Titrations

Question 1

What is the “known” solution which as a precise and accurate concentration?

Answer 1

the titrant

Question 2

Where is the equivalence point for the titration between a weak acid and a strong base?

Answer 2

pH > 7

Question 3

What is the duration of a titration?

Answer 3

o A titration is performed until the solution has essentially experienced the entire range of pH conditions from acidic to basic (or basic to acidic)

Question 4

Why are titrations performed?

Answer 4

o Titrations are performed to either measure the concentration of an unknown solution and/or to determine the Ka of an unknown acid (or Kb of an unknown base)

Question 5

What was titrated for the equivalence point to be at a pH < 7?

Answer 5

strong acid and weak base

Question 6

Where is the equivalence point for the titration between a weak base and a strong acid?

Answer 6

pH < 7

Question 7

What are the 2 solutions of a titration?

Answer 7

the analyte and the titrant

Question 8

What was titrated for the equivalence point to be at a pH > 7?

Answer 8

weak acid and strong base

Question 9

At what point will a weak acid’s pH = pKa or a weak base’s pOH = pKb?

Answer 9

half-equivalence point

Question 10

What is the point at which half of the original analyte has been neutralized?

Answer 10

half-equivalence point

Question 11

What is a procedure in which a strong acid/base of accurate concentration is added stepwise in small amounts (aliquots) to incrementally neutralize the solution?

Answer 11

titration

Question 12

Define Equivalence Point (stoichiometric point)

Answer 12

the point at which the number of moles of added base are equal to the number of moles of the acid in the analyte solution

Question 13

What was titrated for the equivalence point to be at a pH = 7?

Answer 13

strong acid and strong base

Question 14

What is the analyte?

Answer 14

 The analyte is the “unknown” solution for which you would like to know the concentration or the equilibrium constant
• The analyte can either be an acid or base, and it can be either weak or strong

Question 15

Where is the equivalence point for the titration between a strong acid and strong base?

Answer 15

pH = 7

Question 16

What is the range of an indicator?

Answer 16

o The approximate range of a typical indicator is +/- 1 off the pKa value

Question 17

Define half-equivalence point

Answer 17

the point at which half of the original analyte has been neutralized

Question 18

What part of the titration is the “unknown” solution for which you would like to know the concentration or the equilibrium constant?

Answer 18

the analyte

Question 19

What are indicators?

Answer 19

o Acid/base indicators are nothing more than a “special” type of weak acid or weak base

Question 20

Define titration

Answer 20

procedure in which a strong acid/base of accurate concentration is added stepwise in small amounts (aliquots) to incrementally neutralize the solution

Question 21

On a titration curve, where is the equivalence point?

Answer 21

near the end of the point of inflection

Question 22

What is the titrant?

Answer 22

 The titrant is the “known” solution which as a precise and accurate concentration
• The titrant is generally a strong acid or base

Question 23

What is the point at which the number of moles of added base are equal to the number of moles of the acid in the analyte solution?

Answer 23

Equivalence Point (stoichiometric point)

Question 24

How do indicators work?

Answer 24

o The acid form (protonated) will be one color while the base form (deprotonated) will have a different color