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ANACHEM LEC > Stoich And Measurement > Flashcards

Stoich And Measurement Flashcards

1
Q

has only one marking; used in measuring volume precisely.

A

Volumetric flask

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2
Q

Determination of the dimensions, capacity, quantity, or extent of
something

A

Measurement

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3
Q

It is the process of obtaining the magnitude of a quantity relative to an
agreed standard.

A

Measurement

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4
Q

It is composed of a number and a unit and is meaningless without the unit.

A

Measurement

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5
Q

→ a property that is measured
→ Can be derived or fundamental
− Ex. mass, volume, length, time, temperature, pressure

A

Quantity

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6
Q

Fundamental: simplest quantities

A

mass, volume, length, time, temperature, pressure

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7
Q

Quantities (7)

A

Force, velocity, energy, electric current, acceleration, power

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8
Q

A standard quantity against which a quantity is measured

− Ex.kg,L,m,s,K,Pa

A

Unit

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9
Q

Used to describe quantities.

A

Unit

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10
Q

Kg is a unit used to describe ?

A

Mass

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11
Q

L is a unit used to describe

A

volume

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12
Q

m describes

A

Length

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13
Q

S describes

A

Time

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14
Q

describes temperature,

A

K

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15
Q

Unit of pressure

A

Pa

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16
Q

− Units in commerce

− Units: Inch, foot, pound, quart, and gallon

A

English System

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17
Q

− Used in scientific work

− Units: grams, meter, and liter

A

Metric System

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18
Q

Measurement systems should be understandable to everyone hence
the creation of ?

A

SI system

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19
Q

SI means?

A

“Système International d’Unités”

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20
Q

The internationally adopted system which defines or expresses all quantities in terms of seven basic units, the six used by chemists being:

A

SI system

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21
Q

the only unit not commonly used by chemists

A

Candela

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22
Q

basis for 1 second. The old basis of a second was observed from the pendulum.

A

Cesium hyperfine splitting frequency

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23
Q

the basis for luminous intensity.

A

Luminous efficacy of a specified monochromatic source

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24
Q

Kg stands for?

A

Mass

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25
Q

m stands for?

A

Length

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26
Q

S stands for?

A

Second

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27
Q

K stands for?

A

Temperature

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28
Q

Mol stands for?

A

Amount of substance

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29
Q

A stands for?

A

Electric current

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30
Q

fixed value; does not change

A

Constant

31
Q

logical extension of the metric system

A

SI units

32
Q

SI units speed

A

m/s

33
Q

SI unit of density

A

kg/m3

34
Q

are used with these base units and other derived units to express small or large measured quantities in terms of a few simple digits

A

Prefixes

35
Q

1 kg = _____g

A

1000 g

36
Q

1 milligram (mg) =_______g

A

0.001 g

37
Q

What is the multplier of giga

A

10^9

38
Q

What is the multplier of mega

A

10 ^6

39
Q

What is the multplier of kilo

A

10^3

40
Q

What is the multplier of deci

A

10^-1

41
Q

What is the multplier of centi

A

10^-2

42
Q

What is the multplier of milli

A

10^-3

43
Q

results from counting objects or is part of a definition.

A

exact number

44
Q

results from a measurement or observation and contains some uncertainty.

A

inexact number

45
Q

Digits in a measurement that are known with certainty plus one digit that
is estimated.

A

Significant figures

46
Q

Unit of density for solids

A

g/cm3

47
Q

Unit of density in liquid

A

g/mL

48
Q

Unit of density for gases

A

g/L

49
Q

Ratio of the density of a substance to the density of water. It is one of the few unitless quantities in Chemistry.

A

Specific gravity

50
Q

If is the density of the 𝑔/𝑚𝑙 substance the density of water that you will you use is the constant value is

A

1 𝑔 / 𝑚𝑙

51
Q

ρ𝑠𝑢𝑏𝑠𝑡𝑎𝑛𝑐𝑒 formula

A

𝑠𝑝𝑔𝑟𝑥ρ𝐻2O

52
Q

The specific gravity of a substance is equal to its _______, but contains no units

A

Density

53
Q

The specific gravity of a substance is equal to its density, but contains no units

A

MOLES

54
Q

SI unit for the amount of a chemical species

A

Mol

55
Q

Avogadro’s

number

A

(6.022 × 1023)

56
Q

Mass, in grams, of a substance that is numerically equivalent to the formula mass of the substance

A

Molar Mass

57
Q

is 1/1000 of a mole

A

Millimole

58
Q

A homogeneous mixture of two or more substances with each substance retaining its own chemical identity

A

SOLUTIONS

59
Q

cannot identify or distinguish the individual components in a mixture

A

homogeneous

60
Q

solution in which water is the solvent

A

Aqueous solution

61
Q

A solution in which a substance other than water is the solvent

A

→Nonaqueous solution

62
Q

Component of a solution that is usually present in the

greatest amount

A

Solvent

63
Q

Component of a solution that is usually present in a lesser amount relative to that of the solvent

A

Solutr

64
Q

A solution that contains a large amount of solute relative to the amount that could be dissolved

A

Concentrated solution:

65
Q

A solution that contains a small amount of solute relative to the amount that could be dissolved

A

Dilute solution:

66
Q

The process in which more solvent is added to a solution in order to lower its concentration

A

Dilution

67
Q

How would you prepare 100 mL of 0.9% saline solution in water from a 10% saline solution?

A

9 mL of 10% saline solution + 91 mL of water

68
Q

The amount of solute present in a specified amount of solution

A

PERCENT CONCENTRATION

69
Q

What is the percent by mass concentration of glucose in a solution made by dissolving 5.5 g of glucose in 78.2 g of water?

A

6.6% (m/m)

70
Q

Calculate the volume percent of solute in 30.0 mL of methyl alcohol in enough water to give 435 mL of solution.

A

6.90% (v/v)

71
Q

How many grams of sodium chloride are needed to prepare 150 mL of 0.9% (m/v) sodium chloride?

A

1.35 g of NaCl

72
Q

Moles of solute in a solution divided by the liters of solution

A

Molarity

73
Q

Calculate the molarity of a solution made from 20.0 g of NaOH in 250 mL of solution. ( ) moles of solute Molarity M = liters of solution

A

2.00 M

74
Q

The most common measure of concentration in the laboratory is?

A

Molarity

ANACHEM LEC (4 decks)

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