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1 Ksp Some useful data: Compound Ksp Compound Ksp AgCl 1.8 x 10–10 Ag2CrO4 9 x 10–12 PbSO4 1.8 x 10–8 CaF2 4.0 x 10–11 Mg(OH)2 1.5 x 10–11 BaSO4 1.1 x 10–10 Simple Introductory Stuff 1. To what kind of solutions is the proper use of the solubility product principle limited? (A) dilute solutions of moderately soluble electrolytes (B) dilute solutions of slightly soluble electrolytes (C) saturated solutions of moderately soluble electrolytes (D) saturated solutions of slightly soluble electrolytes (E) supersaturated solutions of moderately soluble electrolytes 2. Which is the correct expression for the solubility product constant for Ag2CrO4? (A) Ksp = [Ag+]2 [CrO42–] (D) Ksp = [2Ag+]2 [CrO42–] (B) Ksp = [Ag+] [CrO42–] (E) Ksp = [Ag+] [CrO42–] (C) Ksp = [2Ag+] [CrO42–] Ksp and Solubility 3. If the concentration of a saturated solution of SrCO3 is 0.000040 mol L–1, what is the value for the solubility product constant of this salt? (A) 4.0 x 10–4 (B) 1.6 x 10–9 (C) 4.0 x 10–5 (D) 1.6 x 10–11 (E) 1.6 x 10–7 4. The solubility of Cu2CrO4 in water at 25 °C is 1 x 10–4 mol L–1. The solubility product constant at this temperature is (A) 1 x 10–12 (B) 4 x 10–12 (C) 1 x 10–8 (D) 4 x 10–8 5. What is the solubility product constant, Ksp, of Tl2CrO4 given that the molar concentration of CrO42- in a saturated solution is 6.3 x 10-5 M? (A) 2.5 x 10-13 (B) 4.0 x 10-9 (C) 1.0 x 10-12 (D) 8.0 x 10-9 (E) 6.3 x 10-5 6. What is the Ksp of Mg3(PO4)2 in water at 25 °C if its molar solubility is 8.6 x 10-6? (A) 4.7 x 10-26 (B) 5.1 x 10-24 (C) 8.0 x 10-8 (D) 8.6 x 10-7 (E) 7.4 x 10-11 7. The solubility of the ionic compound Al2(PO4)3 is 0.020 moles per liter. Calculate the Ksp. (A) 3.5 x 10-7 (B) 3.2 x 10-9 (C) 1.5 x 10-7 (D) 6.4 x 10-11 (E) 8.0 x 10-62 8. The solubility of BaCO3 is 7.9 x 10–3 g L–1. Calculate the solubility product, Ksp ignoring hydrolysis. (A) 1.6 x 10–2 (B) 4.0 x 10–5 (C) 1.6 x 10–9 (D) 6.2 x 10–5 9. The solubility of silver acetate, AgC2H3O2, is 1.02 g per 100 mL. What is the Ksp? (A) 3.7 x 10–5 (B) 2.8 x 10–4 (C) 1.0 x 10–4 (D) 3.7 x 10–3 10. Calculate the molar solubility of Ag2CrO4? (A) 8.1 x 10–23 (B) 3 x 10–6 (C) 2.1 x 10–4 (D) 1.7 x 10–4 (E) 1.3 x 10–4 11. Given that the Ksp for strontium fluoride (SrF2) is 2.6 x 10-9, calculate the solubility in pure water. (A) 1.4 x 10-3 (B) 3.4 x 10-4 (C) 8.7 x 10-4 (D) 5.1 x 10-4 (E) 2.6 x 10-9 Other Concentrations 12. Calculate the concentration of Fe3+ in blood using the fact that the pH = 7.41 and the Ksp of Fe(OH)3 is 4.0 x 10-38. (A) 2.4 x 10-18 M (B) 1.2 x 10-19 M (C) 2.0 x 10-10 M (D) 1.3 x 10-38 M (E) 4.0 x 10-38 M 13. What is [OH–] in a saturated solution of Mg(OH)2 where [Mg2+] = 1.5 x 10–5 M? (A) 2.2 x 10–10 M (B) 5.0 x 10–4 M (C) 3.0 x 10–5 M (D) 1.0 x 10–3 M 14. Silver chloride is precipitated by adding HCl to a solution of a silver salt until the concentration of chloride ions (Cl–) is 0.20 M. Neglecting the effects of interatomic attraction, what is the concentration of silver ions? (A) 0.0042 M (B) 1.8 x 10–10 M (C) 0.0095 M (D) 9.0 x 10–10 M 15. Typical “hard” water contains about 2.0 x 10–3 mol of Ca2+ per liter. Calculate the maximum concentration of fluoride ion which could be present in hard water. (A) 1.4 x 10–4 M (B) 4.0 x 10–3 M (C) 2.0 x 10–3 M (D) 2.0 x 10–8 M 16. What is the concentration of Ag+ in a 0.010 M KCl solution saturated with AgCl? (A) 1.3 x 10–5 M (B) 1.8 x 10–8 M (C) 1.0 x 10–7 M (D) 1.8 x 10–11 M 17. What is the molar concentration of silver ion in a solution containing 1.3 x 10–4 M CrO42–, saturated with Ag2CrO4? (A) 1.3 x 10–16 (B) 2.6 x 10–4 (C) 7 x 10–16 (D) 7 x 10–3 (E) 9 x 10–123 Common Ion 18. If two salts, AX and BX2, have the same Ksp values of 4.0 x 10–12, then (A) their molar solubilities in water are the same. (B) the salts are more soluble in 0.1 M NaX than in water. (C) the molar solubility of AX in water is less than that of BX2. (D) addition of NaX will not affect the solubilities of the salts. 19. What is the molar solubility of lead sulfate in 1.0 x 10–3 M Na2SO4? (A) 1.8 x 10–2 (B) 1.8 x 10–5 (C) 1.3 x 10–4 (D) 5.0 x 10–6 20. The Ksp of PbCl2 is 1.7 x 10-5. Calculate its molar solubility in a solution that is 0.200 M NaCl. (A) 4.3 x 10-5 (B) 8.5 x 10-5 (C) 4.3 x 10-4 (D) 4.1 x 10-3 (E) 4.1 x 10-4 21. For which salt would the solubility be MOST sensitive to pH? (A) Ca(NO3)2 (B) CaF2 (C) CaCl2 (D) CaBr2 (E) CaI2 22. Which of the following salts would NOT be more soluble in acidic solution? (A) Mg(OH)2 (B) AgCl (C) Ag3PO4 (D) AgF 23. For which salt of the following pairs will the solubility depend on pH? i) PbF2, PbCl2 ii) Sr(NO3)2 Sr(NO2)2 (A) They all depend on pH (B) i. PbCl2 ii. Sr(NO2) 2 (C) i. PbCl2 ii. Sr(NO2) 2 (D) i. PbF2 ii. Sr(NO2) 2 (E) i. PbF2 ii. Sr(NO3) 2 Precipitation? 24. The addition of solid Na2SO4 to an aqueous solution in equilibrium with solid BaSO4 will cause (A) no change in [Ba2+] in solution. (B) more BaSO4 to dissolve. (C) precipitation of more BaSO4. (D) an increase in the Ksp of BaSO4. 25. Which of the following mixtures would result in the formation of a precipitate? (A) 0.10 M NaNO3 and 0.05 M BaCl2 (B) 1 x 10-8 M Na2SO4 and 0.0005 M M BaCl2 (C) 1 x 10-5 M Fe2(SO4) 3 and 1 x 10-5 M BaCl2 (D) 1 x 10-2 M CuSO4 and 1 x 10-8 M BaCl2 26. In a solution of 2.0 x 10-3 M Pb2+(aq), what is the concentration of I- necessary to just begin precipitation of PbI2 (Ksp = 1.4 x 10-8)? (A) 1.4 x 10-8 M (B) 2.6 x 10-3 M (C) 4.9 x 10-11 M (D) 2.8 x 10-11 M (E) 7.0 x 10-6 M4 27. Given the following values of Ksp, select the mixture below that would give rise to the formation of a precipitate. AgCl Ksp = 1.8 x 10-10 BaSO4 Ksp = 1.1 x 10-10 PbI2 Ksp = 7.9 x 10-9 CaF2 Ksp = 3.2 x 10-11 AgCN Ksp = 2.2 x 10-16 (A) A solution that is 1.00 x 10-5 M AgNO3 and 1.00 x 10-5 M NaCl (B) A solution that is 1.00 x 10-4 M …

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