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(CaC2O4) contains 0.0061 g of CaC,O4. Calculate solubility-product constant for this salt at 25 °C. 17.55 A 1.00-L solution saturated at contains 0,54 g of Pbl,. Calculate the solubility-product constant for this salt at 25 °C. 17.56 A 1.00-L solution saturated at 25 °C with lead(II) iodide (a) pure water, (b) 3.0 × 10-2 M AgNO3 solution, (c) 0.10 M NaBr solution. 17.57 Using Appendix D, calculate the molar solubility of AgBr in 17.58 Calculate the solubility of LaF, in grams per liter in (a) pure water, (b) 0.010 M KF solution, (c) 0.050 M LaCl3 solution. 17.59 Consider a beaker containing a saturated solution of CaF2 in equilibrium with undissolved CaF(s). Solid CaCl2 is then added to the solution. (a) Will the amount of solid CaF, at the bottom of the beaker increase, decrease, or re- main the same? (b) Will the concentration of Ca² + ions in solution increase or decrease? (c) Will the concentration of F ions in solution increase or decrease? 17.60 Consider a beaker containing a saturated solution of PbI2 in equilibrium with undissolved PbI2(s). Now solid KI is added to this solution. (a) Will the amount of solid Pbl2 at the bottom of the beaker increase, decrease, or remain the same? (b) Will the concentration of Pb2+ ions in solution increase or decrease? (c) Will the concentration of I ions in solution increase or decrease? 17.61 Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH (a) 7.0, (b) 9.5, (c) 11.8. 17.62 Calculate the molar solubility of Ni(OH)2 when buffered at pH (a) 8.0, (b) 10.0, (c) 12.0. 17.63 Which of the following salts will be substantially more soluble in acidic solution than in pure water: (a) ZNCO, (b) ZnS, (c) Bil3, (d) AGCN, (e) Ba3(PO4)2? 17.64 For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with a st

(CaC2O4) contains 0.0061 g of CaC,O4. Calculate solubility-product constant for this salt at 25 °C. 17.55 A 1.00-L solution saturated at contains 0,54 g of Pbl,. Calculate the solubility-product constant for this salt at 25 °C. 17.56 A 1.00-L solution saturated at 25 °C with lead(II) iodide (a) pure water, (b) 3.0 × 10-2 M AgNO3 solution, (c) 0.10 M NaBr solution. 17.57 Using Appendix D, calculate the molar solubility of AgBr in 17.58 Calculate the solubility of LaF, in grams per liter in (a) pure water, (b) 0.010 M KF solution, (c) 0.050 M LaCl3 solution. 17.59 Consider a beaker containing a saturated solution of CaF2 in equilibrium with undissolved CaF(s). Solid CaCl2 is then added to the solution. (a) Will the amount of solid CaF, at the bottom of the beaker increase, decrease, or re- main the same? (b) Will the concentration of Ca² + ions in solution increase or decrease? (c) Will the concentration of F ions in solution increase or decrease? 17.60 Consider a beaker containing a saturated solution of PbI2 in equilibrium with undissolved PbI2(s). Now solid KI is added to this solution. (a) Will the amount of solid Pbl2 at the bottom of the beaker increase, decrease, or remain the same? (b) Will the concentration of Pb2+ ions in solution increase or decrease? (c) Will the concentration of I ions in solution increase or decrease? 17.61 Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH (a) 7.0, (b) 9.5, (c) 11.8. 17.62 Calculate the molar solubility of Ni(OH)2 when buffered at pH (a) 8.0, (b) 10.0, (c) 12.0. 17.63 Which of the following salts will be substantially more soluble in acidic solution than in pure water: (a) ZNCO, (b) ZnS, (c) Bil3, (d) AGCN, (e) Ba3(PO4)2? 17.64 For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with a st

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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(CaC2O4) contains 0.0061 g of CaC,O4. Calculate solubility-product constant for this salt at 25 °C. 17.55 A 1.00-L solution saturated at contains 0,54 g of Pbl,. Calculate the solubility-product constant for this salt at 25 °C. 17.56 A 1.00-L solution saturated at 25 °C with lead(II) iodide (a) pure water, (b) 3.0 × 10-2 M AgNO3 solution, (c) 0.10 M NaBr solution. 17.57 Using Appendix D, calculate the molar solubility of AgBr in 17.58 Calculate the solubility of LaF, in grams per liter in (a) pure water, (b) 0.010 M KF solution, (c) 0.050 M LaCl3 solution. 17.59 Consider a beaker containing a saturated solution of CaF2 in equilibrium with undissolved CaF(s). Solid CaCl2 is then added to the solution. (a) Will the amount of solid CaF, at the bottom of the beaker increase, decrease, or re- main the same? (b) Will the concentration of Ca² + ions in solution increase or decrease? (c) Will the concentration of F ions in solution increase or decrease? 17.60 Consider a beaker containing a saturated solution of PbI2 in equilibrium with undissolved PbI2(s). Now solid KI is added to this solution. (a) Will the amount of solid Pbl2 at the bottom of the beaker increase, decrease, or remain the same? (b) Will the concentration of Pb2+ ions in solution increase or decrease? (c) Will the concentration of I ions in solution increase or decrease? 17.61 Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH (a) 7.0, (b) 9.5, (c) 11.8. 17.62 Calculate the molar solubility of Ni(OH)2 when buffered at pH (a) 8.0, (b) 10.0, (c) 12.0. 17.63 Which of the following salts will be substantially more soluble in acidic solution than in pure water: (a) ZNCO, (b) ZnS, (c) Bil3, (d) AGCN, (e) Ba3(PO4)2? 17.64 For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with a st
Transcribed Image Text:(CaC2O4) contains 0.0061 g of CaC,O4. Calculate solubility-product constant for this salt at 25 °C. 17.55 A 1.00-L solution saturated at contains 0,54 g of Pbl,. Calculate the solubility-product constant for this salt at 25 °C. 17.56 A 1.00-L solution saturated at 25 °C with lead(II) iodide (a) pure water, (b) 3.0 × 10-2 M AgNO3 solution, (c) 0.10 M NaBr solution. 17.57 Using Appendix D, calculate the molar solubility of AgBr in 17.58 Calculate the solubility of LaF, in grams per liter in (a) pure water, (b) 0.010 M KF solution, (c) 0.050 M LaCl3 solution. 17.59 Consider a beaker containing a saturated solution of CaF2 in equilibrium with undissolved CaF(s). Solid CaCl2 is then added to the solution. (a) Will the amount of solid CaF, at the bottom of the beaker increase, decrease, or re- main the same? (b) Will the concentration of Ca² + ions in solution increase or decrease? (c) Will the concentration of F ions in solution increase or decrease? 17.60 Consider a beaker containing a saturated solution of PbI2 in equilibrium with undissolved PbI2(s). Now solid KI is added to this solution. (a) Will the amount of solid Pbl2 at the bottom of the beaker increase, decrease, or remain the same? (b) Will the concentration of Pb2+ ions in solution increase or decrease? (c) Will the concentration of I ions in solution increase or decrease? 17.61 Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH (a) 7.0, (b) 9.5, (c) 11.8. 17.62 Calculate the molar solubility of Ni(OH)2 when buffered at pH (a) 8.0, (b) 10.0, (c) 12.0. 17.63 Which of the following salts will be substantially more soluble in acidic solution than in pure water: (a) ZNCO, (b) ZnS, (c) Bil3, (d) AGCN, (e) Ba3(PO4)2? 17.64 For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with a st
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