How much water must be added to 40.0 g of CaCl₂ to produce a solution that is 35.0 wt% CaCl₂? A)54.0 g B)74.2 g C)87.5 g D)114 g

Question

Quizplus · Accepted Answer

First, we need to calculate the mass of CaCl2 needed in the final solution. Since the solution is 35.0 wt%, meaning that 35.0% of the total mass of the solution is CaCl2, then:

mass of CaCl2 = 40.0 g / (1 - 35.0%) = 61.5 g

This means that we need to add 61.5 - 40.0 = 21.5 g of CaCl2 to the solution. Now, we can use the definition of wt% to calculate the mass of the final solution:

40.0 g + x g = (35.0/100) * (40.0 g + x g)

Solving for x, we get:

x = 74.2 g

Therefore, we need to add 74.2 - 40.0 = 34.2 g of water to the initial 40.0 g of CaCl2 to obtain a final solution that is 35.0 wt% CaCl2.

How Much Water Must Be Added to 40