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April 16, 2014

Homework Help: Chemistry

Posted by Kw1h on Friday, September 28, 2012 at 2:33am.

You are asked to prepare 500. mL of a 0.150 M acetate buffer at pH 5.00 using only pure acetic acid, 3.00 M NaOH, and water. Calculate the quantities needed for each of the following steps in the buffer preparation.

1. Add acetic acid to ~400 mL of water in a 500 mL beaker. How many grams of acetic acid do you need?

2. Add 3.00 M NaOH solution while stirring and monitoring the pH with a pH electrode until the pH is 5.00. What volume of NaOH solution do you calculate that you will need?

By taking the desired moles of the solution (0.15M x 0.5L = 0.075 moles), I was able to calculate the needed Acetic Acid (Question #1 = 4.5g)

(Desired Moles) 0.075 x (Formula Weight) 60.05 = 4.5g Acetic Acid.

Where I am stuck is Question 2. After using HH:

(AC/HAC)=10^(5-4.76), (AC/HAC)=1.74

After this, I multiplied my HAC (0.075) by my 1.74 to achieve my AC (0.13).

I know I need to incorporate this with my Molarity of base (3.00M), but am not sure how. Am I even on the right track?

Thank you very much in advance.

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