Chapter 14 Problems

1.Classify each of these as an Arrhenius acid or a base. Which are strong and which are weak? What ions are produced when each is dissolved in water?

a.       `LiOH`

b.      `Mg(OH)_2`

c.       `HClO`

d.      `HBr`

e.       `KOH`

f.       `H_2SO_3`

2. Why is HA considered a Bronsted-Lowery Acid?

3. In the equation depicting the autoionization of water, 

`H_2O+H_2O -> H_3 O^(+) +OH^(-)`

would we say that the equilibrium lies to left, right, or neither?

4. Use chemical equations to illustrate the amphoteric properties of `HCO_3^(-)`.

5. What products will result when HSO₄^- is added to water? Complete and balance the reaction below.

`HSO_4^(-) + H_2O -> ?`

6. Identify the parent acid, parent base, conjugate acid and conjugate base for the following reaction:

1.  
   1. `HF+H_2O -> F^(-)+H_3O^(+)`
   2. `HSO_4^(-)+NH_3 -> SO_4^(-2)+NH^(+4)`
   3. `C_2H_3O_2^(-) +HCl -> HC_2H_3O_2+Cl^(-)`
   4. `HNO_2+H-2O-> H_3O^(+)+NO_2^(-)`
   5. `HCN+H_2O -> H-3O^(+) +CN^(-)`

7. Compare HCl with H₂S in terms of acid strength.

1. Compare H₃PO₄, NaH₂PO₄, Na₂HPO₄, and Na₃PO₄ with respect to acidity.

9. Identify the nature of each of the following as either a Lewis Acid or a Lewis Base:

a.      `NH_3`

b.      `Ag^(+)`

c.       `Ni^(2+)`

d.      `Pt^(4+)`

e.     ` H_2 O`

f.        `SO_2`

10.      Explain why SiF₄ can act as a Lewis Acid.

11. Identify each of the following as an acid or a base and write a chemical equation showing how it is an acid or base according to the Arrhenius definition:

a.      `HNO_3 (aq)`

b.      NH_4^(+) (aq)`

c.       `KOH`

d.      `HC_2 H_3 O_2 (aq)`

12.   Identify each of the following as an acid or a base, then write the conjugate base of the acids and the conjugate acids of the bases.

a.      `HCl`

b.      `NH_3`

c.       `H_2 SO_3

d.      `ClO_4^(-)`

e.      `HCHO_2`

f.        `HF`

g.      `CO_3^(2-)`

h.      `HSO_4^(-)

13. Write chemical equations to show the amphoteric properties of H₂PO₄^-

14. Order the following acids according to acid strength and explain how you determined this order:

`HClO`, `HClO_2`, `HClO_3`, `HClO_4`

15. Write the balanced equations for the following reactions between acid-base pairs.

a.      `H_2CO_3 + Ba(OH)_2 ->`

b.      `HBr + NaOH ->`

c.       `H_2SO_4 + NH_3 ->`

d.      `CH_3COOH + NaOH ->`

16. What are acidic salts?

17. Draw H₂SO₄ using a molecular modeling program and insert the electrostatic potential map. Take a screen capture of this molecule and identify the areas that cause sulfuric acid to be called a polyprotic acid. What does this term mean?

18. What is the relationship between the value of the equilibrium constant for the autoionization of liquid water and the tabulated value of the ion-product constant of liquid water (K_w)?

19. Show that water is amphiprotic by writing balanced chemical equations for the reactions of water with HNO₃ and NH₃. In which reaction does water act as the acid? In which does it act as the base?

20. The autoionization of sulfuric acid can be described by the following chemical equation:

At 25°C, K = 3 × 10^-4. Write an equilibrium constant expression for KH₂SO₄ that is analogous to K_w. The density of H₂SO₄ is 1.8 g/cm³at 25°C. What is the concentration of H₃SO₄⁺? What fraction of H₂SO₄ is ionized?