HA(aq) + H_2O(l) H_3O^+(aq) + A^-(aq) Consider the following acids and their equ
ID: 539082 • Letter: H
Question
HA(aq) + H_2O(l) H_3O^+(aq) + A^-(aq) Consider the following acids and their equilibrium constants for reaction with water at 25 degree C. If all the acids have the same initial concentration, which is the strongest acid (i.e. which donates the most protons to water)? A) HBrO, K_C = 2.0 times 10^-9 B) HNO_2, K_C = 4.5 times 10^-4 C) HF, K_C = 3.5 times 10^-4 D) HIO_3, K_C = 1.7 times 10^-1 Salt solubilities can be compared by the concentration of cation formed when the salt dissolves in the general reaction: M_a X_b (s) a M^b+ (aq) + b X^a- (aq). Given the following salts and their equilibrium constants for the reaction above at 25 degree C, which salt is the least soluble? A) AgCl, K_C = 1.8 times 10^-10 B) Ag_2SO_4, K_C = 1.2 times 10^-5 C) CaCO_3, K_C = 2.6 times 10^-9 D) CaF_2, K_C = 1.5 times 10^-10 Consider the reaction HCO^-_3 (aq) + H_2O(l) CO^-2_3 (aq) + H_3O+ (aq) The K_eq for this reaction is 5.6 times 10^-11. Describe what will happen to the reaction if the concentration of each reactant is [HCO^-_3] = 5.6 times 10^-11 [H_3O^+] = 1.2 times 10^-11 [CO^-_3] = 5.6 times 10^-11Explanation / Answer
Ans 24. HIO3 Kc = 1.7 x 10-1
The equillibrium constant of the acid is the ratio of concentration of products to that of concentration of reactants .
The acid with most amount of protons , will have highest Kc value amongst all .
So the strongest acid amongst all here is HIO3.
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