A solution is formed by dissolving 83.2 grams of copper II chloride (CuCl2
) in 2.5 liters of water. The molar mass of CuCl2
is 134.45 g/mol.
What is the molarity of the solution?
First, we need to convert the mass of CuCl2 in grams to moles:
83.2 g CuCl2 ÷ 134.45 g/mol = 0.619 moles CuCl2
Next, we need to find the volume of the solution in liters:
2.5 liters
Finally, we can use the equation for molarity:
Molarity = moles of solute ÷ volume of solution (in liters)
Molarity = 0.619 moles ÷ 2.5 liters
Molarity = 0.248 M
Therefore, the molarity of the solution is 0.248 M.
To find the molarity of a solution, you need to divide the number of moles of solute by the volume of the solution in liters.
Firstly, let's find the number of moles of CuCl2:
Number of moles = mass of CuCl2 / molar mass of CuCl2
Number of moles = 83.2 g / 134.45 g/mol
Number of moles = 0.6183 mol (rounded to four decimal places)
Now, we can calculate the molarity of the solution:
Molarity (M) = moles of solute / volume of solution in liters
Molarity = 0.6183 mol / 2.5 L
Molarity = 0.2473 M (rounded to four decimal places)
Therefore, the molarity of the solution is 0.2473 M.