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

Publisher: MAC HIGHER

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Chapter 6, Problem 6.11E

Interpretation Introduction

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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Transmitance 3. Which one of the following compounds corresponds to this IR spectrum? Point out the absorption band(s) that helped you decide. OH H3C OH H₂C CH3 H3C CH3 H3C INFRARED SPECTRUM 0.8- 0.6 0.4- 0.2 3000 2000 1000 Wavenumber (cm-1) 4. Consider this compound: H3C On the structure above, label the different types of H's as A, B, C, etc. In table form, list the labeled signals, and for each one state the number of hydrogens, their shifts, and the splitting you would observe for these hydrogens in the ¹H NMR spectrum. Label # of hydrogens splitting Shift (2)

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Chapter 6 Solutions

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

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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.

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.