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Chemistry > Acids, Bases, Salts > Flashcards

Acids, Bases, Salts Flashcards

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1
Q

Acid

A

A H+ donator.

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2
Q

Weak Acid

A

partially dissociates (only some H+ ions dissosisted)

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3
Q

Examples of weak acids

A

ethanoic acid CH3COOH
citric acid C6H8O7
formic acid CHOOH
phosphoric acid H3PO4

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4
Q

Strong acid

A

Fully dissosisted in aqueous solution

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5
Q

Examples of strong acids

A

Hydrochloric Acid HCl
Sulfuric Acid H2SO4
Nitric Acid HNO3

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6
Q

Base

A

A h+ ion acceptor

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7
Q

Alkali

A

A soluble base and release OH- ions in solution

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8
Q

Salt

A

An ionic substance formed when the H+ ions of an acid are replaced by metal ions or ammonium ions.

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9
Q

Concentration

A

The amount in moles of acid per until vol of solution.

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10
Q

Strength (of acid)

A

Related to the proportion of the acid that is dissosisted in aqueous solution.

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11
Q

Test for sulfate ions

A

Add barium nitrate

White precipitate formed

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12
Q

Test for Carbonate ions

A

Add dilute HCl
Effervescent occurs
Bubble gas through limewater
White precipitate formed

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13
Q

Test for ammonia ions

A 
Add sodium hydroxide 
Ammonia gas formed
Warm solution in water bath
Place damp red litmus in mouth if test tube 
Litmus paper will turn blue
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14
Q

Test for Chloride ions

A

Add silver nitrate
White precipitate formed
When added to dilute and concentrated ammonia precipitate redesolves

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15
Q

Test for bromide ions

A

Add silver nitrate
Cream precipitate forms
When added to dilute ammonia precipitate remains
When added to concentrated ammonia precipitate redesolves

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16
Q

Test for iodide ions

A

Add silver nitrate
Yellow precipitate formed
When added to dilute and concentrated ammonia precipitate remains

17
Q

How does the equation showing the dissociation of acids

A

strong acids fully dissociate so reaction is one way:
HCl –> H+ + Cl-
weak acids partially dissociate so reaction is reversible:
CH3COOH CH3COO- + H+

18
Q

Coomon Alkalis

A

Sodium Hydroxide NaOH
Potassium Hydroxide KOH
Ammonia NH3

19
Q

Types of bases

A

Metal Hydroxides - OH- can accept 1 H+ ion to form water

Metal Oxides - Can accept 1 H+ ion to form a hydroxide or 2 to form water

20
Q

Ammonia as a base and alkali

A

Ammonia is an alkali as it’s soluble in water however can act as a base as it contains a nitrogen with a lone pair of electrons which can form a bond with a H+ ion to form NH4+

21
Q

how can water act as an acid and a base

A

Water can act as an acid as it can donate a H+ ion:
H2o -> OH- + H+

Water can also act as a base by accepting a H+ ion:
H2O + H+ -> H3O+ (hydronium ion)

22
Q

Acid + Alkali

A

Salt + Water

23
Q

Acid + Metal Oxide

A

Salt + Water

24
Q

Acid + Metal carbonate

A

Salt + Carbon Dioxide + Water

25
Q

Acid+ Metal hydrogen carbonate

A

Salt + Carbon Dioxide + Water

26
Q

Acid + Metal Hydroxide

A

Salt + Water

27
Q

Acid + Reactive Metal

A

Salt+ Hydrogen

28
Q

Always soluble ions

A

Group 1 ions
Ammonium NH4+
Nitrate NO3-
Hydrogen carbonate HCO3-

29
Q

Soluble ions with exeption

A 
Halide ions ( Cl- Br- I-) expect when combined with Ag+ Pb2+ Hg2+(mercury)
Sulfate SO42- except when combined with Ag+ Pb2+ Ca2+ Sr2+ Ba2+
30
Q

insoluble ions

A

oxide unless combined with group 1 metal or Ca2+ or Ba2+
Carbonate unless combined with group 1 metal or ammonium
phosphate unless combined with group 1 metal or ammonium

31
Q

insoluble ions

A

hydroxide unless combined with group 1 metal or ammonium or Ca2+ Mg2+ Sr2+ or Ba2+
Sulfide unless combined with group 1 metal or ammonium
Dichromate (cr2O72-) unless combined with group 1 metal or ammonium or Ca2+ or Mg2+

Chemistry (10 decks)

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