What concentrations of acetic acid (pKa = 4.76) and acetate would be required to

Question

What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.9? Note that the concentration and/or pH value may differ from that in the first question. STRATEGY 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [A–]/[HA]. 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. Step 1: The ratio of base to acid is 1.4. Step 2: The mole fraction of acetate is 0.58, and the concentration of acetate is 0.088. Step 3: Calculate the concentration of acetic acid. What concentrations of acetic acid (pKa 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.97 Note that the concentration and/or pH value may differ from that in the first question STRATEGY 1. Rearrange gtenderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetie acid), IA V 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid That is, there are 1.4 molecules Step 1: The ratio of base to acid is 1.4. of acetate for each molecule of acetic acid Step 2: The mole fraction of acetate is 0.58, and the concentration of acetate is 0.088. Step 3: Calculate the concentration of acetic acid. Number lacetic acid]- D acetic acid)- Previous Give Up & View Solution Check Answer Next Exi Hint about us |careers partners prvacy policy terms of use contact us 21 f8 20 od F4 F7 FS

Explanation / Answer

from the given data

[acetate]/[aceticacid] = 1.4 ----- 1

[acetate] = 0.088 M    -- -2

from 1&2

[Aceticacid] = 0.088/1.4 = 0.0628 M

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