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In experiments D-1 and D-3, hyhrochloric acid was added one drop at a time to a buffer solution and to deionized water. Did the buffer minimize changes in ph with each addition compared to water? If it did, explain in general terms how the buffer was able to do it.

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Related questions

1. Compare the pHs of deionized water and tap water. Explain why the pH is not 7 and why the samples have different pHs.

2. Equal amounts of H+ and HO- are added to a buffer. What is the effect on the pH of the buffer? Explain.

3. How do you identify a suitable buffer system to maintain a pH of 3.0 in an aqueous solution?

1. A buffer is made by mixing 1.250 mol formic acid, HCOOH, with 0.750 mol sodium formate, HCOONa in enough water for a total volume of 1.00L. The Ka of formic acid is 1.87 x 10-4

a. What is the pH of this buffer?

b. If 0.075 mol HCl is added to this buffer, what is the pH of the resulting buffer? (assume no volume changes)

c. If 0.055 mol NaOH is added to this buffer, what is the pH of the resulting buffer? (Assume no volume changes)

2. A buffer solution contains 0.120 moles of propionic acid, HC3H5O2, and 0.100 moles of sodium propionate, NaC3H5O2, in 1.00 L of solution. Ka = 1.32 x 10-5 a. What is the pH of this buffer?

b. What is the pH of this buffer after the addition of 0.010 mol of NaOH?

c. Beginning with the initial buffer from part a, what is the pH of the buffer after the addition of 0.010 mol of HBr?

Help Please!

A) preparation of buffer solution:

6.606g of sodium acecate trihydrate was weighed out (MM=136 g/mole) in a small beaker. 25 ml of water was added to 100 ml volumetric flask. 8.00 ml of a 6 M acetic solution was added.

B) pH of water with added NaOH and HCl

Prepare two beakers (Beaker 1 and Beaker 2) and pipet 25 mL of deionized water into each beaker. Measure the pH of the water in the beaker. In Beaker 1, add 1 drop of 1 M NaOH into the beaker. Stir and read the pH of the resulting mixture. Add an additional drop of the 1 M NaOH solution to the beaker, stir and measure the pH. Add an addition 4 drops for a total of 6 mL and then 4 more drops for a total of 10 drops, add 10 more drops and finally using a volumetric or graduated pipet, add 1 mL of 1M NaOH and read the pH after each addition. To Beaker 2, add 1 drop of 1 M HCl into the beaker. Stir and read the pH of the resulting mixture. Add an addition 1 drop of the 1 M HCl solution to the beaker, stir and measure the pH. Add an addition 4 drops for a total of 6 drops and then an additional 4 drops for a total of 10 drops, add 10 more drops and finally add 1 mL of 1 M HCl, read the pH after each addition.

C) pH of buffer solution with added NaOH and HCl

Prepare two additional beakers (Beaker 3 and Beaker 4). Pipet 25 mL of the prepared buffer solution from part A into each beaker. Measure the pH of the buffer solution. To Beaker 3, using a graduated pipet, add 1 mL of 1 M NaOH. Stir and read the pH of the resulting mixture. Add an addition 1 mL of the 1 M NaOH solution to the beaker, stir and measure the pH. Add 4 mL more for a total of 6 mL and then an additional 4 mL for a total of 10 mL, finally add two 10 mL additions, read the pH after each addition. To Beaker 4 containing 25 mL of buffer, repeat the steps of beaker 3 with the addition of 1 M HCl into the beaker. Stir and read the pH after each addition.

Questions: only need 4-6

4)Calculate the pH of the buffer solution after 2 mL of NaOH was added to Beaker 3 and after 2 mL of HCl was added to Beaker 4. Compare this to your measured pH

5)Compare the measured pH for the addition of 1M NaOH and 1 M HCl to beaker 3 and 4 with the buffer solutions to the measured pH in Beaker 1 and 2 with the water.

6)From the measured pH of the acetic acid buffer solution above before the addition of any NaOH or HCl solution, calculate the K?a for acetic acid. Compare to CH3COOH Ka value which is 9.1x10^-6?

Water

Buffer solution

Beaker 1

Beaker 2

Beaker 3

Beaker 4

Total Volume of

1 M NaOH

added

pH

Total Volume of

1 M HCl

added

pH

Total Volume of

1 M NaOH

added

pH

Total Volume of

1 M HCl

added

pH

0 mL

7.08

0 mL

7.01

0 mL

6.02

0 mL

6.05

1 drop

9.86

1 drop

3.13

1 mL

11.87

1 mL

5.52

2 drops

10.38

2 drops

2.69

2 mL

12.38

2 mL

5.22

6 drops

10.86

6 drops

2.25

6 mL

12.74

6 mL

4.46

10 drops

11.08

10 drops

2.02

10 mL

12.87

10 mL

3.53

20 drops

11.35

20 drops

1.76

20 mL

12.99

20 mL

1.04

2 mL =
(40 drops)

11.68

2 mL

1.47

30 mL

13.06

30 mL

0.89

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