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Chapter 13: Problem 24

Describe how you would prepare 250.0 \(\mathrm{mL}\) of a. 0.500 \(\mathrm{M}\) solution of \(\mathrm{NaCl}\) by using apparatus found in a chemistry lab.

Short Answer

Expert verified
To prepare 250.0 mL of a 0.500 M solution of NaCl, firstly calculate the amount of NaCl needed, which is approximately 7.305 g. Measure this amount of NaCl using a lab scale, then dissolve it in some distilled water. Transfer the solution to a 250 mL volumetric flask, and adjust the water volume up to the mark on the flask. Ensure the solution is well mixed.

Step by step solution

01

Calculate the amount of NaCl required

Firstly, it is necessary to calculate the amount of solute (\(\mathrm{NaCl}\)) required. This can be done using the formula:\\[n=M \cdot V\]where \(M\) is the molarity, \(V\) is the volume of the solution in litres and \(n\) is the amount of solute in moles. As we have 0.500 M solution and 250.0 mL = 0.250 L, the moles of \(\mathrm{NaCl}\) required can be calculated as follows:\[n = 0.500 M \times 0.250 L = 0.125 \text{ moles}\]
02

Convert moles to grams

To convert moles to grams, use the molar mass of \(\mathrm{NaCl}\) (approximately 58.44 \(\mathrm{g/mole}\)). The equation is \( \text{mass} = n \times \text{molar mass}\), so the mass of \(\mathrm{NaCl}\) required is:\[\text{mass} = 0.125 \text{ moles} \times 58.44 \mathrm{g/mole} = 7.305 \mathrm{g}\]
03

Prepare the solution

To prepare the solution with the correct molarity, measure out 7.305 g of \(\mathrm{NaCl}\) using a lab scale and dissolve it in some distilled water. Mix until it's fully dissolved, then transfer this solution to a 250 mL volumetric flask. Add additional distilled water up to the 250 ml mark on the flask (not above or below), then stopper the flask and invert it several times to ensure that the solute is evenly distributed throughout the solution.

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