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AP Chemistry : Reactions and Equilibrium

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Example Question #1 : Using Base Dissociation Constant (Kb)

A 1M solution of a monoprotic acid has a pH of 4.6. What is the $\small K_{b}$ value for the conjugate base of the acid?

Possible Answers:

$\small 3.98*10^{-10}$

$\small 4.68*10^{-6}$

$\small 1.58*10^{-5}$

$\small 2.00*10^{-5}$

Correct answer:

$\small 1.58*10^{-5}$

Explanation:

In order to find the base dissociation constant for the conjugate base, we can start by finding the acid dissociation constant for the acid. Since a 1M solution of the acid has a pH of 4.6, we can find the proton concentration of the solution.

$pH=-\log[H^+]\rightarrow [H^+]=10^{-pH}$

$\small [H^{+}] = 10^{-4.6} = 2.51*10^{-5}$

Since the acid is monoprotic, we can set the following equilibrium expression equal to its acid dissociation constant.

$\small K_{a} = \frac{[H^{+}][A^{-}]}{[HA]}$

We can see that, since the acid is monoprotic, the concntration of protons will be equal to the concentration of the acid anion. The final concentration of the acid molecule will be equal to the initial concentration, minus the amount of protons formed. Using these values, we can solve for the equilibrium constant for the acid.

$K_a= \frac{[2.51*10^{-5}]^{2}}{[1-2.51*10^{-5}]} = 6.31*10^{-10}$

Now that we have the acid dissociation constant, we can find the conjugate base's dissociation constant by setting the product of the two values equal to the autoionization of water.

$\small K_{w} = K_{a}K_{b}$

$\small 1*10^{-14} = K_{b}(6.31*10^{-10})$

$\small K_{b} = 1.58*10^{-5}$

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Example Question #181 : Reactions And Equilibrium

Would H₂SO₄ or HNO₃ produce a more acidic solution?

Possible Answers:

HNO₃ since it has a higher pKa

HNO₃ since it has a lower pKa

H₂SO₄ since it has a lower pKa

H₂SO₄ since it has a higher pKa

Correct answer:

H₂SO₄ since it has a lower pKa

Explanation:

Both are strong acids, but H₂SO₄ is bivalent, realeasing 2 protons for each molecule dissolved in solution. Further, a more acidic solution would have a lower pKa.

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Example Question #91 : Acid Base Reactions

Which of the following species will not be present in an aqueous solution of H_2SO_4 ?

Possible Answers:

H_2O

H_3O^+

OH^-

All of these will be present in the solution

H^+

Correct answer:

OH^-

Explanation:

The hydroxide ion (OH–) is a strong base and therefore would not be present in an acidic solution. Protons, the hydronium ion, and water will all be present in relatively large amounts within the solution.

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Example Question #21 : P H And Poh Of Strong Acids And Bases

Which of the following anions is the strongest base?

Possible Answers:

C_2H_3O_2^-

NO_3^-

I^-

ClO_4^-

Correct answer:

C_2H_3O_2^-

Explanation:

Weaker acids dissociate less in water and therefore, reverse reaction is favored in

$HX_{(aq)} + H_{2}O_{(l)} \rightleftharpoons H_{3}O_{(aq)} + X^{-}_{(aq)}$ . This indicates that the weaker the acid, the stronger its conjugate base.

HI, HClO_4 , and HNO_3 are all strong acids. Their conjugates are weak bases.

C_2H_3O_2^- has the weakest conjugate acid among the all the choices, so it is the strongest base.

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AP Chemistry : Reactions and Equilibrium

Study concepts, example questions & explanations for AP Chemistry

All AP Chemistry Resources

Example Questions

Example Question #1 : Using Base Dissociation Constant (Kb)

Example Question #181 : Reactions And Equilibrium

Example Question #91 : Acid Base Reactions

Example Question #21 : P H And Poh Of Strong Acids And Bases

All AP Chemistry Resources

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