× There is no additional information about the initial concentration. There is o

Question

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There is no additional information about the initial concentration. There is only a hint that reads.."Given the buffer pH, what is the hydroxide ion concentration? Write the solubility product expression for chromium(III) hydroxide and determine the concentration of Cr3+ in solution using the Ksp value. The Cr3+ in solution complexes with the hydroxide to form the complex ion [Cr(OH)4]. What is the formation equation for this complex ion? How do you use the Kf, the formation constant, and the concentrations of Cr3+ and OHto determine the molar solubility of chromium(III) hydroxide?"

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A saturated solution of AgCl is treated with solid NaCl until the [Cl] is 0.72 M. What will be the resulting [Ag+] in solution? Enter your answer in scientific notation.

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10 M

What percent of Ag+ remains in solution at this point?

%

Explanation / Answer

Answer (1)

First you will need the solubility product constant of AgCl which is 1.6x10^-10.

If AgCl was placed in pure water,
AgCl(s) <-----> Ag^+(aq) + Cl^-(aq)
would dissolved according to the equation given above.
Ksp = [Ag^+][Cl^-] = 1.6x10^-10
[Ag^+][0.72] = 1.6x10^-10
[Ag^+] = 2.22 x10^-10 M

(2.22 x 10^-7 M) divided by (0.72 M) x 100%

= 3.08 x 10^-5 %

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