You are asked to prepare 500. mL of a 0.100 M acetate buffer at pH 5.00 using on
ID: 505177 • Letter: Y
Question
You are asked to prepare 500. mL of a 0.100 M acetate buffer at pH 5.00 using only pure acetic acid (MW = 60.05 g/mol, pK_a = 4.76), 3.00 M NaOH, and water. Answer the following questions regarding the preparation of the buffer. How many grams of acetic acid will you need to prepare the 500 mL buffer? Note that the given concentration of acetate refers to the concentration of all acetate species in solution. What volume of 3.00 M NaOH must you add to the acetic acid to achieve a buffer with a pH of 5.00 at a final volume of 500 mL? (Ignore activity coefficients.) Pour the beaker contents into a 500 mL volumetric flask. Rinse the beaker several times and add the rinses to the flask. Swirl the flask to mix the solution. Add water to the mark to make the volume 500 mL. Stopper the flask and invert how many times to ensure complete mixing? 1 2 20Explanation / Answer
Answer:
By taking the desired moles of the solution (0.100 M x 0.5L = 0.05 moles), I was able to calculate the needed Acetic Acid
Acetic Acid needed (g) = (Desired Moles) x (Formula Weight)
Acetic Acid (g)=0.05 X 60.05
=3.025g
2. What volume of 3.00 M NaOH must you add to the acetic acid to achieve a buffer with a pH of 5.00 at a final volume of 500 mL? (Ignore activity coefficients.)
You want 0.05 mols to start HAc. You're right there (and the 3.05 g is correct).
5.00 = 4.75 + log (b/a)
b/a = 1.77 or
b = 1.77*a or
a = 0.564*b.
Substitute this into the below for a.
b+ a = 0.100 M x 0.5L = 0.05 moles.
b + 0.564b = 0.05
1.564b = 0.05
b = 0.0319 moles.
3.0M = 0.0319 mols/L
Molarity = Moles /Volume
Volume=0.0319/3.00
=0.01063 L=10.63 ml
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