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Phantasy [73]
3 years ago
14

Calculate the pH of a solution prepared by dissolving 0.370 mol of formic acid (HCO2H) and 0.230 mol of sodium formate (NaCO2H)

in water sufficient to yield 1.00 L of solution. The Ka of formic acid is
Chemistry
1 answer:
Veronika [31]3 years ago
5 0

The question is incomplete, here is the complete question:

Calculate the pH of a solution prepared by dissolving 0.370 mol of formic acid (HCO₂H) and 0.230 mol of sodium formate (NaCO₂H) in water sufficient to yield 1.00 L of solution. The Ka of formic acid is 1.77 × 10⁻⁴

a) 2.099

b) 10.463

c) 3.546

d) 2.307

e) 3.952

<u>Answer:</u> The pH of the solution is 3.546

<u>Explanation:</u>

We are given:

Moles of formic acid = 0.370 moles

Moles of sodium formate = 0.230 moles

Volume of solution = 1 L

To calculate the molarity of solution, we use the equation:

\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}

To calculate the pH of acidic buffer, we use the equation given by Henderson Hasselbalch:  

pH=pK_a+\log(\frac{[salt]}{[acid]})

pH=pK_a+\log(\frac{[HCOONa]}{[HCOOH]})

pK_a = negative logarithm of acid dissociation constant of formic acid = 3.75

[HCOONa]=\frac{0.230}{1}  

[HCOOH]=\frac{0.370}{1}

pH = ?  

Putting values in above equation, we get:  

pH=3.75+\log(\frac{0.23/1}{0.37/1})\\\\pH=3.54

Hence, the pH of the solution is 3.546

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