In which direction will the following equilibria I and II proceed?
`I:H_(2)SO_(4)(aq)+NH_(3)(aq)hArrNH_(4)^(+)(aq)+HSO_(4)^(-)(aq)`
`II: HCO_(3)^(-)(aq)+SO_(4)^(-)(aq)hArr HSO_(4)^(-)(aq)+CO_(3)^(2-)(aq)`

Options

A. I forward &II backward
B. I backward & II forward
C. Both forward
D. Both backward

Explanation

To determine the direction in which the given equilibria will proceed, we need to analyze the strength of the acids and bases involved in each reaction.

### Equilibrium I:
**Reaction:**
\[ H_2SO_4(aq) + NH_3(aq) \rightleftharpoons NH_4^+(aq) + HSO_4^-(aq) \]

1. **Identify the acids and bases:**
- \( H_2SO_4 \) (sulfuric acid) is a strong acid.
- \( NH_3 \) (ammonia) is a weak base.
- \( NH_4^+ \) (ammonium ion) is a weak acid.
- \( HSO_4^- \) (hydrogen sulfate ion) is a weak base.

2. **Determine the direction of the equilibrium:**
- The reaction involves a strong acid (\( H_2SO_4 \)) and a weak base (\( NH_3 \)) reacting to form a weak acid (\( NH_4^+ \)) and a weak base (\( HSO_4^- \)).
- According to the principle of equilibrium, the reaction will shift from strong acid/base to weak acid/base. Therefore, the equilibrium will shift **forward**.

### Equilibrium II:
**Reaction:**
\[ HCO_3^-(aq) + SO_4^{2-}(aq) \rightleftharpoons HSO_4^-(aq) + CO_3^{2-}(aq) \]

1. **Identify the acids and bases:**
- \( HCO_3^- \) (bicarbonate) is a weak acid.
- \( SO_4^{2-} \) (sulfate) is a weak base.
- \( HSO_4^- \) (hydrogen sulfate) is a strong acid.
- \( CO_3^{2-} \) (carbonate) is a strong base.

2. **Determine the direction of the equilibrium:**
- The reaction involves a weak acid (\( HCO_3^- \)) and a weak base (\( SO_4^{2-} \)) reacting to form a strong acid (\( HSO_4^- \)) and a strong base (\( CO_3^{2-} \)).
- The equilibrium will shift from strong acid/base to weak acid/base. Therefore, the equilibrium will shift **backward**.

### Summary of Results:
- For Equilibrium I, the equilibrium shifts **forward**.
- For Equilibrium II, the equilibrium shifts **backward**.