If the concentration of [Ag^+] In solution is 3.5 Times 10^-5 M, what is the max

Question

If the concentration of [Ag^+] In solution is 3.5 Times 10^-5 M, what is the maximum concentration of the other ion before precipitation will occur? Consider the reaction: What is the solubility of AgCl in pure water? What is the solubility of AgCl in a 7.6 mM NaCI solution? A solution contains 5 Times 10^-7 M Zn^2+, Ni^2+, and Mn^2+. Adding in saturating amounts of S^2- solution will precipitated out all of the metal ions. The K_sp for each are as follows: Which solid will precipitate first? What is the concentration of Zn^2+ ions remaining in solution when NiS begins to precipitate out?

Explanation / Answer

1. a)

     concentration = 3.5 * 10-5/5.5 * 10-5

                            = 0.63 mol/L

b) concentration = 8.1 * 10-5/(3.5 * 10-5)2

                            = 6.6 * 10-3 mol/L

c) concentration = 6.0 * 10-51/(3.5 * 10-5)2

                            = 0.49 * 10-41 mol/L

2. Ksp = S2

S = (1.8 * 10-10)^!.2

S = 1.43 *10 -5 mol/L

3. lower ksp values precipitate first therefore Mns is precipitate first.

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