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Chapter 4: Q15E (page 216)

Silver can be separated from gold because silver dissolves in nitric acid while gold does not. Is the dissolution of silver in nitric acid an acid-base reaction or an oxidation-reduction reaction? Explain your answer.

Short Answer

Expert verified

It is an oxidation-reduction reaction.

The balanced equations for the dissolution areas given below:

\(\begin{aligned}{}3Ag\left( s \right) + 4HN{O_3}\left( {Cold\& diluted} \right) \to 3AgN{O_3}\left( {aq} \right) + NO + 2{H_2}O\left( l \right)\\Ag\left( s \right) + 2HN{O_3}\left( {hot\& concentrated} \right) \to AgN{O_3}\left( {aq} \right) + N{O_2} + {H_2}O\left( l \right)\end{aligned}\)

Step by step solution

01

Reaction between silver and cold, dilute nitric acid

The corresponding balanced equation is as follows:

\(3Ag\left( s \right) + 4HN{O_3}\left( {Cold\& diluted} \right) \to 3AgN{O_3}\left( {aq} \right) + NO + 2{H_2}O\left( l \right)\)

In this case, silver is oxidised from 0 to +1 state and nitrogen reduced from +5 to +2 state (NO).

02

Reaction between silver and hot,concentrated nitric acid

The corresponding balanced equation is as follows:

\(Ag\left( s \right) + 2HN{O_3}\left( {hot\& concentrated} \right) \to AgN{O_3}\left( {aq} \right) + N{O_2} + {H_2}O\left( l \right)\)

In this case, silver is oxidised from 0 to +1 state and nitrogen reduced from+5 to +4 state (NO2)

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Most popular questions from this chapter

Write a balanced equation describing each of the following chemical reactions.

(a) Solid potassium chlorate, KClO3 decomposes to form solid potassium chloride and diatomic oxygen gas

(b) Solid aluminium metal reacts with solid diatomic iodine to form solid Al2I6

(c) When solid sodium chloride is added to aqueous sulfuric acid, hydrogen chloride gas and aqueous sodium sulfate are produced.

(d) Aqueous solutions of phosphoric acid and potassium hydroxide react to produce aqueous potassium dihydrogen phosphate and liquid water.

Classify the following as acid-base reaction or oxidation-reduction reactions.

(a)\(N{a_2}S\left( {aq} \right) + 2HCl\left( {aq} \right) \to 2NaCl\left( {aq} \right) + {H_2}S\left( g \right)\)

(b)\(2Na\left( s \right) + 2HCl\left( {aq} \right) \to 2NaCl\left( {aq} \right) + {H_2}\left( g \right)\)

(c)\(Mg\left( s \right) + C{l_2}\left( g \right) \to MgC{l_2}\left( s \right)\)

(d)\(MgO\left( s \right) + 2HCl\left( {aq} \right) \to MgC{l_2}\left( {aq} \right) + {H_2}O\left( l \right)\)

(e)\({K_3}P\left( s \right) + 2{O_2}\left( g \right) \to {K_3}P{O_4}\left( s \right)\)

(f)\(3KOH\left( {aq} \right) + {H_3}P{O_4}\left( {aq} \right) \to {K_3}P{O_4}\left( {aq} \right) + 3{H_2}O\left( l \right)\)

A 0.025-g sample of a compound composed of boron and hydrogen, with a molecular mass of ~28 amu, burns spontaneously when exposed to air, producing 0.063 g of B2O3. What are the empirical and molecular formulas of the compound?

Which solution could be used to precipitate barium ion Ba2+, in a water sample, Sodium chloride, sodium hydroxide, or sodium sulfate. What is the formula for the expected precipitate?

Colourful fireworks often involve the decomposition of barium nitrate and potassium chlorate and the reaction of metals magnesium, aluminium, and iron with oxygen.

(a)Write the formulae of barium nitrate and potassium chlorate.

(b)The decomposition of solid potassium chlorate leads to the formation of solid potassium chloride and diatomic oxygen gas. Write an equation for the reaction.

(c) The decomposition of solid barium nitrate leads to the formation of solid barium oxide, diatomic nitrogen gas and diatomic oxygen gas. Write an equation for the reaction.

(d)Write separate equations for the reactions of the solid metals magnesium, aluminium and iron and oxygen gas to yield the corresponding metal oxides.(Assume the iron oxide contains \(F{e^{3 + }}\)ions.)
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