what mass of potassium chloride is required to prepare 5.00L of a 2.00M solution of KCL
How many mols do you need? That will be M x L = ?
Then use this example to convert from moles to grams.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine the mass of potassium chloride (KCl) required to prepare a 2.00M solution in 5.00L of water, you need to use the formula for molarity:
Molarity (M) = moles of solute / volume of solution (in liters)
First, rearrange the formula to solve for moles of solute:
moles of solute = Molarity × volume of solution
Now, plug in the values:
moles of solute = 2.00M × 5.00L
moles of solute = 10.00 mol
Next, find the molar mass of KCl, which consists of potassium (K) and chlorine (Cl). The molar mass is the sum of the atomic masses of its components.
Molar mass of K: 39.10 g/mol
Molar mass of Cl: 35.45 g/mol (approximately)
Molar mass of KCl = molar mass of K + molar mass of Cl
Molar mass of KCl = 39.10 g/mol + 35.45 g/mol
Molar mass of KCl = 74.55 g/mol
Finally, use the equation:
mass = moles of solute × molar mass of KCl
mass = 10.00 mol × 74.55 g/mol
mass = 745.5 g
Therefore, 745.5 grams of potassium chloride (KCl) are required to prepare a 2.00M solution of KCl in 5.00L of water.