make an aqueous solution of 0.176 M copper(II) chloride for an experiment in lab, using a 300 mL volumetric flask. How much solid copper(II) chloride should you add
How many mols CuCl2 do you need? That's M x L = 0.176 x 0.300 = ?
How many grams is that? grams CuCl2 = mols CuCl2 x molar mass CuCl2 = ?
.0528
To determine the amount of solid copper(II) chloride to add, we need to use the formula:
Molarity (M) = moles of solute / volume of solution in liters
First, we need to calculate the moles of solute required using the given molarity and volume of solution:
Molarity = 0.176 M
Volume of solution = 300 mL = 0.3 L
Rearranging the formula, we have:
moles of solute = Molarity × Volume of solution
moles of solute = 0.176 M × 0.3 L
moles of solute = 0.0528 moles
Since copper(II) chloride (CuCl2) has a 1:1 stoichiometric ratio, the moles of copper(II) chloride required will be the same.
Now, we need to determine the molar mass of copper(II) chloride (CuCl2) to convert moles to grams. The molar mass of copper (Cu) is 63.55 g/mol, and the molar mass of chlorine (Cl) is 35.45 g/mol.
Molar mass of CuCl2 = (63.55 g/mol × 1) + (35.45 g/mol × 2)
Molar mass of CuCl2 = 134.45 g/mol
Now, we can calculate the mass of solid copper(II) chloride needed:
Mass of solid copper(II) chloride = moles of copper(II) chloride × molar mass of CuCl2
Mass of solid copper(II) chloride = 0.0528 moles × 134.45 g/mol
Mass of solid copper(II) chloride = 7.06272 grams
Therefore, you should add approximately 7.06 grams of solid copper(II) chloride to make a 0.176 M aqueous solution in a 300 mL volumetric flask for your lab experiment.