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The pH of a solution that is 0.50 M in HCOOH is 2.045.
How do we calculate the pH?
pH of the solution will be calculated by taking the negative logarithm of the concentration of H⁺ ion.
Given chemical reaction will be:
HCOOH(aq) ⇄ H⁺(aq) + HCOO⁻(aq)
Initial: 0.50 0 0
Equilibrium: 0.50-x x x
Given that, pKa = 3.75
Ka = [tex]10^{-pKa}[/tex]
Ka = [tex]10^{-3.75}[/tex] = 0.000178
Ka for the above equation will be written as:
Ka = [H⁺][HCOO⁻]/[HCOOH]
Ka = (x)² / (0.50-x)
x is negligible as compared to 0.5, so the equation becomes
0.000178 = (x)² / 0.50
x² = (0.000178)(0.5) = 0.000089
x = 0.009
[H⁺] = 0.009M
pH will be calculated as:
pH = -log(0.009) = -(-2.045) = 2.045
Hence pH of the solution is 2.045.
To know more about pH, visit the below link:
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