Prepare 250mls of 0.1NaCl stock solutions. Calculate how much grams of NaCl is needed to prepare 0.1N NaCl stock solution in 250mls of deionized water?

To prepare a 0.1N NaCl solution in 250mls of deionized water, we first need to calculate the molecular weight of NaCl, which is 58.44 g/mol.

Now, we can calculate the amount of NaCl needed to prepare the solution:

0.1N = 0.1 moles/L
0.1 moles/L * 0.25 L = 0.025 moles

Now, we can convert moles to grams using the molecular weight:

0.025 moles * 58.44 g/mol = 1.46 grams

Therefore, you will need 1.46 grams of NaCl to prepare a 0.1N NaCl stock solution in 250mls of deionized water.

Calculating the mass of NaCl needed:

Step 1: Convert normality to molarity:
1N = 1 mole of solute per liter of solution

Step 2: Calculate the number of moles of NaCl needed:
0.1N - 0.25L = 0.025 moles of NaCl

Step 3: Convert moles to grams using the molar mass of NaCl:
Molar mass of NaCl = 58.44 g/mol

0.025 moles of NaCl - 58.44 g/mol = 1.46 grams of NaCl

Preparing the 250mL of 0.1N NaCl stock solution:

1. Weigh out 1.46 grams of NaCl.
2. Dissolve the NaCl in a small amount of deionized water (e.g., 50 mL).
3. Transfer the solution to a 250mL volumetric flask.
4. Add deionized water to the 250mL mark.
5. Mix thoroughly to ensure homogeneity.

The resulting solution will be 250 mL of 0.1N NaCl stock solution.