# Chem2 hw7s - Yoon, Seong Meen – Homework 7 – Due: Oct...

This preview shows pages 1–3. Sign up to view the full content.

Yoon, Seong Meen – Homework 7 – Due: Oct 29 2007, 11:00 pm – Inst: James Holcombe 1 This print-out should have 24 questions. Multiple-choice questions may continue on the next column or page – fnd all choices beFore answering. The due time is Central time. 001 (part 1 oF 1) 10 points The curve For the titration oF hypochlorous acid (HOCl) with NaOH(aq) base is given below. 0 2 4 6 8 10 12 14 0 20 40 60 80 100 120 140 Volume oF base (mL) pH Estimate the p K a oF hypochlorous acid. C a = 0 . 75, C b = 0 . 5775, and the volume oF HOCl is 100 mL. 1. 77 2. 38 . 5 3. None oF these 4. 10 . 2 5. 7 . 5 correct Explanation: K a = 3 . 5 × 10 - 8 C a = 0 . 75 C b = 0 . 5775 V HOCl = 100 mL 0 2 4 6 8 10 12 14 0 20 40 60 80 100 120 140 Volume oF base (mL) pH (77,10 . 2) (38 . 5,7 . 5) The equivalence point oF this titration is when the curve is at an in±ection point (nearly vertical); i.e. , at a volume oF 77 mL . The pH at the equivalence point oF this titration is 10 . 2 pH . The p K a can be Found at one-halF the vol- ume oF the equivalence point; i.e. , at 38 . 5 mL. The p K a is 7 . 5 pH From looking at the graph. The Formula is p K a = - log ( K a ) = - log 3 . 5 × 10 - 8 · = 7 . 45593 pH . Note : The p K a is the pH when the mole Fraction is 0.5. 002 (part 1 oF 1) 10 points It required 25.0 mL oF 0.333 M NaOH solution to completely neutralize 15.0 mL oF H 2 SO 4 so- lution. What was the molarity oF the H 2 SO 4 ? 1. 0.555 M 2. 0.200 M 3. 1.11 M 4. 0.278 M correct Explanation: V NaOH = 25.0 mL [NaOH] = 0.333 M

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

View Full Document
Yoon, Seong Meen – Homework 7 – Due: Oct 29 2007, 11:00 pm – Inst: James Holcombe 2 V H 2 SO 4 = 15.0 mL The balanced equation for the reaction is H 2 SO 4 + 2 NaOH Na 2 SO 4 + 2 H 2 O We determine the moles of NaOH used. ? mol NaOH = 0 . 025 L soln × 0 . 333 mol NaOH 1 L soln = 0 . 00832 mol NaOH Using the mole ratio from the balanced chemical equation we calculate the moles of H 2 SO 4 needed to react with this amount of NaOH: ? mol H 2 SO 4 = 0 . 00832 mol NaOH × 1 mol H 2 SO 4 2 mol NaOH = 0 . 00416 mol H 2 SO 4 This is the amount of H 2 SO 4 that must have been in the 15.0 mL sample. Molarity is moles solute per liter of solution: ? M H 2 SO 4 = 0 . 00416 mol H 2 SO 4 0 . 0150 L solution = 0 . 277 M H 2 SO 4 003 (part 1 of 3) 10 points Below is the pH curve of a weak acid (HA) titrated with strong base. Answer the fol- lowing question based on the interpretation of this pH curve. Be as accurate as possible. 0 5 10 15 20 25 30 35 40 45 50 55 60 0 1 2 3 4 5 6 7 8 9 10 11 12 13 Titration Curve Amount of Base added (mL) pH What is the pH at the equivalence point of this titration? Your answer must be within ± 10%. Correct answer: 6 . 3 pH. Explanation: The inFection points are shown below. 0 5 10 15 20 25 30 35 40 45 50 55 60
This is the end of the preview. Sign up to access the rest of the document.

## This note was uploaded on 05/14/2009 for the course CH 53575 taught by Professor Hackert during the Spring '09 term at University of Texas at Austin.

### Page1 / 9

Chem2 hw7s - Yoon, Seong Meen – Homework 7 – Due: Oct...

This preview shows document pages 1 - 3. Sign up to view the full document.

View Full Document
Ask a homework question - tutors are online