Problem: Calculate the pH of the solution that results from each of the following mixtures.55.0 mL of 0.17 M HCHO2 with 80.0 mL of 0.13 M NaCHO2

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FREE Expert Solution

We’re being asked to calculate the pH of a solution the containing HCHO2 (formic acid) and NaCHO(sodium formate)

A solution that contains a weak acid and its conjugate base is a buffer solution. The pH of a buffer solution can be determined using the Henderson-Hasselbalch equation.

pH = pKa + log(conjugate baseweak acid)

Given solution:

The solution is composed of 0.17 M HCO2 and 0.13 M NaCHO2

 HCHO2 is a weak acid where NaCHO2 is its conjugate base

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Problem Details

Calculate the pH of the solution that results from each of the following mixtures.

55.0 mL of 0.17 M HCHO2 with 80.0 mL of 0.13 M NaCHO2

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Our tutors have indicated that to solve this problem you will need to apply the Buffer concept. You can view video lessons to learn Buffer. Or if you need more Buffer practice, you can also practice Buffer practice problems.

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Based on our data, we think this problem is relevant for Professor Subedi's class at Murray State University.