Chemistry, 18.03.2020 04:30 xwalker6772

Precipitation reactions and ionic equations
(look at attachment)

Precipitation reactions and ionic equations (look at attachment)

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Answer from: Isaiahgardiner5143

Net ionic equation: 2OH⁻(aq) + Fe²⁺(aq) → Fe(OH)₂(s)

Net ionic equation: 2K⁺(aq) + CH₃COO⁻ (aq) + 2Na⁺(aq) + S⁻²(aq) → NO REACTION

Net ionic equation: CO₃⁻²(aq) + Pb⁺²(aq) → PbCO₃(s)

Explanation:

a. Solutions of calcium hydroxide and Iron (II) chloride are mixed:

We identify the reactants:

Ca(OH)₂ , FeCl₂

In excess, the Fe(OH)₂ can make precipitate

Salts from chlorides with elements from group II are soluble.

The reaction is: Ca(OH)₂(aq) + FeCl₂(aq) → Fe(OH)₂(s) + CaCl₂(aq)

Ca(OH)₂(aq) + FeCl₂(aq) → Fe(OH)₂(s) + CaCl₂(aq)

We dissociate the compounds, except for the solid

Ca²⁺(aq) + 2OH⁻(aq) + Fe²⁺(aq) + 2Cl⁻(aq) → Fe(OH)₂(s) + Ca²⁺ + 2Cl⁻(aq)

Net ionic equation: 2OH⁻(aq) + Fe²⁺(aq) → Fe(OH)₂(s)

b. Solutions of potassium acetate and sodium sulfide are mixed:

The reactants are: KCH₃COOH and Na₂S

In this case there are no precipitates, because all the salts are soluble

We make the complete reaction:

2KCH₃COO (aq) + Na₂S(aq) → K₂S(aq) + 2NaCH₃COO (aq)

Net ionic equation is:

2K⁺(aq) + CH₃COO⁻ (aq) + 2Na⁺(aq) + S⁻²(aq) → 2K⁺(aq) + S⁻²(aq) + 2Na⁺(aq) + CH₃COO⁻ (aq)

c. Solutions of ammonium carbonate and lead(II) nitrate are mixed:

In this case, the reactants are: (NH₄)₂CO₃ and Pb(NO₃)₂

All salts from nitrate are soluble.

Carbonate makes a precipitate when it bonds Pb.

The complete reaction is:

(NH₄)₂CO₃(aq) + Pb(NO₃)₂(aq) → PbCO₃(s) + 2NH₄NO₃(aq)

We dissociate all of the compounds, except for the solid in order to make the net ionic equation:

2NH₄⁺(aq) +CO₃⁻²(aq) + Pb⁺²(aq) +2NO₃⁻(aq) → PbCO₃(s) + 2NH₄⁺ (aq) + 2NO₃⁻(aq)

The net ionic equation is: CO₃⁻²(aq) + Pb⁺²(aq) → PbCO₃(s)

The ions that are repeated, are called spectators ions. We all cancel them.

Answer from: Quest

the only liquid elements at standard temperature and pressure are bromine (br) and mercury (hg). although, elements caesium (cs), rubidium (rb), francium (fr) and gallium (ga) become liquid at or just above room temperature.

explanation:

Answer from: Quest

b is the correct

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