What is the molarity of a saturated sucrose solution at 25 degrees Celsius?

To find the molarity of the saturated sucrose solution, we follow these steps:

Determine the number of moles of sucrose:
The molar mass of sucrose (C₁₂H₂₂O₁₁) is approximately 342.3 g/mol. If 211.4 grams of sucrose dissolve, we can calculate the moles of sucrose as follows:
```
  Moles of sucrose = mass / molar mass = 211.4 g / 342.3 g/mol = 0.617 moles
  
```
Calculate the volume of the saturated solution:
Since the density of the solution is given as 1.34 g/mL, we need to find the total mass of the saturated solution. We know that 100 g of water and 211.4 g of sucrose gives us:
```
  Total mass of solution = mass of water + mass of sucrose = 100 g + 211.4 g = 311.4 g
  
```
The volume of the solution can then be calculated using density:
```
  Volume = mass / density = 311.4 g / 1.34 g/mL ≈ 232.4 mL
  
```

Convert volume from mL to L:

  Volume in liters = 232.4 mL / 1000 = 0.2324 L

Calculate molarity:
Molarity is defined as moles of solute per liter of solution. Thus, we can calculate the molarity of the sucrose solution:
```
  Molarity (M) = moles of sucrose / volume of solution in liters
  M = 0.617 moles / 0.2324 L ≈ 2.65 M
  
```

Conclusion: The molarity of the saturated sucrose solution at 25 degrees Celsius is approximately 2.65 M.

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