homework6

homework6 - savage(jws775 – Homework#6 – Holcombe...

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Unformatted text preview: savage (jws775) – 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 . 14 M Ba(OH) 2 aqueous solution? 1. 8.7 2. 10 . 0854 3. 1 . 34472 4. . 552842 5. 13 . 4472 correct 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 . 14 M Ba(OH) 2 produces 0 . 28 M OH- . Ba(OH) 2 → Ba 2+ + 2 OH- ini . 14 M 0 M 0 M Δ- . 14 M +0 . 14 M 2(0 . 14 M) fin 0 M +0 . 14 M +0 . 28 M pH = 14- pOH = 14- (- log 0 . 28) = 13 . 4472 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 A is more acidic and has a greater pH. 4. Solution B is more acidic, but Solution A has a greater pH. 5. Both solutions have identical acidities and pH. correct 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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This note was uploaded on 04/22/2011 for the course CHEM 302 taught by Professor Mccord during the Spring '10 term at University of Texas.

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homework6 - savage(jws775 – Homework#6 – Holcombe...

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