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OCR A Level Chemistry > 2.1.14 Acids and Bases > Flashcards

2.1.14 Acids and Bases Flashcards

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1
Q

What is the formula for: sulphuric acid?

A

H2SO4;

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2
Q

What is the formula for: hydrochloric acid?

A

HCl;

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3
Q

What is the formula for: nitric acid?

A

HNO3;

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4
Q

What is the formula for: a carboxylic acid?

A

CH3COOH

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5
Q

What do all acids have in common and how is this written?

A
  1. They all DONATE the H+ ions they contain IN SOLUTION; AKA ‘protons,’ because they are an H atom with no electron. These H+ ions are responsible for all of the reactions as seen with acids.
  2. This is written as H+(small)(aq).
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6
Q

What is the difference between acids and alkalis in terms of donating ions and accepting ions?

A

Acids: donate H+ ions; and are known as PROTON DONORS
Alkalis: accept ions;
NOTE: how this is an alkali and NOT a base, because bases do not dissolve in water - and so ion transactions cannot occur - they occur only IN SOLUTION.

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7
Q

What is the difference between a weak acid and a strong acid?

A

Weak acids are:

  1. Very good at accepting back H+ ions and so only PARTIALLY DISSOCEATE; this is why they have an equilibrium.
  2. Are not very good at giving many ‘protons’ away;
  3. They have an equilibrium, and so reactions between ammonia and an acid are said to have only produced an ammonium salt (as the water has partially formed).

Strong acids:

  1. Form no equilibrium, as everything reacts;
  2. FULLY DISSOCEATE, as give away all of their H+ ions.
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8
Q

Define dissociate.

A

The extent to which an acid donates all of its H+ ions / protons (same thing). A strong acid would have fully dissociated, and a weak acid would have partially dissociated.

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9
Q

Why are acids known as proton donors? If so, what are alkalis (NOT BASES) known as?

A
  1. Because they give away their protons/ H+ ions (same thing) depending on how strong they are.
  2. Alkalis (NOT BASES) accept these protons, and so are known as proton acceptors.
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10
Q

What are MgO and CuO examples of?

A

Metal oxides, they are BASES.

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11
Q

What are NaOH and Mg(OH)2 examples of?

A

Metal hydroxides, they are BASES.

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12
Q

What are amines?

A

CH3NH2 - they are organic compound which are examples of BASES.

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13
Q

What is NH3?

A

Ammonia, a WEAK, ORGANIC BASE.

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14
Q

What is the difference in the type of ions that acids and alkalis have? How is this shown in the neutralisation reaction?

A
  1. Acids: H+ ions in solution;
  2. Alkalis: OH- ions in solution;
  3. In a neutralisation reaction, these two attract to form water.
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15
Q

What is NaOH?

A

Sodium hydroxide;

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16
Q

What is the formula for sodium hydroxide?

A

NaOH;

17
Q

What is KOH?

A

Potassium hydroxide;

18
Q

What is the formula for potassium hydroxide?

A

KOH;

19
Q

What is the general formula for a hydroxide?

A

OH, these are alkalis as they produce Oh- ions in solution.

20
Q

What is sodium hydroxide used as, and when can it be classified as corrosive?

A
  1. Used in oven cleaners and wall paint strippers;

2. It is classified as corrosive as dilute a 0.5mol/dm^3

21
Q

Why is ammonia a weak base?

A
  1. Because it dissolves in water (so is an alkali ), to form a weak alkaline solution.
  2. It produces an equilibrium, with NH3(aq)+H2O(l)equilib arrowNH4+(aq)+OH-(aq) - it has stripped an H+ ion from water, forming ammonium.
  3. It is only PARTIALLY DISSOCEATED.
22
Q

What is the name for something that behaves as bases and acids?

A

Amphoteric;

23
Q

What does amphoteric mean, produce examples?

A
  1. A substance that behaves as an acid and a base.
  2. Examples: water, carboxyl acids (COOH, which is able to donate a proton, but has an acidic part) and an amino acid basic group, NH2, which could accept a proton.
24
Q

What is the state symbol one should utilise when noting water?

A

(l), NOT AQ, because water cannot be dissolved in itself.

OCR A Level Chemistry (83 decks)

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