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For the next three problems, consider 1.0 L of a solution which is 0.6 M HC2H3O2...

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Chemistry

For the next three problems, consider 1.0 L of a solution whichis 0.6 M HC2H3O2 and 0.2 MNaC2H3O2 (Ka forHC2H3O2 = 1.8 x 10-5).Assume 2 significant figures in all of the given concentrations sothat you should calculate all of the following pH values to twodecimal places.

1. Calculate the pH of this solution.

2. Calculate the pH after 0.10 mol of HCl has been added to theoriginal solution. Assume no volume change on addition ofHCl.

3. Calculate the pH after 0.20 mol of NaOH has been added to theoriginal buffer solution. Assume no volume change on addition ofNaOH.

Answer & Explanation Solved by verified expert
4.4 Ratings (964 Votes)
Solution Given solution is the solution of weak acid and its conjugate base therefore its buffer solution Using the Henderson equation we can calculate its pH pH pka log baseacid pka log ka pka log 18105 pka 474 lets use the pka value in the above equation pH474 log 0206 pH 4740477 pH426 2    See Answer
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