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30 Jun 2020

0.01 M of Cl is present in a solution. If AgCl will be dissolved in the solution, what would be its solubility? (K_sp = 1.77 x 10^-10)

Solve problems involving solubility equilibria

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Related questions

A solution is 5.0 x 10^-5 M in each of these ions: Ag⁺, SO₄^2-, Cl^-, CO₃^2-. Which precipitate will form?

A) Ag₂SO₄ (Ksp = 1.12 x 10^-5)

B) AgCl (Ksp = 1.77 x 10^-10)

C) Ag₂CO₃ (Ksp = 8.46 x 10^-12)

orangeelephant440

What is the molar solubility of AgCl in 4 M NH₃? K_sp of AgCl = 1.77 x 10^-10, K_f of Ag(NH₃)₂ = 1.7 x 10⁷.

What is the solubility of AgCl in water (g/L); the Ksp for AgCl is 1.1x10-9. What would happen to the solubility of AgCl in a 0.300 M NaCl solution?

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