Explanation The given equation is as follows, HNO 2 (aq) + NH 3 (aq) ⇌ NH 4 + (aq) + NO 2 − (aq) Now, write the expression for equilibrium constant from the above reaction. K = [ NH 4 + ] [ NO 2 − ] [ HNO 2 ] [ NH 3 ] The NH 4 + ion formation reaction equation is the combination of the following two equations and it can be written as, HNO 2 (aq) + H 2 O (l) ⇌ H 3 O + (aq) + NO 2 − (aq) NH 3 (aq) + H 2 O (l) ⇌ NH 4 + (aq) + OH - (aq) The equations represents the weak acid dissociation and weak base dissociation. Now, write the expressions for both acid and base dissociation constants for the above two equation as below. K a = [ H 3 O + ] [ NO 2 − ] [ HNO 2 ] K b = [ NH 4 + ] [ OH - ] [ NH 3 ] At 298K, K a of HNO 2 is 4 .3×10 -4 K b of NH 3 is 1 .8×10 -5 . Now, substitute these values in the above expression and it becomes, 4 .3×10 -4 = [ H 3 O + ] [ NO 2 − ] [ HNO 2 ] 1 .8×10 -5 = [ NH 4 + ] [ OH - ] [ NH 3 ] Now, multiply the above equations, 4 .3×10 -4 ×1

ACHIEVE/CHEMICAL PRINCIPLES ACCESS 2TERM

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ISBN: 9781319403959

Author: ATKINS

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Chapter 6, Problem 6.11E

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Interpretation:

The equilibrium constant for the following reaction and the value of K at 298 K for the reaction HNO2(aq) + NH3(aq) ⇌ NH4+(aq) + NO2−(aq) has to be calculated.

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Chapter 6, Problem 6.10E

Chapter 6, Problem 6.12E

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ACHIEVE/CHEMICAL PRINCIPLES ACCESS 2TERM

Ch. 6 - Prob. 6A.1AST Ch. 6 - Prob. 6A.1BST Ch. 6 - Prob. 6A.2AST Ch. 6 - Prob. 6A.2BST Ch. 6 - Prob. 6A.3AST Ch. 6 - Prob. 6A.3BST Ch. 6 - Prob. 6A.1E Ch. 6 - Prob. 6A.2E Ch. 6 - Prob. 6A.3E Ch. 6 - Prob. 6A.4E

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The equilibrium constant for the following reaction and the value of K at 298 K for the reaction HNO 2 (aq) + NH 3 (aq) ⇌ NH 4 + (aq) + NO 2 − (aq) has to be calculated.

Solution Summary: The author explains that the equilibrium constant for the following reaction and the value of K at 298 K is to be calculated. The NH_4+ ion formation reaction equation is the

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Interpretation:

The equilibrium constant for the following reaction and the value of K at 298 K for the reaction HNO2(aq) + NH3(aq) ⇌ NH4+(aq) + NO2−(aq) has to be calculated.

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Chapter 6 Solutions

The equilibrium constant for the following reaction and the value of K at 298 K for the reaction HNO 2 (aq) + NH 3 (aq) ⇌ NH 4 + (aq) + NO 2 − (aq) has to be calculated.

Solution Summary: The author explains that the equilibrium constant for the following reaction and the value of K at 298 K is to be calculated. The NH_4+ ion formation reaction equation is the

Concept explainers

Videos

Interpretation: The equilibrium constant for the following reaction and the value of K at 298 K for the reaction HNO2(aq) + NH3(aq) ⇌ NH4+(aq) + NO2−(aq) has to be calculated.

Want to see the full answer?

Chapter 6 Solutions

Interpretation:

The equilibrium constant for the following reaction and the value of K at 298 K for the reaction HNO2(aq) + NH3(aq) ⇌ NH4+(aq) + NO2−(aq) has to be calculated.