Lab 11 - Acid-Base Studies
Purpose
To measure pHs in a variety of solutions and mixtures and to account for the results obtained.Goals
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•To learn to use pH paper and a pH meter to measure the pH of a given solution.
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•To become familiar with the pH scale.
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•To observe pH changes produced upon addition of acid or base to a solution.
Introduction
Many substances can be classified as acids or bases. There are three definitions used to describe acids and bases, but we consider only the Brønsted definition here. In this theory, an acid is a proton (H+) donor and acids can usually be recognized because protons that can be transferred are written first in the chemical formula. For example, acetic acid has the formula HC2H3O2. Although it contains four protons, only one is acidic. A base is a proton (H+) acceptor. Protons have positive charge, so their acceptors usually have negative charge, i.e., most anions are bases. NH3 is the most common base that is not an anion. A Brønsted acid-base reaction is the transfer of a proton from the acid to the base to form their conjugate acid-base pairs. Conjugate acid-base pairs differ by exactly one proton. Thus, the conjugate base of an acid is obtained by removing one H+, so the conjugate base of HF is the F- ion. The conjugate acid of a base is obtained by adding one H+ to the base, so the conjugate acid of CN- is HCN. Brønsted acid-base reactions contain two conjugate acid-base pairs and nothing else.Figure 1
( 1 )
HA + H2O A- + H3O- | Ka =
|
( 2 )
A- + H2O HA + OH- | Kb =
|
( 3 )
H2O + H2O H3O+ + OH- | Kw = [H3O+][OH-] |
( 4 )
pH = -log[H3O+]
pH = -log[H3O+]
can be solved for the hydronium ion concentration to obtain equation 5[H3O+] = 10-pH
.
( 5 )
[H3O+] = 10-pH
Equipment
Reagents
Safety
HCl, NaOH, HC2H3O2 and NH3 are corrosive. They can attack the skin and cause permanent damage to the eyes. If any of these solutions splash into your eyes, use the eyewash immediately. Hold your eyes open and flush with water. If contact with skin or clothing occurs, flush the affected area with water. Have your lab partner notify your instructor about the spill. HCl, HC2H3O2 and NH3 solutions give off highly irritating vapors. Do not inhale them. Work with concentrated solutions under the hood so vapors do not build up in the lab. If you do inhale enough vapor to have a problem, move to fresh air. Have your lab partner notify your instructor about the accident. Acid-base reactions are highly exothermic. They can cause water to boil and splash hot, corrosive solution out of the vessel in which they were mixed. Do not directly combine solutions with concentrations greater than 0.1 M. Use caution when pouring solutions or disposing of them.Waste Disposal
All wastes should be put into the large waste container designated by your instructor. When disposing of concentrated solutions, pour them slowly.Lab Procedure
Please print the worksheet for this lab. You will need this sheet to record your data. In this experiment, you will be using pH meters. They have electrodes with a thin glass bulb at the tip. They break easily and are costly to replace. Be careful not to shove the electrode into the bottom of a test tube or drop the electrode. There is a protective guard around the tip, which should remain in place at all times. The guard will not protect against careless treatment. Please use extreme care when using this equipment. When the pH electrode is not in use, it should be capped with the pH 7 buffer solution.Part A: pH Measurements of Some Common Acid and Base Solutions
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1Number seven test tubes 1 - 7.
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2Fill each test tube ~ 1/4 - 1/2 full with solutions 1 - 7 listed in Table A.
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3Use a pH meter to measure the pH of each solution and record them in Table A. Rinse the pH meter thoroughly with deionized water between each measurement.
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4Discard the solutions and rinse each of the test tubes.
Part B: Acidity and Basicity of Some Household Chemicals
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1Place ten small strips of pH paper on the plastic work surface provided.
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2Put one or two drops of each of the solutions listed in Table B on a separate piece of paper. Because ammonia vapors will react with the pH paper, add ammonia (NH3) last! The bleach will oxidize the pH paper quickly; be sure to observe the initial color change of the pH paper.
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3Observe and record your results in Table B.
Part C: Acid-Base Reactions
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1Measure 10.0 mL of 0.10 M HCl in a 10 mL graduated cylinder and place in a clean 30 mL beaker.
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2Use a pH meter to measure the pH. Record this value in Table C as 0.0 mL NaOH.
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3Rinse the graduated cylinder used in Step 1 thoroughly and dry.
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4Measure 3.0 mL of 0.10 M NaOH and add it carefully to the HCl solution in the beaker and stir. Record the pH of the new solution in Table C as 3.0 mL NaOH.
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5Add an additional 3.0 mL of 0.10 M NaOH to the beaker, stir, and record the pH in Table C as 6.0 mL NaOH. The total volume in the beaker should now be 16 mL.
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6Add a final 6.0 mL of 0.10 M NaOH to the beaker and record the pH in Table C as 12.0 mL NaOH. The total volume should now be 22 mL.
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7Turn off the pH probe.
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8Discard the solution, wash and dry all your glassware and return it to the set-up area where you found it.
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9Before leaving, go to a computer in the laboratory and enter your results in the In-Lab assignment. If all results are scored as correct, log out. If not all results are correct, try to find the error or consult with your lab instructor. When all results are correct, note them and log out of WebAssign. The In-Lab assignment must be completed by the end of the lab period. If additional time is required, please consult with your lab instructor.