# Yo what volume should 5.0g of KCl be diluted in order to prepare a 0.25 M solution?

Mar 22, 2018

0.268L

#### Explanation:

$G i v e n :$
Mass = 5.0g of KCl
Concentration = 0.25M KCl
Molar Mass KCl = 74.5513g/mol
Volume = ?

We can use the molarity formula to solve this, which is

$\text{Molarity"="moles of solute"/"litres of solution}$

However since we are trying to find the volume, we use the following formula (rearranged):

$\text{Volume"="moles of solute"/"molarity}$

Also, our value 5.0g KCl is not in moles quite yet so we convert that in terms of moles of KCl, using the mole formula,

$\text{Moles"="mass"/"molar mass}$

${n}_{K C l} = \text{5.0g"/"74.5513g/mol}$

${n}_{K C l} = 0.067067 \ldots . . m o l$

Next we plug in the given values into the volume formula.

$\text{Volume"="moles of solute"/"molarity}$

${V}_{K C l} = \text{0.067067.....mol"/"0.25L}$

${V}_{K C l} = 0.268 \ldots L$

$\therefore$ $\text{5.0 g KCl}$ should be diluted to $\text{0.268 L}$ in order to prepare a $\text{0.25 M KCl}$ solution.