Determine the molar solubility of Ba (ClO)_2 in pure water. K_ap for Ba(ClO)_2 =

Question

Determine the molar solubility of Ba (ClO)_2 in pure water. K_ap for Ba(ClO)_2 = 2.45 times 10^-5 A) 6.13 times 10^-6 M B) 1.23 times 10^-5 M C) 2.90 times 10^-2 M D) 4.95 times 10^-3 M E) 1.83 times 10^-2 Which of the following statements is true? A) K_sp is related to acid dissociation B) K_f is related to the solubility of ionic species C) K_b is related to base dissociation D) K_H is related to the formation of complexes E) K_w is related to the solubility of gases A solution containing CaCl_2 is mixed with a solution of Li_2C_2O_4 (lithium oxalate) to form a solution that is 1.15 times 10^-5 M in calcium ion and 2.00 times 10^-4 M in oxalate ion. What will happen once these solutions are mixed? K_sp (CaC_2O_4) = 2.3 times 10^-9. A) Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds. B) Nothing will happen K_sp > Q for all possible precipitants. C) A precipitate will form as calcium oxalate is not soluble to any extent. D) A precipitate will form since Q > K_sp for calcium oxalate. E) The solution will be saturated, since K_sp - Q. Consider the following reaction: CO_2(g) + C(s, graphite) = 2 CO(g) A reaction mixture initially contains 0.82 atm CO_2, 50 mol of graphite, and nothing else in a close container. Determine the equilibrium of CO if K_p for the reaction at this is 2.25. A) 0.91 atm B) 0.45 atm C) 1.36 atm D) 0.57 atm E) 1.14 atm what is the conjugate acid of H_2PO_4^-? A) HPO_4^2- B) PO_4^3- C) H_3PO_4 D) H_3O^+ E) OH^- The following titration curve indicates the titration of what kind of substance? A) strong monoprotic acid B) weak monoprotic acid C) diprotic acid D) triprotic acid E) weak base (bonus) What can small, multiply charged metal ions do when in an aqueous solution? A) Form a complex B) Make the solution acidic C) Be D) All of the above

Explanation / Answer

(15)

Ba(ClO2) (s) = Ba2+ (aq.) + 2 ClO2- (aq.)
Ksp = [Ba2+][ClO2-]2

2.45 * 10-5 = S * (2S)2

S3 = 2.45 * 10-5 / 4

S = 1.83 * 10-2 M

(E)

(16)

(C) Kb is related to base dissociation

where as ,

Ksp is related to solubility of ionic solids

Kf is the formation constant of complexes

Kw is related to ionic product of water

KH is Henry's law constant

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