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Ceutics - Exam 1 - Preformulation Part 2 - Yang

Total questions: 107

Worksheet time: 1hrs 2mins

Name
Class
Date
1.

What are the different factors of preformulation

a)

solid state properties

b)

solubility

c)

hydroscopicity

d)

lipophilicity

2.

What is solubility

a)

concentration of solute in a saturated solution at certain temperature

b)

concentration of solute in an unsaturated solution at certain temperature

c)

concentration of solute in a saturated solution at varying temperatures

d)

opposites attract

e)

like dissolves like

3.

What are correct descriptions of solubility designations in USP

a)

the higher the solubility range, the more soluble it is

b)

the higher the solubility range, the less soluble it is

c)

the lower the solubility range, the more soluble it is

d)

the lower the solubility range, the less soluble it is

4.

How to you convert micrograms to milligrams

a)

1 mcg x 1000 = 1 mg

b)

1 mg x 1000 = 1 mcg

c)

1 mcg x 100 = 1 mg

d)

1 mg x 100 = 1 mcg

e)

1 mcg x 10,000 = 1 mg

5.

If the aqueous solution has a solubility of < 100 mcg/mL, what does that indicate

a)

soluble

b)

insoluble

c)

practically insoluble

6.

What equation is this

a)

Drug Solubility in Ideal Solution

b)

Temperature and Solubility

c)

Stoke's-Einstein Equation

d)

Solubility Prediction

e)

Solubility and Particle Size

7.

What is X2

a)

Mole Fraction Solubility

b)

Heat of Fusion

c)

Gas Constant

d)

Melting Point

e)

Temperature of Measurement

8.

What is Hf

a)

Mole Fraction Solubility

b)

Heat of Fusion

c)

Gas Constant

d)

Melting Point

e)

Temperature of Measurement

9.

What is R

a)

Mole Fraction Solubility

b)

Heat of Fusion

c)

Gas Constant

d)

Melting Point

e)

Temperature of Measurement

10.

What is T

a)

Mole Fraction Solubility

b)

Heat of Fusion

c)

Gas Constant

d)

Melting Point

e)

Temperature of Measurement

11.

What is T0

a)

Mole Fraction Solubility

b)

Heat of Fusion

c)

Gas Constant

d)

Melting Point

e)

Temperature of Measurement

12.

What are the possible gas constants you can use for R

a)

1.987 cal/mol

b)

8.314 J/mol*K

c)

8.314 x 107 erg/mol*K

d)

8.314 x 107 dyn/cm

e)

0.0821 L*atm/mol*K

13.

What is the heat of fusion

a)

4540 cal/mol

b)

353.2 K

c)

293 K

d)

1.987 cal/mol

14.

What is the temperature of measurement

a)

4540 cal/mol

b)

353.2 K

c)

293 K

d)

1.987 cal/mol

15.

What is the melting point

a)

4540 cal/mol

b)

353.2 K

c)

293 K

d)

1.987 cal/mol

16.

What is the gas constant

a)

4540 cal/mol

b)

353.2 K

c)

293 K

d)

1.987 cal/mol

17.

What equation is this

a)

Drug Solubility in Ideal Solution

b)

Temperature and Solubility

c)

Stoke's-Einstein Equation

d)

Solubility Prediction

e)

Solubility and Particle Size

18.

Which solute-solvent interactions involves compounds without a permanent dipole

a)

Van der Waals Forces

b)

Hydrogen Bonds

c)

Electrostatic Force

d)

Alpha-linkages

19.

Which solute-solvent interactions results in permanent, positively charged dipole of a hydrogen atom (functional groups can be H-bond donors or acceptors)

a)

Van der Waals Forces

b)

Hydrogen Bonds

c)

Electrostatic Force

d)

Alpha-linkages

20.

Which solute-solvent interactions occurs between two ions from induced dipoles (attractive force can be calculated)

a)

Van der Waals Forces

b)

Hydrogen Bonds

c)

Electrostatic Force

d)

Alpha-linkages

21.

What equation is this

a)

Drug Solubility in Ideal Solution

b)

Temperature and Solubility

c)

Stoke's-Einstein Equation

d)

Attractive force of electrostatic interactions

e)

Solubility and Particle Size

22.

What are the different types of Solute-Solvent Interactions

a)

Van der Waals Forces

b)

Hydrogen Bonds

c)

Electrostatic Force

d)

Alpha linkages

23.

What are the different classifications of solvents

a)

Polar

b)

Semipolar

c)

Nonpolar

d)

Covalent

e)

Hydrogen bonds

24.

What is a polar solvent and what is an example of a polar solvent

a)

exhibit strong dipolar bonds and hydrogen bond properties

b)

water

c)

exhibit strong dipolar bonds but not strong hydrogen properties

d)

glycerin, propylene glycol, ethanol, acetone

e)

chloroform, ethyl ester, benzene, carbon tetrachloride

25.

What is a semipolar solvent and what is an example of a semipolar solvent

a)

exhibit strong dipolar bonds and hydrogen bond properties

b)

water

c)

exhibit strong dipolar bonds but not strong hydrogen properties

d)

glycerin, propylene glycol, ethanol, acetone

e)

chloroform, ethyl ester, benzene, carbon tetrachloride

26.

What is a nonpolar solvent and what is an example of a nonpolar solvent

a)

exhibit low to little dipolar character and immiscible with water

b)

water

c)

exhibit strong dipolar bonds but not strong hydrogen properties

d)

glycerin, propylene glycol, ethanol, acetone

e)

chloroform, ethyl ester, benzene, carbon tetrachloride

27.

Which solvents are semipolar

a)

glycerin, propylene glycol

b)

water

c)

ethanol, acetone

d)

benzene, carbon tetrachloride

e)

chloroform, ethyl ether

28.

Which solvents are nonpolar

a)

glycerin, propylene glycol

b)

water

c)

ethanol, acetone

d)

benzene, carbon tetrachloride

e)

chloroform, ethyl ether

29.

What are some solubility enhancements that can be made during preformulation

a)

chemical modification; reduce the particle size

b)

addition of co-solvent

c)

pH adjustment; advanced formulation

d)

addition of complexing agent

e)

addition of surfactant

30.

What are examples of co-solvents

a)

water, alcohol

b)

caffeine, EDTA

c)

glycerin

d)

cyclodextrin

e)

span

31.

What are examples of complexing agents

a)

Tween

b)

caffeine, EDTA

c)

SLS

d)

cyclodextrin

e)

span

32.

What are examples of surfactants

a)

tween

b)

caffeine, EDTA

c)

SLS

d)

cyclodextrin

e)

span

33.

What equation is this

a)

Drug Solubility in Ideal Solution

b)

Temperature and Solubility

c)

Stoke's-Einstein Equation

d)

Solubility Prediction

e)

Solubility and Particle Size

34.

What does S represent

a)

solubility of particles

b)

solubility of solid

c)

surface tension

d)

radius of particles

e)

molar volume

35.

What does S0 represent

a)

solubility of particles

b)

solubility of solid

c)

surface tension

d)

radius of particles

e)

molar volume

36.

What does lowercase gamma represent

a)

solubility of particles

b)

solubility of solid

c)

surface tension

d)

radius of particles

e)

molar volume

37.

What does V represent

a)

solubility of particles

b)

solubility of solid

c)

surface tension

d)

radius of particles

e)

molar volume

38.

What does r represent

a)

solubility of particles

b)

solubility of solid

c)

absolute temperature

d)

radius of particles

e)

gas constant

39.

What does R represent

a)

solubility of particles

b)

solubility of solid

c)

absolute temperature

d)

radius of particles

e)

gas constant

40.

What does T represent

a)

solubility of particles

b)

solubility of solid

c)

absolute temperature

d)

radius of particles

e)

gas constant

41.

What are the possible gas constants you can use for R

a)

1.987 cal/mol

b)

8.314 J/mol*K

c)

8.314 x 107 erg/mol*K

d)

8.314 x 107 dyn/cm

e)

0.0821 L*atm/mol*K

42.

What is the log (S/S0)

a)

log(1.10)

b)

log(100)

c)

log(1)

d)

log(50)

e)

log(0.90)

43.

What is lowercase gamma

a)

100 dynes/cm

b)

1.10

c)

50 cm3

d)

300 K

e)

8.314*107 dynes/cm

44.

What is V

a)

100 dynes/cm

b)

1.10

c)

50 cm3

d)

300 K

e)

8.314*107 dynes/cm

45.

What is T

a)

100 dynes/cm

b)

1.10

c)

50 cm3

d)

300 K

e)

8.314*107 dynes/cm

46.

What is the best R to use

a)

100 dynes/cm

b)

8.314 J/mol*K

c)

0.0821 L*atm/mol*K

d)

8.314*107 erg/K*mol

e)

8.314*107 dynes/cm

47.

The solubility of ____ can be affected by pH

a)

weak electrolytes

b)

weak acid

c)

weak base

48.

What relationship does this equation establish

a)

Drug Solubility in Ideal Solution

b)

Temperature and Solubility

c)

Stoke's-Einstein Equation

d)

Solubility Prediction

e)

Solubility and pH

49.

What is St

a)

Total Solubility

b)

Starting Solubility

c)

Acid Dissociation Constant

d)

Acid Concentration

e)

Molecular Weight

50.

What is S0

a)

Total Solubility

b)

Starting Solubility

c)

Acid Dissociation Constant

d)

Acid Concentration

e)

Molecular Weight

51.

What is Ka

a)

Total Solubility

b)

Starting Solubility

c)

Acid Dissociation Constant

d)

Acid Concentration

e)

Molecular Weight

52.

What is [H+]

a)

Total Solubility

b)

Starting Solubility

c)

Acid Dissociation Constant

d)

Acid Concentration

e)

Molecular Weight

53.

What are characteristics of a cosolvent system

a)

used when a drug is not completely soluble in water

b)

must be biocompatible and miscible in each other

c)

the mole fraction of the cosolvent system affects the dielectric constant of the mixture

d)

used when a drug is not soluble in water

54.

What equation is this

a)

Drug Solubility in Ideal Solution

b)

Temperature and Solubility

c)

Stoke's-Einstein Equation

d)

Solubility Prediction

e)

Mole fraction

55.

What relationship does this equation establish

a)

Drug Solubility in Ideal Solution

b)

Temperature and Solubility

c)

Stoke's-Einstein Equation

d)

Solubility Prediction

e)

Solubility and pH

56.

What is X2

a)

Mole Fraction Solubility

b)

Heat of Fusion

c)

Gas Constant

d)

Melting Point

e)

Temperature of Measurement

57.

What is Delta Hf

a)

Mole Fraction Solubility

b)

Heat of Fusion

c)

Gas Constant

d)

Melting Point

e)

Temperature of Measurement

58.

What is R

a)

Mole Fraction Solubility

b)

Heat of Fusion

c)

Gas Constant

d)

Melting Point

e)

Temperature of Measurement

59.

What is T

a)

Mole Fraction Solubility

b)

Heat of Fusion

c)

Gas Constant

d)

Starting Temperature

e)

Temperature of Measurement

60.

What is T0

a)

Mole Fraction Solubility

b)

Heat of Fusion

c)

Gas Constant

d)

Starting Temperature

e)

Temperature of Measurement

61.

What type of process is dissolution typically and what is the exception

a)

endothermic

b)

exothermic

c)

Ca(OH)2

d)

Ce2(SO4)3

62.

What can you use to initially investigate solubility if resources were limited

a)

water

b)

saline

c)

0.1M HCl

d)

0.1M NaOH

e)

propylene glycol

63.

What can you use to initially investigate solubility if resources were sufficient

a)

PEG 400

b)

oils

c)

0.1M HCl

d)

surfactant systems

e)

propylene glycol

64.

Hygroscopy is the ability of a substance to

a)

attract and hold water molecules from the surrounding environment

b)

repel and push away water molecules from the surrounding environment

c)

attract and use water molecules from the surrounding environment

65.

What is hygroscopicity

a)

the degree which a substance is hygroscopic

b)

the degree which a substance is hydroscopic

66.

Hygroscopicity refers to how moisture affects

a)

flow

b)

compaction

c)

dissolution

d)

stability

e)

storage/packaging

67.

What are ways in which a hygroscopic compound can retain water

a)

bulk or surface adsorption

b)

capillary condensation

c)

chemical reaction

d)

deliquescence

e)

efflorescence

68.

What is deliquescence

a)

a solid dissolves and saturates a thin film of water on its surface

b)

moisture is absorbed to the extent that deliquescence takes place, the liquid film surrounding the solid is saturated

c)

process dictated by vapor diffusion and heat transport rates

d)

a crystal loses water of crystallization below a critical water vapor pressure

69.

What is efflorescence

a)

a solid dissolves and saturates a thin film of water on its surface

b)

moisture is absorbed to the extent that deliquescence takes place, the liquid film surrounding the solid is saturated

c)

process dictated by vapor diffusion and heat transport rates

d)

a crystal loses water of crystallization below a critical water vapor pressure

e)

the opposite of deliquescence

70.

What equation is this

a)

Drug Solubility in Ideal Solution

b)

Temperature and Solubility

c)

Relative Humidity

d)

Solubility Prediction

e)

Mole fraction

71.

What is relative humidity normally expressed as

a)

a percentage

b)

a decimal

c)

a fraction

d)

a temperature

72.

What does phi represent

a)

relative humidity

b)

water vapor

c)

equilibrium vapor pressure of water

d)

temperature

e)

pressure

73.

What does ew represent

a)

relative humidity

b)

water vapor

c)

equilibrium vapor pressure of water

d)

temperature

e)

pressure

74.

What does ew* represent

a)

relative humidity

b)

water vapor

c)

equilibrium vapor pressure of water

d)

temperature

e)

pressure

75.

RH (phi) depends on the ___ and ____ of the system of interest

a)

relative humidity

b)

water vapor

c)

equilibrium vapor pressure of water

d)

temperature

e)

pressure

76.

Vapor pressure or equilibrium vapor pressure is defined as the pressure exerted by a vapor in thermodynamic equilibrium with its (1) at a (2) in a (3)

a)

1 - condensed phases; 2 - given temperature; 3 - closed system

b)

1 - condensed phases; 2 - any temperature; 3 - closed system

c)

1 - condensed phases; 2 - given temperature; 3 - open system

d)

1 - condensed phases; 2 - any temperature; 3 - open system

77.

Which equation is displayed and what does it relate to

a)

Antoine equation

b)

August equation

c)

Vapor Pressure

d)

Relative Humidity

78.

Which equation is displayed and what does it relate to

a)

Antoine equation

b)

August equation

c)

Vapor Pressure

d)

Relative Humidity

79.

What are the hygroscopicity classifications

a)

non-hygroscopic

b)

slightly hygroscopic

c)

moderately hygroscopic

d)

very hygroscopic

80.

What is a class 1: non-hygroscopic classification

a)

essentially no moisture increase occur at relative humidities below 90%

b)

essentially no moisture increase occur at relative humidities below 80%

c)

moisture content does not increase more than 5% after storage for 1 week at relative humidities below 60%

d)

moisture content increase may occur at relative humidities as low as 40-50%

81.

What is a class 2: slightly hygroscopic classification

a)

essentially no moisture increase occur at relative humidities below 90%

b)

essentially no moisture increase occur at relative humidities below 80%

c)

moisture content does not increase more than 5% after storage for 1 week at relative humidities below 60%

d)

moisture content increase may occur at relative humidities as low as 40-50%

82.

What is a class 3: moderately hygroscopic classification

a)

essentially no moisture increase occur at relative humidities below 90%

b)

essentially no moisture increase occur at relative humidities below 80%

c)

moisture content does not increase more than 5% after storage for 1 week at relative humidities below 60%

d)

moisture content increase may occur at relative humidities as low as 40-50%

83.

What is a class 4: very hygroscopic classification

a)

essentially no moisture increase occur at relative humidities below 90%

b)

essentially no moisture increase occur at relative humidities below 80%

c)

moisture content does not increase more than 5% after storage for 1 week at relative humidities below 60%

d)

moisture content increase may occur at relative humidities as low as 40-50%

84.

In lipophilicity, what is the partition coefficient

a)

ratio of the concentration of the compound in the two phases of a mixture of two immiscible solvents at equilibrium

b)

ratio of the concentration of the compound in the two phases of a mixture of two immiscible solvents not at equilibrium

c)

ratio of the concentration of the compound in the two phases of a mixture of two miscible solvents at equilibrium

d)

ratio of the concentration of the compound in the two phases of a mixture of two miscible solvents not at equilibrium

85.

What does this equation represent

a)

octanol-water partition coefficient

b)

immiscible solvent coefficient

c)

hygroscopicity

d)

octanol-water hygroscopicity

86.

If the logP is = 0

a)

the mixture is in equal amounts

b)

the mixture is more lipid soluble

c)

the mixture is more water soluble

87.

If the logP is > 0

a)

the mixture is in equal amounts

b)

the mixture is more lipid soluble

c)

the mixture is more water soluble

88.

If the logP is < 0

a)

the mixture is in equal amounts

b)

the mixture is more lipid soluble

c)

the mixture is more water soluble

89.

What partition coefficient substituents increase P

a)

-alkyl

b)

-aryl

c)

-OH, -COOH

d)

-O, -CO

e)

-NH2

90.

What partition coefficient substituents decrease P

a)

-alkyl

b)

-aryl

c)

-OH, -COOH

d)

-O, -CO

e)

-NH2

91.

To increase lipophilicity,

a)

most programs use a group additivity approach

b)

some programs use more complicated algorithms

c)

most use clogP

d)

most programs use a group reductive approach

e)

some programs use more basic algorithms

92.

What is apparent partition coefficient (Papp)

a)

the effective lipophilicity of a compound at a given pH

b)

a function of both the lipophilicity of the unionized compound and the degree of ionization

c)

the ineffective lipophilicity of a compound at a given pH

d)

a function of both the lipophilicity of the ionized compound and the degree of ionization

93.

What equation is this

a)

Apparent Partition Coefficient for Weak Acids

b)

Apparent Partition Coefficient for Weak Bases

c)

Apparent Partition Coefficient

d)

Effective Lipophilicity

94.

What equation is this

a)

Apparent Partition Coefficient for Weak Acids

b)

Apparent Partition Coefficient for Weak Bases

c)

Apparent Partition Coefficient

d)

Effective Lipophilicity

95.

What is this equation for

a)

weak acids

b)

weak bases

c)

strong acids

d)

strong bases

96.

What is the slope

a)

1/Papp

b)

1/P

c)

Ka/P

d)

1/[H+]

97.

What is the y-intercept

a)

1/Papp

b)

1/P

c)

Ka/P

d)

1/[H+]

98.

What is the y-axis

a)

1/Papp

b)

1/P

c)

Ka/P

d)

1/[H+]

99.

What is the x-axis

a)

1/Papp

b)

1/P

c)

Ka/P

d)

1/[H+]

100.

What is this equation for

a)

weak acids

b)

weak bases

c)

strong acids

d)

strong bases

101.

What is the x-axis

a)

1/Papp

b)

1/P

c)

1/Ka*P

d)

[H+]

102.

What is the y-axis

a)

1/Papp

b)

1/P

c)

1/Ka*P

d)

[H+]

103.

What is the y-intercept

a)

1/Papp

b)

1/P

c)

1/Ka*P

d)

[H+]

104.

What is the slope

a)

1/Papp

b)

1/P

c)

1/Ka*P

d)

[H+]

105.

What are the applications of log P when using it to predict the solubility of a drug

a)

drugs with high logP values have low aq solubility

b)

drugs with low logP values have high aq solubility

c)

drugs with high logP values have high aq solubility

d)

drugs with low logP values have low aq solubility

106.

What are the applications of log P when using it to predict the drug absorption

a)

drugs with high logP values are easily bound to protein, have low aq solubility, and bind to extraneous sites

b)

drugs with low logP values may be too hydrophilic to have any affinity for the membranes and may be poorly absorbed

c)

drugs with low logP values are easily bound to protein, have low aq solubility, and bind to extraneous sites

d)

drugs with high logP values may be too hydrophilic to have any affinity for the membranes and may be poorly absorbed

107.

LogP helps to discover the preservation of oral liquid pharmaceutical dosage forms because

a)

the preservatives take effects under their unionized forms

b)

in emulsion, the unionized preservative is lipid soluble whereas microbes grow in aq phases where the ionic form of the preservatives likes to accumulate

c)

the preservatives take effects under their ionized forms

d)

in emulsion, the ionized preservative is lipid soluble whereas microbes grow in aq phases where the ionic form of the preservatives likes to accumulate

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