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Chem (2022) Sem. 1 > Acids + Bases (excl. Titrations) (2) > Flashcards

Acids + Bases (excl. Titrations) (2) Flashcards

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1
Q

Acid + Metal —> ____ + _______

A

Acid + Metal —> Salt + Hydrogen

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2
Q

Acid + Metal Hydroxide —> ____ + _____

A

Acid + Metal Hydroxide —> Salt + Water

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3
Q

Acid + Metal Oxides —> ____ + _____

A

Acid + Metal Oxides —> Salt + Water

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4
Q

Group 1 Metal + Water —> _____ _______ + ________

A

Group 1 Metal + Water —> Metal Hydroxide + Hydrogen

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5
Q

Acid + Carbonates —> ____ + _____ + ______ _______

A

Acid + Carbonates —> Salt + Water + Carbon Dioxide

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6
Q

Properties of Acids & Bases

A

Acids:

  • Taste sour
  • Turns litmus red
  • Corrosive
  • Molecular in structure

Bases:

  • Taste bitter
  • Turn litmus blue
  • Feel slippery
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7
Q

Explain the Davy Theory on Acids + Bases

A

Acid:
- Substances containing replaceable hydrogen that could be partly or totally replaced by metals

Base:
- Substances that reacted with acids to form salts and water

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8
Q

Explain the Arrhenius Theory on Acids + Bases

A

Acids:

  • Produces a hydrogen ion in solution
    • HCl —> H^+ + Cl^-

Bases:

  • Produces a hydroxide ion in solution
    • NaOH —> Na^+ + OH^-
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9
Q

Explain the Bronstead-Lowry Theory on Acids + Bases

A

Acids:
- Substance that can donate a proton (hydrogen ion) in a reaction

Bases:
- Substance that can accept a proton (hydrogen ion) in a reaction

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10
Q

What are the disadvantages and advantages of the Bronsted Lowry theory?

A

Advantages:

  • Isn’t limited to reactions in aqueous solutions
  • Can include any reaction where acids donate proton to base
    • HCL + NH3 —> NH4Cl

Disadvantages:

  • Can’t be applied to reactions between acidic & basic oxides
    • CaO + CO2 —> CaCO3
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11
Q 
Show the conjugate acid-base pairs of:
HCl 
H2SO4
HNO3
CH3COOH
H3O^+
NH4^+
H2O
A

(From acid , base)

HCl:

  • HCl , Cl-
  • H3O ^+, H2O

H2SO4:

  • H2SO4 , HSO4^-
  • H3O^+ , H2O

HNO3:

  • HNO3 , NO3^-
  • H2O^+ , H2O

CH3COOH:

  • CH3COOH , CH3COO-
  • H3O^+ , H2O

H3O^+:

  • H3O^+ , H2O
  • H3O^+ , H2O

NH4^+:

  • NH4^+ , NH3^-
  • H3O^+ , H2O

H2O:

  • H2O , OH-
  • H3O^+ , H2O
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12
Q

What is an amphiprotic substance?

A

A substance which can function as either an acid or a base dependent upon what it is reacting with

E.g.
H2O
- Base: OH-
- Acid: H3O^+

HCO3^-

  • Base: CO3^2-
  • Acid: H2CO3

H2PO4^-

  • Base: HPO4^2-
  • Acid: H3PO4
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13
Q

What is monoprotic acid?

A

Can donate only 1 proton per molecule

E.g. HCl, HNO3, CH3COOH

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14
Q

What is diprotic acid?

A

Can donate 2 protons per molecule

E.g. H2SO4, H2CO3

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15
Q

What is polyprotic acid?

A

Can donate more than 1 proton per molecule

E.g. H2SO4, H3PO4, H2S, H2SO3

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16
Q

What is a triprotic acid?

A

Can donate 3 protons per molecule

E.g. H3PO4, H3BO3

17
Q

What are strong acids?

A
  • Molecules completely ionises in water
  • Resulting solution: mainly ions and few molecules

E.g. only nitric acid (HNO3), sulfuric acid (H2SO4) & hydrochloric acid (HCL)

18
Q

What are strong bases?

A
  • Molecules completely dissociates in water
  • Form separate ions (E.g. NaOH –> Na^+ + OH^-)

E.g. G1 & G2 hydroxides & oxides

19
Q

What are weak acids?

A
  • Molecules only partly ionise in water
  • Resulting solution: consists of molecules and few ions

E.g. Vinegar + citric acid

20
Q

What are weak bases?

A
  • Molecules partially ionise in water
  • Few ions formed

E.g. Ammonia

21
Q

What is Ka?

A

The equilibrium expression is rearranged to give the acid/base dissociation equilibrium constant, which is a measure of the strength of acid/base.

Ka = products/reactants

E.g. HF + H2O –>

22
Q

How do you determine if Carbonic acid (H2CO3) is a weak or strong acid (use hydrolysis)?

A
  1. H2CO3 + H2O —>
23
Q

Is Ammonia (NH3) a weak or strong base (use hydrolysis)?

A
  1. NH3 + H2O —>
24
Q

Define salts + examples

A

Is an ionic compound containing + ions other than a hydrogen ion or - ions other than the oxide ion or the hydroxide ion.

  • E.g. CaCO3, FeSO4 & KF
25
Q

What happens when a salt dissolves in water?

A

Completely dissolves in water and dissociates completely into ions

26
Q

What is it called when one or both ions produced in dissociation can undergo a further reaction with water?

A

Hydrolysis

27
Q

A salt formed between a strong acid and a strong base is ______

A

Neutral

28
Q

A salt formed between a strong acid and a weak base is _______

A

Acidic

29
Q

A sat formed in the reaction between a weak acid and a strong base is ______

A

Basic

30
Q

Define buffer

A
  • Are solutions that have the ability to resist pH change when small amounts of either acids or bases are added to them
  • Generally contain a weak acid and its conjugate base OR a weak base and its conjugate acid
  • They work as weaker acid + weak base can CO-EXIST in solution without neutralising one another but react to neutralise any strong acid or strong base added to buffer
31
Q

Define buffer capacity

A
  • The ability of a buffer solution to neutralise excess acid or base without a major change in pH
  • Can be also defined as:
    The amount of acid or base the buffer can neutralise before pH changes dramatically

Chem (2022) Sem. 1 (5 decks)

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