Molarity (M) = moles of solute (mol) / Volume of the solution (L)
Molarity of the solution = 3.000 M Volume of the solution = 250.0 mL = 0.25 L moles in 250.0 mL = molarity x volume of the solution = 3.000 M x 0.25 L = 0.75 mol
Hence, 0.75 mol of NaCl is needed to prepare 250.0 mL of 3.000 M NaCl solution.
Moles (mol) = mass (g) / molar mass (g/mol)
Moles of NaCl in 250.0 mL = 0.75 mol Molar mass of NaCl = <span>58.44 g/mol Mass of NaCl in 250.0 mL = Moles x Molar mass = 0.75 mol x </span><span>58.44 g/mol = 43.83 g
Hence, 43.83 g of NaCl is needed to prepare 250.0 mL of 3.000 M solution.</span>
True water is wet because when something is wet in this case it's water it has water on it at a molecular level. Water molecules are bonded on top of each other so it's wet.
