A 0.15 M sulfuric acid (H2SO4) solution is titrated with 0.12 M sodium hydroxide (NaOH). Calculate the volume of NaOH solution required to neutralize 25.0 mL of H2SO4 solution.
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To calculate the volume of NaOH solution required to neutralize the sulfuric acid solution, we can use the equation:
M1V1 = M2V2
Where:
M1 = molarity of the sulfuric acid solution = 0.15 M
V1 = volume of the sulfuric acid solution = 25.0 mL = 0.0250 L (convert to liters)
M2 = molarity of the sodium hydroxide solution = 0.12 M
V2 = volume of the sodium hydroxide solution (to be determined)
Substituting the given values into the equation, we have:
(0.15 M)(0.0250 L) = (0.12 M)(V2)
Rearranging the equation to solve for V2:
V2 = (0.15 M)(0.0250 L) / (0.12 M)
V2 ≈ 0.03125 L
Therefore, approximately 0.03125 liters (or 31.25 mL) of the sodium hydroxide solution is required to neutralize 25.0 mL of the sulfuric acid solution.
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