--------------------SKIP NH3------------------------------------

SOLVE THE TWO QUESTIONS BELOW

Calculation of the expected pHs of the weak acid and base are not required but recommended. Extra points for correct results. Show calculations only for one pH value of each. For the determination of [H_3O^+] and [OH^-], in table 3 show calculations only for the HCl solutions (in beakers A, B, C, and D).

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A lab experiment was conducted utilizing software to general a titration curve. 25 mL of an unknown analyte was titrated with .1015 M of NaOH solution.

The pH at the equivalence point for solution 1 = 7.83.

12.61mL of NaOH titrant added.

The pH at the equivalence point for solution 2 = 8.53. Total volume of NaOH titrants for solution 1

12.47mL of NaOH titrant added.

What is Ka for the weak acid?

Please help with any calculations here.

Part 2 consists of unknown acid solutions with added base in which the pH was measured. Please help calculate the [A-]/[HA] of buffers.

PLEASE HELP ANSWERING THE 3 PRELAB QUESTIONS FOR A BUFFER EXPERIMENT. Here is the back ground information:

1. Imagine you add some HCl to two solutions. One contains a pH buffer and the other is just plain water with no buffer. a. How would the addition of HCl affect the pH of these solutions? b. Would these solutionsâ pHs change to the same extent if the same amount of HCl were added? Why or why not?

2. If a solution contained formic acid (HCO2H) at a concentration of 0.414 M and its conjugate base, formate (HCO2 ï ), at a concentration of 0.303 M, what would the pH of the solution be? The pKa of formic acid is 3.77

3. You are asked to make a buffer to a pH of 3.00. Which acid (and its conjugate base) would be a good choice for this? Explain your choice.

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