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Precipitation Titration

Total questions: 87

Worksheet time: 44mins

Name
Class
Date
1.

What is the process called where a solid forms from a solution in precipitation titration?

a)

Precipitation formation

b)

Evaporation

c)

Condensation

d)

Sublimation

2.

Which curve is studied in precipitation titration to understand the reaction progress?

a)

Titration curves

b)

Absorption curves

c)

Calibration curves

d)

Solubility curves

3.

Which of the following is an end point detection method in precipitation titration?

a)

Mohr method

b)

Volhard method

c)

Fajan’s method

d)

All of the above

4.

Name one end point detection method used in precipitation titration.

a)

Mohr method

b)

Volhard method

c)

Fajans method

d)

Karl Fischer method

5.

Name another end point detection method used in precipitation titration.

a)

Volhard method

b)

Mohr method

c)

Fajans method

d)

Karl Fischer method

6.

Precipitation Formation: Analyte is titrated with a ________ of a precipitating agent in accordance with defined reaction stoichiometry. Fill in the blank.

a)

standard solution

b)

buffer solution

c)

dilute acid

d)

indicator

7.

Precipitation Formation: Titrations with ________ are useful for determining certain analytes, e.g. Cl⁻ can be determined when titrated with AgNO₃. Fill in the blank.

a)

precipitating agents

b)

oxidizing agents

c)

complexing agents

d)

reducing agents

8.

A titration curve for a precipitation titration can be constructed by plotting mL Ag⁺ against pX. Which of the following can X be?

a)

Cl⁻

b)

Br⁻

c)

I⁻

d)

SCN⁻

e)

All of the above

9.

In argentometric titration, plots of titration curves are normally sigmoidal curves consisting of pAg (or pAnalyte) vs. volume of AgNO3 solution added. What is the shape of the titration curve in argentometric titration?

a)

Linear

b)

Sigmoidal

c)

Exponential

d)

Parabolic

10.

In the titration of chloride with silver, what is the chemical reaction that occurs?

a)

AgNO3 + NaCl → AgCl + NaNO3

b)

Ag+ + Cl- → AgCl

c)

Ag + Cl2 → AgCl2

d)

AgNO3 → Ag+ + NO3-

11.

The points on the titration curve can be calculated, given the analyte concentration, AgNO3 concentration and the appropriate _______.

a)

Ksp

b)

pH

c)

molarity

d)

temperature

12.

Calculate the [Ag+], [Cl-] and pAg in a titration of 20.00 mL of 0.100 M AgNO3 with 0.100 M NaCl.

a)

[Ag+] = 0.100 M, [Cl-] = 0.100 M, pAg = 1.00

b)

[Ag+] = 0.050 M, [Cl-] = 0.050 M, pAg = 1.30

c)

[Ag+] = 0.010 M, [Cl-] = 0.010 M, pAg = 2.00

d)

[Ag+] = 0.001 M, [Cl-] = 0.001 M, pAg = 3.00

13.

What is the pAg when 0.00 mL of titrant is added?

a)

1.00

b)

2.00

c)

3.00

d)

0.50

14.

What is the pAg when 10.00 mL of titrant is added?

a)

1.48

b)

2.35

c)

0.98

d)

3.12

15.

What is the pAg when 20.00 mL of titrant is added?

a)

4.87

b)

2.15

c)

6.32

d)

8.01

16.

What is the pAg when 25.00 mL of titrant is added?

a)

7.79

b)

5.32

c)

8.45

d)

6.21

17.

At the start of the titration, [Ag+] = 0.100 M. Calculate the pAg using the formula pAg = -log [Ag+].

a)

1.00

b)

0.10

c)

2.00

d)

0.50

18.

Given: 10.00 mL titrant added (Pre-equivalence Region). Calculate the mmol of Ag+ started if 20.00 mL of 0.100 mM Ag+ solution is used.

a)

2.00 mmol

b)

0.20 mmol

c)

0.002 mmol

d)

20.0 mmol

19.

Given: 10.00 mL titrant added (Pre-equivalence Region). Calculate the mmol of Cl- added if 10.00 mL of 0.100 mM Cl- solution is used.

a)

1.00 mmol

b)

0.10 mmol

c)

10.0 mmol

d)

0.01 mmol

20.

Given: 10.00 mL titrant added (Pre-equivalence Region). Calculate the mmol of Ag+ left after reaction if 2.00 mmol Ag+ started and 1.00 mmol Cl- added.

a)

1.00 mmol

b)

0.50 mmol

c)

2.00 mmol

d)

0.00 mmol

21.

Given: 10.00 mL titrant added (Pre-equivalence Region). What is the total volume of solution after mixing 20 mL Ag+ and 10 mL Cl-?

a)

30 mL

b)

20 mL

c)

10 mL

d)

25 mL

22.

Calculate the concentration of Ag+ left in solution if 1.00 mmol Ag+ is left in 30 mL solution.

a)

0.0333 M

b)

0.00333 M

c)

0.333 M

d)

0.0300 M

23.

Given: 10.00 mL titrant added (Pre-equivalence Region). Calculate the pAg if [Ag+] = 0.0333 M. Use the formula pAg = -log[Ag+].

a)

1.48

b)

2.48

c)

0.48

d)

3.48

24.

At the equivalence point, what is the number of mmol Ag+ started if 20.00 mL of 0.100 mM Ag+ solution is used?

a)

2.00 mmol

b)

0.20 mmol

c)

0.002 mmol

d)

20.0 mmol

25.

At the equivalence point, what is the number of mmol Cl- added if 20.00 mL of 0.100 mM Cl- solution is used?

a)

2.00 mmol

b)

0.20 mmol

c)

0.002 mmol

d)

0.020 mmol

26.

At the equivalence point, the concentration of Ag+ and Cl- are equal. If Ksp=[Ag+][Cl−]Ksp = [Ag+][Cl-] and Ksp=1.8×10−10Ksp = 1.8 \times 10^{-10} , what is the value of s (the concentration of Ag+ or Cl-)?

a)

1.34 × 10^{-5} M

b)

1.8 × 10^{-10} M

c)

9.0 \times 10^{-6} M

d)

2.0 × 10^{-5} M

27.

Calculate pAg = pCl at the equivalence point using the formula pAg=pCl=−log(1.34×10−5pAg = pCl = -log(1.34 \times 10^{-5} . What is the value?

a)

4.87

b)

3.87

c)

5.87

d)

6.87

28.

After the stoichiometric point, excess NaCl is being added into the solution. After 25 mL of 0.100 M NaCl has been added, what is the mmol of Ag+ started?

a)

2.00 mmol

b)

1.50 mmol

c)

2.50 mmol

d)

0.50 mmol

29.

After the stoichiometric point, excess NaCl is being added into the solution. After 25 mL of 0.100 M NaCl has been added, what is the mmol of Cl- added?

a)

2.50 mmol

b)

0.25 mmol

c)

25.0 mmol

d)

0.025 mmol

30.

After the stoichiometric point, excess NaCl is being added into the solution. After 25 mL of 0.100 M NaCl has been added, what is the mmol of Cl- in excess?

a)

0.50 mmol

b)

2.5 mmol

c)

0.25 mmol

d)

1.0 mmol

31.

After the stoichiometric point, excess NaCl is being added into the solution. After 25 mL of 0.100 M NaCl has been added, what is the total volume of solution? Volume of solution = 20 + 25 = ______ mL

a)

45 mL

b)

40 mL

c)

25 mL

d)

50 mL

32.

Given the calculation: [Cl⁻] ≅ (0.50 mmol)/45 mL, what is the value of [Cl⁻]?

a)

0.0111

b)

0.0011

c)

0.111

d)

0.051

33.

What is the solubility product (Ksp) expression for AgCl?

a)

Ksp = [Ag⁺][Cl⁻]

b)

Ksp = [Ag⁺]/[Cl⁻]

c)

Ksp = [Ag⁺] + [Cl⁻]

d)

Ksp = [Ag⁺] - [Cl⁻]

34.

Calculate the value of s in the equation: 1.8 × 10⁻¹⁰ = s × (0.0111).

a)

s = 1.62 × 10⁻⁸ M

b)

s = 1.62 × 10⁻⁹ M

c)

s = 1.98 × 10⁻⁸ M

d)

s = 1.80 × 10⁻⁷ M

35.

What is the value of pAg calculated from the equation: pAg = - log 1.62 × 10⁻⁸?

a)

7.79

b)

8.79

c)

6.79

d)

9.79

36.

In this calculation, [Cl⁻] contributed by the solubility of AgCl is considered negligible.

a)

True

b)

False

37.

Observations About Argentometric Titrations: High reagent concentrations give ________, more dramatic equivalence point changes in pAg and better endpoints. Fill in the blank.

a)

sharper

b)

slower

c)

duller

d)

weaker

38.

The smaller the Ksp, the more complete the precipitation reaction and the ________ the equivalence region changes.

a)

sharper

b)

slower

c)

broader

d)

weaker

39.

Which of the following factors affect the choice and use of an endpoint indicator?

a)

Only Ksp

b)

Only reagent concentrations

c)

Both Ksp and reagent concentrations

d)

Neither Ksp nor reagent concentrations

40.

Calculate the pCl for the titration of 100.0 mL of 0.1000 M Cl⁻ with 0.1000 M AgNO₃ for the addition of 0.00 mL AgNO₃ solution.

a)

pCl = 1.00

b)

pCl = 2.00

c)

pCl = 0.50

d)

pCl = 0.10

41.

Calculate the pCl for the titration of 100.0 mL of 0.1000 M Cl⁻ with 0.1000 M AgNO₃ for the addition of 20.00 mL AgNO₃ solution.

a)

pCl = 1.00

b)

pCl = 2.00

c)

pCl = 0.50

d)

pCl = 0.70

42.

Calculate the pCl for the titration of 100.0 mL of 0.1000 M Cl⁻ with 0.1000 M AgNO₃ for the addition of 99.00 mL AgNO₃ solution.

a)

pCl = 1.00

b)

pCl = 2.00

c)

pCl = 0.50

d)

pCl = 0.00

43.

Calculate the pCl for the titration of 100.0 mL of 0.1000 M Cl⁻ with 0.1000 M AgNO₃ for the addition of 99.50 mL AgNO₃ solution.

a)

pCl = 1.00

b)

pCl = 2.00

c)

pCl = 0.50

d)

pCl = 1.50

44.

Calculate the pCl for the titration of 100.0 mL of 0.1000 M Cl⁻ with 0.1000 M AgNO₃ for the addition of 100.00 mL AgNO₃ solution.

a)

pCl = -log(0.1000) = 1.00

b)

pCl = -log(0.0500) = 1.30

c)

pCl = -log(0.2000) = 0.70

d)

pCl = -log(0.0100) = 2.00

45.

Calculate the pCl for the titration of 100.0 mL of 0.1000 M Cl⁻ with 0.1000 M AgNO₃ for the addition of 100.50 mL AgNO₃ solution.

a)

pCl = 1.00

b)

pCl = 2.00

c)

pCl = 0.50

d)

pCl = 0.00

46.

Calculate the pCl for the titration of 100.0 mL of 0.1000 M Cl⁻ with 0.1000 M AgNO₃ for the addition of 110.00 mL AgNO₃ solution.

a)

pCl = 1.00

b)

pCl = 2.00

c)

pCl = 0.50

d)

pCl = 3.00

47.

Titrations with Ag+ are called _________?

a)

argentometric titrations

b)

acidimetric titrations

c)

complexometric titrations

d)

alkalimetric titrations

48.

Which of the following is NOT a classical method for end point detection in argentometric titrations?

a)

Mohr Titration

b)

Volhard Titration

c)

Fajan's Titration

d)

Benedict's Test

49.

Name any one classical method used for end point detection in argentometric titrations.

a)

Mohr's method

b)

Volhard's method

c)

Fajans method

d)

Kjeldahl method

50.

Mohr Method is an example of which type of titration?

a)

Direct titration

b)

Back titration

c)

Complexometric titration

d)

Redox titration

51.

In which year was the Mohr Method first published as a method for chloride analysis?

a)

1855

b)

1870

c)

1901

d)

1825

52.

What is the basis of endpoint in the Mohr Method?

a)

Formation of a colored secondary precipitate

b)

Change in pH

c)

Formation of a gas

d)

Change in temperature

53.

Which of the following is used as an indicator in the Mohr Method?

a)

Phenolphthalein

b)

Soluble chromate salt (Na2CrO4, K2CrO4)

c)

Methyl orange

d)

Bromothymol blue

54.

In the precipitation of Cl- by Ag+, what is the color of the Ag2CrO4 precipitate formed when excess Ag+ is present?

a)

White

b)

Reddish

c)

Yellow

d)

Blue

55.

What is the chemical equation for the Mohr indicator reaction (end point) in the Mohr Method?

a)

2Ag++CrO42−→Ag2CrO4(s)2Ag^+ + CrO_4^{2-} \rightarrow Ag_2CrO_4(s)

b)

Ag+ + OH- → AgOH(s)

c)

CrO42−+2H+→H2CrO4CrO4^{2-} + 2H^{+} \rightarrow H2CrO4

d)

H2CrO4↔2H++CrO42−H2CrO4 \leftrightarrow 2H^+ + CrO4^{2-}

56.

Fill in the blank: The Mohr Method has to be performed only in ______ or slightly weak basic medium (pH 7-10).

a)

neutral

b)

acidic

c)

strongly basic

d)

saline

57.

In a pH (acid solution), which compound will be formed according to the Mohr Method? Select the correct option.

a)

Silver hydroxide

b)

Chromic acid

c)

Ag2CrO4

d)

Sodium chloride

58.

Fill in the blank: In a pH (basic solution), ______ will be formed according to the Mohr Method.

a)

silver hydroxide

b)

silver chloride

c)

silver nitrate

d)

potassium chromate

59.

What is the color of the precipitate formed at the end point in the Mohr Method?

a)

White

b)

Reddish

c)

Yellow

d)

Blue

60.

Which reagent is used to precipitate Cl⁻ in the Volhard Method?

a)

KSCN

b)

AgNO₃

c)

FeCl₃

d)

NaCl

61.

What is the color of the precipitate formed when Ag⁺ reacts with Cl⁻?

a)

Red

b)

White

c)

Blue

d)

Yellow

62.

Excess Ag⁺ is titrated with ______ in the presence of Fe³⁺.

a)

KSCN (potassium thiocyanate)

b)

NaCl (sodium chloride)

c)

KBr (potassium bromide)

d)

KI (potassium iodide)

63.

What is the color of the complex ion formed when Ag⁺ has been consumed and Fe³⁺ reacts with SCN⁻?

a)

White

b)

Red

c)

Blue

d)

Green

64.

What is the indicator used in the Volhard Method for back titration of excess Ag+ with SCN-?

a)

Fe2+

b)

Fe3+

c)

Cu2+

d)

Mn2+

65.

What color indicates the endpoint in the Volhard Method titration when excess SCN- reacts with Fe3+?

a)

Blue

b)

White

c)

Red

d)

Green

66.

Volhard Method: The AgCl precipitate is filtered, and the excess Ag+ is titrated with SCN-, producing a _______ precipitate of AgSCN.

a)

white

b)

yellow

c)

red

d)

black

67.

Volhard Method: The titration is usually done in _______ pH medium to prevent precipitation of iron hydroxides, Fe(OH)3.

a)

acidic

b)

neutral

c)

basic

d)

alkaline

68.

The appearance of the red color in the Volhard Method titration indicates the endpoint.

a)

True

b)

False

69.

Volhard Method – Separation of AgCl Precipitate The AgCl precipitate must be separated from the thiocyanate to prevent the reaction: Which compound is less soluble?

a)

AgCl

b)

AgSCN

c)

Both are equally soluble

d)

None of the above

70.

Fill in the blank: The solubility product constant (Ksp) of AgSCN is _______.

a)

1.1 x 10⁻¹²

b)

2.3 x 10⁻⁸

c)

6.6 x 10⁻¹⁰

d)

4.5 x 10⁻⁶

71.

The equilibrium will shift to the right, causing a negative error for the chloride analysis if AgCl is not separated from SCN⁻.

a)

True

b)

False

72.

What is the purpose of adding nitrobenzene before titrating with SCN⁻?

a)

To increase solubility

b)

To form an oily layer and prevent reaction

c)

To filter AgCl

d)

To shift equilibrium to the left

73.

What are adsorption indicators? Adsorption indicators are ______ compounds that tend to be adsorbed onto the surface of the solid precipitate in the titration.

a)

organic

b)

inorganic

c)

metallic

d)

ionic

74.

Adsorption indicators work best when: (a) They do not precipitate out Ag+ when the indicators are at low concentration. (b) They bind to the precipitate only when excess Ag+ is present to produce color. Which of the following is NOT a condition for adsorption indicators to work best?

a)

They do not precipitate out Ag+ at low concentration

b)

They bind to the precipitate only when excess Ag+ is present

c)

They precipitate out Ag+ at high concentration

d)

They produce color only in the absence of Ag+

75.

Give an example of an adsorption indicator mentioned in Fajan's Method.

a)

Fluorescein

b)

Phenolphthalein

c)

Methyl orange

d)

Thymol blue

76.

Fluorescein is a polycyclic compound that ionizes in solution to yield ______ fluoresceinate ions.

a)

yellow-green

b)

blue

c)

red

d)

violet

77.

What color does the surface of a precipitate become when fluoresceinate adsorbs to Ag+ ions and excess Ag+ is present?

a)

reddish-colored

b)

blue-colored

c)

green-colored

d)

yellow-colored

78.

Adsorption indicators bind to the precipitate only when excess Ag+ is present to produce color.

a)

True

b)

False

79.

Only the ionized fluoresceinate produces the _____

a)

blue color

b)

green color

c)

red color

d)

yellow color

80.

In the titration of NaCl with AgNO3, what is the white precipitate formed?

a)

NaCl

b)

AgNO3

c)

AgCl

d)

Cl2

81.

During the titration, _____ are formed.

a)

colloids

b)

precipitates

c)

ions

d)

gases

82.

Before the equivalence point, the surface of the precipitant particles will be _____ charged due to the adsorption of excess Cl- to the surface of the particles.

a)

positively

b)

negatively

c)

neutrally

d)

not

83.

A diffuse positive counter-ion layer will _____ the particles.

a)

repel

b)

surround

c)

dissolve

d)

neutralize

84.

The primary adsorption layer is _____ charged and the anionic indicator is repelled.

a)

positively

b)

negatively

c)

neutrally

d)

not

85.

Which ion is present in the 1° Layer surrounding AgCl?

a)

Na+

b)

Cl-

c)

In-

d)

Ag+

86.

Before the end point in Fajan's Method, which ion is present in excess?

a)

Cl-

b)

Ag+

c)

NO3-

d)

SO42−SO4^2-

87.

When the equivalence point is reached in Fajan's Method, what happens to the surface of the colloidal particles?

a)

The surface of the colloidal particles becomes largely neutral.

b)

The surface of the colloidal particles becomes highly positive.

c)

The surface of the colloidal particles becomes highly negative.

d)

The colloidal particles dissolve completely.

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