A 0.010 M solution of the weak acid, HB, is 1.0% ionized. K_a = ? a. 1.0 X 10^-6
ID: 510785 • Letter: A
Question
A 0.010 M solution of the weak acid, HB, is 1.0% ionized. K_a = ? a. 1.0 X 10^-6 b. 3.3 X 10^-6 c. 5.0 X 10^-6 d. 1.0 X 106-3 e. none of these 25. Acid ionization constants for H_2 Z and HZ are K_a1 = 10^-7 and K_a2 = 10^-15, respectively. Determine the molar concentration of the Z^2- ion produced in a 0.10 M aqueous solution of H_2 Z. a. 10^-30 b. 10^-22 c. 10^-15 d. 10^-7 e. none of these Determine the pH of 5.0 X 10^-7 M aqueous sulfuric acid; K_a1 > > > LARGE, K_a2 = 0.013. a. 1.0 b. 5.0 c. 6.0 d. 6.3 e. none of these A 0.1 M solution of the hypothetical weak acid HSp is found to have a pH of exactly 4.0. The ionization constant, K_a, of the acid is: a. 1 X 10^-4 b. 1 X 10^-5 c. 1 X 10^-6 d. 1 x 10^-7 e. none of theseExplanation / Answer
24)HB+H2O<-->B- +H3O+ [ionization rxn of HB]
ka=[B-][H3O+]/[HB] [H2O is in excess so taken to be at constant concentrtion throughout th rxn]
given,[HB]=0.01M
[B-]=1.0% of [HB]=1/100*0.01M=0.0001M
[B-]=[H3O+]=0.0001M
ka=(0.0001M)(0.0001M)/0.01M)=1.0*10^-6 M (a)
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