Multiple Choice
In an acid-base titration, what is the volume of added base required to reach the equivalence point if 50.0 mL of 0.1 M hydrochloric acid (HCl) is titrated with 0.1 M sodium hydroxide (NaOH)?
18. Aqueous Equilibrium
Intro to Acid-Base Titration Curves
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Consider the titration of 100.0 mL of 0.40 M HCl with 0.40 M NaOH. If sodium hydroxide is the titrant, which volume would place it in excess?
a) 70.0 mL b) 25.0 mL c) 100.0 mL d) 110.0 mL e) 9.0 mL
A
70.0 mL
B
25.0 mL
C
100.0 mL
D
110.0 mL
E
9.0 mL
Verified step by step guidance1
Start by understanding the concept of titration. In a titration, a solution of known concentration (the titrant) is added to a solution of unknown concentration until the reaction reaches the equivalence point, where the amount of titrant equals the amount of substance in the solution being titrated.
Calculate the moles of HCl present initially. Use the formula: \( \text{moles} = \text{concentration} \times \text{volume} \). For HCl, the concentration is 0.40 M and the volume is 100.0 mL (or 0.100 L).
Determine the moles of NaOH needed to reach the equivalence point. Since HCl and NaOH react in a 1:1 molar ratio, the moles of NaOH required will be equal to the moles of HCl calculated in the previous step.
Calculate the volume of NaOH needed to reach the equivalence point using the formula: \( \text{volume} = \frac{\text{moles}}{\text{concentration}} \). The concentration of NaOH is 0.40 M.
Compare the calculated volume of NaOH needed to reach the equivalence point with the given options. Any volume greater than the equivalence point volume will place NaOH in excess.
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