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Problem 47b
Calculate the pH at the equivalence point for titrating 0.200 M solutions of each of the following bases with 0.200 M HBr: (b) hydroxylamine 1NH2OH2.
Problem 48a
Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH: (a) hydrobromic acid (HBr).
Problem 48b
Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH: (b) chlorous acid (HClO2).
Problem 48c
Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH: (c) benzoic acid (C6H5COOH).
- For each statement, indicate whether it is true or false. (c) The solubility of a slightly soluble salt is independent of the presence of a common ion. (d) The solubility product of a slightly soluble salt is independent of the presence of a common ion.
Problem 49
Problem 50c
The solubility of two slightly soluble salts of M2 + , MA and MZ2, is the same, 4 * 10-4 mol/L. (c) If you added an equal volume of a solution saturated in MA to one saturated in MZ2, what would be the equilibrium concentration of the cation, M2+?
- Write the expression for the solubility-product constant for each of the following ionic compounds: Fe(OH)2.
Problem 51
Problem 52a
(a) True or false: 'solubility' and 'solubility-product constant' are the same number for a given compound.
Problem 52b
(b) Write the expression for the solubility-product constant for each of the following ionic compounds: MnCO3, Hg(OH)2, and Cu3(PO4)3.
Problem 53a
(a) I f t he molar solubility of CaF2 at 35°C i s 1.24 × 10–3 mol/L, what is Ksp at this temperature?
Problem 53b
(b) It is found that 1.1 × 10-2 g SrF2 dissolves per 100 mL of aqueous solution at 25°C. Calculate the solubility product for SrF2.
- (c) Using the appropriate Ksp value from Appendix D, calculate the pH of a saturated solution of Ca(OH)2.
Problem 54
Problem 54b
(b) If 0.0490 g of AgIO3 dissolves per liter of solution, calculate the solubility-product constant.
Problem 55
A 1.00-L solution saturated at 25 C with calcium oxalate 1CaC2O42 contains 0.0061 g of CaC2O4. Calculate the solubility-product constant for this salt at 25 C.
Problem 56
A 1.00-L solution saturated at 25 C with lead(II) iodide contains 0.54 g of PbI2. Calculate the solubility-product constant for this salt at 25 C.
- Using Appendix D, calculate the molar solubility of AgBr in (b) 3.0 × 10^-2 M AgNO3 solution and (c) 0.10 M NaBr solution.
Problem 57
Problem 58a
Calculate the solubility of LaF3 in grams per liter in (a) pure water.
Problem 58b
Calculate the solubility of LaF3 in grams per liter in (b) 0.010 M KF solution.
Problem 58c
Calculate the solubility of LaF3 in grams per liter in (c) 0.050 M LaCl3 solution.
- Consider a beaker containing a saturated solution of CaF2 in equilibrium with undissolved CaF2(s). Solid CaCl2 is then added to the solution. (b) Will the concentration of Ca2+ ions in solution increase or decrease? (c) Will the concentration of F- ions in solution increase or decrease?
Problem 59
Problem 59a
Consider a beaker containing a saturated solution of CaF2 in equilibrium with undissolved CaF21s2. Solid CaCl2 is then added to the solution. (a) Will the amount of solid CaF2 at the bottom of the beaker increase, decrease, or remain the same?
Problem 61
Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH (a) 7.0 (b) 9.5 (c) 11.8.
Problem 62a
Calculate the molar solubility of Ni(OH)2 when buffered at pH (a) 8.0.
Problem 62b
Calculate the molar solubility of Ni(OH)2 when buffered at pH (b) 10.0.
Problem 62c
Calculate the molar solubility of Ni(OH)2 when buffered at pH (c) 12.0.
- Which of the following salts will be substantially more soluble in acidic solution than in pure water: (a) ZnCO3, (b) ZnS, (c) BiI3, (d) AgCN, (e) Ba3(PO4)2?
Problem 63
Problem 64
For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with a strong acid: (a) MnS (b) PbF2 (c) AuCl3 (e) CuBr (d) Hg2C2O4.
Problem 65
From the value of Kf listed in Table 17.1, calculate the concentration of Ni2 +1aq2 and Ni1NH326 2+ that are present at equilibrium after dissolving 1.25 g NiCl2 in 100.0 mL of 0.20 M NH31aq2.
- From the value of Kf listed in Table 17.1, calculate the concentration of NH3 required to just dissolve 0.020 mol of NiC2O4 (Ksp = 4 * 10^-102) in 1.00 L of solution? (Hint: You can neglect the hydrolysis of C2O4^2- because the solution will be quite basic.)
Problem 66
- Use values of Ksp for AgI and Kf for [Ag(CN)2]- to (a) calculate the molar solubility of AgI in pure water. (b) calculate the equilibrium constant for the reaction AgI(s) + 2 CN⁻(aq) ⇌ [Ag(CN)2]⁻(aq) + I⁻(aq). (c) determine the molar solubility of AgI in a 0.100 M NaCN solution.
Problem 67