Question

Initial NaOH volume mL |
Final NaOH volume mL |
Total volume of NaOH used mL |

9 |
0 |
9 |

9 |
0.2 |
8.8 |

9 |
0.3 |
8.7 |

Three trials, average volume of NaOH used mL = 8.8

Average volume of NaOH used mL |
Concentration CH3COOH in vinegar mol/L |
% CH3COOH in vinegar |

8.8 |
72 |
83 |

1. The manufacturer of the vinegar used in the experiment stated that the vinegar contained 5.0% acetic acid. What is the percent error between your result and the manufacturer statement? Show your work.

2. If a 7.0 mL sample of vinegar was titrated to the stoichiometric equivalence point with 7.5 mL of 1.5M NaOH, what is the mass percent of CH3COOH in the vinegar sample? Show your work.

Answer #1

1. From data in the first table,

average volume of NaOH used = 8.8 ml

moles of NaOH used = 1.5 M x 8.8 ml = 13.2 mmol

mass of acetic acid in vinegar = 13.2 mmol x 60.0 g/mol/1000 = 0.80 g

% CH3COOH in vinegar = 0.80 g x 100/volume of vinegar solution

volume of vinegar solution is not given above. Feed the value and determine the % final answer.

2. moles NaOH used = 1.5 M x 7.5 ml = 11.25 mmol = 0.01125 mol

mass percent CH3COOH in vinegar = (0.01125 mol x 60 g/mol x 100)/7.0 ml = 9.64%

A. The manufacturer of the vinegar used in the experiment stated
that the vinegar contained 5.0% acetic acid. What is the percent
error between your result and the manufacturerâ€™s statement? B. What
challenges would you encounter with the titration if you had used
apple cider vinegar or balsamic vinegar as the analyte instead of
white vinegar? The issue with using a dark color vinegar is the
coloring in the end. C. How would your results have differed if the
tip...

Please check my answers and let me know if they correct.
Thanks
Exercise 1: Determining the Concentration of Acetic Acid
Data Table 1. NaOH Titration Volume.
Initial NaOH Volume (mL)
Final NaOH Volume (mL)
Total volume of NaOH used (mL)
Trial 1
9 ml
0
9
Trial 2
9 ml
0.2
8.8
Trial 3
9 ml
0.3
8.7
Average Volume of NaOH Used (mL) : 8.8
Data Table 2. Concentration of
CH3COOH in Vinegar.
Average volume of NaOH used (mL)...

1)
A 21.30 mL volume of 0.0975
M NaOH was used to titrate 25.0
mL of a weak monoprotic acid solution to the
stoichiometric point. Determine the molar
concentration of the weak acid solution.
2.08 M
0.114 M
0.0831 M
0.00390 M
2.44 M
2)
For a weak acid (CH3COOH) that is
titrated with a strong base (NaOH), what species
(ions/molecules) are present in
the solution at the stoichiometric point?
CH3COO-
H2O
Na+
NaCl
HCl

A
sample of acetic acid (weak acid) was neutralized with .05M NaOH
solution by titration. 34 mL of NaOH had been used. Show your work.
CH3COOH + NaOH-----CH3COONa + H2O
a) Calculate how many moles of NaOH were used?
b) How many moles of aspirin were in a sample?
c) Calculate how many grams of acetic acid were in the
sample
d) When acetic acid is titrated with NaOH solution what is the
pH at the equivalence point? Circle the...

What volume of a 0.1048 M NaOH is needed to neutralize (get to
the equivalence point) 50.00 mL of a 0.0876 M acetic acid solution?
What is the pH at the equivalence point? Show your work please!

please find the following and show work so i have a better
understanding:
- volume of NaOH used
- moles of NaOH used
- moles of HC2H3O2
- mass of HC2H3O2
- mass percent of vinegar solution
- molarity of HC2H3O2
- deviation
- percent error
- average mass percent of vinegar
- average molarity of vinegar
Table 2: Titration of standard
NaOH with a HC2H3O2
Solution
Trail 1
Trial 2
Trial 3
M of NaOH
0.4936 M
0.4936 M...

NH3/NH4 buffer:
Mass NH4Cl used 1.3738g
volume NaOH used 21.2 ml
initial pH (0f the buffer) 9.6, pH after 1 drop HCl 9.03, pH
after 10 drops HCl 8.91
Dilute NaOH solution
Initial pH 10.35
pH :1 drop HCl 10.21, 10 drops HCl 2.85
Acetate buffer (0.500)
Mass of CH3COONa * 3H2O 10.935
volume CH#COOH 44.3 ml
initial pH 4.89
1.0 ml of NaOH pH 4.93
initial volume 2.2
final volume 16.2
final pH 5.91
Acetate buffer (0.100)
Mass of...

Water Hardness Lab follow up Questions
Trial
Initial EDTA Volume (mL)
Final EDTA Volume (mL)
Total Volume of EDTA Used (mL)
1
8.5
6
2.5
2
5.0
3.0
2.0
3
3.0
0.5
2.3
Average Volume of EDTA Used (mL):
2.3
Average Volume of EDTA Used (mL)
Concentration Ca2+ Ions Per Liter of Water
(mol/L)
Water Hardness (ppm CaCO3)
2.3
0.0023
230
2.Approximately how much calcium would you ingest by drinking
six, 8-oz glasses of your local water? Hint: 1 oz...

Data:
Trial
Initial Volume of EDTA (mL)
Final Volume of EDTA (mL)
1
10ml
9ml
2
9ml
8ml
3
8ml
7ml
Calculate the concentration of Ca+2 ions per liter of water
using the following equation.
Calculate the water hardness using your results from part 2 and
the following equation.
Calculate the average water hardness for the three trials
conducted. Show all work.

Use your mean NaOH molarity, the mean acid/base volume ratio
from Project D, and the HCl/NaOH stoichiometric ratio from the
balanced equation of Project D to calculate a precise concentration
for (to standardize) your 0.1 M HCl. Show this as a single, sample
calculation with explicit units in your notebook and on your report
sheet. Given the information of mass of KHP is 0.9191g, Volume
delivered is 45.03 mL, mean of molarity NaOH is 0.09971 mol/L,
acid/base ration is 1.018,...

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