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Clinical Chemistry Lecture > Preparation of Solutions and Dilutions > Flashcards

Preparation of Solutions and Dilutions Flashcards

1
Q

Two Major Systems in the Unit of Measurement:

A

English System
Metric System

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2
Q

Measurements of analytes in a biochemistry laboratory may either use the _____ or _____

A

Conventional Unit
Syteme Internationale

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3
Q

What is the Metric System Unit of Measurement and the English System Unit of Measurement of:

Length

A

Metric System: Meter
English System: Inch, Foot, Mile

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4
Q

What is the Metric System Unit of Measurement and the English System Unit of Measurement of:

Mass

A

Metric System: Gram
English System: Ounce, Pound, Ton

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5
Q

What is the Metric System Unit of Measurement and the English System Unit of Measurement of:

Volume

A

Metric System: Liter
English System: Pint, Quart, Gallon

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6
Q

What is the Metric System Unit of Measurement and the English System Unit of Measurement of:

Power

A

Metric System: Watt
English System: Horsepower

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7
Q

What is the Metric System Unit of Measurement and the English System Unit of Measurement of:

Torque

A

Metric System: Newton-meter
English System: Pound-foot

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8
Q

What is the Metric System Unit of Measurement and the English System Unit of Measurement of:

Temperature

A

Metric System: Degree Celsius
English System: Degree Fahrenheit

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9
Q

Components of a Laboratory Result:

A

Actual Value
Unit

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10
Q

It is recommended that analytes be reported using _____

A

Moles per solute per volume of solution (substance concentration)

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11
Q

Reporting laboratory results is often expressed in terms of _____ or _____

A

Substance concentration
Mass of a substance

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12
Q

International d’Unités is also known as the _____ in French or the _____

A

Systeme International
SI Unit

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13
Q

The SI Unit is based on the _____

A

Metric System

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14
Q

The SI Unit consists of how many independent base units?

A

7 independent base units

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15
Q

What are the 7 independent base units?

A

Time
Length
Mass
Electric Current
Thermodynamic Temperature
Amount of Substance
Luminous Intensity

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16
Q

Typical Symbol of:

Time

A

t

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17
Q

Typical Symbol of:

Length

A

l, x, r, etc.

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18
Q

Typical Symbol of:

Mass

A

m

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19
Q

Typical Symbol of:

Electric Current

A

l, i

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20
Q

Typical Symbol of:

Thermodynamic Temperature

A

T

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21
Q

Typical Symbol of:

Amount of Substance

A

n

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22
Q

Typical Symbol of:

Luminous Intensity

A

lv

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23
Q

Identify the Symbol of:

Second

A

s

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24
Q

Identify the Symbol of:

Meter

A

m

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25
Q

Identify the Symbol of:

Kilogram

A

kg

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26
Q

Identify the Symbol of:

Ampere

A

A

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27
Q

Identify the Symbol of:

Kelvin

A

K

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28
Q

Identify the Symbol of:

Mole

A

mol

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29
Q

Identify the Symbol of:

Candela

A

cd

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30
Q

Matter is divided into _____ and _____

A

Pure Substances
Mixtures

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31
Q

Pure Substances is divided into _____ and _____

A

Elements
Compounds

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32
Q

Mixtures is divided into _____ and _____

A

Homogenous
Heterogenous

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33
Q

The amount of solute in a solution can be measured as a _____

A

Percentage of the total volume of the solution

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34
Q

Percent Solutions is expressed as _____

A

Equal parts per hundred or the amount of solute per 100 total units of solution

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35
Q

There are how many expressions under Percent Solution:

A

3 Expressions

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36
Q

What are the 3 Expressions of Percent Solution:

A

Percent by Mass
Percent by Volume
Mass-volume Percent

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37
Q

This is the mass of solute in a solution divided by the total mass of solution, multiplied by 100.

A

Percent by Mass

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38
Q

Formula of Percent by Mass:

A

(Mass of solute/Mass of Solution) x 100

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39
Q

This is the volume of solute in a solution divided by the total volume of solution, multiplied by 100.

A

Percent by Volume

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40
Q

Formula of Percent by Volume:

A

(Volume of Solute/Volume of Solution) x 100

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41
Q

This is the mass of solute in a solution (in grams) divided by the total volume of solution (in milliliters), multiplied by 100.

A

Mass-volume Percent

42
Q

Formula for Mass-volume Percent:

A

(Mass of Solute in Grams/Volume of Solution in Milliliters) x 100

43
Q

_____ is two or more substances with each substance retaining its own chemical identity.

A

Homogenous Mixture

44
Q

Components of Solution:

A

Solute
Solvent

45
Q

The component of a solution that is present in the greatest amount.

46
Q

The component of a solution that is present in a lesser amount.

47
Q

Practice Question:

What is the percent-by-mass concentration of sucrose in a solution made by dissolving
7.5g of sucrose in 86.5g of water?

A

Formula Used: Percent by Mass
Final Answer: 7.98% Sucrose Solution

48
Q

Refers to the weight or volume of the solute present in a specified amount of solvent or a
solution.

A

Concentration of Solutions

49
Q

Basic Types of Solutions:

A

Percent Solutions
Molar Solutions
Molal Solutions
Normal Solutions

50
Q

Practice Question:

What is the percent-by-volume concentration if a 2mL of concentrated HCl is diluted with 80mL distilled water?

A

Formula Used: Percent by Volume
Final Answer: 2.44% HCl Solution

51
Q

Practice Question:

What is the concentration of a 200 mL solution containing 1.8g of NaCl?

A

Formula Used: Mass-volume Percent
Final Answer: 0.9% NaCl Solution and 0.9g/ml NaCl Solution

52
Q

Practice Question:

10% bleach (sodium hypochlorite) is used to disinfect benches before and after work. It denatures protein in micro-organisms and is therefore effective in killing bacteria, fungus and viruses. How much bleach is needed to make 100mL of 10% bleach (sodium hypochlorite) solution? How much distilled water is needed to dilute the bleach?

A

Formula Used: Percent by Volume
Final Answer: 10ml Bleach (Sodium hypochlorite)

53
Q

Practice Question:

10% bleach (sodium hypochlorite) is used to disinfect benches before and after work. It denatures protein in micro-organisms and is therefore effective in killing bacteria, fungus and viruses. How much bleach is needed to make 100mL of 10% bleach (sodium hypochlorite) solution? How much distilled water is needed to dilute the bleach?

A

Final Answer: 90ml dH2O

54
Q

Practice Question:

Normal saline solution (NSS) is used to dissolve drugs for IV use which is 0.9%w/v NaCl in water. How many grams of NaCl is needed to prepare a 35mL NSS?

A

Formula Used: Mass-volume Percent
Final Answer: 0.32g NaCl

55
Q

This is a solution containing one gram molecular weight (one mole of the solute in one liter solution) of the substance per liter of the solution.

A

Molar Solution

56
Q

What are the Formula for Molar Solutions?

A

Formula 1: mol of Solute/L of Solution
Formula 2: g of Solute/MW x L of Solution

57
Q

Practice Question:

Determine the molarity of a solution containing 4.35 moles of KMnO4 dissolved in
enough water to give 750 mL solution.

A

Formula Used: Molar Solutions = mol of Solute/L of Solution
Final Answer: 5.8M KMnO4

58
Q

Practice Question:

Determine the molarity of a solution containing 20g NaOH dissolved in enough water to give 1.50L solution.
(Na-23; O-16, H-1)

A

Formula Used: Molar Solutions = g of Solute/MW x L of Solution
Final Answer: 0.33M NaOH Solution

59
Q

This is the solution containing one gram molecular weight (one mole of the solute in one kilogram of solution) of the substance per kilogram of the solution.

A

Molal Solutions

60
Q

What are the Formulas used for Molal Solutions?

A

Formula 1: mol of Solute/Kg of Solution
Formula 2: g of Solute/MW x Kg of Solution

61
Q

Practice Question:

How many grams of FeSO4 is needed to prepare 0.30 L of 0.10M FeSO4 solution?
(Fe-55.85; S-32.06; O-14)

A

Formula Used: Molarity Solution = g of Solute/MW x L of Solution
Final Answer: 4.56g FeSo4

62
Q

This is the least likely to be encountered of the four concentration expressions to be encountered in the clinical laboratories, but is often used in chemical titrations and chemical reagent classification.

A

Normal Solutions

63
Q

What is the Formula for Normal Solution?

A

Formula: g of Solute/Equivalent Weight x L of Solution

64
Q

What is the Formula to get the Equivalent Weight?

A

Equivalent Weight = Molecular Weight x Valence

65
Q

In identifying the Valence of Acids, we count the _____

A

Number of Hydrogen Ions

66
Q

In identifying the Valence of Bases, we count the _____

A

Number of Hydroxide Ions

67
Q

In identifying the Valence of Salts, we _____

A

Multiply the Absolute Value of Ions

68
Q

Normality is _____ Molarity of that compound.

A

Always equal or Greater than

69
Q

Practice Question:

What is the molarity of a 2N NaCl solution?

A

Formula Used: Molarity = Normality/Valence
Final Answer: 2M of NaCl Solution

70
Q

Practice Question:

What is the normality of a 5M H2SO4 solution?

A

Formula Used: Normality = Molarity x Valence
Final Answer: 10N H2SO4 Solution

71
Q

Practice Question:

Determine the normality of a solution containing 15g KCl dissolved in enough water to give 0.20L solution.
(K-39.10; Cl-35.45)

A

Formula Used; Normality of Solution = g of Solute/EW x L of Solution
Final Answer: 1.01N KCl Solution

72
Q

Represents the ratio of concentrated or stock material to the total final volume of a solution and consists of the volume or weight of the concentrate plus the volume of the diluent, with the concentration units remaining the same.

73
Q

Whenever the solution is diluted, the volume is _____ and its concentration is _____ but the total amount of solute _____.

A

Increased
Decreased
Remain Unchanged

74
Q

What is the Formula for Dilutions?

A

C1V1 = C2V2

75
Q

Practice Question:

What is the initial volume of a 40% formaldehyde diluted to prepare 100mL of 10% formaldehyde solution?

A

Formula Used: Dilutions = C1V1 = C2V2
Final Answer: 25mL

76
Q

Practice Question:

What is the final concentration of a 50mL 90% methanol diluted to prepare a 200mL methanol solution?

A

Formula Used: Dilutions = C1V1 = C2V2
Final Answer: 22.5% Methanol Solution

77
Q

Formula in Converting Celsius to Fahrenheit:

A

F = 1.8C + 32

78
Q

Formula in Converting Fahrenheit to Celsius:

A

C = (F-32) x 5/9

79
Q

Identify the Value of the Analyte:

Albumin

A

10 mmol/l CF

80
Q

Identify the Value of the Analyte:

Ammonia

A

0.587 mmol/l CF

81
Q

Identify the Value of the Analyte:

Bicarbonate

A

1 mmol/l CF

82
Q

Identify the Value of the Analyte:

Bilirubin

A

17.1 mmol/l CF

83
Q

Identify the Value of the Analyte:

BUN

A

0.357 mmol/l CF

84
Q

Identify the Value of the Analyte:

Calcium

A

0.25 mmol/l CF

85
Q

Identify the Value of the Analyte:

Chloride

A

1 mmol/l CF

86
Q

Identify the Value of the Analyte:

Cholesterol

A

0.026 mmol/l CF

87
Q

Identify the Value of the Analyte:

Creatinine

A

88.4 mmol/l CF

88
Q

Identify the Value of the Analyte:

Glucose

A

0.0555 mmol/l CF

89
Q

Identify the Value of the Analyte:

Iron

A

0.179 mmol/l CF

90
Q

Identify the Value of the Analyte:

Lithium

A

1 mmol/l CF

91
Q

Identify the Value of the Analyte:

Magnesium

A

0.5 mmol/l CF

92
Q

Identify the Value of the Analyte:

Phospholipid

A

0.01 mmol/l CF

93
Q

Identify the Value of the Analyte:

Phosphorus

A

0.323 mmol/l CF

94
Q

Identify the Value of the Analyte:

Potassium

A

1 mmol/l CF

95
Q

Identify the Value of the Analyte:

Sodium

A

1 mmol/l CF

96
Q

Identify the Value of the Analyte:

Thyroxine

A

12.9 mmol/l CF

97
Q

Identify the Value of the Analyte:

Total Protein

A

10 mmol/l CF

98
Q

Identify the Value of the Analyte:

Triglyceride

A

0.0113 mmol/l CF

99
Q

Identify the Value of the Analyte:

Uric Acid

A

0/0595 mmol/l CF

100
Q

Identify the Value of the Analyte:

Pc02

A

0.133 mmol/l CF

101
Q

Identify the Value of the Analyte:

p02

A

0.133 mmol/l CF

Clinical Chemistry Lecture (3 decks)

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