You are given 60 ml of 0.50 M acetic acid/acetate buffer to test. The starting c

Question

You are given 60 ml of 0.50 M acetic acid/acetate buffer to test. The starting composition of the two major species are:

Concentration of CH3COOH is 0.300 M, Concentration of CH3COO- is 0.200 M

a) Use the Handerson-Hasselbach equation to estimate the initial pH of the buffer.

b) You add 1.0 ml of 1.00 M HCl to the buffer. Calculate the molarity of H3O+ added as HCl, and the final molarities of acetic acid and acetate ion at equilibrium. What is the new value of pH?

c)Now take a fresh 60 ml of the buffer and add 1.0 ml of 1.00 M NaOH. Using steps similar to those above, calculate the new pH of the solution.

Explanation / Answer

a) pH = pKa + log [Csalt]/[Cacid]

b) pH = pKa + log [moles of salt- moles of HCl added]/[moles of acid + moles of HCL added]

c) pH = pKa + log [moles of salt+ moles of HCl added]/[moles of acid - moles of HCL added]

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