What is the molarity of a solution prepared by dissolving 5.844 g of NaCl in 1.000 L of solution?

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Multiple Choice

What is the molarity of a solution prepared by dissolving 5.844 g of NaCl in 1.000 L of solution?

Explanation:
Molarity is moles of solute per liter of solution. First determine the amount of NaCl in moles: NaCl has a molar mass of 58.44 g/mol, so n = 5.844 g ÷ 58.44 g/mol = 0.100 mol. The volume is 1.000 L, so M = n/V = 0.100 mol ÷ 1.000 L = 0.100 M. This equals one-tenth of a mole per liter, since the given mass corresponds to exactly 0.1 mol in one liter. The other possibilities would require more or less NaCl per liter than what was provided.

Molarity is moles of solute per liter of solution. First determine the amount of NaCl in moles: NaCl has a molar mass of 58.44 g/mol, so n = 5.844 g ÷ 58.44 g/mol = 0.100 mol. The volume is 1.000 L, so M = n/V = 0.100 mol ÷ 1.000 L = 0.100 M. This equals one-tenth of a mole per liter, since the given mass corresponds to exactly 0.1 mol in one liter. The other possibilities would require more or less NaCl per liter than what was provided.

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