You make 1.000 L of an aqueous solution that contains 35.0 g of sucrose (C12H22O11).

A) What is the molarity of sucrose in this solution? (I got 0.102 M for Part A) I just can't figure out part B.

B) How many liters of water would you have to add to this solution to reduce the molarity you calculated in Part A by a factor of two?

For A: The molarity of sucrose solution is 0.102 M

For B: The volume of water that would be added to the solution is 2 liters

Explanation:

To calculate the molarity of solution, we use the equation:

Given mass of sucrose = 35.0 g

Molar mass of sucrose = 342.3 g/mol

Volume of solution = 1.000 L

Putting values in above equation, we get:

Hence, the molarity of sucrose solution is 0.102 M

To calculate the volume of the diluted solution, we use the equation:

where,

are the molarity and volume of the concentrated sucrose solution

are the molarity and volume of diluted sucrose solution

We are given:

Putting values in above equation, we get:

Hence, the volume of water that would be added to the solution is 2 liters

b is the correct answer

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