What volume of 0.5 molarity of BaCl2 is needed to have 0.1 moles of BaCl2?
mols = M x L
0.1 = 0.5 x ? L
L = ?
To calculate the volume of a solution needed, we can use the equation:
Molarity (M) = Moles (mol) / Volume (L)
In this case, we know the molarity (0.5 M) and moles (0.1 mol) of BaCl2, and we need to calculate the volume.
Let's rearrange the equation to solve for Volume:
Volume (L) = Moles (mol) / Molarity (M)
Plugging in the values:
Volume (L) = 0.1 mol / 0.5 M
Volume (L) = 0.2 L
Therefore, 0.2 liters of the 0.5 M BaCl2 solution is needed to have 0.1 moles of BaCl2.
To find the volume of 0.5 M BaCl2 needed to have 0.1 moles of BaCl2, we can use the formula:
Molarity = Moles / Volume
Rearranging the formula, we get:
Volume = Moles / Molarity
Substituting the given values, we have:
Volume = 0.1 moles / 0.5 M
Calculating this, we find:
Volume = 0.2 liters or 200 milliliters
Therefore, 0.2 liters or 200 milliliters of 0.5 M BaCl2 solution is needed to have 0.1 moles of BaCl2.