SPRING BREAK PRACTICE III

# SPRING BREAK PRACTICE III - What is the pH of the buffer...

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Thursday, March 17, 2011 – SPRING BREAK PRACTICE III =] 1. 2 H 2 O(l) H 3 O + (aq) + OH - (aq) K w = 1.0 x 10 -14 at 25 ° C | K w = 3.8 x 10 -14 at 40 ° C What is the pH of pure water at 40 ° C? 2. Sodium azide, NaN 3 is an ionic compound consisting of Na + ions and N 3 - ions. A 0.50 M solution of NaN 3 has a pH of 9.21. Calculate K a for hydrazoic acid, HN 3 . 3. Calculate the pH of a 0.50 M KCN solution. K a (HCN) = 6.2 x 10 -10

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4. Aqueous buffer solutions can be prepared conveniently by partially neutralizing a weak acid with a strong base or a weak base with a strong acid.
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Unformatted text preview: What is the pH of the buffer solution prepared by adding 0.200 mol of solid NaOH to 1.000 L of 0.500 M HCN solution? (K a = 6.2 x 10-10 for HCN; assume no change in volume when the NaOH is added.) 5. Consider a titration in which NaOH is being added to a flask which originally contains 1.0 liter of 1.0 M HX. The titration curve for this process is shown below. pH Volume NaOH added Based on this data, what is the approximate K a for acid HX?...
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## This note was uploaded on 12/22/2011 for the course CHEM 01:160:162 taught by Professor Donaldseigel during the Spring '10 term at Rutgers.

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SPRING BREAK PRACTICE III - What is the pH of the buffer...

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