HW7_Solutions

# I mixed it with some water i had sitting in a pan it

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I mixed it with some water I had sitting in a pan. It really mixed up nicely, I thought that I would say the solution was ? on this lovely day. 1. still neutral 2. now just basic 3. now acidic correct Explanation: Ammonium sulfate is the salt of a strong acid, so it is an acidic salt. 020 10.0 points Consider the ionization constants hypochlorous acid (HOCl) : K a = 3 . 5 × 10 - 8 ; ammonia (NH 3 ) : K b = 1 . 8 × 10 - 5 . A solution of ammonium hypochlorite (NH 4 OCl) is 1. neutral, because the anion hydrolyzes to a greater extent than the cation. 2. neutral, because the cation and the anion hydrolyze to the same extent. 3. basic, because the cation hydrolyzes to a greater extent than the anion. 4. neutral, because NH 4 OCl is a weak base/weak acid salt. 5. acidic, because the anion hydrolyzes to a greater extent than the cation. 6. acidic, because the cation and the anion hydrolyze to the same extent. 7. basic, because the cation and the anion hydrolyze to the same extent. 8. neutral, because the cation hydrolyzes to a greater extent than the anion. 9. basic, because the anion hydrolyzes to a greater extent than the cation. correct 10. acidic, because the cation hydrolyzes to a greater extent than the anion. Explanation: Compare NH + 4 + H 2 O NH 3 + H 3 O + K a = 1 K b = 1 1 . 8 × 10 - 5 = 55555 . 6 OCl - + H 2 O HOCl + OH - K b = 1 K a = 1 3 . 5 × 10 - 8 = 2 . 85714 × 10 7 The production of OH - occurs to the greater extent, making the solution basic. 021 10.0 points The pH of a 1 × 10 - 8 M solution of HNO 3 is 1. 8 2. 6 3. 6.96 correct 4. 7 Explanation: [H + ] HNO 3 = 1 × 10 - 8 M HNO 3 is a strong acid and dissociates com- pletely, but since the acid is so dilute, water makes a great contribution of hydronium ions to the solution that needs to be taken into consideration. [H + ] H 2 O = 1 × 10 - 7

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estrada (gse77) – Homework 7 – Sutcliffe – (52410) 6 [H + ] total = 1 . 1 × 10 - 7 pH = - log ( 1 . 1 × 10 - 7 ) = 6 . 95861 022 10.0 points This last question needs very little math if you think about it carefully..
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• Fall '07
• Holcombe

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