Concept explainers
(a)
Interpretation:
The solubility product constant for
Concept Introduction:
Solubility product is the equilibrium constant for the reaction that occurs when an ionic compound is dissolved to produce its constituent ions. It is represented by
The expression for its
(a)
Answer to Problem 14.69QE
The solubility product constant of
Explanation of Solution
The dissociation reaction of
The solubility of
The formula to calculate the molar solubility of
Substitute
Therefore the solubility product constant of
(b)
Interpretation:
The solubility product constant for
Concept Introduction:
Refer to part (a).
(b)
Answer to Problem 14.69QE
The solubility product constant of
Explanation of Solution
The dissociation reaction of
The formula to calculate the molar solubility of
The solubility of
The formula to convert solubility of
Substitute
The solubility of
Substitute
Therefore the solubility product constant of
(c)
Interpretation:
The solubility product constant for
Concept Introduction:
Refer to part (a).
(c)
Answer to Problem 14.69QE
The solubility product constant of
Explanation of Solution
The dissociation reaction of
The ICE table for the above reaction is as follows:
The formula to calculate the molar solubility of
Substitute
Therefore the solubility product constant of
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Chapter 14 Solutions
Chemistry: Principles and Practice
- Some barium chloride is added to a solution that contains both K2SO4 (0.050 M) and Na3PO4 (0.020 M). (a) Which begins to precipitate first: the barium sulfate or the barium phosphate? (b) The concentration of the first anion species to precipitate, either the sulfate or phosphate, decreases as the precipitate forms. What is the concentration of the first species when the second begins to precipitate?arrow_forwardConsider the reaction BaF2(s)+SO42(aq)BaSO4(s)+2 F(aq) (a) Calculate K for the reaction. (b) Will BaSO4 precipitate if Na2SO4 is added to a saturated solution of BaF2?arrow_forwardUse the solubility product constant from Appendix F to determine whether a precipitate will form if 10.0 mL of 1.0 106 M iron(II) chloride is added to 20.0 mL of 3.0 104 M barium hydroxide.arrow_forward
- Because barium sulfate is opaque to X-rays, it is suspended in water and taken internally to make the gastrointestinal tract visible in an X-ray photograph. Although barium ion is quite toxic, barium sulfate’s /Csp of 1.1 X 10-,<) gives it such low solubility' that it can be safely consumed. What is the molar solubility' of BaSO4. What is its solubility' in grams per 100 g of water?arrow_forwardThe Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)arrow_forwardAn analytical chemist has a solution containing chloride ion, Cl¯. She decides to determine the amount of chloride ion in the solution by titrating 50.0 mL of this solution by 0.100 M AGNO3. As a way to indicate the endpoint of the titration, she added 1.13 g of potassium chromate, K2CrO4. As she slowly added the silver nitrate to the solution, a white precipitate formed. She continued the titration, with more white precipitate forming. Finally, the solution turned red, from another precipitate. The volume of the solution at this point was 60.8 mL. How many moles of chloride ion were there in the original solution? How many moles of chloride ion were there in the final solution? You may make any reasonable approximations. Ksp for Ag, CrO4 is 1.1 x 10-12, K, for AgCl is 1.8 x 10-10 moles of Cl¯ in the original solution moles of Cl¯ in the final solutionarrow_forward
- The Solubility Product Constant for manganese(II) carbonate is 1.8 × 10−¹¹ The molar solubility of manganese(II) carbonate in a water solution is M.arrow_forwardThe solubility of an ionic compound in water can be expressed in terms of the mass that will dissolve in a given volume of water, or in terms of the solubility product, Ksp. If only 0.303 g of Ca(OH)2 dissolves in enough water to give 0.243 L of aqueous solution at a given temperature, what is the Ksp value for calcium hydroxide at this temperature?arrow_forward7. The separate samples of nitric and acetic acids are both titrated with a 0.100 M solution of NaOH(aq). (Y) 25.0mL of 1.0 M HNO3(aq) (Z) 25.0 mL of 1.0 M CH3COOH(aq) Determine whether each of the following statements concerning this titration is true or false. (A) A larger volume of NaOH(aq) is needed to reach the equivalence point in the titration of HNO3 (B) The pH at the equivalence point in the HNO3 titration will be lower than the pH at the equivalence point in the CH3COOH titration (C) Phenolphthalein would be a suitable indicator for both titrations Group of answer choices a.) A) False B) True C) True b.) A) False B) False C) True c.) A) False B) True C) False d.) A) True B)True C)Truearrow_forward
- The solubility product constant for ruthenium perchlorate (RuClO4) is 3.0 x 10-3. What is the molar solubility (in mol/L)?arrow_forwardThe solubility of an ionic compound in water can be expressed in terms of the mass that will dissolve in a given volume of water, or in terms of the solubility product, Ksp.If only 0.264 g of Ca(OH)2 dissolves in enough water to give 0.165 L of aqueous solution at a given temperature, what is the Ksp value for calcium hydroxide at this temperature?arrow_forwardDetermine the molar solubility for Mg(OH)₂ (Ksp = 1.0 × 10⁻³¹) in an aqueous solution that has a pH of 8.90 at 25 °C.arrow_forward
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