If 3.251 grams of CaCl_2 were dissolved in enough water to make 150.00 mL of sol

Question

If 3.251 grams of CaCl_2 were dissolved in enough water to make 150.00 mL of solution, what is the molarity of the solution? In the total mass of the solution in question 1 was 151.632 grams, what is the concentration of the solute in question 1 in percent mass? Solution #1 was prepared by adding 10.0 g of liquid acetone to 25.0 ml of water. Solution #2 was prepared by dissolving 10.0 g of liquid acetone in enough water to make 25.0 ml of solution. Find the m/v% of each solution and tell which would be more concentrated. The density of acetone is 0.789 g/mL.

Explanation / Answer

The problem 1 and problem 2 are solved correctly, i have looked the solution

Problem 3:

Case 1: Density of water = 1 gm/mL

Mass of water = 25 mL * 1 gm/mL = 25 gm

Hence in the first case, we are adding 10g of acetone to 25g of water

Case 2: Density of acetone = 0.789 g/mL

Volume of acetone = 10g/0.789g/mL = 12.674 mL

Volume of solution = Volume of water + Volume of acetone

25 mL = Volume of water + 12.674

Volume of water = 12.35 mL

Hence the solution 2 is more concentrated, since the mass/volume percentage is higher for solution 2

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