Chapter 13, Fundamental Equilibrium Concepts Video Solutions, Chemistry

Chapter Questions

01:25

Problem 1

What does it mean to describe a reaction as "reversible"?

Matthew H.

Numerade Educator

03:47

Problem 1

Write equations that show $\mathrm{NH}_{3}$ as both a conjugate acid and a conjugate base.

Jasmine H.

Numerade Educator

00:26

Problem 2

When writing an equation, how is a reversible reaction distinguished from a nonreversible reaction?

Rikhil M.

Numerade Educator

00:42

Problem 2

Write equations that show $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$ acting both as an acid and as a base.

Aadit S.

Numerade Educator

02:01

Problem 3

If a reaction is reversible, when can it be said to have reached equilibrium?

Matthew H.

Numerade Educator

Show by suitable net ionic equations that each of the following species can act as a Brønsted-Lowry acid:
(a) $\mathrm{H}_{3} \mathrm{O}^{+}$
(b) $\mathrm{HCl}$
(c) $\mathrm{NH}_{3}$
(d) $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}$
(e) $\mathrm{NH}_{4}^{+}$
(f) $\mathrm{HSO}_{4}^{-}$

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00:39

Problem 4

Is a system at equilibrium if the rate constants of the forward and reverse reactions are equal?

Rikhil M.

Numerade Educator

Problem 4

Show by suitable net ionic equations that each of the following species can act as a Brønsted-Lowry acid:
(a) $\mathrm{HNO}_{3}$
(b) $\mathrm{PH}_{4}^{+}$
(c) $\mathrm{H}_{2} \mathrm{~S}$
(d) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COOH}$
(e) $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$
(f) HS-

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01:19

Problem 5

If the concentrations of products and reactants are equal, is the system at equilibrium?

Matthew H.

Numerade Educator

Problem 5

Show by suitable net ionic equations that each of the following species can act as a Brønsted-Lowry base:
(a) $\mathrm{H}_{2} \mathrm{O}$
(b) $\mathrm{OH}^{-}$
(c) $\mathrm{NH}_{3}$
(d) $\mathrm{CN}^{-}$
(e) $S^{2-}$
(f) $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$

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01:14

Problem 6

Explain why there may be an infinite number of values for the reaction quotient of a reaction at a given temperature but there can be only one value for the equilibrium constant at that temperature.

Rikhil M.

Numerade Educator

Problem 6

Show by suitable net ionic equations that each of the following species can act as a Brønsted-Lowry base:
(a) $\mathrm{HS}^{-}$
(b) $\mathrm{PO}_{4}^{3-}$
(c) $\mathrm{NH}_{2}^{-}$
(d) $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$
(e) $\mathrm{O}^{2-}$
(f) $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$

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01:44

Problem 7

Explain why an equilibrium between $\mathrm{Br}_{2}(l)$ and $\mathrm{Br}_{2}(g)$ would not be established if the container were not a closed vessel shown in Figure 13.4 .

Matthew H.

Numerade Educator

03:02

Problem 7

What is the conjugate acid of each of the following? What is the conjugate base of each?
(a) $\mathrm{OH}^{-}$
(b) $\mathrm{H}_{2} \mathrm{O}$
(c) $\mathrm{HCO}_{3}^{-}$
(d) $\mathrm{NH}_{3}$
(e) $\mathrm{HSO}_{4}^{-}$
(f) $\mathrm{H}_{2} \mathrm{O}_{2}$
(g) HS $^{-}$
(h) $\mathrm{H}_{5} \mathrm{~N}_{2}+$

Sima S.

Numerade Educator

00:32

Problem 8

If you observe the following reaction at equilibrium, is it possible to tell whether the reaction started with pure $\mathrm{NO}_{2}$ or with pure $\mathrm{N}_{2} \mathrm{O}_{4} ?$
$2 \mathrm{NO}_{2}(g) \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{4}(g)$

Rikhil M.

Numerade Educator

00:54

Problem 8

What is the conjugate acid of each of the following? What is the conjugate base of each?
(a) $\mathrm{H}_{2} \mathrm{~S}$
(b) $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$
(c) $\mathrm{PH}_{3}$
(d) $\mathrm{HS}^{-}$
(e) $\mathrm{HSO}_{3}^{-}$
(f) $\mathrm{H}_{3} \mathrm{O}_{2}^{+}$
(g) $\mathrm{H}_{4} \mathrm{~N}_{2}$
(h) $\mathrm{CH}_{3} \mathrm{OH}$

Aadit S.

Numerade Educator

Problem 9

Among the solubility rules previously discussed is the statement: All chlorides are soluble except $\mathrm{Hg}_{2} \mathrm{Cl}_{2}$, AgCl, $\mathrm{PbCl}_{2}$, and CuCl.
(a) Write the expression for the equilibrium constant for the reaction represented by the equation $\mathrm{AgCl}(s) \rightleftharpoons \mathrm{Ag}^{+}(a q)+\mathrm{Cl}^{-}(a q) .$ Is $K_{c}>1,<1,$ or $\approx 1 ?$ Explain your answer.
(b) Write the expression for the equilibrium constant for the reaction represented by the equation $\mathrm{Pb}^{2+}(a q)+2 \mathrm{Cl}^{-}(a q) \rightleftharpoons \mathrm{PbCl}_{2}(s)$. Is $K_{c}>1,<1,$ or $\approx 1$ ? Explain your answer.

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Problem 9

Identify and label the Brønsted-Lowry acid, its conjugate base, the Brønsted-Lowry base, and its conjugate acid in each of the following equations:
(a) $\mathrm{HNO}_{3}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{NO}_{3}^{-}$
(b) $\mathrm{CN}^{-}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{HCN}+\mathrm{OH}^{-}$
(c) $\mathrm{H}_{2} \mathrm{SO}_{4}+\mathrm{Cl}^{-} \longrightarrow \mathrm{HCl}+\mathrm{HSO}_{4}^{-}$
(d) $\mathrm{HSO}_{4}^{-}+\mathrm{OH}^{-} \longrightarrow \mathrm{SO}_{4}^{2-}+\mathrm{H}_{2} \mathrm{O}$
(e) $\mathrm{O}^{2-}+\mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{OH}^{-}$
(f) $\left[\mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)_{3}(\mathrm{OH})\right]^{+}+\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+} \longrightarrow\left[\mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\right]^{2+}+\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5}(\mathrm{OH})\right]^{2+}$
(g) $\mathrm{H}_{2} \mathrm{~S}+\mathrm{NH}_{2}^{-} \longrightarrow \mathrm{HS}^{-}+\mathrm{NH}_{3}$

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01:21

Problem 10

Among the solubility rules previously discussed is the statement: Carbonates, phosphates, borates, and arsenates - except those of the ammonium ion and the alkali metals- -are insoluble.
(a) Write the expression for the equilibrium constant for the reaction represented by the equation $\mathrm{CaCO}_{3}(s) \rightleftharpoons \mathrm{Ca}^{2+}(a q)+\mathrm{CO}_{3}^{2-}(\mathrm{aq}) .$ Is $K_{c}>1,<1, \mathrm{or} \approx 1 ?$ Explain your answer.
(b) Write the expression for the equilibrium constant for the reaction represented by the equation $3 \mathrm{Ba}^{2+}(a q)+2 \mathrm{PO}_{4}^{3-}(a q) \rightleftharpoons \mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s) .$ Is $K_{c}>1,<1,$ or $\approx 1 ?$ Explain your answer.

Nicole S.

Numerade Educator

Problem 10

Identify and label the Brønsted-Lowry acid, its conjugate base, the Brønsted-Lowry base, and its conjugate acid in each of the following equations:
(a) $\mathrm{NO}_{2}^{-}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{HNO}_{2}+\mathrm{OH}^{-}$
(b) $\mathrm{HBr}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{H}_{3} \mathrm{O}^{+}+\mathrm{Br}^{-}$
(c) $\mathrm{HS}^{-}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{H}_{2} \mathrm{~S}+\mathrm{OH}^{-}$
(d) $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}+\mathrm{OH}^{-} \longrightarrow \mathrm{HPO}_{4}^{2-}+\mathrm{H}_{2} \mathrm{O}$
(e) $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}+\mathrm{HCl} \longrightarrow \mathrm{H}_{3} \mathrm{PO}_{4}+\mathrm{Cl}^{-}$
(f) $\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5}(\mathrm{OH})\right]^{2+}+\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+} \longrightarrow\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}+\left[\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5}(\mathrm{OH})\right]^{2+}$
(g) $\mathrm{CH}_{3} \mathrm{OH}+\mathrm{H}^{-} \longrightarrow \mathrm{CH}_{3} \mathrm{O}^{-}+\mathrm{H}_{2}$

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