The K_a of acetic acid is 1.8 * 10^-5. What is the PH at 25.0 degree C of an aqu

Question

The K_a of acetic acid is 1.8 * 10^-5. What is the PH at 25.0 degree C of an aqueous solution that is 0.100 M in acetic acid? +2.87 -2.87 -11.13 +11.13 +6.61 The acid-dissociation constants of sulfurous acid are K_al=1.7* 10^ -2and K_a2 = 6.4 *10^-8 at 25.0 degree C. Calculate the PH of a 0.163 M aqueous solution of sulfurous acid. 4.53 l.28 1.86 6.21 1.93 The acid-dissociation constants of phosphoric acid are K_al=7.5 * 10^-3, K_a2=6.2 * 10^-8. and K_a3 = 4.2*10^-13 at 25.0 degree C. What is the pH of a 2.5 M aqueous solution of phosphoric acid? 1.82 0.40 2.51 0.86 0.13 The pH of a 0.55 M aqueous solution ammonia, NH_3. at 25.0 degree C is 11.50. What is the value ofK_bforNH_3?

Explanation / Answer

14. H+ concentration of acetic acid is ( ka1 * concentration).5 = .0013M

so PH = - log .0013 = 2.87 answer A

15 H+ concentration of acetic acid is ( ka1 * concentration).5 = .05

so PH = - log .05 = 1.28 answer B

16. H+ concentration of acetic acid is ( ka1 * concentration).5 = .137

so PH = - log .137 = .86 answer D

17.

concentration of OH- = 10-2.5    ( POH = 14 - PH)

KB = (10-2.5)2 / .55 = 1.8 * e-5

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