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Chem 20 > solutions > Flashcards

solutions Flashcards

1
Q

two primary uses of acid base indicators

A

mark end of titration

Estimate pH of a solution by using a different number of indicators, replace more expensive pH metre

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2
Q

What are acid base indicators

A

substances that change colour when The acidity of the solution changes

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3
Q

What is litmus

A

common indicator obtained from lichen, prepared by soaking absorbent paper with witness solution then drying

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4
Q

Why are acid-base indicators unique chemicals

A

can exist in two forms each with a distinctly different color, form of colour depends on acidity of a solution

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5
Q

Two forms of any indicator depend on

A

Whether a particular hydrogen atom is present in indicator molecule

HIn

In

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6
Q

given 2 pHs and volume one find volume two

A

show hydronium or hydroxide ions formed,

find to hydronium/hydroxide concentrations with formulas,

use dilution formula to solve

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7
Q

given concentration and two volumes, find PH

A

show hydronium or hydroxide ions formed

and determine ratio, calculate new concentration different ratio than 1 to 1,

use pH formula to solve

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8
Q

Give into volume and concentration, find concentration of diluted

A

Show hydroxide or hydromium formed,

determine ratio and calculate concentration is greater than 1 to 1,

identify that concentration of diluted equals C2,

use dilution formula to solve

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9
Q

Given two volumes and concentration, find pH of diluted solution

A

Find concentration of diluted solution,

use pH formula

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10
Q

what has an Inverse square relationship

A

exists between ion concentration and pH or POH

Greater hydronium ion concentration equals lower pH,

greater hydroxide ion concentration equals lower POH

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11
Q

Sig dig rules for hydro/hydrox ion concentrations and ph/poh

A

only use for POH and hydroxide and hydronium ion calculations

number of digits after the decimal in PH equals number of sig digs in ion concentrations

number of sig digs in ion concentration equals number of digits after the decimal in ph

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12
Q

what was hydronium ion concentration improved to and why

A

improved to pH formula, because we need pH measurements to one or more decimal places

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13
Q

monoprotic base and example

A

react with water wants to produce hydroxide ions

CH3COO-(aq)

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14
Q

polyprotic base and example

A

can react more than once with water but reactions are much less than 50%

week whose reactions with water decrease with each successive step

CO3 2-(aq)

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15
Q

Polyprotic base indicator

A

negative charge higher than one

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16
Q

non-polyprotic base and example

A

no possibility of successions with water

Ba(OH)2

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17
Q

What does pure water do

A

Self ionizes, contains hydroxide and hydronium ion’s

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18
Q

conductivity test of pure water

A

Concentrations are so low conductivity test would be negative

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19
Q

adding acid to water ads _____ which causes_____which makes the solution

A

Hydronium ion‘s, causing hydronium ion concentration to increase, makes solution conductive

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20
Q

adding base to water ads _____ which causes_____which makes the solution

A

hydroxide ions, causing hydroxide ion concentration to increase, makes solution conductive

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21
Q

exception to polyprotic acid being weak whose reaction with water decreases every time

A

H2SO4

strong acid because it’s first reaction with water is essentially complete, second reaction much less than 50% complete

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22
Q

polyprotic acid and example

A

weak whose Reaction with water decreases with each successive step

have more than one acidic hydrogen

H3PO4

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23
Q

Monoprotic acids

A

have only one acidic hydrogen atom in their compound formula

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24
Q

Strong acids classification and trick

A 
HCL  
HBr
HI
HCIO4
H2SO4 
HNO3
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25
Q

weak acids classification

A

all other species that produce Hydronium ions in solution

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26
Q

strong bases classification and trick

A

Group 1 and two cations with hydroxide ions

1 and 2 are the strongest numbers because they’re first

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27
Q

weak bases classification and trick

A

All other species that produces hydroxide ions in solution

e and a in weak is like a and o in all other

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28
Q

Neutral species

A 
Group 1 and two cations
NO3-
Br-
I-
Cl-
CIO4- 
BrO4-
Be O3- 
IO4 4- 
IO3-
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29
Q

Strong acid empirical properties

A

high conductivity
very low ph
fast reaction rate

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30
Q

strong acids modified arrhenius theory

A

completely react with water to form hydronium ions

> 99%

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31
Q

weak acids empirical properties

A

low conductivity
med to low ph
slow reaction rate

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32
Q

weak acids modified arrhenius theory

A

partially react with water to form hydronium ions

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33
Q

strong bases empirical properties

A

high conductivity
very high ph
fast reaction rate

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34
Q

strong bases modified arrhenius theory

A

completely react with water to form hydroxide ions

100
>99%

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35
Q

weak bases empirical properties

A

low conductivity (molecular)
med to high ph
slow reaction rate

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36
Q

weak bases modified Arrhenius theory

A

partially react with water to form hydroxide ions

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37
Q

weak acids food and drink examples

A

lactic acid in dairy

carbonic acid in drinks

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38
Q

Neutralization reactions and example

A

reaction between hydronium and hydroxide ions to produce water

HCL+NaOH——>NaCl+H2O

H3O+OH——>2H2O

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39
Q

Amphiprotic

A

can donate or accept H+

can write equations for both

Na…

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40
Q

steps for explaining basic/acidic properties

A

write dissociation (base) or ionization (acid) make sure it’s balanced

If haven’t already shown hydronium or hydroxide ions formed, add water (don’t include element in second equation if doesn’t have H or O)

41
Q

two ways acids and bases can be defined

A

empirically and theoretically

42
Q

Empirical definition of acid

A

a substance which dissolves in water to produce a solution that

tastes sour 
turns blue litmus red 
conducts electricity 
reacts with active metals to produce H2(g) 
neutralizes bases
43
Q

Empirical definition of base

A

asubstance which dissolved in water to produce a solution that

tastes bitter 
feels slippery 
turns red litmus blue 
conducts electricity 
neutralizes acids
44
Q

acid arrhenius theoretical definition and example

A

a substance that forms an acidic solution by dissolving in water to produce free hydrogen ions (H+) in solution

45
Q

base arrhenius theortical definition and example

A

A substance that forms a basic solution by dissolving in water to produce free hydroxide ions (OH-) in solution

46
Q

Acid modified theoretical definition and example

A

Hey species that forms in acidic solution by reacting with water to produce hydronium ion‘s

HCl+H2O—>H3O+Cl

47
Q

Base modified theoretical definition

A

A species that forms a basic solution by reacting with water to produce hydroxide ions

48
Q

what did scientists think about a hydrogen ion

A

but it wasn’t likely that a hydrogen ions could exist on its own in an aqueous solution,

thought it would bond strongly to polar water molecules

49
Q

Paul Giguère provided ____

A

empirical evidence

discovered hydrated protons commonly called hydronium ions (H3O+)

50
Q

modern view of acids and bases is that the hydronium ions

A

(H3O+) are responsible for acidic properties and hydroxide ions

(OH-) are responsible for basic properties

51
Q

Dilution definition

A

Decreasing the concentration of a solution

52
Q

How is dilution accomplished

A

adding more solvent

53
Q

do the number of moles of solute change when a solution is diluted

A

no, number of moles before equals number of moles after

54
Q

Why is dilution important

A

in manipulating the concentration of solutions for better control of reactions

55
Q

Problem with concentrated solution reactions

A

could be too violent to be safe and too fast to observe

56
Q

Stock solution definition

A

initial starting solution from which samples are taken for a dilution, usually very high concentration

57
Q

Dilution formula

A

C1 V1=C2 V2

58
Q

Dilution formula is used for

A

Determining the volume of stock solution for a standard solution

59
Q

what stays the same and what changes when diluting a solution

A

Number of moles stays the same, concentration and volume change

60
Q

Volumetric techniques

A

Standard solution

used chemical analysis to precisely control chemical reactions

precision equipment is required to measure mass of solute and volume of solution

61
Q

Standard solution definition

A

Solutions with precisely known concentration, a solution of accurate concentration

62
Q

Volumetric flask

A

Glass flask with a long narrow neck

used to prepare a highly precise volume of solution

precise to +0.16 ml at 20°C

63
Q

Graduated cylinder

A

Glass cylinder with regular markings

used to measure a fairly precise volume of liquid or solution

64
Q

Erlenmeyer flask

A

Glass cone shaped flask with a large flat bottom

used to mix a solution sample during titration

markings only approximate volume

65
Q

Beaker

A

Glass wide body cylinder with regular markings

used for transferring and storing solutions or solids and contain reactions

markings are only approximate volume precise to only +5 ml

66
Q

Why is there no way of knowing how much solute is present in a solution by looking at it

A

most solutions are colourless and aqueous

67
Q

what is concentration Comparing

A

Comparing the quantity of solute to the quantity of solution

68
Q

Concentration formula

A

concentration=quantity of solute/quantity of solvent

69
Q

Dilute definition

A

A relatively small quantity of solute per volume of solution

70
Q

Concentrated definition

A

A relatively large quantity of solute per volume of solution

71
Q

Different ways to express concentration

A

percent concentration

parts per million (ppm)

amount concentration/more concentration (mol/L)

72
Q

Percent concentration formulas and concentration

A

volume of solute (ml)/volume of solution (ml) times 100

mass of solute (g)/volume of
solution (ml) times 100

mass of solute (g)/mass of solution (g) times 100

73
Q

Parts per million formula and units

A

mass of solute (g) times 10 to the sixth/ mass of solution (g)

74
Q

Like dissolves like

A

factor of solubility

polar substances tend to dissolve in polar solvents

Nonpolar substances tend to dissolve in nonvolatile solvents

75
Q

intermolecular attractions

A

Factor affecting solubility

The stronger the intermolecular attractions between solute and solvent the more likely the solute will dissolve

76
Q

Temperature

A

Factor affecting solubility

solubility of a solid solid and liquid solving increase with increasing temperature

77
Q

solubility of liquids and solids does not change with

A

pressure

78
Q

increasing pressure above the solution ____

A

forces more gas to dissolve

79
Q

solubility of a gas in a liquid is ____

A

directly proportional to its pressure

80
Q

Degrees of saturation

A

Saturated solution, unsaturated solution, supersaturated solution

81
Q

Saturated solution

A

solvent holds as much salt as is possible at that temperature

unresolved solid remains in flask

dissolved solute is in dynamic equilibrium with solid solute particles

82
Q

Unsaturated solution

A

less than the maximum amount of solute is dissolved in a solvent

No solid remains in flask

83
Q

Super saturated solution

A

solvent holds more slowly than normally possible at that temperature

solution is unstable:
crystallization can often be stimulated by adding a seed crystal or scratching the side of the flask

84
Q

dissociation is a ______ change

A

physical change, can get back the original solute by evaporate in the solvent

85
Q

Reaction

A

Cannot get back to the original solute, substance didn’t dissolve it reacted

86
Q

Process to determine the energy change

A

1) separation of solute particles
2) separation of a solvent particles to make holes
3) formation of new interactions between solute and solvent

87
Q

Endothermic energy change

A

have to break bonds

88
Q

exothermic energy change

A

have to make bonds

89
Q

Hydronium ion concentration goes with

A

PH

90
Q

Hydroxide ion concentration goes with

A

POH

91
Q

percentages for polyprotics

A

First one: less than 50 percent
<50%

Every one after: less than 1 percent
<1%

92
Q

How can ph changes be deceptive and example

A

adding vinegar to pure water might change the ph from 7 to 4

even though the ph only changed 3 units, the hydronium ion concentration increased by 10 to the third

93
Q

how does hydronium ion concentration change when ph decreases and example

A

difference in ph change=exponent of hydronium ion concentration change

ex) change from 6 to 2 in ph is 10 to the fourth in hydronium ion concentration

94
Q

concentration formula

A

concentration=moles/volume

95
Q

mole formula

A

moles=mass/molar mass

96
Q

different ways to express concentration

A

parts per million (ppm)
percent concentration
amount concentration

97
Q

percentage for strong acid and strong base

A

> 99%

98
Q

percentage for weak acid and weak base

A

> 5%

99
Q

what is volume measured in for calculations

A

litres

Chem 20 (5 decks)

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