What is the molarity of a solution prepared by dissolving 543g ofCa(NO3)2 into 355ml of water?
First, you need to calculate the number of moles of Ca(NO3)2 in 543g:
molar mass of Ca(NO3)2 = 164 g/mol
moles of Ca(NO3)2 = mass / molar mass
moles of Ca(NO3)2 = 543g / 164 g/mol = 3.31 mol
Next, you need to calculate the volume of the solution in liters:
355 ml = 0.355 L
Finally, you can calculate the molarity of the solution:
molarity = moles of solute / volume of solution in liters
molarity = 3.31 mol / 0.355 L = 9.31 M
Therefore, the molarity of the solution is 9.31 M.
What is the final concentration (M) of a solution prepared by diluting 50.0ml of a6.00m KCl solution to a volume of 2.00L?
To find the final concentration of the solution, you can use the equation:
C1V1 = C2V2
where C1 is the initial concentration, V1 is the initial volume, C2 is the final concentration, and V2 is the final volume.
Substituting the given values:
C1 = 6.00 M
V1 = 50.0 mL = 0.0500 L
V2 = 2.00 L
Solving for C2:
C2 = (C1V1) / V2
C2 = (6.00 M x 0.0500 L) / 2.00 L
C2 = 0.150 M
Therefore, the final concentration of the solution is 0.150 M.
To find the molarity of a solution, you need to know the number of moles of solute (Ca(NO3)2) and the volume of the solution (in liters).
1. First, calculate the number of moles of Ca(NO3)2:
- The molar mass of Ca(NO3)2 is 164.09 g/mol (40.08 g/mol for Ca + 2 * 14.01 g/mol for N + 6 * 16.00 g/mol for O).
- Divide the mass of Ca(NO3)2 (543 g) by its molar mass to get the number of moles:
moles = 543 g / 164.09 g/mol = 3.31 mol
2. Next, convert the volume of water from milliliters to liters:
- Divide the volume of water (355 mL) by 1000 to get the volume in liters:
volume = 355 mL / 1000 = 0.355 L
3. Finally, calculate the molarity (M) by dividing the number of moles by the volume in liters:
- Molarity (M) = moles / volume
M = 3.31 mol / 0.355 L = 9.31 M
Therefore, the molarity of the solution prepared by dissolving 543g of Ca(NO3)2 in 355ml of water is 9.31 M.