DE Unit 9: Titrations

What is the main purpose of acid-base titrations?

• To test if reactants react.

• To calculate the concentration of unknown solution.

• To calculate the concentration of known solution.

• 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.

The pH at the equivalence point of the titration of a strong acid with a strong base is usually:

• acidic 3.9
• acidic 4.5
• neutral 7.0
• basic 8.2

What volume of NaOH was needed to reach the equivalence point

• 50ml

• 100ml

• 150ml

• 200ml

If it takes 25 mL of 0.05 M HCl to neutralize 345 mL of NaOH solutions, what is the concentration of the NaOH solution?

• 0.043 M

• 276 M

• 0.0036 M

• 0.11 M

The reaction of perchloric acid (HClO₄) with lithium hydroxide (KOH) is described by the equation

HClO₄ + KOH → KClO₄ + H₂O

Suppose 100 mL of perchloric acid is neutralized by exactly 50.0 mL of 1.0 M of Potassium hydroxide. What is the concentration of the perchloric acid?

• 0.5M

• 50M

• 2.0M

• 1.0M

A weak acid that is titrated with a strong base will have a pH at the equivalence that is___

• acidic

• basic

• neutral

• it will depend on the Ka of the acid

A strong acid that is titrated with a weak base will have a pH at the equivalence that is ___

• acidic

• basic

• neutral

• depends on the Kb of the base

It takes 22.0 mL of 1.0 M NaOH to titrate 30.0 mL of acetic acid (Ka = 1.8x10^-5). What is the pH at the equivalence point?

• 7.0

• 8.62

• 9.19

• 4.81

How many mL of 0.25M NaOH would be required to titrate 50.0 mL of a 0.15 M HBr solution?

• 30.0

• 0.030

• 50.0

• 7.0