Titration Problems

Acid + Base ₋--> 

• salt + hydrogen
• salt + water
• salt + carbon dioxide + water
• salt

What is the endpoint of a titration

• Where the amount of acid and base are equal as shown by a colour change 
• Where there is no base
• When the volume of base in the burette is used up 
• When there is no acid

What is the volume in this burette?

• 25.80mL
• 25.30mL
• 24.70mL
• 24.20mL

What solution usually goes in the burette?

• Acid
• Base
• Indicator
• Water

What indicator is commonly used in titrations?

• Phenolphthalein
• Bromothymol Blue 
• Litmus
• Universal 

What is the long graduated piece of equipment called?

• Pipette
• Tube
• Burette
• Measuring Cylinder

what is the reading on this burette?

• 4.40mL
• 3.50mL
• 3.60mL
• 4.50mL

If phenolphthalein turns bright pink, it indicates

• an acid 
• a base
• a neutral

The following neutralization reaction occurs in the classroom.
HCl  +  KOH  -->  H₂O  +  KCl
If a student uses 25.0 mL of a 0.5M solution of KOH, what is the molarity of the acid if the is 15.0mL of acid neutralized?

• 0.8M
• 1.2M
• 12.5M

In a titration, 15.5 g of oxalic acid was dissolved in a flask and neutralized with 31.2 mL of NaOH.  Determine the molarity of the NaOH.

Hint: Primary standards (like oxalic acid, here) incude water in their formula.  As a result, they do not absorb atmospheric water.  Oxalic acid has the chemcial formula: H₂C₂O₄⋅2H₂O (so be sure to include the 2 extra water molecules).

• 7.88 mol/L
• 8.33 M
• 3.55 M
• 0.333 mol/L