The acids have to be arranged in the increasing order of acid strength and the reason has to be justified.

Question

For the following acid-base reaction, (1) predict the products, showing both reactants and products complete Lewis structures and arrows showing electron flow; (2) label each structure with the lowing: Bronsted acid, Bronsted base, conjugate acid, conjugate base; (3) give a brief definition of a ronsted acid and Bronsted base; (4) predict the direction of the equilibrium and justify your answer. HC0OH + CH3 Nta PRん106Y pkb = 3.36

Answer 1

Question

Chapter 11, Problem 11D.35E

Interpretation Introduction

Interpretation:

The acids have to be arranged in the increasing order of acid strength and the reason has to be justified.

Expert Solution & Answer

Trending nowThis is a popular solution!

See solution

Check out sample textbook solution

Students have asked these similar questions

For the following acid-base reaction, (1) predict the products, showing both reactants and products complete Lewis structures and arrows showing electron flow; (2) label each structure with the lowing: Bronsted acid, Bronsted base, conjugate acid, conjugate base; (3) give a brief definition of a ronsted acid and Bronsted base; (4) predict the direction of the equilibrium and justify your answer. HC0OH + CH3 Nta PRん106Y pkb = 3.36

In a Bronsted acid-base reaction, the stronger acid reacts with the stronger base to produce a weaker acid and a weaker base. Thus, whether a reaction “goes” or “does not go” can be used to determine the relative strength of the Bronsted acids and bases in the reaction. From the data below, determine the order of the strengths of the three Bronsted acids. Reaction 1: NH4 + + (CH3)3N → (CH3)3NH+ + NH3 goes Reaction 2: H2TeO3 + (CH3)3N → (CH3)3NH+ + HTeO3 - goes Reaction 3: NH4 + + HTeO3 - → H2TeO3 + NH3 does not go

Calculate the hydrogen-ion concentration and the pH of a solution of 0.0001M H2CO3, and also calculate what fraction of the H2CO3 has been dissociated. Compare this fraction with the fraction dissociated when the concentration is 0.01M (given that the pH is 4.2 in a 0.01M solution). What generalization can you make regarding the effect of dilution on the degree of dissociation?