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ch7 acid base Flashcards

1
Q

Fill in the blanks.

More acid means more ___ ions.
More alkaline means more ___ ions

A

More acid means H+ ions
More alkali means OH- ions

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2
Q

Define strength of acid.

A
  1. ability, acid, release hydrogen ion (acidity)
  2. weaker acid, release less H+ ion
  3. yet releases same vol., H2 gas
  4. hence rate of reaction decreases

(less H+ ion released, therefore less no. collision, therefore less freq of effective collision)

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3
Q

name of salt produced if reacted with…

  1. sulfuric acid
  2. nitric acid
  3. hydrochloric acid
  4. phosphoric acid
  5. ethanoic acid
A
  1. sulfate
  2. nitrate
  3. chloride
  4. phosphate
  5. ethanoate (CH₃COO)₂
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4
Q

4 eqn.

(acid + ___)

A

alkali + ammonium salt -> ammonia + salt + water
acid + alkali/base -> salt + water
acid + reactive metal -> salt + hydrogen
acid + carbonate -> salt + carbon dioxide + water

ammonium only found in salts

ALKALIIIIIII!!!!!!

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5
Q

3 unreactive metals

A
  • gold
  • silver
  • copper

just happens to correspond to 3 tiers of medals

however, silver, copper oxide exists while gold oxide dosent

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6
Q

which keywords signalises a base/akali?

A
  • (all metal except gold) oxide
  • (all metal except gold) hydroxide

definition of base is still:
oxide formed w/ reactive metal, reacts w/ acid to form salt, water

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7
Q

what is —> in chemical eqn? What does it show?

A
  • strong acid/alkali
  • complete ionisation
  • irreversible reaction

vol of gas same
rate of reaction faster

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8
Q

what is
⇌

in chemical eqn? what does it show?

A
  • weak acid/alkali
  • partial ionisation
  • reversible reaction

vol of gas same
rate of reaction slower

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9
Q

in which solution can acid ionise, and in which solution can acid not ionise?

A

Ionise in water
Does not ionise in anything else, including alcohol

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10
Q

If I have 10,000 HCL molecules and add water into it, how many H+ and Cl- ions there are?

A

10,000 H+ ions
10,000 Cl- ions

strong acid -> complete ionisation

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11
Q

ethanoic, nitric acid formulas

A

ethanoic: CH3COOH
nitric: HNO3

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12
Q

acids properties (6 pointers)

A
  • sour taste
  • conduct electricity in (aq) state
  • turns blue litmus paper red
  • turns Universal Indicator from green towards red
  • corrosive when conc.
  • pH 1-6
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13
Q

define acids

A
  • substances that produce H+ ions when dissolved in water
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14
Q

1 Can acids/akali be solid?
2 Can acids/alkali be covalent compounds?

A

1 no.

2 yes!! Just need water
Example: Hydrogen chloride dissolves to become hydrochloric acid

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15
Q

1 Does Lead react with dilute HCl and H2So4?

2 Does Lead react with dilute nitric acid? HNo3?

A

1 Partially
2 Yes.

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16
Q

Why dosen’t lead react/not react with dilute HCl and H2SO4?

A

LINK
It partially reacts.

REASON
- insoluble layer forms, prevents further reaction

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17
Q

What is sulfuric acid used for? (2 uses)

A
  • fertilisers, car batteries
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18
Q

What is ethanoic acid used for? (1 uses)

A
  • manufacture vinegar
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19
Q

List 3 Strong and 1 Weak acid

A

Strong
Hcl, H2So4, HNo3

weak
- all organic acids
- e.g. CH3COOH

What does organic mean in Chem?
Anything with Carbon in the formula

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20
Q

What does organic mean in Chem?

A

Anything with Carbon in the formula

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21
Q

what is hydrochloric acid used for? (1 use)

A

remove rust -> clean metal surfaces

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22
Q

Volume of gas released affected by ___ of acid?

A

Basicity of acid.

Find out basicity by writing balanced eqn.

Strength of acid based on reversible/non reversible, and will only affect no. of H+ ions released, NOT vol of h2 released

23
Q

Define alkali

A
  • Substance that produce OH- ions when dissolve in water
  • Base soluble in water
24
Q

alkalis to memorise

A
  • aqueous ammonia nh3 (aq)

NH4 OH is rejected!! will penalise if write that. Use nh3 (aq) for aqueous ammonia

25
5 Properties of alkali
- bitter taste - feel slippery - conduct electricity in (aq) state - turn universal indicator towards violet - pH 8-14 - turns red litmus paper blue
26
Are alkalis corrosive?
- Yes, for Conc. forms of strong alkalis
27
2 irl Uses of alkali
- toothpaste - antacid
28
in neutral solution, what is the concentration of H+ ions and OH- ions?
Conc. of H+ ions = Conc. of OH- ions ## Footnote Common misconception: There are no ions -> THIS IS NOT TRUE!! **ACTUALLY, THERE ARE EQUAL CONC. OF H+ and OH- IONS**
29
# pH<7 means...?** when pH<7, what can be concluded about conc. of H+ and OH- ions? **Fill in the blanks** The ___ the pH value, the ___ the conc. of H+ ions
conc. of H+ ions > conc. of OH- ions **Fill in the blanks** higher, lower *or* lower, higher
30
What does pH actually measure?
- conc. of H+, OH- ions
31
when pH>7, what can be concluded about conc. of H+ and OH- ions?
H+ ions < OH- ions ## Footnote alt. answer: OH- ions > H+ ions
32
conc. vs strength
**conc:** amt of dissolved substance - can be changed - dilute/conc. - affect rate of reaction - if its limiting will affect vol. of gas release **strength:** ease of dissociation of acid molecules - fixed in every acid - strong/weak - will **NOT** affect vol of gas release no such thing as "very strong" | olvl syllablus only "strong" or "weak"
33
which one reacts more? X reacts readily to Y Z reacts vigorously to Y
Z reacts more. Vigorously > Readily in terms of reaction
34
Write the eqn. for ionisation of HOCL (Hypochlorous acid) given that it is a weak acid
HOCL ⇌ H+ + OCl- **Must add charges. This is ionisation**
35
# magnesium is a **metal** weak acid vs strong acid **with same amount of H+ ions released upon dissolving in water** reaction w/ magnesium differences, similarities
difference: - weak acid releases lower conc., H+ ions similarity: - weak acid releases **same vol of gas as strong acid (only if same amt of H+)**
36
Which keywords signalises an alkali?
**LINK**: Alkali is base that is soluble in water ammo**nium**/(grp1) oxide/hydroxide
37
ammonium vs ammonia full list of differences
**nium** - only found in salt - all states **nia** - base - gas/(aq) state - default state: gas - NH3 ## Footnote **LINK** - all bases can dissociate in water and will give out OH- (hydroxide ions)
38
I have weak acid X. What can I conclude about it?
- reactions, reversible - undergo partial ionisation when dissolve -> water ## Footnote **Not all weak acids have Carbon inside of them, but all acids that are organic (have Carbon) are weak acids**
39
How to identify Acidic oxides
All non-metal oxides - So2, So3, SiO2 e.g. **except for** - NO, CO, H2O ## Footnote no cold water NO CO H2O
40
Define oxide?
compound formed from oxygen w/ other element/compounds ## Footnote Any chemical formula containing **oxygen** (can be o, O2, O3...)
41
How to identify Neutraic Oxides
NO CO H2O ## Footnote No Cold Water **Does not apply to other higher subscript oxide formulas** i.e. CO is neutraic but Co2, Co3 isnt i.e. NO is neutraic, but No2 isnt. *unrelated: N2 is neutral (**btw n2 isn't an oxide, no oxygen in formula**)
42
Acidic oxides 1 chem 2 phys property
- React w/ alkali to form salt, water - usually **GAS** at r.t.p. - soluble, water ## Footnote acts like any other acid, can jst react with any other alkali.
43
Neutraic oxide properties
- does **NOT** react w acid/alkali
44
ALL ___ oxides are basic oxide?
*all* **metal** oxides are basic - e.g. Na2O, MgO, Fe2O3... except Zn Al Pb ## Footnote ZAP
45
Properties of basic oxides 2 phys properties 1 chem property
- Usually solid in r.t.p. - **insouble** in water **except** (Grp1) oxides - react w/ acids, form salt+ water ## Footnote **Ammonium oxide does not exsist.** **MISCONCEPTION** Base needs to dissolve to react. Nope! It just dosen't show alkali properties. Still will react.
46
Amphoteric Oxides
Zn Al Pb ## Footnote ZAP
47
Properties of Amphoteric Oxides
- insoluble in water - show both basic acidic properties ## Footnote Zn Al Pb (ZAP)
48
Acid XH₂ complete ionisation __ basic acid.
XH₂ -> X2- + 2H+ ## Footnote dibasic 2H+
49
does base need to dissolve to react with acid
**MISCONCEPTION** Base needs to be (aq) to react **ACTUAL** Nope! Insol. base dosen't show alkali properties. Still will react. **WHERE IS THIS USED IN?** i.e. excess solid reactant method aq. acid + **insoluble** base **HOWEVER** acid needs to be (aq). Acid **CANNOT** be solid.
50
nitric acid or HCl **Stronger** acid?
Nitric acid
51
define base
metal oxides, react w/ acids -> salt + Water
52
ammonia (aq) + acid reaction whats atypical, and why?
1. acid + Nh3 (aq) -> ammonium salt 2. no water, Nh3(aq) no hydroxide group
53
pH scale indicator for what
pH scale: measure relative acidity/alkalinity indicator: mixture substaces, shows diff colours, diff pH

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