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Chapter 10: Q.10.84 (page 359)

Identify the weaker acid in each of the following pairs:

a. HNO2and H2CO3

b. HF or HCO3-

c. HBrorHSO4鈭�

d. NH4+orH3PO4

Short Answer

Expert verified

Part a. H2CO3

Part b. HCO3鈭�

Part c.HSO4鈭�

Part d.NH4+

Step by step solution

01

Given Information (Part a)

An acid is any hydrogen-containing substance that is fit for donating a proton (hydrogen ion) to another substance. A base is a particle or ion ready to acknowledge a hydrogen ion from an acid. Acidic substances are normally identified by their acrid taste.

02

Explanation Part (a)

H2CO3 is the weaker acid as it has a stronger conjugate base.

03

Explanation Part (b)

HCO3-is the weaker acid as it has a stronger conjugate base.

04

Explanation Part (c)

HSO4-is the weaker acid as it has a stronger conjugate base.

05

Explanation Part (d)

NH4+is the weaker acid as it has a stronger conjugate base.

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Most popular questions from this chapter

Write the formula for the conjugate base for each of the following acids:

a.HF

b.H2O

c.H2PO3-

d.HSO4-

Calculate the [OH-]of each aqueous solution with the following [H3O+]:

a. coffee, 1.0脳10-5M

b. soap, 1.0脳10-8M

c. cleanser, 5.0脳10-10M

d. lemon juice,2.5脳10-2M

In the blood plasma. pH is maintained by the carbonic acid bicarbonate buffer system, (10,8)

a. How is pH maintained when acid is added to the buffer system?

b. How is pH maintained when base is added to the buffer system?

Which of the following are at equilibrium?

a. The rate of the forward reaction is twice as fast as the rate of the reverse reaction.

b. The concentrations of the reactants and the products do not change.

c. The rate of the reverse reaction does not change.

Which of the following represents a buffer system? Explain.

a. NaOHandNaCl

b. H2CO3andNaHCO3

c. HFandKF

d. KClandNaCl
See all solutions

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