Consider following solutions: (I) I M glucose(aq) (II) 1 M sodium choride(aq)
(III) 1 M acetic acid in benzene (IV) 1 M ammonium phosphate (aq)

Options

A. all are isotonic solutions
B. III is hypotonic of I, II, IV
C. I, II, Ivare hypertonic of III
D. IV is hypertonic I, II, III

Answer

To solve the problem regarding the four solutions provided, we need to analyze each solution based on its osmotic pressure, which is determined by the Van't Hoff factor (I). The osmotic pressure (π) can be calculated using the formula:

\[ \pi = iCRT \]

Where:
- \(C\) is the concentration of the solution (in molarity),
- \(R\) is the gas constant,
- \(T\) is the temperature in Kelvin,
- \(i\) is the Van't Hoff factor, which indicates the number of particles the solute dissociates into.

### Step-by-Step Solution:

1. **Identify the Van't Hoff factor (i) for each solution:**
- **(I) 1 M Glucose (aq):**
- Glucose does not dissociate in solution; hence, \(i = 1\).
- **(II) 1 M Sodium Chloride (aq):**
- Sodium chloride dissociates into two ions: Na\(^+\) and Cl\(^-\); hence, \(i = 2\).
- **(III) 1 M Acetic Acid in Benzene:**
- Acetic acid is a weak acid and does not dissociate significantly in a non-polar solvent like benzene. Thus, we can assume \(i \approx 1\).
- **(IV) 1 M Ammonium Phosphate (aq):**
- Ammonium phosphate dissociates into four ions: \(NH_4^+\) and \(PO_4^{3-}\); hence, \(i = 4\).

2. **Calculate the osmotic pressure for each solution:**
- Since \(C\), \(R\), and \(T\) are constant for all solutions, the osmotic pressure will depend solely on the Van't Hoff factor \(i\):
- **(I) Glucose:** \(\pi = 1 \cdot C \cdot R \cdot T\)
- **(II) NaCl:** \(\pi = 2 \cdot C \cdot R \cdot T\)
- **(III) Acetic Acid:** \(\pi \approx 1 \cdot C \cdot R \cdot T\)
- **(IV) Ammonium Phosphate:** \(\pi = 4 \cdot C \cdot R \cdot T\)

3. **Compare the osmotic pressures:**
- From the calculated values, we can see:
- Glucose and Acetic Acid have the same osmotic pressure (both have \(i = 1\)).
- Sodium Chloride has a higher osmotic pressure than Glucose and Acetic Acid (\(i = 2\)).
- Ammonium Phosphate has the highest osmotic pressure (\(i = 4\)).

4. **Determine the relationships between the solutions:**
- **Isotonic Solutions:** Solutions that have the same osmotic pressure.
- Glucose and Acetic Acid are isotonic.
- **Hypotonic Solutions:** Solutions with lower osmotic pressure compared to others.
- Acetic Acid is hypotonic compared to Glucose, NaCl, and Ammonium Phosphate.
- **Hypertonic Solutions:** Solutions with higher osmotic pressure.
- Sodium Chloride and Ammonium Phosphate are hypertonic compared to Acetic Acid.

5. **Conclusion:**
- The correct statements based on the analysis are:
- (b) Acetic Acid is hypotonic compared to 1, 2, and 4.
- (c) Solutions 1, 2, and 4 are hypertonic compared to 3.
- (d) Solution 4 is hypertonic compared to 1, 2, and 3.

### Final Answer:
The correct options are (b), (c), and (d).