4 is 1.2E-2)
Here ...
- 65
1
vote
1
answer
2k
views
How to calculate ion concentrations for a precipitation from the solubility product constant? [closed]
The equilibrium constant for dissolving the insoluble substance gold (I) iodide, AuI (s), in aqueous
solution is 1.6 × 10^-23
at 25ºC. Write the equilibrium constant expression and calculate the ...
- 75
-1
votes
1
answer
171
views
Why don't we take into account the auto-protonation of water when measuring its concentration?
When we calculate the concentration of water at $ 25~^\circ\rm C $,
why don't we assume dissociation of water at this temperature?
$$\ce{H2O <=> H+ + OH-}$$
- 153
2
votes
1
answer
954
views
What is total concentration of buffer used in derivation of buffer capacity?
ChemBuddy — The buffer capacity provides the following:
$$\ce{HA <=> H+ + A-}$$
Total concentration of the buffer $c_\mathrm{buf}$ is given by
$$c_\mathrm{buf} = [\ce{HA}] + [\ce{A-}]\tag{19.3}$...
- 7,804