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Quantitative Analysis > Quant Exam 1 > Flashcards

Quant Exam 1 Flashcards

1
Q

identification of what chemical constituents are present in a substance; identity of a compound

A

qualitative analysis

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2
Q

measurement of how much of a chemical substance is present; numerical answers

A

quantitative analysis

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3
Q

step one of chemical analysis

A

formulating the question - translating general questions into specific questions

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4
Q

step two of chemical analysis

A

selecting analytical procedures - doing a literature search

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5
Q

step three of chemical analysis

A

sampling - selecting representative materials to be measured

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6
Q

sample/material composition is the same everywhere

A

homogeneous

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7
Q

sample/material composition differs from region to region

A

heterogeneous

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8
Q

step four of chemical analysis

A

sample preparation - converting the sample into a suitable form

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9
Q

step five of chemical analysis

A

analysis - repeating measurements, applying different analytical methods

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10
Q

step six of chemical analysis

A

reporting and interpreting

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11
Q

step seven of chemical analysis

A

drawing conclusions

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12
Q

substance being measured or detected; also called “measured”

A

analyte

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13
Q

a solution whose composition is known by virtue of the way it was made from a reagent of known purity or by virtue of its reaction with a known quantity of a standard reagent

A

standard solution

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14
Q

liquid remaining above the solid after precipitation

A

supernatant - also called “supernate”

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15
Q

a portion of a substance

A

aliquot

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16
Q

a solution of anything in water

A

aqueous

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17
Q

a suspension of a solid in a solvent

A

slurry

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18
Q

to pour liquid off a solid or, perhaps, a denser liquid; the denser phase is left behind

A

decant

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19
Q

a complete transfer

A

quantitative transfer

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20
Q

a homogenous mixture of two or more substances

A

solution

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21
Q

the minor species in a solution

A

solute

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22
Q

the major species in a solution

A

solvent

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23
Q

formula for molarity (M)

A

moles solute / liters solution

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24
Q

formula for molality (m)

A

moles solute / kilograms solvent

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25
Q

formula for weight percent (% wt)

A

(grams solute / grams solution) x 100

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26
Q

formula for parts per million (ppm)

A

milligrams solute / liters solution

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27
Q

chemical analysis based on weighing the final product

A

gravimetric analysis

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28
Q

Avogadro’s Number

A

6.022 x 10^23

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29
Q

formula for dilution

A

M1V1 = M2V2

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30
Q

how close together a set of measurements are; reproducibility

A

precision

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31
Q

how close a measurement is to the true/accepted value; nearness to the truth

A

accuracy

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32
Q

True or False: In addition/subtraction, the number of significant figures is determined by the number with the fewest decimal places.

A

T

33
Q

True or False: In multiplication/division, the number of significant figures is determined by the factor with the smallest number of digits.

A

T

34
Q

True or False: In logarithms, the number of significant figures determines the number of decimal places.

A

T

35
Q

True or False: In antilogs, the number of decimal places determines the number of significant figures.

A

T

36
Q

a built-in error, consistent, reproducible; in principle, detectable and correctable

A

systematic error

37
Q

from uncontrollable variables in the measurement; inconsistent error value; can be reduced by repeated trials, but cannot be completely eliminated

A

random error

38
Q

expresses the margin of uncertainty associated with a measurement

A

absolute uncertainty

39
Q

compares the sizes of the absolute uncertainty with the size of its associated measurements

A

relative uncertainty

40
Q

formula for relative uncertainty

A

absolute uncertainty / magnitude of measurement

41
Q

formula for percent relative uncertainty

A

(absolute uncertainty / magnitude of measurement) x 100

42
Q

True or False: The number of significant figures in the answer is limited by the number of decimal places in the uncertainty.

A

T

43
Q

True or False: Random error can be expressed as the standard deviation/standard deviation of the mean/confidence interval.

A

T

44
Q

True or False: Random errors in arithmetic processes propagate through calculations.

A

T

45
Q

analyze known samples/certified reference materials, analyze blank samples, use different analytical methods to measure the same quantity, round-robin experiments

A

ways to detect systematic error

46
Q

formula for relative standard deviation/coefficient of variation

A

(standard deviation / mean) x 100

47
Q

the absolute value of the highest value minus the lowest value

A

range

48
Q

True or False: When given an even number of data points, the median is the average of the two middle values.

A

T

49
Q

True or False: When finding the confidence interval, the degree of freedom is the number of samples minus one.

A

T

50
Q

EXCEL command for finding the mean

A

= AVERAGE ( : )

51
Q

EXCEL command for finding the standard deviation

A

= STDEV ( : )

52
Q

EXCEL command for finding the number of samples

A

= COUNT ( : )

53
Q

replicate measurements of a sample made by a single analytical technique are compared to an accepted value

A

case one

54
Q

comparing replicate measurements of a sample measured by two analytical techniques or samples created from two methods measured by one analytical technique

A

case two

55
Q

multiple samples are measured by two different analytical techniques and the results are compared

A

case three

56
Q

True or False: For case one, if the known value does not lie within the 95% confidence interval range, then the methods give different results.

A

T

57
Q

calculated F value < table F value

A

the difference in standard deviations is not significant; use the s pooled formula to find t

58
Q

calculated F value > table F value

A

the difference in standard deviations is significant; use the regular t formula

59
Q

calculated t value < table t value

A

not significantly different mean values

60
Q

calculated t value > table t value

A

significantly different mean values

61
Q

calculated G value > table G value

A

questionable value can be discarded

62
Q

calculated G value < table G value

A

questionable value cannot be discarded

63
Q

True or False: When constructing a standard/calibration curve, the blank value should be subtracted from the measured values.

A

T - called corrected values

64
Q

True or False: Concentrations of pure solids/liquids/solvents are omitted from the equilibrium constant formula because they are unity.

A

T

65
Q

reverse reaction equilibrium constant calculation

A

K’ = 1 / K

66
Q

added equilibrium constant calculation

A

K3 = K1 x K2

67
Q

if a system is subjected to a change/disturbance, the direction in which the system proceeds back to equilibrium will attempt to offset the change

A

Le Chatelier’s Principle

68
Q

Q < K (Le Chatelier’s)

A

the system will shift to the right until Q = K

69
Q

Q > K (Le Chatelier’s)

A

the system will shift to the left until Q = K

70
Q

True or False: Heat is a reactant in an endothermic reaction. (H > 0)

A

T

71
Q

True or False: Heat is a product in an exothermic reaction. (H < 0)

A

T

72
Q

(+) G, K < 1

A

disfavored reaction

73
Q

(-) G, K > 1

A

favored reaction

74
Q

the equilibrium constant for the reaction in which a solid salt dissolves to give its constituent ions in solution

A

solubility product

75
Q

Q > Ksp (precipitation)

A

a precipitate will be formed

76
Q

Q < Ksp (precipitation)

A

a precipitate will not be formed

77
Q

a salt is less soluble if one of its ions is already present in the solution

A

common ion effect

78
Q

True or False: A smaller Ksp value means a more soluble salt.

A

T

Quantitative Analysis (3 decks)

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