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kozerog [31]
3 years ago
8

What is the pH of a solution that contains 0.83M HCN (Ka = 4.9x10-10) and 0.64 M potassium cyanide?

Chemistry
1 answer:
oksian1 [2.3K]3 years ago
5 0

Answer:

pH= 9.2

Explanation:

Henderson hasselbach equation

pKa= log Ka= log (4.9 x 10^-10)=9.3

pH=Pka+log \frac{[A-]}{[HA]}

pH=9.3+log \frac{[CN-]}{[HCN]}

pH=9.3+log \frac{[0.64 M]}{[0.83 M]}

pH= 9.2

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How many moles of HCl are required to completely neutralize 0.30 moles of Ca(OH)2?
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Read 2 more answers
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