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Chemistry > Acids, Bases and Salts > Flashcards

Acids, Bases and Salts Flashcards

1
Q

Give the molecular formula of hydrochloric acid.

A

HCl

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2
Q

Give the molecular formula of sulfuric acid.

A

H2SO4

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3
Q

Give the molecular formula of nitric acid.

A

HNO3

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4
Q

Give the molecular formula of phosphoric acid.

A

H3PO4

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5
Q

Give the molecular formula of ethanoic acid.

A

CH3COOH

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6
Q

Define an acid.

A

A proton donor that releases H+ ions in solution.

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7
Q

What is a carboxylate ion?

A

The ion formed when an organic acid dissociates.

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8
Q

What is a weak acid?

A

An acid that only partially disociates in water, according to an equilibrium.

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9
Q

How can water act as a weak acid?

A

H2O OH- + H+

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10
Q

What is the difference between the strength and the concentration of an acid?

A

The strength of an acid determines the extent of dissociation in solution, whereas the concentration determines the number of molecules per unit volume.

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11
Q

Define a base.

A

A proton acceptor.

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12
Q

Name the three types of base.

A

Metal oxides, metal hydroxides, and ammonium.

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13
Q

How can water act as a base?

A

H2O can accept a proton to give a hydronium ion: H3O+

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14
Q

Define an alkalis.

A

A soluble base that releases OH- ions in solution.

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15
Q

Name the three most common alkalis,

A

Sodium hydroxide, potassium hydroxide and aqueous ammonia

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16
Q

Give the reaction of ammonia and water.

A

NH3 + H2O ——> OH- + NH4+

17
Q

Explain why ammonia is a base in solution.

A

When ammonia reacts with water it accepts a proton to give an ammonium ion, and OH- ions are released.

18
Q

What does ‘aqua’ mean in a chemical equation?

A

A reaction involving water where water is not actually reacting chemically, eg. when water acts as a solvent.

19
Q

Define a salt.

A

Salts are ionic compounds formed when the H+ ions in acids are replaced by metal ions or ammonium ions.

20
Q

Give the equation of a hydrogen carbonate ion.

A

HCO3-

21
Q

Give the equation of carbonic acid.

A

H2CO3

22
Q

Give 4 equations for the common acid base reactions.

A

acid + metal —–> salt + hydrogen
acid + metal oxide ——> salt + water
acid + metal hydroxide ——> salt + water
acid + metal carbonate ——> salt + water + carbon dioxide

23
Q

What is a neutralisation reaction?

A

Any reaction in which the H+ from an acid reacts with OH- from an alkali to form water.

24
Q

Describe an ionic compound dissolving in water.

A

The charged ions in a n ionic compound attract the polar water molecules, which surround the ions pulling them away from the ionic structure/lattice. The ions “dissolve” when they are surrounded by water molecules.

25
Q

Which ions always form soluble compounds?

A

Group 1 ions, ammonium ions, nitrate ions and hydrogen carbonate ions.

26
Q

Describe the solubility of halides.

A

Soluble except when combined with Ag+, Pb2+ or Hg2+

27
Q

Describe the solubility of SO4- ions

A

Soluble except when combined with Ag+, Pb2+, Ca2+, Sr2+ , Ba2+

28
Q

Which ions are almost always insoluble (except when with group 1, ammonium or nitrate ions)?

A

Carbonates, phosphates and sulphides.

29
Q

Describe the appearance of the 3 silver halides.

A

Silver chloride- white precipitate
Silver bromide- cream precipitate
Silver iodide- yellow precipitate

30
Q

Describe the reactions of the three silver halides with dilute and concentrated ammonia solution.

A

Silver chloride- dissolves in dilute NH4+
Silver bromide- dissolves only in concentrated NH4+
Silver iodide- does not dissolve in NH4+

31
Q

Describe the test for halide salts

A

React with acidified silver nitrate solution. If a precipitate forms, a halide is present. Add first dilute, and then concentrated ammonia soluion to identify that halide.

32
Q

Describe the test for sulphate salts.

A

Add a solution of Ba2+ ions in the form of barium chloride or barium nitrate solution. If SO4 2- ions a re present, a white precipitate forms.

33
Q

Describe the test for carbonate ions.

A

Add dilute nitric acid to the test substance. If bubbles/effervescence is seen then the unknown compound could be a carbonate. The gas could be further tested by bubbling it through limewater, if the limewater turns milky then this is a positive test for CO2

34
Q

Describe the test for ammonium ions in solution.

A

Add sodium hydroxide solution and warm gently. If ammonium ions are present you get a smell of ammonia and a piece of damp red litmus will turn blue.

Chemistry (13 decks)

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