a chemist wants to make 5.5L of a .3M Cacl2 solution. What mass of CaCl2 should the chemist use?
How many moles do you want? That'x M x L = ?
Then mols = grams/molar mass.
To determine the mass of CaCl2 needed, you will need to use the formula:
Mass (g) = Concentration (M) x Volume (L) x Molar Mass (g/mol)
1. First, find the molar mass of CaCl2:
Ca = 40.08 g/mol
Cl = 35.45 g/mol (x2 since there are two chlorine atoms)
Molar mass of CaCl2 = 40.08 g/mol + (35.45 g/mol x 2) = 110.98 g/mol
2. Convert the desired volume (5.5 L) to liters:
5.5 L
3. Now, calculate the mass of CaCl2:
Mass (g) = 0.3 M x 5.5 L x 110.98 g/mol
Simplifying the equation:
Mass (g) = 18.1545 g
Therefore, the chemist should use approximately 18.15 grams of CaCl2 to make a 5.5L 0.3M CaCl2 solution.
To determine the mass of CaCl2 that the chemist should use, we need to use the formula:
Molarity (M) = (moles of solute) / (volume of solution in liters)
Given:
Molarity = 0.3 M
Volume of solution = 5.5 L
First, let's rearrange the formula to solve for moles of solute:
moles of solute = Molarity × volume of solution
moles of solute = 0.3 M × 5.5 L
moles of solute = 1.65 mol
Now, we need to find the molar mass of CaCl2, which is the sum of the atomic masses of calcium (Ca) and chlorine (Cl):
1 calcium atom (Ca) = 40.08 g/mol
2 chlorine atoms (Cl) = 2 × 35.45 g/mol
Molar mass of CaCl2 = 40.08 g/mol + 2 × 35.45 g/mol
Molar mass of CaCl2 = 110.98 g/mol
Finally, we can calculate the mass of CaCl2:
Mass of CaCl2 = moles of solute × molar mass of CaCl2
Mass of CaCl2 = 1.65 mol × 110.98 g/mol
Mass of CaCl2 = 182.937 g
Therefore, the chemist should use 182.937 grams of CaCl2 to make a 5.5L 0.3M CaCl2 solution.