If 33.6 grams of KCl are dissolved in 192 grams of water, what is the concentration of the solution in percent by mass? AND if 2.1 moles of CaCl2 are dissolved in enough water to make a .92 liter solution what is the resulting molarity? Please help and explain or anything?!

% w/w = (grams solute/total grams) x 100 =

[33.6 g KCl/(33.6+192)]*100 = ?

M = moles/L soln = 2.1 mols/0.92L = ?

14.9%

To calculate the concentration of a solution, you need to know the amount of solute (in grams or moles) and the total mass or volume of the solution.

1. Calculating the concentration in percent by mass:
First, find the total mass of the solution by adding the mass of the solute (KCl) and the mass of the solvent (water). In this case, it would be 33.6 grams (KCl) + 192 grams (water) = 225.6 grams (total mass of solution).

Next, divide the mass of the solute (KCl) by the total mass of the solution and multiply by 100 to express it as a percentage:
(33.6 grams / 225.6 grams) x 100 = 14.9% (concentration of the KCl solution in percent by mass).

Therefore, the concentration of the solution is 14.9% by mass.

2. Calculating the molarity of a solution:
Molarity is defined as the number of moles of solute per liter of solution (mol/L).

To calculate the molarity (M) of the CaCl2 solution, divide the number of moles of solute (CaCl2) by the volume of the solution in liters:
Molarity (M) = Moles of solute / Volume of solution in liters

Given that 2.1 moles of CaCl2 are dissolved in 0.92 liters of solution:
Molarity (M) = 2.1 moles / 0.92 L = 2.28 M (resulting molarity of the CaCl2 solution)

Therefore, the resulting molarity of the solution is 2.28 M.

By following these steps, you can determine the concentration of a solution in percent by mass and the molarity of a solution.