a) We define pH as pH = -log [H + ]; therefore, pH = -log (8.8*10 -7 ) = 6.055 (

Question

a) We define pH as pH = -log [H+]; therefore,

pH = -log (8.8*10-7) = 6.055 (ans).

b) We know that [H+]*[OH-] = Kw = 1.0*10-14 where Kw is the ionic product of water. Use the relation to find out the value of [OH-].

[OH-] = Kw/[H+] = (1.0*10-14)/(8.8*10-7) = 1.136*10-8 M (ans).

c) The equilibrium constant (acid ionization constant), Ka is written as

Ka = [H+][A-]/[HA] where the square braces denote equilibrium concentrations.

Plug in values and get

Ka = (2.00*10-4)*(2.00*10-4)/(0.150) 2.667*10-7 (ans).

Ka is an equilibrium constant and hence, must be dimensionless.

Explanation / Answer

12/22/2017 1205 AM 63.9/100 Print 11 Gialatr Periodic Table Question 14 of 14 Maz saplingearning - Answer the following three questions: a) What is the pH of an aqueous solution with a hydrogen ion concentration of [H1-8.8 x10-7 M7 Number b) What is the hydroxide ion concentration, [OH"], in an aqueous solution with a hydrogen ion concentration Number OH c) A monoprotic acid, HA, dissociates: The equilibrium concentrations of the reactants and products are HA]-0.150 M H)=2.00 × 10-4 M [A-1-200-10-4 M Calculate the K, value for the acid HA below careers privacy policyterms of use c

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