solution9_pdf

# solution9_pdf - valdez(vv689 – Homework#9 – Holcombe...

This preview shows pages 1–2. Sign up to view the full content.

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: valdez (vv689) – Homework #9 – Holcombe – (52460) 1 This print-out should have 14 questions. Multiple-choice questions may continue on the next column or page – find all choices before answering. 001 10.0 points A 1 M solution of NaOH is used to titrate a 1 M solution of C 6 H 5 COOH (benzoic acid). If the K a of C 6 H 5 COOH is 5 × 10- 5 , what is the pH of the solution at the equivalence point? 1. 7 2. 13 3. not enough information 4. 5 5. 9 correct Explanation: Equal volumes of the titrant and analyte will be used to reach the equivalance point. Regardless of the starting volume, at the equivalance point the volume will be double the starting value and all of the benzoic acid will have been converted to benzoate. The solution will be 0 . 5 M C 6 H 5 COO- . K b = K w /K a = 10- 14 / (5 × 10- 5 ) = 2 × 10- 10 [OH- ] = ( K b C b ) 1 / 2 = (2 × 10- 10 · . 5) 1 / 2 = (10- 10 ) 1 / 2 = 10- 5 pOH = 5 pH = 9 002 10.0 points It was found that 25 mL of 0.012 M HCl neutralized 40 mL of NaOH solution. What was the molarity of the base solution? 1. 0.050 M 2. 0.0075 M correct 3. 0.012 M 4. 0.006 M Explanation: V HCl = 25 mL M HCl = 0 . 012 M V NaOH = 40 mL = 0 . 04 L The base is NaOH. To neutralize, mol H + = mol OH- . n H + = . 012 mol L (25 mL HCl) × 1 L 1000 mL × 1 mol H + 1 mol HCl = 0 . 0003 mol H + = n OH- = n NaOH M NaOH = mol L = . 0003 mol NaOH . 04 L = 0 . 0075 M NaOH 003 10.0 points What is the pH when 100 mL of 0.1 M HCl is titrated with 50 mL of 0.2 M NaOH?...
View Full Document

{[ snackBarMessage ]}

### Page1 / 4

solution9_pdf - valdez(vv689 – Homework#9 – Holcombe...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document
Ask a homework question - tutors are online