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Z2, is the same, 4 × 10-4 mol/L. (a) Which has the Targer numerical value for the solubility product constant? (b) In a saturated solution of each salt in water, which has the higher concentration of M² + ? (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+? 17.51 Write the expression for the solubility-product con- nc stant for each of the following ionic compounds: Agl, SISO4, Fe(OH)2, and Hg2Br2. 17.52 (a) True or false: "solubility" and "solubility-product con- stant" are the same number for a given compound. (b) Write the expression for the solubility-product constant for each mui of the following ionic compounds: MNCO3, Hg(OH)2, and Cu3(PO4)2. 1618 17.53 (a) If the molar solubility of CaF2 at 35°C is 1.24 × 10 3 mol/L, what is Ksp at this temperature? (b) It is found that 1.1 × 10-2 g SrF, dissolves per 100 mL of aque- ous solution at 25 °C. Calculate the solubility product for SrF2. (c) The Ksp of Ba(IO3)2 at 25 °C is 6.0 × 10-10. What is the molar solubility of Ba(IO3)2? sp 7.54 (a) The molar solubility of PBB12 at 25°C is 1.0 × 10-² mol/L. Calculate Ksp. (b) If 0.0490 g of AgIO3 dis- solves per liter of solution, calculate the solubility-product constant. (c) Using the appropriate Ksp value from Appen- dix D, calculate the pH of a saturated solution of Ca(OH)2.

Z2, is the same, 4 × 10-4 mol/L. (a) Which has the Targer numerical value for the solubility product constant? (b) In a saturated solution of each salt in water, which has the higher concentration of M² + ? (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+? 17.51 Write the expression for the solubility-product con- nc stant for each of the following ionic compounds: Agl, SISO4, Fe(OH)2, and Hg2Br2. 17.52 (a) True or false: "solubility" and "solubility-product con- stant" are the same number for a given compound. (b) Write the expression for the solubility-product constant for each mui of the following ionic compounds: MNCO3, Hg(OH)2, and Cu3(PO4)2. 1618 17.53 (a) If the molar solubility of CaF2 at 35°C is 1.24 × 10 3 mol/L, what is Ksp at this temperature? (b) It is found that 1.1 × 10-2 g SrF, dissolves per 100 mL of aque- ous solution at 25 °C. Calculate the solubility product for SrF2. (c) The Ksp of Ba(IO3)2 at 25 °C is 6.0 × 10-10. What is the molar solubility of Ba(IO3)2? sp 7.54 (a) The molar solubility of PBB12 at 25°C is 1.0 × 10-² mol/L. Calculate Ksp. (b) If 0.0490 g of AgIO3 dis- solves per liter of solution, calculate the solubility-product constant. (c) Using the appropriate Ksp value from Appen- dix D, calculate the pH of a saturated solution of Ca(OH)2.

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Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Z2, is the same, 4 × 10-4 mol/L. (a) Which has the Targer numerical value for the solubility product constant? (b) In a saturated solution of each salt in water, which has the higher concentration of M² + ? (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+? 17.51 Write the expression for the solubility-product con- nc stant for each of the following ionic compounds: Agl, SISO4, Fe(OH)2, and Hg2Br2. 17.52 (a) True or false: "solubility" and "solubility-product con- stant" are the same number for a given compound. (b) Write the expression for the solubility-product constant for each mui of the following ionic compounds: MNCO3, Hg(OH)2, and Cu3(PO4)2. 1618 17.53 (a) If the molar solubility of CaF2 at 35°C is 1.24 × 10 3 mol/L, what is Ksp at this temperature? (b) It is found that 1.1 × 10-2 g SrF, dissolves per 100 mL of aque- ous solution at 25 °C. Calculate the solubility product for SrF2. (c) The Ksp of Ba(IO3)2 at 25 °C is 6.0 × 10-10. What is the molar solubility of Ba(IO3)2? sp 7.54 (a) The molar solubility of PBB12 at 25°C is 1.0 × 10-² mol/L. Calculate Ksp. (b) If 0.0490 g of AgIO3 dis- solves per liter of solution, calculate the solubility-product constant. (c) Using the appropriate Ksp value from Appen- dix D, calculate the pH of a saturated solution of Ca(OH)2.
Transcribed Image Text:Z2, is the same, 4 × 10-4 mol/L. (a) Which has the Targer numerical value for the solubility product constant? (b) In a saturated solution of each salt in water, which has the higher concentration of M² + ? (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+? 17.51 Write the expression for the solubility-product con- nc stant for each of the following ionic compounds: Agl, SISO4, Fe(OH)2, and Hg2Br2. 17.52 (a) True or false: "solubility" and "solubility-product con- stant" are the same number for a given compound. (b) Write the expression for the solubility-product constant for each mui of the following ionic compounds: MNCO3, Hg(OH)2, and Cu3(PO4)2. 1618 17.53 (a) If the molar solubility of CaF2 at 35°C is 1.24 × 10 3 mol/L, what is Ksp at this temperature? (b) It is found that 1.1 × 10-2 g SrF, dissolves per 100 mL of aque- ous solution at 25 °C. Calculate the solubility product for SrF2. (c) The Ksp of Ba(IO3)2 at 25 °C is 6.0 × 10-10. What is the molar solubility of Ba(IO3)2? sp 7.54 (a) The molar solubility of PBB12 at 25°C is 1.0 × 10-² mol/L. Calculate Ksp. (b) If 0.0490 g of AgIO3 dis- solves per liter of solution, calculate the solubility-product constant. (c) Using the appropriate Ksp value from Appen- dix D, calculate the pH of a saturated solution of Ca(OH)2.
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