All Questions
12
questions
-2
votes
2
answers
732
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Isolating potassium chloride from sodium chloride and potassium hydroxide
Assume that you have an aqueous solution of sodium chloride and potassium hydroxide. Is it possible to isolate potassium chloride from this?
$$\ce{Na+(aq) + Cl-(aq) + K+(aq) + OH-(aq) -> Na+(aq) + ...
user123142
0
votes
0
answers
126
views
Why is the Ag+ concentration in a beaker fixed in the reaction between excess AgCl (s) and KI (aq) from the start? [duplicate]
This arises as a sub-question for the following question: Calculate the concentration of I- in a solution obtained by mixing 0.10 M KI with an excess of AgCl(s).
I tried to look at How does addition ...
1
vote
1
answer
2k
views
Using solubility product to determine the mass of the precipitate of a reaction
I mix together $\pu{100 mL}$ of an aqueous $\ce{NaCl}$ solution at $\pu{0.5 M}$ and $\pu{100 mL}$ of an aqueous $\ce{AgNO3}$ solution at $\pu{0.3 M}$. Assuming that the solubility of $\ce{NaCl}$ in ...
- 11
2
votes
2
answers
345
views
Calculating equilibrium concentrations of silver and halide ions
$\pu{500 ml}$ of $\pu{0.01 M}$ $\ce{AgNO3}$ is mixed with $\pu{500 ml}$ of solution containing $\pu{0.1 M}$ $\ce{NaCl}$ and $\pu{0.1 M}$ $\ce{NaBr}$. $K_\mathrm{sp}$ of $\ce{AgCl}$ is $10^{-10}$ and $...
- 224
2
votes
1
answer
958
views
How to find the concentration of barium ions in a mixture of barium sulfate and barium thiosulfate?
I have a hard time with selective precipitation problem.
A mixture of $\ce{BaSO4}$ and $\ce{BaS2O3}$ is shaken with pure water until a saturated solution is formed. Both solids remain in excess. ...
- 23
2
votes
0
answers
34
views
Cleaning a stubborn Electrospray residue
I have an electrospray ionization capillary tip that sprays into a chamber that contains some circuit boards. An aqueous CsI sample is apparently causing a white residue to build up on these boards ...
1
vote
0
answers
47
views
how can I predict the rate of water ions precipitation on a surface?
Consider a titanium pot that contains 1kg water with the following ions:
$[Ca^{2+}]=22000$ ppm, $[Mg^{2+}]=1500$ ppm,$[Sr^{2+}]=791$ ppm,$[Na^{1+}]=48000$ ppm,$[Cl^{1-}]=120000$ ppm,$[SO_4^{2-}]=...
- 17
0
votes
3
answers
148
views
Finding ions in water samples
So for a school chemistry assignment I was given 5 water samples and a bunch of different reagents to help me find out what was in the solutions. I'm stuck on two.
The first one had a pH of 7 and ...
- 11
4
votes
4
answers
32k
views
Difference between precipitation and crystallisation
What is the main difference between precipitation and crystallization.
Is precipitation a chemical change and crystallization a physical change.
How can we say that the resulting solute is precipitate ...
- 93
1
vote
1
answer
166
views
Is NaCl in water considered "solution" despite of NaCl's having some precipitation?
Is $\ce{NaCl}$ in water aqueous? For a certain amount of $\ce{NaCl}$, it can dissolve in water but if you add more $\ce{NaCl}$ it can't dissolve any more.
So, if in a certain reaction $\ce{NaCl}$ is ...
- 393
4
votes
1
answer
4k
views
How to determine which salt will precipitate from a solution containing multiple ions?
I have a solution containing $0.2\:\mathrm{mol}$ of $\ce{Br^-}$ ions and $\ce{SO_4^2-}$ ions each.
Now if I add excess $\ce{AgNO3}$ in this solution,
what will precipitate?
$\ce{Ag2SO4}$ or $\ce{...
- 801
6
votes
2
answers
1k
views
How to find the mass of dissolved AgCl when placed in a solution of NaCl?
I think the following problem in my textbook is malformed:
Solid $\ce{AgCl}$ is placed in $1\,\mathrm{L}$ of $0.55\,\mathrm{M}$ $\ce{NaCl}$. Find the mass of $\ce{AgCl}$ which dissolves.
I know ...
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