Calculate the K_b value for NO_2^- given K_a for HNO_2 is 4.5 Times 10^-4. 2.2 T

Question

Calculate the K_b value for NO_2^- given K_a for HNO_2 is 4.5 Times 10^-4. 2.2 Times 10^-11 4.5 Times 10^10 4.5 Times 10^-4 2.2 Times 1063 1.7 Times 10^-9 Given the following acids and K_a values: HClO_4 1 Times 10^7 CH_3 COOH 1.8 Times 10^-5 HCN 4.9 Times 10^-10 HF 3.5 Times 10^-4 What is the order of increasing base strength? (weakest base rightarrow strongest base) CN^-, F^-, CH_3COO^-, ClO_4^- CN^-, CH_3COO^-, F^-, ClO_4^-. CN^-, ClO^-, F^-, CH_3COO^- ClO_4^, CH_3COO^-, -CN^-, F^- ClO_4^-, F^-, CH_3COO^-, CN^- a 0.6 M solution of a weak acid (HA) The pH of the acid solution is 4.0. Calculate the concentration of H* in the solution. 1 Times 10^4 M 4.0 M 0.6 M 2 Times 10^-3 M

Explanation / Answer

Problem 1

Ka x Kb = Kw

(4.5 x 10-4) Kb = (1.0 x 10-14)

Kb = 2.22 x 10-11

Problem 2

The larger the Ka the greater the ionization of the acid, the stronger it is, the lower the pH.

HClO4 = 1x107

CH3COOH = 1.8x10-5

HCN = 4.9x10-10

HF = 3.5x10-4

HClO4 > HF > CH3COOH > HCN increasing acidity (observe greater than sign)

HClO4 , HF , CH3COOH , HCN increasing base strength

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