This is a buffer problem. I know the answer is simple but I\'m just not getting

Question

This is a buffer problem. I know the answer is simple but I'm just not getting to it. Here is the setup:

I have created a buffer with the theoretical pH of 4.4 from 0.7315 g of Citiric Acid Monohydrate and 0.4468 g Sodium Citrate Dihydrate. This buffer was dissolved and brought to volume in 100 mL of DI water. The measured pH was 3.38.

I calculated the Ionic strength to be 0.091 and the Activity Coefficient to be 0.1185. This gave a "real" pH of 3.47.
To bring the pH to my desired pH of 4.4 I added 3.61 mL of a 1.02 M NaOH stock solution.

I now need to calculate the concentrations, the theoretical pH, the new ionic strength, activity Coefficient, and new "real" pH. I know I need to use an I.C.E. table, but I'm not quite sure how or where to start. Again, I know it's simple I'm just not able to see it. Please help.

Explanation / Answer

To prepare buffer of pH 4.4 of citric acid and sodium citrate, kindly follow this method:

Prepare 0.1 M solution of citric acid monohydrate.

Prepare 0.1 M solutin of sodium citrate dihydrate.

Now, for pH = 4.4; take 49.5ml 0.1 M citric acid solution and 50.5ml of 0.1M sodium citrate solution and mix well together.

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