Consider a 1.0 L buffer containing 0.092 mol L-1 HCOOH and 0.100 mol L-1 HCOO-. What is the pH of the solution after adding 1.9 x 10-3 mol of HCl? Express your answer to 2 decimal places.
Molarity of hcl = moles / volume
= 1.9*10^-3 / 1
= 1.9*10^-3 M
Now it will reduce the amount of conjugate base and increases the amount of acid
Base = 0.1 - (1.9*10^-3 )
= 0.0981
Acid = 0.092 + (1.9*10^-3 )
= 0.0939
pKa of HCOOH = 3.8
pH = pKa + log ( conjugate base / acid )
= 3.8 + log ( 0.0981 / 0.0939)
= 3.82
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Consider a 1.0 L buffer containing 0.092 mol L-1 HCOOH and 0.100 mol L-1 HCOO-. What...
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