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)
Chapter10: Effect Of Electrolytes On Chemical Equilibria
Section: Chapter Questions
Problem 10.16QAP
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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)
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