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38. Calculate the (Ca2+] required to start the precipitation of calcium fluoride, CaF2, from a solution containing 0.0025 MF-at 25°C. Ksp for CaF2 = 3.9 x 10-11. a. 6.4 x 10-7 M b. 5.2 x 10-10 M c. 4.8 x 10-3 M d. 6.2 x 10-6 M e. 1.6 x 10-8 M
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35. Calculate the concentration of OH' ions in a saturated Mn(OH)2 solution. The solubility product for Mn(OH)2 is 4.6 x 10-14 a. 1.0 x 10-5 M b. 2.0 x 10-5 M c. 1.6 x 10-5 M d. 3.2 x 10-5 M e. 4.5 x 10-5 M
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1. Which of the following solubility product expressions is incorrect? d. Aul, K, = [AT][I-] 2. At 25°C, 1.4x 10-mole of Cd(OH) dissolves to give 1.0 liter of saturated aqueous solution. What is the solubility product for Cd(OH)2? a. 1.7 x 10- b. 2.9 x 10 C. 1.1 x 10-4 d. 5.8 x 10-1 e. 4.1 x 10-2 3. IfX the molar solubility (mol/L) of Ni(OH)a, which of the following represents the...
Question For the following equilibrium, if Ksp 1.0 x 1022, what is the molar solubility of silver arsenate? Ag3AsO4(s)3 Ag (aq) AsO(aq) Report your answer in scientific notation with the correct number of significant figures.
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Ch. 18 Values The following values will be useful for problems in this chapter. Acid Substance or Species HF HNO2 CH3COOH HOCI HOBr HOCN HCN H2SO4 KA = 7.2 x 10-4 Ka = 4.5 x 10-4 Ka = 1.8 x 10-5 Ka = 3.5 x 10-8 = 2.5 x 10-9 K4 = 3.5 x 10-4 Ka = 4.0 x 10-10 Kai = very large Kq2 = 1.2...
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36. Calculate the pH of a saturated aqueous solution of Co(OH)2. Ksp is 2.5 x 10-16. a. 8.60 b. 8.90 c. 9.10 d. 9.20 e. 9.40
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12. Refer to Ch. 18 Values. The pH of a 0.10 M solution of a monoprotic acid is 2.85. What is the value of the ionization constant of the acid? a. 6.3 x 10-5 b. 3.8 x 10-6 c. 2.0 x 10-5 d. 4.0 x 10-8 e. 7.2 x 104 12. Refer to...
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Equilibrium Constants The following equilibrium constants will be useful for some of the problems. Substance H2CO3 Substance HCOH HNO2 НОСІ (COOH)2 Constant K = 1.8 x 10-4 Ka = 4.5 x 10-4 KA = 3.5 x 10-8 K = 7.2 x 10-4 KA = 4.0 x 10-10 Ki = very large K = 1.2 x 10-2 Ka=2.5 x 10-9 Constant Ki = 4.2 x...
1) Write the solubility-product expression for the following mercury salts: Hg2Cl2 and HgCl2. 2) Exactly 0.133 mg of AgBr will dissolve in 1.00 L of water. What is the value of Ksp for AgBr? 3) By experiment, it is found that 1.2 x 10-3 mol of lead (II) iodide, PbI2, dissolves in 1.0 L of water at 25°C. What is the Ksp at this temperature? 4) What is the molar solubility of silver chloride in 1.0 L of solution that...
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ID: A 15. Refer to Ch. 18 Values. The (OH) = 1.3 x 105 M for a 0.025 M solution of a weak base. Calculate the value of K, for this weak base. a. 5.2 x 10-5 b. 3.1 x 10-7 c. 7.7 x 10-4 d. 4.0 x 10- e. 6.8 x 10-11