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hw6sol - valdez(vv689 Homework#6 Holcombe(52460 This...

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valdez (vv689) – Homework #6 – Holcombe – (52460) 1 This print-out should have 13 questions. Multiple-choice questions may continue on the next column or page – find all choices before answering. 001 10.0 points What is the pH of a 0 . 1 M Ba(OH) 2 aqueous solution? 1. 1 . 3301 2. 0 . 69897 3. 8.7 4. 13 . 301 correct 5. 9 . 97577 Explanation: [Ba(OH) 2 ] = 0 . 15 M Ba(OH) 2 is a strong base which dissociates in aqueous solution to produce two moles of OH - for every mole of Ba(OH) 2 , so 0 . 1 M Ba(OH) 2 produces 0 . 2 M OH - . Ba(OH) 2 Ba 2+ + 2 OH - ini 0 . 1 M 0 M 0 M Δ - 0 . 1 M +0 . 1 M 2(0 . 1 M) fin 0 M +0 . 1 M +0 . 2 M pH = 14 - pOH = 14 - ( - log 0 . 2) = 13 . 301 002 10.0 points Solution A contains HCl and has a H + con- centration of 10 - 5 M. Solution B contains CH 3 COOH and has an H + concentration of 10 - 5 M. Which solution is more acidic and which solution has a greater pH? 1. Solution B is more acidic and has a greater pH. 2. Solution A is more acidic, but Solution B has a greater pH. 3. Solution B is more acidic, but Solution A has a greater pH. 4. Both solutions have identical acidities and pH. correct 5. Solution A is more acidic and has a greater pH. Explanation: [H + ] A = [H + ] B = 10 - 5 M pH = - log[H + ] We are told that both solutions have the same concentration of H + , so they will have identical acidities and an identical pH.
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