(1). What will be the pH when 50.0 ml of 2.00 M carbonic acid is mixed 20.0 ml of 3.00 M sodium bicarbonate? The Ka of carbonic is 4.30 x 10-7 (2). For the buffer system in Problem no. 1, what will be the pH when: (a) 15.0 ml of 0.500 M HCl and (b) when 15.0 ml of 0.750 M NaOH is added to the buffer?
(1). What will be the pH when 50.0 ml of 2.00 M carbonic acid is mixed 20.0 ml of 3.00 M sodium bicarbonate? The Ka of carbonic is 4.30 x 10-7 (2). For the buffer system in Problem no. 1, what will be the pH when: (a) 15.0 ml of 0.500 M HCl and (b) when 15.0 ml of 0.750 M NaOH is added to the buffer?
Chemistry
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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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(1). What will be the pH when 50.0 ml of 2.00 M carbonic acid is mixed 20.0 ml of 3.00 M sodium bicarbonate? The Ka of carbonic is 4.30 x 10-7
(2). For the buffer system in Problem no. 1, what will be the pH when:
(a) 15.0 ml of 0.500 M HCl and (b) when 15.0 ml of 0.750 M NaOH is added to the buffer?
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