9.0.1 moles of weak acid is dissolved into 1L of water and the pH is 3.2. What s

Question

9.0.1 moles of weak acid is dissolved into 1L of water and the pH is 3.2. What s the percentage ionization? 4.3percentage 1.6 percentage 0.63 percentage 5.0 percentage not enough information For the reaction: AB_3(g) A(g) + 3B (g) What is the equilibrium constant expression if the initial concentration of AB_3 is 0.1 M and the equilibrium concentration of A is represented by x? Assume the initial concentrations of A and B are both zero. K = x-3x/0.1-x K = x-x^3/(0.1 -x)^3 K = x x^3/(0.1-3x)^3 K = x (3x)^3/0.1-x none of the above 9. What is the pK_a, of the conjugate acid of Pyridine, which has a K_b of 1.7 times 10^-9? 5.23 0 7.05 0 5.8 times 10^-7 0 6.95 More information is needed. Calculate K_a, for the acid HNO_2, that has the following concentrations at equilibrium: [HNO_2]=9.87 M, [NO_2]=0.026 M, and [H^+]=0.026 M. 1.55 times 10^-4 1.12 times 10^-2 1.21 times 10^-2 3.43 times 10^-3 None of the above

Explanation / Answer

Ans 9 . C . 0.63 %

Since pH is 3.2 , so [H+] = 10-3.2 = 6.3 x 10-4 M

percent ionisation is the relative number of acid molecules that have dissociated

= (6.3 x 10-4/ 0.1) x 100

= 0.63%

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