0.100 moles of HF and 0.200 moles of NaCN in 1.00 liter solution. (This is a lit
ID: 774300 • Letter: 0
Question
0.100 moles of HF and 0.200 moles of NaCN in 1.00 liter solution.
(This is a little bit tricky, because here you are mixing a weak acid with a weak base! This is not a common situation that we have encountered before. Can you write the Bronsted Lowry acid - base reaction between this weak acid and this weak base? Can you calculate the value of the equilibrium constant for this reaction? What can you conclude about this reaction based on the numerical value (or size!) of the equilibrium constant? You should see that you can essentially run this reaction to completion! After this reaction is complete, can you calculate the pH of the resulting solution? Hint: Is there a buffer?)Type your question here
Explanation / Answer
NaCN ? Na++ CN-SinceCN-is the conjugate base of a very weak acid, it is a relatively strong base.
Na+, on the other hand, is the conjugate acid of an extremely strong base, NaOH, and is extremely weak.
The CN-can be expected to react with water to control the pH in the salt solution.
CN-+H2O?HCN+OH-
Initial0.20M-----00
Change
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