9.R: Titration of Vinegar (Report)
- Page ID
- 306784
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| Trial 1 | Trial 2 | Trial 3 | |
|---|---|---|---|
| Initial Buret Reading | |||
| Final Buret Reading | |||
| Volume of NaOH used | |||
| Molarity of NaOH used | |||
| Volume of vinegar used |
Data Analysis
- Write the balanced equation for the neutralization reaction between aqueous sodium hydroxide and acetic acid.
| Trial 2 | Trial 2 | Trial 3 | |
|---|---|---|---|
| Moles of NaOH used in titration | |||
| Moles of acetic acid neutralized in vinegar sample | |||
| Molarity of acetic acid in vinegar | |||
| Average molarity | |||
2. Determine the molarity of acetic acid in vinegar. Show all calculations for one trial below.
| Trial 1 | Trial 2 | Trial 3 | |
|---|---|---|---|
| Mass of HC2H3O2 in vinegar sample | |||
| Mass of vinegar sample (assume density = 1.00 g/mL) | |||
| Mass Percent of HC2H3O2 in vinegar | |||
| Average Mass Percent | |||
3. Determine the mass percent of acetic acid in vinegar. Show all calculations for one trial below.
Questions
- What was the purpose of the phenolphthalein indicator in this experiment? Be specific.
- Suppose you added 40 mL of water to your vinegar sample instead of 20 mL. Would the titration have required more, less or the same amount of NaOH (aq) for a complete reaction? Explain.
- Consider a 0.586 M aqueous solution of barium hydroxide, Ba(OH)2 (aq). How many grams of Ba(OH)2 are dissolved in 0.191 dL of 0.586 M Ba(OH)2 (aq)?
- What volume (in L) of 0.586 M Ba(OH) 2 (aq) contains 0.466 ounces of Ba(OH)2 dissolved in it?
- If 16.0 mL of water are added to 31.5 mL of 0.586 M Ba(OH)2 (aq), what is the new solution molarity?