A solution has 12% of sucrose by weight (molar mass 342.3 g mol-1).
The osmotic pressure of the red blood cell is 5.94 bar at 25 °C, how much (in terms of volume) of the 12% sucrose solution do you need to make 1 L of isotonic (isosmotic) solution for the red blood cell?

To find the volume of the 12% sucrose solution needed to make 1 L of an isotonic solution for the red blood cell, we can apply the concept of osmotic pressure and the van 't Hoff equation for osmotic pressure.

The van 't Hoff equation for osmotic pressure (\( \Pi \)) is:
\[
\Pi = i \cdot C \cdot R \cdot T
\]
where:
- \( \Pi \) is the osmotic pressure in bar,
- \( i \) is the van 't Hoff factor (1 for sucrose, a non-electrolyte),
- \( C \) is the molarity of the solution (mol/L),
- \( R \) is the gas constant (\(0.0831 \, \text{L bar K}^{-1} \text{mol}^{-1}\)),
- \( T \) is the temperature in Kelvin.

Given values:
- Osmotic pressure (\( \Pi \)) = 5.94 bar
- Temperature \( T = 25^\circ \text{C} = 298 \, \text{K} \)

### Step 1: Calculate the required molarity (C)
Rearrange the van 't Hoff equation to solve for \( C \):
\[
C = \frac{\Pi}{i \cdot R \cdot T}
\]
Substitute values:
\[
C = \frac{5.94}{1 \times 0.0831 \times 298}
\]
\[
C \approx 0.241 \, \text{mol/L}
\]

### Step 2: Determine the amount of sucrose in 1 L of solution
Since we need a 1 L isotonic solution with a molarity of \( 0.241 \, \text{mol/L} \), the moles of sucrose required are:
\[
\text{moles of sucrose} = 0.241 \, \text{mol}
\]

### Step 3: Convert moles to mass of sucrose
Using the molar mass of sucrose (\( 342.3 \, \text{g/mol} \)):
\[
\text{mass of sucrose} = 0.241 \times 342.3
\]
\[
\text{mass of sucrose} \approx 82.5 \, \text{g}
\]

### Step 4: Calculate the volume of the 12% sucrose solution needed
The 12% sucrose solution means there are 12 g of sucrose in every 100 g of solution. To find the total mass of solution that contains 82.5 g of sucrose:
\[
\frac{82.5 \, \text{g sucrose}}{12 \, \text{g sucrose per 100 g solution}} = \frac{82.5}{0.12}
\]
\[
\approx 687.5 \, \text{g of solution}
\]

Assuming the density of the solution is approximately \(1 \, \text{g/mL}\) (a reasonable assumption for dilute solutions), the volume of the solution needed is roughly:
\[
687.5 \, \text{mL}
\]

### Answer
To make a 1 L isotonic solution for the red blood cell, you need approximately **687.5 mL of the 12% sucrose solution**.

Would you like further clarification on any steps? 

Here are some related questions to deepen understanding:
1. How would this calculation change if the sucrose solution concentration were different?
2. What assumptions are made about the solution's properties in this calculation?
3. How would temperature variations affect the volume required?
4. How does the osmotic pressure of different solutes compare for the same molarity?
5. What is the importance of isotonic solutions in biological applications?

**Tip:** When working with osmotic pressure, double-check the units of \( R \) and \( \Pi \) for consistency.

A solution has 12% of sucrose by weight (molar mass 342.3 g mol-1). The osmotic pressure of the red blood cell is 5.94 bar at 25 °C, how much (in terms of volume) of the 12% sucrose solution do you need to make 1 L of isotonic (isosmotic) solution for the red blood cell?

Learn how to calculate the volume of a 12% sucrose solution required to create 1 L of isotonic solution for a red blood cell, based on osmotic pressure and the van 't Hoff equation. Given osmotic pressure of 5.94 bar at 25°C and a sucrose molar mass of 342.3 g/mol, this problem involves understanding molarity, molar mass, and osmotic pressure calculations. Ideal for high school chemistry students.

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