NEW
Font size
WorksheetsA-B TITRATION AND MOLARITY
Total questions: 12
Worksheet time: 3hrs 0mins
Calculate the Molarity in a solution containing 40.0 g of NaCl dissolved in 500.0 ml of H2O.
0.08 M
12.5 M
1.37 M
0.74 M
A solution is made by dissolving 0.50 mole of NaCl in enough water to give a final volume of 400.0 mL. What is the molarity of the solution?
0.10 M
0.40 M
1.25 M
2.33 M
How many moles of solute are present in 50.0 mL of 0.20M KNO3?
10.0 moles solute
0.05 moles solute
1.00 moles solute
0.01 moles solute
NONE OF THESE
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.
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
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
A titration involves the chemical reaction between an analyte solution and the
titrant
titrator
standard
all of the above
