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Chemistry > Things you need to Memorise > Flashcards

Things you need to Memorise Flashcards

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1
Q

Weak Acids

A 
Citric Acid
Hydrofluoric acid
Ethanoic acid
Phosphoric Acid
Carbonic Acid
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2
Q

Soluble: Nag SAG

A

Nitrate
Acetates
Group 1

Sulfates
Ammonium
Group 17

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3
Q

Solubility Exceptions PMS CASTRO BEAR:

A

PMS with SULFATES & GROUP 17

P (Pb, Lead)
M (Hg, Mercury)
S (Silver, Ag)

CASTRO BEAR with SULFATES

Ca (Calcium)
Sr (Strontium)
Ba (Barium)

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4
Q

Acidic and Basic salts

A

ACIDIC always NH4 (ammonium)

Strong Base + Strong Acid = Neutral
Strong Base + Weak Acid = Basic
Weak Base + Strong Acid = Acidic

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5
Q

Strong Bases

Weak base

A

NaOH
KOH
Ca(OH)2 –> Calcium hydroxide
Any other hydroxide with Group 1 & 2 Metals

Ammonia and everything else

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6
Q

Indicator and pH range for titration reactions

A

Indicator pH range of colour change

Methyl orange Strong Acid + Weak Base (Low pH)

Phenolphthalein Strong Base + Weak Acid (High pH)

Bromothymol blue Strong Acid + Strong Base (Neutral)

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7
Q

4 reasons that show a chemical system has reached equilibrium:

A
  1. It is a closed system - no matter enters or leaves the system
  2. Macroscopic properties (e.g. state, colour, temperature and pressure) stay constant
  3. Concentrations of reactant and products stay constant
  4. Rate of forward reaction = rate of reverse reaction
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8
Q

What is the enthalpy, entropy, and Gibbs free energy for Photosynthesis?

A

Enthalpy ∆H

  • Positive
  • Endothermic reaction

Entropy ∆S

  • Negative
  • Decrease in particles

Gibbs Free Energy ∆G

  • Positive
  • Non-spontaneous
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9
Q

What is the enthalpy for combustion?

A

Negative because it is an exothermic reaction

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10
Q

2, Effect of concentration on equilibrium

A

If concentration of a reactant or product is increased, the equilibrium will shift to the other side to use up the added chemical.

If concentration of a reactant or product is decreased, the equilibrium shifts to replace the substance removed.

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11
Q

2, Effect of Pressure and Volume Changes on Equilibrium

A

If pressure is increased, volume decreases. This will be towards the side with fewer gaseous particles. Because there are fewer collisions.

If pressure is decreased, volume increases. This will be towards the side with more gaseous particles. Because there are more collisions.

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12
Q

2, Effect of Temperature Changes on Equilibrium

A

If temperature of an equilibrium system increases the equilibrium position moves in whichever direction absorbs heat

If temperature of an equilibrium system is decreased, the system will move in whichever direction produces more heat.

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13
Q

2, Effect of a Catalyst on Equilibrium

A

Adding a catalyst will provide an alternative pathway of lower activation energy - this will allow both the forward and reverse reactions to occur at a faster rate

No visible effect

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14
Q

Changes in Temperature - Equilibrium Graph

A

It is going to gradually affect both reactants and products

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15
Q

Changes in Concentration - Equilibrium Graph

A

After the equilibrium is disturbed the change will show a sharp spike - ONLY one spike

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16
Q

Changes in Pressure - Equilibrium Graph

A

There will be a sharp spike for BOTH reactants and products

17
Q

Hydrogen Bonding FON

A

Fluorine, Oxygen, Nitrogen

18
Q

KSp

A

The Smaller the Ksp, the more insoluble and less dissociation

The Larger the Ksp, the more soluble and more dissociation

19
Q

Compare Q to Ksp results

A

Q < Ksp
Unsaturated
No precipitation

Q = Ksp
Saturated
Solution at equilibrium precipitation

Q > Ksp
Supersaturated
Precipitation

20
Q

Acid and Base Formula

A

Acid + Base → Salt + Water

Proton Transfer to form water

21
Q

Acid and Carbonate Formulas

A

Acid + Carbonate → Salt + Water + Carbon Dioxide

Acid + Hydrogen carbonate → Salt + Water + carbon dioxide

22
Q

Acid and Metal Formula

A

Metal + Acid (dilute) → Salt + Hydrogen

Nitric acid and concentrated sulfuric acid do not react in this way metals

23
Q

Can a base be a metal carbonate?

A

Yes

24
Q

Applications of Neutralisation Reactions

A

Antacids are substances such as sodium bicarbonate (NaHCO3). They are used to neutralise the stomach acid (HCl).

25
Q

Conductivity V-Shape

A

Strong Acid - Strong Base

26
Q

Conductivity L-Shape

A

Strong Acid - Weak Base

27
Q

Conductivity Opposite-L with a flick

A

Weak Acid - Strong Base

28
Q

Blood as a buffer with 2 equilibrium reactions

A

CO2 + H2O –>

Chemistry (2 decks)

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