practexam2 - 1 When 40.0 mL of 1 104 M Ba(OH)2 are mixed...

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1. When 40.0 mL of 1 × 10 4 M Ba(OH) 2 are mixed with 60.0 mL of 2 × 10 5 M La 2 (SO 4 ) 3 ( K sp for La(OH) 3 is 1.0 × 10 19 and K sp for BaSO 4 is 1.1 × 10 10 ) A. a precipitate of BaSO 4 is obtained. B. a precipitate of La(OH) 3 is obtained. C. two precipitates are obtained. D. no precipitate is obtained. 2. How much sodium hydroxide can be added to a solution of a 100 ml solution of 0.2M acetic acid and 0.1 M lithium acetate before the pH begins to change significantly? A. B. C. D. 3. What is the sum of the coefficients for the charge balance equation of lithium valonate, a triprotic acid? A. 7 B. 6 C. 8 D. 9 E. 11 4. What is the solubility of iodide ion in AuI ( K sp = 4 × 10 12 ) in 0.100 M solution AuNO 3 ? A. B.
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C. D. 5. What is the simple rule that allows one to estimate the molar solubility of ions from the Ksp? Answer 6. What will be the pH in a titration in which 50.0 mL of 0.120 M HNO 3 (aq) is added to 25.0 mL of 0.240 M KOH(aq)? A. 0.74 B. 7 C. 13.33 D. 13.38 7. What is the pH of a 1 M Lithium maleiate solution? The pKas for this salt of a diprotic acid are 2 and 6. Answer 8. What can you say about the pH of 10 -9 M solutions of HCl, citric acid, acetic acid, ammonia and lithium hydroxide? Answer 9. In performing a buffer neutralization calculation which has a weak acid, a weak base and a strong acid or base present initially, if you follow through all the steps in the neutralization if can take a lot of work to find the equilibrium pH. Why is it that this problem can often be done quite efficiently in
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