Question

Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected. (a) AgCl(s) in 0.025 M NaCl (b) CaF2(s) in 0.00133 M KF (c) Ag2SO4(s) in 0.500 L of a solution containing 19.50 g of K2SO4 (d) Zn(OH)2(s) in a solution buffered at a pH of 11.45\

Answer 1

Step-by-step explanation:

a) AgCl(s) in 0.025 M NaCl

Equation: AgCl(s) ⇄ Ag⁺ (aq) + Cl⁻ (aq)

Initial conc : S O O

equili conc : O S S

NaCl(s) ⇒ Na⁺ (aq) + Cl⁻ (aq)

Initial conc : 0.025 0 0

equili conc : 0 0.025 0.025

Therefore the concentration: Ag⁺ = 6.4 * 10^-9 M, Cl⁻ = 0.025 M

attached below is the detailed solution of the