객관식
What is the pH at the equivalence point when titrating a 0.200 M solution of sodium hydroxide (NaOH) with 0.200 M HBr?
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18. Aqueous Equilibrium
Intro to Acid-Base Titration Curves
객관식
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)?
A
100.0 mL
B
50.0 mL
C
25.0 mL
D
75.0 mL
검증된 단계별 안내1
Understand the concept of the equivalence point in a titration: It is the point at which the amount of titrant added is chemically equivalent to the amount of substance present in the sample.
Identify the balanced chemical equation for the reaction: Hydrochloric acid (HCl) reacts with sodium hydroxide (NaOH) to form water (H₂O) and sodium chloride (NaCl). The equation is:
Calculate the moles of HCl present initially: Use the formula , where is the number of moles, is the concentration (0.1 M), and is the volume in liters (50.0 mL converted to 0.050 L).
Determine the moles of NaOH required to reach the equivalence point: Since the reaction is a 1:1 molar ratio, the moles of NaOH needed will be equal to the moles of HCl calculated in the previous step.
Calculate the volume of NaOH needed: Use the formula , where is the moles of NaOH and is the concentration of NaOH (0.1 M).
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