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Calculate the pH of the following aqueous solution:
0.35 M NaF (pKa for HF = 3.14)

I'm pretty sure I know how to calculate the pH by itself, but I am confused on how to get the equation. I'm not sure what HF has to do with this, other than it's an acid. I'm probably overthinking it because it's worded differently. Thanks in advance!​

Respuesta :

samueladesida43

The pH of an aqueous solution that has a concentration of 0.35 M NaF and pKa for HF = 3.14 is 3.6.

How to calculate pH?

The pH of a solution refers to the degree of acidity or alkalinity of the solution. It can be calculated using the Henderson-Hasselbalch Equation as follows:

pH = pka + log ([A-]/[HA])

Where;

  • A- = conjugate base
  • HA = weak acid

pH = pKa + log([F-]/[HF])

pH = 3.14 + log(1/0.35)

pH = 3.14 + 0.4559 = 3.595

Therefore, the pH of an aqueous solution that has a concentration of 0.35 M NaF and pKa for HF = 3.14 is 3.6.

Learn more about pH at: https://brainly.com/question/15289741

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