A solution contains 0.01 mole of lactic acid (pk a =3.60). You decide to add sod

Question

A solution contains 0.01 mole of lactic acid (pka =3.60). You decide to add sodium lactate to the solution to make a buffer of pH 4.5. what is the required molarity of sodium lactate in the final buffer solution?
The acid-base equilibrium reaction is, CH3CH(OH)COOH H2O <-- > CH3CH(OH)COO- H3O+ pK= 3.60

Please help, see solution, am not getting the same answers. Please explain if any missing steps?

Question 1A (5 pts). A solution contains 0.01 mole ofiactic acid (pKa 3.60). You decide to add sodium lactate to the solution to make a buffer of pH4.5. what isthe required molarity ofsodium lactate in the final buffer solution? oci 6.13

Explanation / Answer

Formula to calculate pH of acid buffer is,

pH = pKa + Log[salt]/[acid]

4.5 = 3.6 + Log[Salt]/(0.01)

Log[salt]/(0.01) = 0.90

[Salt]/0.01 = 100.90

[Salt]/0.01 = 7.94

[Salt] = 7.94 * 0.01

[Salt] = 0.0794 M

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