How many grams of sodium chloride are needed to prepare 0.5 L of a 0.2 M solutio

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Question: How many grams of sodium chloride are needed to prepare 0.5 L of a 0.2 M solution?

Options:

Correct Answer: 11.68 g

Solution:

Molar mass of NaCl = 58.44 g/mol. Moles needed = 0.2 M * 0.5 L = 0.1 moles. Mass = moles * molar mass = 0.1 * 58.44 g = 5.844 g.

How many grams of sodium chloride are needed to prepare 0.5 L of a 0.2 M solution?

How many grams of sodium chloride are needed to prepare 0.5 L of a 0.2 M solution?

Step 1: Understand that Molarity (M) is the number of moles of solute per liter of solution.
Step 2: Identify the desired concentration of the solution, which is 0.2 M.
Step 3: Identify the volume of the solution you want to prepare, which is 0.5 L.
Step 4: Calculate the number of moles needed using the formula: Moles = Molarity * Volume. So, Moles = 0.2 M * 0.5 L = 0.1 moles.
Step 5: Find the molar mass of sodium chloride (NaCl), which is 58.44 g/mol.
Step 6: Calculate the mass of sodium chloride needed using the formula: Mass = Moles * Molar Mass. So, Mass = 0.1 moles * 58.44 g/mol = 5.844 g.

Molarity – Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution.
Molar Mass – Molar mass is the mass of one mole of a substance, typically expressed in grams per mole.
Mass Calculation – To find the mass of a solute needed for a solution, multiply the number of moles by the molar mass.