Acid-base Titration Assignment solves questions in end. if necessary use notebook to make the curve. A student conducted the following experiment in the lab. 50.00 mL of acetic acid (of unknown concentration) was pipetted into a 150 mL Erlenmeyer flask. An indicator was added and the pH of the solution was recorded. 0.1 M NaOH (a strong base) was added to the Erlenmeyer flask from a buret. The contents of the flask were continuously stirred and the pH was recorded every 2 mL using a pH meter. Data Collected: Volume of NaOH added (mL) pH 0.0 2.87 10.0 4.14 25.0 4.74 40.0 5.35 50.0 8.72 60.0 11.96 75.0 12.30 1. The chemicals involved in the titration are NaOH (a strong electrolyte) and CH3COOH (a weak electrolyte). Predict the shape of the titration curve that would be obtained from the data above. Also predict what the pH at the equivalence point will be. 2. What is the volume of NaOH at the equivalence point? 3. What is the pH at the equivalence point?
Acid-base Titration Assignment solves questions in end. if necessary use notebook to make the curve. A student conducted the following experiment in the lab. 50.00 mL of acetic acid (of unknown concentration) was pipetted into a 150 mL Erlenmeyer flask. An indicator was added and the pH of the solution was recorded. 0.1 M NaOH (a strong base) was added to the Erlenmeyer flask from a buret. The contents of the flask were continuously stirred and the pH was recorded every 2 mL using a pH meter. Data Collected: Volume of NaOH added (mL) pH 0.0 2.87 10.0 4.14 25.0 4.74 40.0 5.35 50.0 8.72 60.0 11.96 75.0 12.30 1. The chemicals involved in the titration are NaOH (a strong electrolyte) and CH3COOH (a weak electrolyte). Predict the shape of the titration curve that would be obtained from the data above. Also predict what the pH at the equivalence point will be. 2. What is the volume of NaOH at the equivalence point? 3. What is the pH at the equivalence point?
Acid-base Titration Assignment solves questions in end. if necessary use notebook to make the curve. A student conducted the following experiment in the lab. 50.00 mL of acetic acid (of unknown concentration) was pipetted into a 150 mL Erlenmeyer flask. An indicator was added and the pH of the solution was recorded. 0.1 M NaOH (a strong base) was added to the Erlenmeyer flask from a buret. The contents of the flask were continuously stirred and the pH was recorded every 2 mL using a pH meter. Data Collected: Volume of NaOH added (mL) pH 0.0 2.87 10.0 4.14 25.0 4.74 40.0 5.35 50.0 8.72 60.0 11.96 75.0 12.30 1. The chemicals involved in the titration are NaOH (a strong electrolyte) and CH3COOH (a weak electrolyte). Predict the shape of the titration curve that would be obtained from the data above. Also predict what the pH at the equivalence point will be. 2. What is the volume of NaOH at the equivalence point? 3. What is the pH at the equivalence point?
solves questions in end. if necessary use notebook to make the curve. A student conducted the following experiment in the lab. 50.00 mL of acetic acid (of unknown concentration) was pipetted into a 150 mL Erlenmeyer flask. An indicator was added and the pH of the solution was recorded. 0.1 M NaOH (a strong base) was added to the Erlenmeyer flask from a buret. The contents of the flask were continuously stirred and the pH was recorded every 2 mL using a pH meter. Data Collected:
Volume of NaOH added (mL)
pH
0.0
2.87
10.0
4.14
25.0
4.74
40.0
5.35
50.0
8.72
60.0
11.96
75.0
12.30
1. The chemicals involved in the titration are NaOH (a strong electrolyte) and CH3COOH (a weak electrolyte). Predict the shape of the titration curve that would be obtained from the data above. Also predict what the pH at the equivalence point will be. 2. What is the volume of NaOH at the equivalence point? 3. What is the pH at the equivalence point? 4. What does the value for pH at the equivalence point tell you about the strength of the acid? 5. Calculate the concentration of the acetic acid solution.
Definition Definition Method of quantitative analysis for determining the concentration of an acid or base by exactly neutralizing it with a standard solution of base or acid having known concentration.
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