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chem > chap 9: salts > Flashcards

chap 9: salts Flashcards

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1
Q

what is a cation?

A

positive ion

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2
Q

what is an anion?

A

negative ion

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3
Q

what are hydrated salts?

A

hydrated salts are salts that contain water of crystallisation

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4
Q

what are anhydrous salts?

A

salts that do not contain water of crystallisation

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5
Q

how can anhydrous salts be obtained?

A

can be obtained by heating hydrated salts

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6
Q

what happens when hydrated salts are heated?

A

they lose their water of crystallisation

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7
Q

what nitrates (NO3^-) are soluble and insoluble?

A

soluble salts: all nitrates
insoluble salts: nil

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8
Q

what carbonates (CO3^2-) are soluble and insoluble?

A

soluble salts: S.P.A and group 1
insoluble salts: all other carbonates

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9
Q

what chlorides (Cl^-) / iodides (I^-) are soluble and insoluble?

A

soluble salts: all chlorides/iodides except silver and lead (ii)
insoluble salts: silver and lead (ii)

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10
Q

what sulfates (SO4^2-) are soluble and insoluble?

A

soluble salts: all sulfates except lead(ii), calcium and barium
insoluble salts: lead (ii), calcium, barium

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11
Q

what hydroxides (OH^-) are soluble and insoluble?

A

soluble salts: group 1, calcium, (sparingly soluble) and barium
insoluble salts: all other hydroxides

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12
Q

what are spectator ions?

A

spectator ions are substances that remain unchanged in their physical state or charge and do not take part in the reaction

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13
Q

when is titration used?

A

to prepare soluble S.P.A and group 1 salts

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14
Q

how to prepare salt using titration?

A
  1. fill up a burette with dilute nitric acid. note the initial burette reading. note the initial burette reading (V1 cm^3)
  2. pipette 25 cm3 of dilute NaOH solution into a conical flask
  3. add 2-3 drops of methyl orange to the NaOH solution. the solution turns yellow
  4. while swirling the conical flask, add dilute nitric acid from the burette slowly until the solution just turns orange permanently. this is the end-point.
  5. record the final burette reading as V2 cm3. the volume of acid required to complete neutralisation ( V2 - V1) cm3
    repeat the reaction without indicator to obtain a pure solution
  6. pipette 25 cm3 of NaOH solution into a conical flask
  7. add (V1- V2) cm3 of dilute nitric acid from the burette
  8. heat the solution to evaporate the water until a hot saturated solution
  9. allow the saturated solution to cool and crystallise
  10. filter to collect the residue
  11. wash crystals with cool distilled water to remove impurities
  12. dry the crystals between sheets of filter paper
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15
Q

when is reaction of acid with B.C.M. (insoluble base, insoluble carbonate, metal) used?

A

it is used to prepare soluble, non-S.P.A salts

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16
Q

how to prepare salts using reaction of an acid with insoluble B.C.M?

A
  1. fill half a beaker with sulfuric acid. add excess zinc and stir continuously until no more zinc will dissolve or when there is no more effervescence
  2. filter to remove excess zinc powder. collect the filtrate which is zinc sulfate solution
  3. heat the filtrate till a hot saturated solution is obtained
  4. when the filtrate is saturated, leave it to cool and crystallise
  5. filter to collect the residue. wash the crystals with a little cold distilled water to remove impurities. dry the crystal between a few sheets of filter paper
17
Q

when is precipitation used?

A

it is used to prepare insoluble salts

18
Q

what are the conditions for an acid + B.C.M reaction to take place?

A

-the base, carbonate or metal must be added in excess so that all the acid is used up. if the acid is not used up, the salt produced will be contaminated with acid.
-starting materials must be insoluble in water. this ensures that the excess starting materials can be removed from the salt solution by filtration

19
Q

what are the conditions for titration to take place?

A

both starting materials are soluble in water. the addition of excess starting material cannot be separated from the salt so the exact volume of reactants are needed.

20
Q

what are the conditions for precipitation to take place?

A

both starting materials are aqueous (one contain the cation and the other contain the anion)
pure and dry sample of the salt can be obtained easily through filtration

21
Q

how to prepare salts using precipitation?

A
  1. add and mix sodium sulfate solution to lead (ii) nitrate solution and stir until no more precipitate forms
  2. filter to collect the residue
  3. wash the residue with small amount of distilled water to remove impurities
  4. allow precipitate to dry on a piece of filter paper

chem (8 decks)

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