In the following chemical equation indicate the Bronsted-Lowry acid: HCl(aq) + H

Question

In the following chemical equation indicate the Bronsted-Lowry acid: HCl(aq) + H_2O(aq) rightarrow H_3O^+(aq) + Cl(aq) What is the conjugate base of the Bronsted-Lowry acids HPO^2-_4? Write a balanced equation for the dissociation of the Bronsted-Lowry acids HSO^-_4 in water. From the following chemical reactions determine the relative Bronsted-Lowry acids strengths (strongest to weakest) HCIO_4(aq) + H_2O(l) rightarrow H_3O^+(aq) + ClO^-_4(aq) HNO_2(aq) + H_2O(l) doubleheadarrow H_3O^+ (aq) + NO^-_2 (aq) + NO^-_2(aq) HClO_4 (aq) > H_3O^+ (aq) > HNO_2(aq) HClO_4 (aq) > HNO_2(aq) > H_3O^+ (aq) H_3O^+ (aq) > HClO_4 (aq) > HNO_2(aq) H_3O^+ (aq) > HNO_2(aq) > HClO_4 (aq)

Explanation / Answer

30) according to Bronsted-Lowry theory molecule which can give H+ ion is said to be acid.

HCl is giving H+ ion so it is acid.

31) he conjugate acid base pairs are just differed by one H+ ion.

if we remove one H+ from HPO4-2 then we got conjugate base

conjugate base = PO4-3

32) HSO4-(aq) +   H2O(l) -------------> H3O+(aq)  + SO4-2(aq)

33) HClO4 is strongst acid HNO2 is weak acid

answer = option a

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