10C- calculating pH Flashcards

1
Q

Define
acidic solution

A

Solution containing a greater concentration of hydronium ions than hydroxide ions

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2
Q

Define
basic solution

A

Solution containing a greater concentration of hydroxide ions than hydronium ions

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3
Q

Define
neutral solution

A

Solution containing an equal concentration of hydronium and hydroxide ions

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4
Q

Define
autoionization

A

Process by which an atom or molecule spontaneously forms ions

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5
Q

Define
ionic product of water (Kw)

A

Expression of the concentration of ions present in water at 25 °C

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6
Q

Define
pH

A

Measure of the concentration of hydronium ions in a solution

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7
Q

Define
pH scale

A

pH values arranged on a logarithmic scale

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8
Q

Ionic(n.) product
definition

A

-Ionic product(n.)=The product of
concentrations of ionic species

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9
Q

Ionisation(v.)
definition

A

-Ionisation(v.)=Conversion of substance into
ions.

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10
Q

Acidity definition

A

-Acidity(adj.)=level of acid in a substance

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11
Q

what happens when water is ionised

A

H2O(l) + H2O(l) H3O+(aq) + OH−(aq)
water acts as a weak acid and weak base

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12
Q

list some monoprotic acids

A

hydrochloric acid (HCl), ammonium (NH4), nitric acid (HNO3), ethanoic acid (CH3COOH)
HANE (hydrochloric acid, ammonium, nitric acid, ethanoic acid)

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13
Q

define monoprotic

A

species that can only donate one proton, H+, during ionisation

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14
Q

list some diprotic acids

A

sulfuric acid (H2SO4), carbonic acid (H2CO3), hydrogen sulfide (H2S), selenous acid (H2SeO3)
SCHS ( sulfuric acid, carbonic acid, hydrogen sulfide, selenous acid)

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15
Q

define diprotic

A

species that can donate up to two protons, H+, during ionisation

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16
Q

list some triprotic acids

A

phosphoric acid (H3PO4), citric acid (C6H8O7), arsenic acid (H3AsO4), boric acid (H3BO3)
PCAB

17
Q

define triprotic

A

species that can donate up to three protons, H+, during ionisation

18
Q

list some amphiprotic acids

A

water (H2O), hydrogen sulfate ( HSO4(-)),hydrogen carbonate (HCO3(-)), di hydrogen phosphate (H2PO4(-)), hydrogen phosphate ( HPO4(2-))

19
Q

define amphiprotic

A

species that can either donate or accept a proton, H+

20
Q

define pH

A

measure of the concentration of hydronium ions in a solution

21
Q

kW formula (aka ionic product formula)

A

Kw = [H3O+] × [OH−]
Kw = (1.00 × 10−7 M) × (1.00 × 10−7 M)
Kw = 1.00 × 10^−14 M2

22
Q

pH formula

A

pH = −log10[H3O+]

23
Q

what is kW

A

the ionic product of water: expression of the concentration of ions present in water at 25°C

Kw is always equal to 1.00 ⨉ 10-14 M^2 at 25°C

This formula only valid at 25 degrees Celsius

24
Q

If neutral pH is still defined as when [H3O+] = [OH–], what would be considered neutral pH at 100°C, assumingKwis equal to 51.3 × 10–14M2?

A

H3O x OH = 51.3 x 10^-14
H3O=OH
H3O x H3O = 51.3 x 10^-14
H3O= √51.3 x 10^-14
H3O= 7.162 x 10^-7
pH= -log 10 (7.16 x 10^-7)
pH=6.14

25
Q

Acid solutions ratio of H3O+ and OH- concentration

A

pH 7 < [H3O+] >1.0 × 10−7 M and [OH−] < 1.0 × 10−7M

26
Q

Neutral solutions ratio of H3O+ and OH- concentration

A

pH = 7, [H3O+] = [OH−] = 1.0 × 10−7 M

27
Q

basic solutions ratio of H3O+ and OH- concentration

A

pH 7 >[H3O+] <1.0 × 10−7 M and [OH−] >1.0 × 10−7M

28
Q

how to calculate pH

A

pH = −log10[H3O+]

29
Q

how to calculate H3O concentration

A

[H3O+] = 10^−pH

30
Q

what factor is pH change

A

every increase or decrease in pH by 1 means that there was a change in the concentration of H3O by a factor of 10

31
Q

Calculate the pH of a 0.30 M solution of hydrochloric acid at 25 .

A

[HCl] = [H3O+] = 0.30 M
pH = −log10[H3O+]
pH = −log10 (0.30 M)
pH = 0.52

32
Q

Explain the
autoionisation of water.

A

-Pure water
undergoes a tiny degree of ionisation with itself
-This is possible
due to water’s amphiprotic nature

H2O(l){acid}
+ H2O(l){Base}⇌ H3O^(+)(aq) + OH^(-)

-There will be
very low concentrations of product as only a small amount of this reaction
will occur due to the strenght of the acid and base being low.

33
Q

What does pH stand
for(not necessary but fun)

A

What
does pH stand for?=Potenz of hydrogen=power of hydrogen=
-p=power=originates
from the german word potenz
-H=hydrogen

34
Q

What is the pH
scales and what does it do

A

-measurement of
acidity= simplified further using measurement of pH
-pH scale=
measurement of acidity of a solution on a scale of 0-14(this only valid at 25 degrees Celsius )