To solve this problem, let's go through the steps required to prepare 135.6 mL of a 0.101 M aqueous solution of NaCl and determine the mass of NaCl needed.
1. Convert Volume from mL to L:
We have a volume of 135.6 mL. Since molarity is defined in terms of liters, we need to convert this volume to liters.
[tex]\[
\text{Volume in Liters} = \frac{135.6 \text{ mL}}{1000} = 0.1356 \text{ L}
\][/tex]
2. Calculate the Number of Moles of NaCl Needed:
Molarity (\(M\)) is defined as the number of moles of solute per liter of solution. Thus:
[tex]\[
\text{Moles of NaCl} = \text{Molarity} \times \text{Volume in Liters} = 0.101 \text{ mol/L} \times 0.1356 \text{ L} = 0.0136956 \text{ mol}
\][/tex]
3. Calculate the Mass of NaCl Needed:
To find the mass of NaCl required, we need to use its molar mass. For NaCl, the molar mass is 58.44 g/mol.
[tex]\[
\text{Mass of NaCl} = \text{Moles of NaCl} \times \text{Molar Mass of NaCl} = 0.0136956 \text{ mol} \times 58.44 \text{ g/mol} = 0.800370864 \text{ g}
\][/tex]
Thus, to prepare 135.6 mL of a 0.101 M aqueous solution of NaCl, you need to use approximately 0.8004 grams of NaCl.
