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WorksheetsACID-BASE TITRATIONS
Total questions: 14
Worksheet time: 4hrs 30mins
NONE OF THESE
What is the main purpose of acid-base titrations?
To test if reactants react.
To calculate the concentration of unknown analyte.
To calculate the concentration of known analyte.
To test quality of reactants.
What is the role of an indicator in a reaction?
To help reactants react successfully.
To bind to the analyte to form a products.
To show when the reaction has reached or past the equivalence point.
To provide a surface for the reaction to occur.
What is an equivalence point?
It is the point when enough analyte has been added.
It is the point when the amount of added titrant is equal to the amount of analyte in the solution.
It is the point when the volume of titrant is equivalent the volume of analyte.
It is the point when the concentration of titrant added is equivalent to the volume of analyte.
Which of the following indicators is the best choice for this titration?
Methyl orange (pH range of color change is 3.2 - 4.4)
Methyl red (pH range of color change is 4.8 - 6.0)
Bromothymol blue (pH range of color change is 6.1 - 7.6)
Phenolphthalein (pH range of color change is 8.2 - 10.0)
A 10.00 mL sample of H2SO4 was neutralized by 13.5 mL of 1.00 M KOH by the following reaction: H2SO4 + 2KOH → K2SO4 + 2H2O
What is the molarity of H2SO4?
0.675 M
0.910 M
1.05 M
1.20 M
How many mL of 1.00 M H2SO4 is needed to neutralize 21.5 mL of 1.50 M KOH?
H2SO4 + 2KOH → K2SO4 + 2H2O
16.1 mL
1.10 mL
5.65 mL
0.900 mL
A 10.00 mL sample of H2SO4 was neutralized by 13.5 mL of 1.00 M KOH. What is the concentration of H2SO4?
H2SO4 + 2KOH → K2SO4 + 2H2O
0.675 M
1.10 M
3.44 M
0.910 M
Which of the following is used as an indicator in the titration of a weak acid and a strong base?
a. Methyl orange (3 to 4.6)
b. Bromothymol blue (6 to 7.5)
c. Phenolphthalein (8 to 9.6)
d. Methyl red (5 to 6.9)
All of these
What is the molarity of a solution of barium hydroxide, if 35 ml if 0.1 M HCl is used in the titration of 25 ml of barium hydroxide solution?
0.28
0.21
0.14
0.07
none of these
Which of the following titrations will have the equivalence point of a pH between 3 to 7?
CH3COOH and NaOH
HCl and NaOH
CH3COOH and NH3
HCl and NH3
all of these
Consider the titrations of the pairs of aqueous acids and bases listed on the left. For which pair is the pH at the equivalence point stated incorrectly?
HCl + NH3 less than 7 (pH at equivalence point)
HNO3 + Ca(OH)2 equal to 7(pH at equivalence point)
HClO4 + NaOH equal to 7 (pH at equivalence point)
HClO + NaOH
less than 7
(pH at equivalence point)
CH3COOH + KOH
greater than 7
(pH at equivalence point)
