Titration Problems

What is the volume in this burette?

• 24.1mL
• 24.3mL
• 24.2L
• 24.2mL

What does pH measure?

• Amount of Oxygen Ions
• Amount of Hydrogen Ions
• The amount of salt in a solution
• The density

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 reading on this burette?

• 4.40mL
• 3.50mL
• 3.60mL
• 4.50mL

I have 25mL of 1M HCl which neutralises 20mL of NaOH. What is the concentration of the NaOH?

• 0.8 M
• 1 M
• 1.25 M

Tags

NGSS.HS-PS1-7

A 50.0 mL sample of Ca(OH)₂ is neutralized by 300.0 mL of HCl solution with a pH of 3. Calculate the molarity of the Ca(OH)₂ solution.

• 1.0 M

• 0.50 M

• 0.006 M

• 0.30 M

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

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 15.0mL of acid neutralized?

• 0.8M
• 1.2M
• 12.5M

Tags

NGSS.HS-PS1-7

pH less than 7.

• Acids
• Bases
• All

Which is the stronger acid?

• pH 1
• pH 4
• pH 8
• pH 13