Question text Calculate the volume of NaOH needed to reach the equivalence point. Consider the titration of 50.0 mL of 0.100 M acetic acid, CH3COOH, with 0.200 M NaOH. Reaction equation: CH3COOH + NaOH → CH3COONa + H2O Volume of NaOH solution required (1 mark)= Answer 1 Question 44[input] mL (I:1)

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Question text Calculate the volume of NaOH needed to reach the equivalence point. Consider the titration of 50.0 mL of 0.100 M acetic acid, CH3COOH, with 0.200 M NaOH. Reaction equation: CH3​COOH + NaOH → CH3​COONa + H2​O Volume of NaOH solution required (1 mark)= Answer 1 Question 44[input] mL (I:1)

BlackTom AI · Accepted Answer

To begin, identify the reactants and the stoichiometry of the neutralization reaction: CH3COOH + NaOH → CH3COONa + H2O, which occurs on a 1:1 mole basis.
First, calculate the moles of acetic acid in the sample: volume = 50.0 mL = 0.0500 L, concentration = 0.100 M. Moles of CH3COOH = 0.0500 L × 0.100 mol/L = 0.00500 mol.
Next, apply the stoichiometric ratio. Since the reaction is 1:1, the moles of NaOH needed to reach the equivalence point are also 0.00500 mol.
Then determine the required volume of NaOH solution. NaOH concentration is 0.200 M, so Volume NaOH = moles / concentration = 0.00500 mol ÷ 0.200 mol/L = 0.0250 L.
Convert this to milliliters: 0.0250 L × 1000 mL/L = 25.0 mL.
Regarding significant figures, the given data (50.0 mL, 0.100 M, and 0.200 M) each have three significant figures, so the final volume should be reported as 25.0 mL to reflect the appropriate precision.
A potential pitfall would be misapplying the molarity or mistaking the reaction ratio; remember the 1:1 stoichiometry means equal moles of base and acid at the equivalence point, so you must first find the acid moles and then convert to the corresponding NaOH volume.
If you inadvertently used a different acid concentration or a different titrant volume without adjusting for the ratio, you would obtain an incorrect volume, underscoring the importance of consistent units and stoichiometric balance.

Question text Calculate the volume of NaOH needed to reach the equivalence point. Consider the titration of 50.0 mL of 0.100 M acetic acid, CH3COOH, with 0.200 M NaOH. Reaction equation: CH3COOH + NaOH → CH3COONa + H2O Volume of NaOH solution required (1 mark)= Answer 1 Question 44[input] mL (I:1)

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