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December 18, 2014

December 18, 2014

Posted by **tomi** on Wednesday, April 15, 2009 at 5:23pm.

a)4.0×10−2M HCl and 8.0×10−2M HOCl

b)0.105M NaNO2 and 5.00×10−2M HNO2

c)5.15x10-2M HCl and 7.62x10-2M NaC2H3O2

- chemistry -
**DrBob222**, Wednesday, April 15, 2009 at 5:42pmI would do the following:

a) This is a weak acid an a strong acid. I would calculate the Cl^- from HOCl with a common ion of H^+ from HCl, and recognize that (Cl^-) = (H^+) from HOCl. Then determine the H^+ from HCl, and add the two H^+ together.

b)This is a common ion problem or you can use the Henderson-Hasselbalch equation.

c)HCl + NaC2H3O2. It appears there is an excess of H^+ which will react with NaC2H3O2 to form HC2H3O2. That gives you a buffer of C2H3O2 and HC2H3O2 and you use the H-H equation to solve for pH.

Post your work if you get stuck.

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