uses of titration

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

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

• 0.8 M

• 1 M

• 1.25 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

pH less than 7.

• Acids
• Bases
• All

Which is the stronger acid?

• pH 1
• pH 4
• pH 8
• pH 13

KOH

• acid
• base
• neutral

What is the molarity of a 30 mL HCl which is neutralized by 48 mL of 0.1 M NaOH?

• 0.16 M
• 6.25 M
• 0.063 M

What are the products of the neutralization shown below?
Ca(OH)₂  +  H₂CO₃  -->  

• H₂O  +  Ca₂CO₃
• CaO +  CO₃
• H₂O  +  CaCO₃