Questions: What is the molarity of a solution prepared by dissolving 4 grams of NaOH in 100 mL of water? 5.00 M 0.50 M 1.00 M 0.01 M

What is the molarity of a solution prepared by dissolving 4 grams of NaOH in 100 mL of water? 5.00 M 0.50 M 1.00 M 0.01 M
Transcript text: What is the molarity of a solution prepared by dissolving 4 grams of NaOH in 100 mL of water? 5.00 M 0.50 M 1.00 M 0.01 M
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Solution

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Solution Steps

Step 1: Calculate the Molar Mass of NaOH
  • Determine the molar mass of NaOH by adding the atomic masses of its constituent elements:
    • Sodium (Na): \( 22.99 \, \text{g/mol} \)
    • Oxygen (O): \( 16.00 \, \text{g/mol} \)
    • Hydrogen (H): \( 1.01 \, \text{g/mol} \)
  • Molar mass of NaOH = \( 22.99 + 16.00 + 1.01 = 40.00 \, \text{g/mol} \)
Step 2: Calculate the Number of Moles of NaOH
  • Use the formula: \[ \text{moles of NaOH} = \frac{\text{mass of NaOH}}{\text{molar mass of NaOH}} \]
  • Substitute the given values: \[ \text{moles of NaOH} = \frac{4 \, \text{g}}{40.00 \, \text{g/mol}} = 0.1 \, \text{mol} \]
Step 3: Calculate the Molarity of the Solution
  • Use the formula for molarity: \[ \text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}} \]
  • Convert 100 mL to liters: \( 100 \, \text{mL} = 0.1 \, \text{L} \)
  • Substitute the values: \[ \text{Molarity} = \frac{0.1 \, \text{mol}}{0.1 \, \text{L}} = 1.00 \, \text{M} \]

Final Answer

\(\boxed{1.00 \, \text{M}}\)

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