Multiple Choice
What will be the color of the indicator in the above question in a solution that has a pH of 6?
18. Aqueous Equilibrium
Intro to Acid-Base Titration Curves
Back18. Aqueous Equilibrium
Intro to Acid-Base Titration Curves
- Multiple Choice
Consider the titration of 60.0 mL of 0.200 M H3PO3 solution with 0.350 M potassium hydroxide, KOH solution. How many milliliters of base would be required to reach each of its equivalence points?
- Multiple ChoiceWhich of the following acids would be needed to combine with its potassium salt to produce a solution buffered at pH 5.00?
Chlorous acid: pKa = 1.95
Nitrous acid: pKa = 3.34
Formic acid: pKa = 3.74
Acetic acid: pKa = 4.74
Hypochlorous acid: pKa = 7.54 - Multiple Choice
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
- Multiple ChoiceA buffer solution is prepared by adding 10.0 g of ammonium chloride (NH₄Cl) to 250 mL of 1.00 M NH₃ solution. What is the pH of the resulting buffer solution?
- Multiple ChoiceWhat is the pH at the equivalence point when titrating a 0.200 M solution of sodium hydroxide (NaOH) with 0.200 M HBr?
- Multiple ChoiceWhen comparing titration curves for two acids with different pKa values, which of the following statements is true?
- Multiple ChoiceIn an acid-base titration, how is the pH at the beginning of the titration determined?
- Multiple ChoiceIn a titration of a weak acid with a strong base, what is the pH at the equivalence point?
- Multiple ChoiceIn 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)?