Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molarity of the HCl, if the solution has a density of 1.20 g/mL.

A 1.00 M solution has an initial volume of 100. mL. Water is evaporated from this solution, and the new solution has a concentration of 5.00 M. Calculate the final volume of the solution and the amount of water removed from the initial solution.

20. How many liters of a 2.00 M solution can be made from 200.0 g MgBr2?The molar mass of MgBr2 is 184.1 g.

1)17.6 g of NaCl is added to water to make 779.5 g of solution. Calculate the mass percent concentration of the solution.   2)38.3 mL of 5.2 M HCl solution is diluted to a volume of 482.4 mL. What is the concentration of the diluted solution?

Concentrated HCl has density of 1.19 g/mL and concentration of 38% by mass. What is the molarity of the solution?

7. For a chemical analysis, 750 mL of a 0.480 mol/L potassium permanganate solution is to be prepared. Calculate the mass of potassium permanganate crystals that will be dissolved to make this solution. d) Baso

Solution of magnesium chloride and sodium chloride are mixed to make brine commonly used to keep roads from becoming slippery because of ice.  The brine solution lowers the freezing point of water by up to 10 degrees C.  A brine solution is made by mixing 60. L of 5.0 M sodium chloride with 30. L of 2.4 M magnesium chloride.  Calculate the concentration of each ion in the solution.

A potasium carbonate solution is 14.6% KCO3 by mass and has a density of 0.68 g/mL. Calculate molarity of the solution. A. 0.72 M B. 6.67 M C. 12.8 M D. 1.44 M

90.0 ml of water are added to 1. ml of a 5.5% ethanol solution. calculate the concentration of final solution

How much KCl and water  must be mixed to prepare 265. grams of a 11.5 % by mass aqueous solution of KCl ?   a. 11.5 g KCl and 253.5 g water   b. 30.5 g KCl and 265 g water   c. 11.5 g KCl and 265 g water   d. 30.5 g KCl and 234.5 g water