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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
weak acids classification
all other species that produce Hydronium ions in solution
26
strong bases classification and trick
Group 1 and two cations with hydroxide ions 1 and 2 are the strongest numbers because they’re first
27
weak bases classification and trick
All other species that produces hydroxide ions in solution e and a in weak is like a and o in all other
28
Neutral species
``` Group 1 and two cations NO3- Br- I- Cl- CIO4- BrO4- Be O3- IO4 4- IO3- ```
29
Strong acid empirical properties
high conductivity very low ph fast reaction rate
30
strong acids modified arrhenius theory
completely react with water to form hydronium ions >99%
31
weak acids empirical properties
low conductivity med to low ph slow reaction rate
32
weak acids modified arrhenius theory
partially react with water to form hydronium ions
33
strong bases empirical properties
high conductivity very high ph fast reaction rate
34
strong bases modified arrhenius theory
completely react with water to form hydroxide ions 100 >99%
35
weak bases empirical properties
low conductivity (molecular) med to high ph slow reaction rate
36
weak bases modified Arrhenius theory
partially react with water to form hydroxide ions
37
weak acids food and drink examples
lactic acid in dairy carbonic acid in drinks
38
Neutralization reactions and example
reaction between hydronium and hydroxide ions to produce water HCL+NaOH——>NaCl+H2O H3O+OH——>2H2O
39
Amphiprotic
can donate or accept H+ can write equations for both Na...
40
steps for explaining basic/acidic properties
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
two ways acids and bases can be defined
empirically and theoretically
42
Empirical definition of acid
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
Empirical definition of base
asubstance which dissolved in water to produce a solution that ``` tastes bitter feels slippery turns red litmus blue conducts electricity neutralizes acids ```
44
acid arrhenius theoretical definition and example
a substance that forms an acidic solution by dissolving in water to produce free hydrogen ions (H+) in solution
45
base arrhenius theortical definition and example
A substance that forms a basic solution by dissolving in water to produce free hydroxide ions (OH-) in solution
46
Acid modified theoretical definition and example
Hey species that forms in acidic solution by reacting with water to produce hydronium ion‘s HCl+H2O—>H3O+Cl
47
Base modified theoretical definition
A species that forms a basic solution by reacting with water to produce hydroxide ions
48
what did scientists think about a hydrogen ion
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
Paul Giguère provided ____
empirical evidence | discovered hydrated protons commonly called hydronium ions (H3O+)
50
modern view of acids and bases is that the hydronium ions
(H3O+) are responsible for acidic properties and hydroxide ions (OH-) are responsible for basic properties
51
Dilution definition
Decreasing the concentration of a solution
52
How is dilution accomplished
adding more solvent
53
do the number of moles of solute change when a solution is diluted
no, number of moles before equals number of moles after
54
Why is dilution important
in manipulating the concentration of solutions for better control of reactions
55
Problem with concentrated solution reactions
could be too violent to be safe and too fast to observe
56
Stock solution definition
initial starting solution from which samples are taken for a dilution, usually very high concentration
57
Dilution formula
C1 V1=C2 V2
58
Dilution formula is used for
Determining the volume of stock solution for a standard solution
59
what stays the same and what changes when diluting a solution
Number of moles stays the same, concentration and volume change
60
Volumetric techniques
Standard solution used chemical analysis to precisely control chemical reactions precision equipment is required to measure mass of solute and volume of solution
61
Standard solution definition
Solutions with precisely known concentration, a solution of accurate concentration
62
Volumetric flask
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
Graduated cylinder
Glass cylinder with regular markings used to measure a fairly precise volume of liquid or solution
64
Erlenmeyer flask
Glass cone shaped flask with a large flat bottom used to mix a solution sample during titration markings only approximate volume
65
Beaker
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
Why is there no way of knowing how much solute is present in a solution by looking at it
most solutions are colourless and aqueous
67
what is concentration Comparing
Comparing the quantity of solute to the quantity of solution
68
Concentration formula
concentration=quantity of solute/quantity of solvent
69
Dilute definition
A relatively small quantity of solute per volume of solution
70
Concentrated definition
A relatively large quantity of solute per volume of solution
71
Different ways to express concentration
percent concentration parts per million (ppm) amount concentration/more concentration (mol/L)
72
Percent concentration formulas and concentration
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
Parts per million formula and units
mass of solute (g) times 10 to the sixth/ mass of solution (g)
74
Like dissolves like
factor of solubility polar substances tend to dissolve in polar solvents Nonpolar substances tend to dissolve in nonvolatile solvents
75
intermolecular attractions
Factor affecting solubility The stronger the intermolecular attractions between solute and solvent the more likely the solute will dissolve
76
Temperature
Factor affecting solubility solubility of a solid solid and liquid solving increase with increasing temperature
77
solubility of liquids and solids does not change with
pressure
78
increasing pressure above the solution ____
forces more gas to dissolve
79
solubility of a gas in a liquid is ____
directly proportional to its pressure
80
Degrees of saturation
Saturated solution, unsaturated solution, supersaturated solution
81
Saturated solution
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
Unsaturated solution
less than the maximum amount of solute is dissolved in a solvent No solid remains in flask
83
Super saturated solution
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
dissociation is a ______ change
physical change, can get back the original solute by evaporate in the solvent
85
Reaction
Cannot get back to the original solute, substance didn’t dissolve it reacted
86
Process to determine the energy change
1) separation of solute particles 2) separation of a solvent particles to make holes 3) formation of new interactions between solute and solvent
87
Endothermic energy change
have to break bonds
88
exothermic energy change
have to make bonds
89
Hydronium ion concentration goes with
PH
90
Hydroxide ion concentration goes with
POH
91
percentages for polyprotics
First one: less than 50 percent <50% Every one after: less than 1 percent <1%
92
How can ph changes be deceptive and example
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
how does hydronium ion concentration change when ph decreases and example
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
concentration formula
concentration=moles/volume
95
mole formula
moles=mass/molar mass
96
different ways to express concentration
parts per million (ppm) percent concentration amount concentration
97
percentage for strong acid and strong base
>99%
98
percentage for weak acid and weak base
>5%
99
what is volume measured in for calculations
litres

Chem 20 (5 decks)

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