The ratio of the concentration of formate to formic acid required in a buffer system is 3.16 : 1.
pH = 4.25; pH of the solution
pKa = 3.75
Henderson–Hasselbalch equation: pH = pKa + log(cs/ck)
4.25 = 3.75 + log(cs/ck)
log(cs/ck) = 4.25 - 3.75
log(cs/ck) = 0.5
cs/ck = 10∧(0.5)
cs/ck = 3.16; ratio of formate to formic acid
A buffer can be defined as a substance that prevents the pH of a solution from changing by either releasing or absorbing H⁺ in a solution.
Buffer is a solution that can resist pH change upon the addition of an acidic or basic components and it is able to neutralize small amounts of added acid or base, pH of the solution is relatively stable.
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