Calculate the pH at the equivalence point in titrating 0.072 M solutions of each of the following with 0.023 MNaOH. (a) hydrobromic acid (HBr) pH (b) hydrocyanic acid (HCN), Ka ==4.9e-10 pH=(c) carbonic acid (H2CO3), Ka= 4.3e-07 pH =

(a) Hydrobromic acid (HBr): Reaction at equivalence point: HBr+NaOH→NaBr+H2O pH=7.0 (neutral) (b)…

Answered: Calculate the pH at the equivalence…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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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in an acidbase titration, 10.0 mL (VB)of NH3 (Ka(NH+) = 5.8*10^ - 19) 0.18 M (CB) are titrated at the equivalence point (EP) with 10.0 ml (VA) of HCI 0.18 M (CA). Calculate (to two decimal places) the pH of the solution at the equivalence point.
A buffer solution contains 0.77 mol of hydrosulfuric acid (H2S) and 0.43 mol of sodium hydrogen sulfide (NaHS) in 5.70 L.The Ka of hydrosulfuric acid (H2S) is Ka = 9.5e-08.(a) What is the pH of this buffer?(b) What is the pH of the buffer after the addition of 0.44 mol of NaOH? (assume no volume change)(c) What is the pH of the original buffer after the addition of 0.08 mol of HI? (assume no volume change)
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Calculate the pH at the equivalence point in titrating 0.072 M solutions of each of the following with 0.023 M NaOH. (a) hydrobromic acid (HBr) pH (b) hydrocyanic acid (HCN), Ka = = 4.9e-10 pH = (c) carbonic acid (H 2CO3), Ka = 4.3e-07 pH =