M5 ACID BASE QUIZ

A neutralization reaction is a reaction between 

• Acid and a Base 

• Acid and water 

• 
  Base and water 

• None of the above 

Which pH number below reflects a weak acid?

• 1

• 6

• 8

• 13

The buffer solution is able to maintain pH by some events, except . . .

• The addition of a little acid

• The addition of a little base

• Dilution

• 
  The addition of excess acid

The following mixture of solutions that form a buffer solution is . . .

• 50 mL CH₃COOH 0.2 M and 50 mL NaOH 0.1 M

• 50 mL CH₃COOH 0.2 M and 100 mL NaOH 0.1 M

• 50 mL HCl 0.2 M and 100 mL NH₄OH 0.1 M

• 50 mL HCl 0.2 M and 50 mL NH₄OH 0.1 M

The pH solution that consist of CH₃COOH 0.01 M and CH₃COONa 0.01 M with Ka = 10^-5 is . . .

• 9

• 8

• 10

• 5

Acidic buffer is made up of

• weak acid and weak base

• weak acid and its conjugate salt

• weak acid and its conjugate base

• strong acid and its conjugate base

Which of the following statements ARE TRUE about buffer solution?

(you may choose more than one answer)

• 
  pH of buffer solution will never change despite addition of small amount of base or acid

• 
  Buffer can be made by mixing weak acid and salt of its conjugate base or by mixing weak base with salt of its conjugate acid

• Buffer has acid and base components that can work specifically to resist pH change

• the closer the ratio of concentration weak acid/base to the concentration of salt of its conjugate base/acid, the less effective the buffer to resist pH change

What is the main purpose of acid-base titrations?

• To test if reactants react.

• To calculate the concentration of known analyte.

• To test quality of reactants.

• To calculate the concentration of unknown analyte.

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.

In the titration of a weak acid of unknown concentration with a standard solution of a strong base, a pH meter was used to follow the progress of the titration. Which of the following is true for this experiment?

• The [H⁺] at the equivalence point equals the ionization constant of the acid.

• 
  The pH at the equivalence point depends on the indicator used.

• The graph of pH versus volume of base added rises gradually at first and then much more rapidly.

• 
  The graph of pH versus volume of base added shows no sharp rise.