Answer:
See explanation below.
Step-by-step explanation:
To solve this problem we use the Henderson-Hasselbach formula:
pH = pKa + log [A⁻]/[HA] where [A⁻]/[HA] is the ratio of the concentration of conjugate base to acid which is what we are seeking to answer, and we are given the values for pH and pKa.
pH = pKa + log [ HCOO⁻]/^[HCOOH]
4.00 = 3.75 + log [ HCOO⁻]/^[HCOOH]
4.00 - 3.75 = log [ HCOO⁻]/^[HCOOH]
0.25 = log [ HCOO⁻]/^[HCOOH]
Taking antilog to both sides of the equation
10^0.25 = [ HCOO⁻]/^[HCOOH]
1.77 = [ HCOO⁻]/^[HCOOH]
This ratio tell us that the concentration of conjugate base is 1.77 times the concentration of HCOOH, so we have a buffer solution since HCOOH is a weak acid and therefore it will not dissociate into H⁺ and HCOO⁻ to an appreciable extent.
Remember buffer solutions are prepared by adding the salt of the conjugate base to the weak acid according to the desired pH.