Titrations
Chemistry ⇒ Analytical Chemistry
Titrations starts at 11 and continues till grade 12.
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See sample questions for grade 12
A 0.250 g sample of KHP (molar mass = 204.22 g/mol) is titrated with NaOH. If 15.0 mL of NaOH is required to reach the endpoint, what is the concentration of the NaOH solution?
A 0.300 M solution of NaOH is used to titrate 40.0 mL of H2SO4. If 60.0 mL of NaOH is required, what is the concentration of the H2SO4?
A 0.500 g sample of oxalic acid (H2C2O4, molar mass = 90.03 g/mol) is titrated with 0.100 M NaOH. How many mL of NaOH are required to reach the endpoint?
A 25.0 mL sample of acetic acid is titrated with 0.100 M NaOH. If the equivalence point is reached after adding 32.5 mL of NaOH, what is the concentration of the acetic acid?
A student titrates 25.0 mL of HCl with 0.100 M NaOH. If 30.0 mL of NaOH is required to reach the equivalence point, what is the concentration of the HCl solution?
A titration is performed using 0.100 M HCl and 0.100 M NaOH. If 25.0 mL of HCl is titrated, what volume of NaOH is needed to reach the equivalence point?
Calculate the volume of 0.200 M NaOH required to neutralize 50.0 mL of 0.150 M H2SO4.
Describe the main characteristics of a good primary standard.
Describe the role of a buffer in a titration.
Describe the steps involved in preparing a standard solution for titration.
Explain the difference between the endpoint and the equivalence point in a titration.
Explain why a burette is preferred over a pipette for delivering the titrant in a titration.
Explain why it is important to swirl the flask during a titration.
Explain why phenolphthalein is not suitable for titrating a weak acid with a weak base.
What is the primary purpose of a titration in analytical chemistry?
