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Titration Calculations

Chemistry ⇒ Acids, Bases, and Salts

Titration Calculations starts at 10 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Titration Calculations. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.
See sample questions for grade 12
A 0.0500 M solution of HCl is titrated with 0.100 M NaOH. If 20.0 mL of HCl is used, what volume of NaOH is required to reach the endpoint?
A 0.100 M solution of Ba(OH)2 is used to titrate 50.0 mL of 0.200 M HCl. What volume of Ba(OH)2 is required?
A 0.100 M solution of H2SO4 is titrated with 0.100 M NaOH. If 25.0 mL of H2SO4 is used, what volume of NaOH is required for complete neutralization?
A 0.100 M solution of HCl is titrated with 0.100 M NaOH. If 20.0 mL of HCl is used, how many moles of NaOH are required to reach the endpoint?
A 0.150 M solution of acetic acid (CH3COOH) is titrated with 0.100 M NaOH. If 25.0 mL of acetic acid is used, what volume of NaOH is needed to reach the equivalence point?
A 0.200 M solution of H2SO4 is titrated with 0.100 M NaOH. If 25.0 mL of H2SO4 is used, what volume of NaOH is needed for complete neutralization?
A 0.250 M solution of NaOH is used to titrate 50.0 mL of H2SO4. If 40.0 mL of NaOH is required, what is the concentration of H2SO4?
A 25.0 mL sample of 0.200 M HNO3 is titrated with 0.100 M KOH. What volume of KOH is needed to reach the endpoint?
A 25.0 mL sample of monoprotic acid is titrated with 0.200 M NaOH. If 30.0 mL of NaOH is required, what is the concentration of the 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 endpoint, what is the concentration of the HCl?
A titration is performed using 0.0500 M H2SO4 and 0.100 M NaOH. If 25.0 mL of H2SO4 is used, what volume of NaOH is required for complete neutralization?
Calculate the volume of 0.200 M H2SO4 required to neutralize 50.0 mL of 0.300 M NaOH. (Assume complete neutralization.)
During a titration, why is it important to swirl the flask while adding titrant?
Explain the difference between a primary standard and a secondary standard in titration.
Explain why a weak acid-strong base titration has a higher pH at the equivalence point than a strong acid-strong base titration.
If 0.0250 mol of HCl is neutralized by 0.0250 mol of NaOH, what is the total volume if both solutions are 0.100 M?
If 40.0 mL of 0.250 M KOH is required to neutralize 20.0 mL of H2SO4, what is the concentration of the H2SO4?
The balanced equation for the reaction between HCl and NaOH is: HCl + NaOH → NaCl + H2O. What is the mole ratio of HCl to NaOH?
What is the purpose of a titration in chemistry?