Silver chloride is classified as an insoluble compound because it dissolves only

Question

Silver chloride is classified as an insoluble compound because it dissolves only to a small extent in water. Consider the balanced equation and equilibrium constant that shows the partial dissolving of silver chloride in water: AgCI(s) Ag (a)C(a) Keq = 1.70 x 10-10 (a) Is this equilibrium classified as a homogeneous or heterogeneous equilibrium? (select) (b) Write the equilibrium constant expression for this reaction. Kec (c) Use the equilibrium constant value and your equilibrium constant expression to calculate the concentration of each ion in a saturated solution of silver chloride. [Ag+] = x 10 [Cl-] = ×10 M Enter your answers in scientific notation.

Explanation / Answer

a) heterogeneous equilibrium

b) Keq = [Ag+][Cl-]

C) 1.7*10^-10 = X*X

   X = concentration of each ion in a saturated solution = x = 1.304*10^-5 M

[Ag+] = x = 1.304*10^-5 M

[Cl-] = x = 1.304*10^-5 M

at 400 k , equilibrium constant(K) = 224

Keq = [NH3]^2/[N2][H2]^3

REACTION quotient(Q) = (0.042/1.34)^2/((0.04/1.34)*(0.042/1.34)^3)

              = 1068.81

Q > K. so that, backward reaction takes place.

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