1. Label four clean 100 and/or 150 mL beakers: A, B, C, and D.

2. Add 40 mL of distilled water to beakers A and C. Be sure that the graduated cylinder is well rinsed before using it.

3. Use a graduated cylinder to add 40 mL of the prepared sodium acetate/acetic acid buffer solution to both beakers B and D.

4. Record the initial pH of each the solutions A-D. Make sure to rinse the pH electrode with distilled water between readings.

5. Pipette 1.0 mL of 6 M HCl, hydrochloric acid solution into beakers A and B. Thoroughly mix the solutions.

6. Pipette 1.0 mL of 6 M NaOH, sodium hydroxide solution into beakers C and D. Thoroughly mix the solutions

-What is the volume of 6HCl used for addition into beaker A,B,C,D?

-Calculate the pH of beaker A and B after the addition of beaker 6M HCL

-Calculate the pH of beaker C and D after the addition of beaker 6M NaOH

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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

The beaker weigh 01 g, 4.1 g of sodium acetate was added intothe beaker, 8.5 mL of 6.0 M acetic acid was added to the beaker andsodium acetate, 91.5 mL of distilled water into the solutions, fourclean 150 mL beakers, 1,2,3,4 were labeled for identification. 40mL of the buffer solution was poured into beaker 1 and beaker 3. 40mL of distilled water was added into beaker 2 and beaker 4. Four PHsolutions were recorded as follows

Beaker PH1 PH2

1 5.33 5.27

2 6.13 2.80

3 5.30 5.32

4 5.26 12.08

1.0 mL of 6.0 M HCL solution waspipetted into beaker 1 and beaker 2.

1.0 mL of 6.0 M NaOH solution was pippeted intobeaker 2 and beaker 4.

To compare the measured Ph, calculate pH of a buffer solution;of water + NaOH (aq)

Could you break it down steps for me to understand how arrive tothe conclusion, including clear formulas. Not just summarizing it.Would be helpful if you break it down in details as I would like tounderstand it. Thanks. Make it a clear formula

Please help me calculate the theoretical pH of a buffer solution containing 0.012mol NaC2H3O2 + 0.012mol of HC2H3O2 in 25mL of solution with an added 6M HCl.