A 0.20 mol L-1 solution of benzoic acid, C6H5COOH, at 25 °C has a pH of 2.45 at equilibrium. What is the Ka for benzoic acid?

(b) Calculate the pH of 0.0005 mol dm-3 ethanois acid when its pKa = 4.75 CH;COOH() -> CH;COO (a H(a + Ka = pH =

Calculate K₂ or K from experimental data. The pH of a 0.14-M solution of chlorous acid (HCIO₂) is measured to be 1.49. Use this information to determine a value of Ka for chlorous acid. HCIO₂(aq) + H₂O(l)=CIO₂ (aq) + H₂O˚(aq) K₂ =

What is the pH of a 0.40 M solution of benzoic acid, C6H5COOH?

Consider a weak acid "HA". What is the pH of a 0.957 mol L-1 solution of HA? The KA of HA is 7.09 x 10-7 .

A 0.018 M solution of salicylic acid, HOC6H4CO2H, has the same pH as 0.0038 M HNO3solution. (a) Write an equation for the ionization of salicylic acid in aqueous solution. (Assume only the –CO2H portion of the molecule ionizes.) (b) What is the pH of solution containing 0.018 M salicylic acid? (c) Calculate the Ka of salicylic acid.

Given the equilibrium reactions below and their equilibrium constants. H3O+ (aq) + A (aq) ⇒ HA(aq) + H₂O (1) Kc1 = 2.5 x 104 A™ + H₂O(1) OH- (aq) (aq) + HA(aq) 2.5 x 10-10 What is the value of Kc for the reaction 2 H₂O) H3O+ + OH (aq) (aq) 1.0 x 10¹4 6.3 x 10-6 1.0 x 10-14 none of the answers are correct Kc2 =

Formic acid, from the Latin formica, is the acid present in ants sting. What is the concentration of HCOO- at equilibrium if the initial concentration of formic acid, HCOOH, is 1.15 M (Ka = 1.7 x 10-4). What is the hydronium concentration at equilibrium of a weak acid whose concentration is 3.10 M and Ka is 2.0 x 10-4? A 1.60 M solution of an unknown acid has a pH of 1.22. What is the Ka?

The pH of an aqueous solution of 0.400 M hydrocyanic acid, (Ka (HCN) = 4.00 × 10-10) is

M11.