Multiple Choice
During the titration of vinegar (acetic acid, CH3COOH) with a strong base such as NaOH, which of the following best describes the pH at the equivalence point?
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18. Aqueous Equilibrium
Titrations: Weak Acid-Strong Base
Back18. Aqueous Equilibrium
Titrations: Weak Acid-Strong Base
- Multiple ChoiceIn the context of titrations involving a weak acid and a strong base, which of the following best describes a back titration?19views
- Multiple ChoiceIn a titration involving a weak acid and a strong base, what is the term for the solution of unknown concentration to which another solution is slowly added?13views
- Multiple ChoiceCalculate the volume (mL) of 0.500 M NaOH required to reach the equivalence point in the titration of 25.0 mL of 0.650 M HF. Ka for HF = 3.5 × 10−4.865views
- Multiple ChoiceFor a titration of a weak acid with a strong base, the pH at the equivalence point ________.814views
- Multiple Choice20.0 mL of 0.500 M HC2H3O2 is titrated with 0.350 M KOH. Determine the pH after 15.0 mL of the base has been added. Ka for HC2H3O2 = 1.8 × 10−5.588views
- Multiple Choice20.0 mL of 0.500 M HC2H3O2 is titrated with 0.350 M KOH. Determine the pH after 15.0 mL of the base has been added. Ka for HC2H3O2 = 1.8 × 10−5.650views
- Multiple ChoiceDetermine the pH when 5.00 mL of excess KOH (beyond the equivalence point) has been added to the titration of 20.0 mL of 0.500 M HC2H3O2 with 0.350 M KOH.657views
- Multiple ChoiceCalculate the pH at the equivalence point for the titration of 20.0 mL of 0.500 M HC2H3O2 with 0.350 M KOH. Ka for HC2H3O2 = 1.8 × 10−5.617views
- Multiple Choice
In order to create a buffer 7.510 g of sodium cyanide is mixed with 100.0 mL of 0.250 M hydrocyanic acid, HCN. What is the pH of the buffer solution after the addition of 12.0 mL of 0.300 M NaH? Ka = 4.9 × 10−10.
578views8rank1comments - Multiple Choice
Consider the titration of 75.0 mL of 0.60 M HNO2 with 0.100 M NaOH at the equivalence point. What would be the pH of the solution at the equivalence point? The Ka of HNO2 is 4.6 × 10−4.
573views6rank - Multiple Choice
Calculate the pH of the solution resulting from the mixing of 55.0 mL of 0.100 M NaCN and 75.0 mL of 0.100 M HCN with 0.0090 moles of NaOH.
538views6rank1comments - Open Question
How will you detect the endpoint of the titration of the borate ion with HCl?
293views - Open Question
Calculate the pH when 50.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10-9)
307views - Multiple Choice20.0 mL of 0.500 M HC2H3O2 is titrated with 0.350 M KOH. Determine the pH after 15.0 mL of the base has been added. Ka for HC2H3O2 = 1.8 × 10⁻⁵.238views