1. Calculate the moles of KHP you titrated for each trial. (KHP is KHC8H4O4). MW = 204.23 g/mol. Determine the number of moles of NaOH required to neutralizw the KHP. Use the mole-mole ratio provided inthe balanced equation. Place answers in data table 2(second picture format) 2. Calculate the volume, in mililiters, of NaOH used to neutralize the KHP. Convert to Liters. Place answers in data table 2. 3. Calculate the molarity of the NaOH solution in units of moles/liter. Place answers in data table 2. Data Table 2:TrialTrial 1Trial 2Trial 3Moles of KHPMoles of NaOHtitratedVolume ofNaOH, LMolarity of NaOHsolution, mols/L4. Find the average molarity of the solution from the results of the three trials in question# 3.5. You will be graded on accuracy in this experiment. Circle the molarity you would like tohave graded, trial #1, trial #2, trial 3 or the average of all three trials. If your trials areclose, it is most often best to have the average value graded. If they differ, choose the trialyou think you did better on. DATA AND OBSERVATIONSPart 1: Reading the buret17.90 mL 21.00 MLFirst buret reading. ml.Second buret reading, mL. 22.80 ML, 25.30 MLPart II: Titration of the sampleData Table 1:Mass KHP (g)Initial buret reading(mL)Final buret reading(mL)Trial 2Trial 1Trial 31.99 g 2.009 1.9990.00ML 0.00ML 0.10ML38.50ML 38.70 38.65MLML

The balanced equation for the reaction between KHP and NaOH can be represented as:…

Answered: 1. Calculate the moles of KHP you…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions

Section4.9: Spectrophotometry

Problem 3.1ACP

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1. Calculate the moles of KHP you titrated for each trial. (KHP is KHC8H4O4). MW = 204.23 g/mol. Determine the number of moles of NaOH required to neutralizw the KHP. Use the mole-mole ratio provided inthe balanced equation. Place answers in data table 2(second picture format)

2. Calculate the volume, in mililiters, of NaOH used to neutralize the KHP. Convert to Liters. Place answers in data table 2.

3. Calculate the molarity of the NaOH solution in units of moles/liter. Place answers in data table 2.

Data Table 2:
Trial
Trial 1
Trial 2
Trial 3
Moles of KHP
Moles of NaOH
titrated
Volume of
NaOH, L
Molarity of NaOH
solution, mols/L
4. Find the average molarity of the solution from the results of the three trials in question
# 3.
5. You will be graded on accuracy in this experiment. Circle the molarity you would like to
have graded, trial #1, trial #2, trial 3 or the average of all three trials. If your trials are
close, it is most often best to have the average value graded. If they differ, choose the trial
you think you did better on.

DATA AND OBSERVATIONS
Part 1: Reading the buret
17.90 mL 21.00 ML
First buret reading. ml.
Second buret reading, mL. 22.80 ML, 25.30 ML
Part II: Titration of the sample
Data Table 1:
Mass KHP (g)
Initial buret reading
(mL)
Final buret reading
(mL)
Trial 2
Trial 1
Trial 3
1.99 g 2.009 1.999
0.00ML 0.00ML 0.10ML
38.50ML 38.70 38.65
ML
ML

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