Fundamentals Of Analytical Chemistry
9th Edition
ISBN: 9781285640686
Author: Skoog
Publisher: Cengage
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4. A weak acid HA has Ka = 4.3 x 10-6. The ionization constant Kb for its conjugate base A- is:
(а) 4.3 х 108
(b) 2.3 x 105
(с) 2.3 х 10-9
(d) 4.3 х
10-20
(a) Calculate the percent ionization of 0.00280 M carbonic acid (K, = 4.3e-07).
% ionization =
%
(b) Calculate the percent ionization of 0.00280 M carbonic acid in a solution containing 0.0380 M sodium hydrogen carbonate.
% ionization =
%
(a) Calculate the percent ionization of 0.00730 M carbonic acid (Ka = 4.3e-07).% ionization(b) Calculate the percent ionization of 0.00730 M carbonic acid in a solution containing 0.0600 M sodium hydrogen carbonate.% ionization
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- Be sure to answer all parts. Calculate the hydroxide ion concentrations of the following solutions at 25°C, given the pOH. (a) pOH= 8.89 x 10 M |-[_HO] (Enter your answer in scientific notation.) (b) рОН - 4.52 M -[ HO] < Prev 15 of 28arrow_forwardWrite the K₂ expression for an aqueous solution of hypochlorous acid: (Note that either the numerator or denominator may contain more than one chemical species. Enter the complete numerator in the top box and the complete denominator in the bottom box. Remember to write the hydronium ion out as H³O+, and not as H†) Ka ||arrow_forward1.What is the pH of 0.400 M ammonia soln? (Kb = 1.8 x 10-5) (Round-off your answer to two decimal place) 2.Predict the direction of the following reactions in aqueous solution: Write FORWARD (if the shift is from left to right)or BACKWARD (if the shift is from right to left) HF (aq)+ HCOO-(aq) ↔ HCOOH (aq) + F-(aq)arrow_forward
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