Experiment 1: Determination of the solubility of potassium bitartrate in water. NaOH concentration (given): 0.05 Balanced reaction equation (titration): Complete the table: Volume HC&H4O6° (cm³) Volume NaOH 0.05 M (cm³) Vend HCH.Or] (mol dm) Vstart AV (Vend-Vaar) (Rough titration) 11.50 I1.50 0 00 1 25.00 11.50 23.10 I1.60 23 3. 34 60 11.60 15.40 26.90 1.50 4 W. S666667 Average Solubility: Solubility constant: 2)
Experiment 1: Determination of the solubility of potassium bitartrate in water. NaOH concentration (given): 0.05 Balanced reaction equation (titration): Complete the table: Volume HC&H4O6° (cm³) Volume NaOH 0.05 M (cm³) Vend HCH.Or] (mol dm) Vstart AV (Vend-Vaar) (Rough titration) 11.50 I1.50 0 00 1 25.00 11.50 23.10 I1.60 23 3. 34 60 11.60 15.40 26.90 1.50 4 W. S666667 Average Solubility: Solubility constant: 2)
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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2 gram potassium bitartrate are put into a 250ml flask. 150ml water is added. The solution is stirred and left to settle.
the solution if filtered through a dry funnel into a 250ml breaker. 25ml of this solution was placed into 4 different flasks each. Approximately 11.5666667ml of NaOH was added to each flask. What is the concentration of the HC4H4O6-? (Asked on the right side of the table)
Transcribed Image Text:2.
Experiment 1: Determination of the solubility of potassium bitartrate in water.
NaOH concentration (given):
Balanced reaction equation (titration):
HO
Complete the table:
Volume NaOH 0.05 M
LOHOH
Volume HC&H.Os"
(cm3)
(mol.dm3)
AV Vend-
Vean)
Vstart
(Rough titration)
1.
23
09 79
3.
4.
Average
L999996 |
Solubility:
Solubility constant:
1.
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