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6. (13 pts) A solution of 0.1000 M HCl was used to titrate 25.00 mL of Na2CO3 (0.0800 M). Calculate the pH of the solution when adding following amount of HCI. For H2CO3 = Ka2 4.69 x 10-11 Kal = 4.46 × 10-7 a) 0.00 mL (before the titration) b) 5.00 mL c) at the first equivalent point d) 45.00 mL

6. (13 pts) A solution of 0.1000 M HCl was used to titrate 25.00 mL of Na2CO3 (0.0800 M). Calculate the pH of the solution when adding following amount of HCI. For H2CO3 = Ka2 4.69 x 10-11 Kal = 4.46 × 10-7 a) 0.00 mL (before the titration) b) 5.00 mL c) at the first equivalent point d) 45.00 mL

Fundamentals Of Analytical Chemistry
Fundamentals Of Analytical Chemistry
9th Edition
ISBN:9781285640686
Author:Skoog
Publisher:Skoog
Chapter14: Principles Of Neutralization Titrations
Section: Chapter Questions
Problem 14.38QAP
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6. (13 pts) A solution of 0.1000 M HCl was used to titrate 25.00 mL of Na2CO3 (0.0800 M). Calculate the pH of the solution when adding following amount of HCI. For H2CO3 = Ka2 4.69 x 10-11 Kal = 4.46 × 10-7 a) 0.00 mL (before the titration) b) 5.00 mL c) at the first equivalent point d) 45.00 mL
Transcribed Image Text:6. (13 pts) A solution of 0.1000 M HCl was used to titrate 25.00 mL of Na2CO3 (0.0800 M). Calculate the pH of the solution when adding following amount of HCI. For H2CO3 = Ka2 4.69 x 10-11 Kal = 4.46 × 10-7 a) 0.00 mL (before the titration) b) 5.00 mL c) at the first equivalent point d) 45.00 mL
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