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1 Dispose of chemicals as instructed by your
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teacher 2 Return all lab equipment to its proper place 3 Report any broken or damaged equipment 4 Wash your hands thoroughly before leaving the laboratory
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Copyright Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc
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Name of substance Hydrochloric acid Sulfuric acid Acetic acid Sodium hydroxide Ammonium hydroxide Calcium hydroxide
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Color of phenolphthalein
Acid or base
4 5 6
Analyze and Conclude
1 Applying Concepts Describe how litmus paper may be used to differentiate between
an acid and a base
2 Classifying Complete the last column of Data Table 1 3 Applying Concepts Describe how phenolphthalein may be used to differentiate
between an acid and a base
Laboratory Manual
Chemistry: Matter and Change 19
Name
Date
Class
LAB 191
LABORATORY MANUAL
4 Observing and Inferring Explain why the phenolphthalein remained colorless when
100 mL of 100M hydrochloric acid and about 9 mL of 100M sodium hydroxide were mixed
5 Observing and Inferring What is the significance of the permanent red color change
in step 6
6 Observing and Inferring Why was a drop of 100M hydrochloric acid added to make
the red color disappear in step 7
7 Observing and Inferring Describe the solid residue remaining after heating the
contents of the evaporating dish to near dryness
8 Drawing a Conclusion Identify the solid residue remaining after heating the contents
of the evaporating dish to near dryness
Copyright Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc
9 Measuring and Using Numbers Write a balanced chemical equation for the reaction
between hydrochloric acid and sodium hydroxide
10 Predicting What quantity of 200M sodium hydroxide would be needed to neutralize
100 mL of 100M hydrochloric acid Explain
11 Error Analysis Compare your answers in Data Table 1 to the answers of other stu-
dents in your class What are some reasons that the answers might be different
Real-World Chemistry
1 Explain the difference between using antacids 2 Explain why neutralization of soil is important
and acid inhibitors in the treatment of excess stomach acid
in the agricultural economy
Chemistry: Matter and Change 19
Laboratory Manual
Name
Date
Class
LABORATORY MANUAL
Use with Section 194
Determining the Percent of Acetic Acid in Vinegar
itration is a procedure used for determining the concentration of an acid or a base by neutralizing a known volume of the acid or base with a solution of a standard base or an acid A standard solution is one whose molarity has been accurately determined experimentally In a titration, one solution is added slowly to the other until the equivalence point is reached At the equivalence point of a neutralization reaction, the moles of acid and moles of base are equal An indicator, placed in the reaction mixture, tells you by means of a color change, when the equivalence point has been reached Your experimental data the volume and molarity of the standard solution and the volume of the unknown acid or base solution are all that you need to calculate the molarity of the unknown acid or base
In this activity, you will first standardize a NaOH solution by using the solution to titrate a known mass of oxalic acid (H2C2O4) Then, you will use your standardized solution to titrate a sample of vinegar Vinegar is a solution of acetic acid (HC2H3O2) From your titration data, you will be able to calculate the number of moles and the mass of the acetic acid in your vinegar sample and determine the percent of acetic acid in vinegar
Problem
Copyright Glencoe/McGraw-Hill, a division of the McGraw-Hill Companies, Inc
Materials
sodium hydroxide pellets (NaOH) acetic acid solution (white vinegar) oxalic acid (H2C2O4 2H2O) phenolphthalein solution 250-mL Erlenmeyer flasks (2) 250-mL beaker 250-mL plastic bottle with screw top 100-mL graduated cylinder ring stand burette burette clamp balance label distilled water
What is the percent of acetic acid in vinegar
Objectives
Prepare a solution of NaOH Determine the molarity of the NaOH solution Determine the percent of acetic acid in vinegar
Safety Precautions
Always wear safety goggles, gloves, and a lab apron Oxalic acid and sodium hydroxide are toxic Sodium hydroxide is caustic, and oxalic acid is corrosive Wipe up any water spills to avoid slippage
Pre-Lab
1 Briefly explain what happens in a neutralization 4 Read the entire laboratory activity Form a
reaction 2 What is a standard solution 3 State the equation used to determine percent error
Laboratory Manual
hypothesis about using a standard solution to determine the concentration of another solution Record your hypothesis on page 151
Chemistry: Matter and Change 19
Name
Date
Class
LAB 192
LABORATORY MANUAL
8 Clean and rinse a 250-mL Erlenmeyer flask
Procedure
Part A: Standardizing an NaOH Solution
1 Label a clean 250-mL plastic bottle Standard
NaOH Solution Write your name and the date of preparation on the label 2 In the 250-mL plastic bottle, dissolve about 50 NaOH pellets in 200 mL of distilled water CAUTION: Sodium hydroxide is caustic 3 Set up the burette, burette clamp, and 250-mL Erlenmeyer flask as shown in Figure A
Figure A
Burette Burette clamp
Stopcock
Ring stand
with distilled water Measure the mass of the empty flask and record it in Data Table 1 Add about 10 g of oxalic acid to the flask and measure its mass again Record the mass of the flask and acid in Data Table 1 Pour about 50 mL of distilled water into the flask containing the acid Gently swirl the flask until the oxalic acid dissolves Add 3 drops of phenolphthalein solution to the flask containing the acid solution Place the flask under the burette so that the tip of the burette is 1 2 cm inside the mouth of the flask Begin the titration by allowing small amounts of the NaOH to flow into the flask containing the acid Swirl the flask to allow the base and acid to mix When the pink color of the indicator begins to take longer to disappear, you are close to the equivalence point Adjust the stopcock of the burette so that the base runs into the acid drop-wise Continue to add drops of base until a permanent light pink color is obtained Record the final volume of the NaOH solution in Data Table 1
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