Volumetric flasks Beakers Serologic pipetters Aspirators Vials/test tubes Cone. H3PO4 (85% w/w, sp gr. 1.70, MM 98) Cone. HCL (37.3% w/w sp. Gr. 1.18, MM 36) Glacial acetic acid (99.7% ww, sp gr. 1.05, MM 60) NaOH pellets NaH2PO4 Na2HPO4 Acid-base indicators: Bromophenol Blue Bromocresol green Phenol red Methyl red Methyl orange Phenolphthalein Thymol Blue pH paper pH meter Weighing balance For chemicals, refer from the template below. Research the chemicals to be used especially those that are new to you and write down the information needed. Name of Chemical Molec. Weight (g/mol) Melting point Boiling point Density (g/mL) General properties Methodolody: (Include a short summary of the overall experimental plan you are going to run. You may use flow chart or bullet form for this part. Sketches of any experimental set-ups used in the experiment or the workup procedures). Preparation of buffers Prepare 250ml of the following buffer solutions. Concentration Buffer solution pka Desired ph 1 0.50 M Phosphate 2.12 2.0 2 0.50 M Phosphate 2.12 3.0 3 0.50 M Acetate 4.70 5.0 4 0.50 M Phosphate 7.21 7.0 5 0.050 M Phosphate 7.21 7.50 6 0.010 M Phosphate 7.21 8.0 7 0.50 M Phosphate 12.32 12.0 Identify the waek acid and conjugate base of the components of each buffer. Compute the buffer components using the Henderson-Hasselbalch equation. Preparation of reagents Prepare 500 ml of the following aqueous solutions. 0 M HCL 0M NaOH Determination of buffer capacity Calibrate the pH meter @ pH 4, 7 and 10. Prepare 100 ml each of 0.1 M HCL and 0.1 M NaOH. Using assigned buffer determine the buffer capacity by adding 0.1 M HCl in 1 ml portions from a buret to a 20 ml of the buffer until its pH changes as monitored with a pH meter. Record the columen added. Repeat this step using 0.1 M NaOH instead

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

Materials/Chemicals:

Volumetric flasks

Beakers

Serologic pipetters

Aspirators

Vials/test tubes

Cone. H3PO4 (85% w/w, sp gr. 1.70, MM 98)

Cone. HCL (37.3% w/w sp. Gr. 1.18, MM 36)

Glacial acetic acid (99.7% ww, sp gr. 1.05, MM 60)

NaOH pellets

NaH2PO4

Na2HPO4

Acid-base indicators:

Bromophenol Blue

Bromocresol green

Phenol red

Methyl red

Methyl orange

Phenolphthalein

Thymol Blue

pH paper

pH meter

Weighing balance

For chemicals, refer from the template below. Research the chemicals to be used especially those that are new to you and write down the information needed.

Name of Chemical	Molec. Weight (g/mol)	Melting point	Boiling point	Density (g/mL)	General properties

Methodolody: (Include a short summary of the overall experimental plan you are going to run. You may use flow chart or bullet form for this part. Sketches of any experimental set-ups used in the experiment or the workup procedures).

Preparation of buffers

Prepare 250ml of the following buffer solutions.

	Concentration	Buffer solution	pka	Desired ph
1	0.50 M	Phosphate	2.12	2.0
2	0.50 M	Phosphate	2.12	3.0
3	0.50 M	Acetate	4.70	5.0
4	0.50 M	Phosphate	7.21	7.0
5	0.050 M	Phosphate	7.21	7.50
6	0.010 M	Phosphate	7.21	8.0
7	0.50 M	Phosphate	12.32	12.0

Identify the waek acid and conjugate base of the components of each buffer. Compute the buffer components using the Henderson-Hasselbalch equation.

Preparation of reagents

Prepare 500 ml of the following aqueous solutions.
1. 0 M HCL
2. 0M NaOH

Determination of buffer capacity

Calibrate the pH meter @ pH 4, 7 and 10.
Prepare 100 ml each of 0.1 M HCL and 0.1 M NaOH.
Using assigned buffer determine the buffer capacity by adding 0.1 M HCl in 1 ml portions from a buret to a 20 ml of the buffer until its pH changes as monitored with a pH meter. Record the columen added. Repeat this step using 0.1 M NaOH instead.

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