HW_2 - 6 H 2 O(NO 2 3(K a = 5.1 x 10-1 6 Determine the pH...

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CHEM 150 HOMEWORK #2 Due: Monday, 6/30/08 1. Determine the pH at the equivalence point of a titration of 200.0 mL solution of 0.100M HNO 2 (K a = 5.1 x 10 -4 ) with 0.250M NaOH. 2. Determine the pH of a 500.0 mL solution of 353.0mg NaCN (K a = 2.1 x 10 -9 for HCN). 3. Determine the pH of a solution of 40.0 mL of 0.0600M HClO 4 mixed with 30.00mL of 0.100M NaOCl (K a = 3.0 x 10 -8 for HOCl). 4. Determine the pH of a 400.0 mL solution of 14.67mg HC 8 H 7 O 3 (K a = 3.88 x 10 -4 ) and 20.59mg Na C 8 H 7 O 3 . 5. Determine the pH of a solution of 25.0 mL of 0.0400M NaOH mixed with 20.00mL of 0.100M HC
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Unformatted text preview: 6 H 2 O(NO 2 ) 3 (K a = 5.1 x 10-1 ). 6. Determine the pH of a solution of 25.0 mL of 0.0400M NaOH mixed with 20.00mL of 0.0750M (NH 4 ) 2 SO 4 (K b = 1.76 x 10-5 for NH 3 ). 7. What volume of 0.307 M NaOH must be added to 200.0mL of 0.425M acetic acid (K a = 1.75 x 10-5 ) to produce a buffer of pH = 4.250? 8. A 0.0450M solution of unknown acid HA is 0.60% dissociated. Determine the pK a for this acid. 9. Given that the pK b for NO 2-is 10.85, find the ratio [HNO 2 ]/[NO 2-] in a solution of sodium nitrite at pH = 2.00....
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This note was uploaded on 08/06/2008 for the course CHEM 150 taught by Professor Buratto during the Summer '08 term at UCSB.

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