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 11

A 0.200 mol/L solution of HNO₃ is titrated with 0.100 mol/L NaOH. If 50.0 mL of NaOH is required, what volume of HNO₃ was titrated?

A 10.0 mL sample of 0.500 mol/L HCl is titrated with NaOH. If the endpoint is reached after 20.0 mL of NaOH is added, what is the concentration of the NaOH?

A 20.0 mL sample of 0.250 mol/L H₂SO₄ is titrated with NaOH. What volume of 0.500 mol/L NaOH is needed to reach the equivalence point?

A 25.0 mL sample of 0.100 mol/L Na₂CO₃ is titrated with HCl. What volume of 0.200 mol/L HCl is required to reach the endpoint? (Na₂CO₃ + 2HCl → 2NaCl + H₂O + CO₂)

A 25.0 mL sample of acetic acid (CH₃COOH) is titrated with 0.150 mol/L NaOH. The endpoint is reached after 40.0 mL of NaOH is added. What is the concentration of the acetic acid?

A 50.0 mL sample of NaOH is titrated with 0.200 mol/L HCl. If 25.0 mL of HCl is required to reach the endpoint, what is the concentration of the NaOH?

A student titrates 25.0 mL of HCl with 0.100 mol/L NaOH. If 30.0 mL of NaOH is required to reach the endpoint, what is the concentration of the HCl?

Describe the steps involved in performing a titration to determine the concentration of an acid.

During a titration, why is it important to swirl the flask while adding titrant?

Explain why a burette is preferred over a pipette for delivering the titrant in a titration.

If 0.0250 L of 0.200 mol/L HCl is neutralized by 0.0500 L of NaOH, what is the concentration of the NaOH?

The balanced equation for the reaction between H₂SO₄ and NaOH is: H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O. If 0.025 mol of H₂SO₄ is titrated, how many moles of NaOH are required?

What is the purpose of a titration in chemistry?

A 0.0250 mol/L solution of Ba(OH)₂ is titrated with 0.0500 mol/L HCl. If 40.0 mL of HCl is required to reach the endpoint, what volume of Ba(OH)₂ was titrated?

A 0.100 mol/L solution of a monoprotic acid HA is titrated with 0.200 mol/L NaOH. If 30.0 mL of acid requires 15.0 mL of NaOH to reach the endpoint, is the result consistent with the stoichiometry of the reaction? Justify your answer.

A 15.0 mL sample of 0.300 mol/L H₂SO₄ is titrated with KOH. If the endpoint is reached after 36.0 mL of KOH, calculate the concentration of the KOH solution. (H₂SO₄ + 2KOH → K₂SO₄ + 2H₂O)

A 25.0 mL sample of a diprotic acid H₂A is titrated with 0.200 mol/L NaOH. The endpoint is reached after 37.5 mL of NaOH is added. Calculate the concentration of the acid solution.

During a titration, a student accidentally overshoots the endpoint by adding excess titrant. Explain how this affects the calculated concentration of the analyte and suggest a method to minimize this error in future titrations.

Explain why it is important to choose an indicator whose color change range closely matches the pH at the equivalence point of a titration.