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Worksheet: Balancing Ionic Equations

Q1:

Write a net ionic equation for the formation of solid calcium fluoride and aqueous sodium chloride from aqueous solutions of calcium chloride and sodium fluoride.

  • A C a ( ) + 2 F ( ) C a ( ) + 2 F ( ) 2 + 2 + a q a q s s
  • B C a C l ( ) + 2 N a F ( ) C a F ( ) + 2 N a C l ( ) 2 2 a q a q s a q
  • C C a ( ) + 2 F ( ) + 2 N a ( ) + 2 C l ( ) C a F ( ) + 2 N a C l ( ) 2 + + 2 a q a q a q a q s a q
  • D C a ( ) + 2 F ( ) C a F ( ) 2 + 2 a q a q s
  • E C a ( ) + 2 C l ( ) + 2 N a ( ) + 2 F ( ) C a ( ) + 2 F ( ) + 2 N a ( ) + 2 C l ( ) 2 + + 2 + + a q a q a q a q s s a q a q

Q2:

When iron(II) ions react with cerium(IV) ions in water, iron(III) and cerium(III) ions are produced.

Write the reduction half-equation for this reaction, including state symbols.

  • A C e ( ) + 2 e C e ( ) 4 + 2 + a q a q
  • B C e ( ) + 3 e C e ( ) 6 + 3 + a q a q
  • C F e ( ) + e F e ( ) 3 + 2 + a q a q
  • D C e ( ) + e C e ( ) 4 + 3 + a q a q
  • E F e ( ) + 2 e F e ( ) 3 + + a q a q

Write a balanced ionic equation for this reaction, including state symbols.

  • A F e ( ) + C e ( ) F e ( ) + C e ( ) 2 + 4 + 3 + 3 + a q a q a q a q
  • B 2 F e ( ) + C e ( ) 2 F e ( ) + C e ( ) 3 + 4 + 2 + 2 + a q a q a q a q
  • C 3 F e ( ) + C e ( ) 3 F e ( ) + C e ( ) 3 + 6 + 2 + 3 + a q a q a q a q
  • D F e ( ) + C e ( ) F e ( ) + C e ( ) 2 + 3 + 3 + 4 + a q a q a q a q
  • E F e ( ) + 2 C e ( ) F e ( ) + 2 C e ( ) + 3 + 3 + 4 + a q a q a q a q

Q3:

Write the reduction half-equation, including state symbols, for the formation of silver from aqueous diamminesilver(I) nitrate, [ A g ( N H ) ] N O 3 2 3 .

  • A A g ( ) + e A g ( ) + a q a q
  • B A g ( ) + e A g ( ) + a q s
  • C [ A g ( N H ) ] ( ) + e A g ( ) + 2 N H ( ) 3 2 + 3 a q a q a q
  • D [ A g ( N H ) ] ( ) + e A g ( ) + 2 N H ( ) 3 2 + 3 a q s a q
  • E [ A g ( N H ) ] N O ( ) + e A g ( ) + 2 N H ( ) + N O ( ) 3 2 3 3 3 a q a q a q a q

Q4:

What name is given to the ions in a reaction equation that are not included in the net ionic equation?

  • A Unreactive ions
  • B Watching ions
  • C Unbalanced ions
  • DSpectator ions
  • E Bystander ions

Q5:

Write a net ionic equation for the following reaction:

  • A 2 K ( ) + C O ( ) + B a ( ) + 2 O H ( ) B a ( ) + C O ( ) + 2 K ( ) + 2 O H ( ) + 2 4 + + 2 4 + a q a q a q a q s s a q a q
  • B 2 K ( ) + C O ( ) + B a ( ) + 2 O H ( ) B a C O ( ) + 2 K ( ) + 2 O H ( ) + 2 4 2 2 + 2 4 + a q a q a q a q s a q a q
  • C B a ( ) + C O ( ) B a ( ) + C O ( ) 2 + 2 4 2 2 + 2 4 2 a q a q s s
  • D B a ( ) + C O ( ) B a C O ( ) 2 + 2 4 2 2 4 a q a q s
  • E B a ( ) + C O ( ) B a C O ( ) + 2 4 2 4 a q a q s

Q6:

Write the reduction half-equation, including state symbols, for the conversion of S n C l 4 to S n C l 2 in water.

  • A S n ( ) + 2 e S n ( ) 4 + 2 + a q a q
  • B C l ( ) + e C l ( ) 2 a q a q
  • C C l ( ) + 2 e 2 C l ( ) 2 a q a q
  • D S n ( ) + 2 e S n ( ) 4 + 2 + a q a q
  • E S n ( ) + e S n ( ) 2 + + a q a q

Q7:

When lead, ammonium, carbonate, and nitrate ions are mixed in aqueous solution, a precipitation reaction takes place. Write a balanced net ionic equation for this reaction, including state symbols.

  • A N H ( ) + N O ( ) N H N O ( ) 4 + 3 4 3 a q a q s
  • B P b ( ) + 2 N O ( ) P b ( N O ) ( ) 2 + 3 3 2 a q a q s
  • C P b ( ) + 2 N O ( ) + 2 N H ( ) + C O ( ) P b ( N O ) ( ) + ( N H ) C O ( ) 2 + 3 4 + 3 2 3 2 4 2 3 a q a q a q a q s s
  • D P b ( ) + C O ( ) P b C O ( ) 2 + 3 2 3 a q a q s
  • E P b ( ) + C O ( ) + N H ( ) + N O ( ) P b C O ( ) + N H N O ( ) 2 + 3 2 4 + 3 3 4 3 a q a q a q a q s s

Q8:

In aqueous solution, carbon dioxide reacts with excess sodium hydroxide to form aqueous sodium carbonate. Write a balanced net ionic equation for this reaction, including state symbols.

  • A C O ( ) + O H ( ) C O ( ) + H ( ) 2 3 2 + a q a q a q a q
  • B C O ( ) + 2 N a O H ( ) N a C O ( ) + H O ( ) 2 2 3 2 a q a q a q l
  • C 2 C O ( ) + 2 O H ( ) 2 C O ( ) + H ( ) 2 3 2 2 a q a q a q g
  • D C O ( ) + 2 O H ( ) C O ( ) + H O ( ) 2 3 2 2 a q a q a q l
  • E 2 C O ( ) + 2 N a O H ( ) 2 N a C O ( ) + H ( ) 2 3 2 a q a q a q g

Q9:

Sodium hydroxide and chlorine gas can be produced by the electrolysis of aqueous sodium chloride. Write a balanced net ionic equation for this reaction, including state symbols.

  • A 2 C l ( ) + 2 H O ( ) 2 O H ( ) + 2 H ( ) C l ( ) 2 + 2 a q l a q a q g
  • B 2 C l ( ) + 2 N a ( ) + 2 H O ( ) 2 N a O H ( ) + 2 H ( ) + C l ( ) + 2 + 2 a q a q l a q a q g
  • C 2 N a C l ( ) + 2 H O ( ) 2 N a O H ( ) + 2 H ( ) + C l ( ) a q l a q a q g 2 + 2
  • D 2 C l ( ) + 2 H O ( ) 2 O H ( ) + H ( ) + C l ( ) 2 2 2 a q l a q g g
  • E 2 N a C l ( ) + 2 H O ( ) 2 N a O H ( ) + H ( ) + C l ( ) a q l a q g g 2 2 2

Q10:

When silver, lithium, chloride, and acetate ions are mixed in aqueous solution, a precipitation reaction takes place. Write a balanced net ionic equation for this reaction, including state symbols.

  • A L i ( ) + C l ( ) + A g ( ) + 2 C H C O ( ) L i C l ( ) + A g ( C H C O ) ( ) + 2 + 3 2 3 2 2 a q a q a q a q s s
  • B A g ( ) + 2 C H C O ( ) A g ( C H C O ) ( ) 2 + 3 2 3 2 2 a q a q s
  • C L i ( ) + C H C O ( ) L i C H C O ( ) + 3 2 3 2 a q a q s
  • D A g ( ) + C l ( ) A g C l ( ) + a q a q s
  • E L i ( ) + C H C O ( ) + A g ( ) + C l ( ) L i C H C O ( ) + A g C l ( ) + 3 2 + 3 2 a q a q a q a q s s

Q11:

When barium, potassium, sulfate, and nitrate ions are mixed in aqueous solution, a precipitation reaction takes place. Write a balanced net ionic equation for this reaction.

  • A B a ( ) + S O ( ) + K ( ) + N O ( ) B a S O ( ) + K N O ( ) 2 + 4 2 + 3 4 3 a q a q a q a q s s
  • B K ( ) + N O ( ) K N O ( ) + 3 3 a q a q s
  • C B a ( ) + S O ( ) + 2 K ( ) + 2 N O ( ) B a ( N O ) ( ) + K S O ( ) 2 + 4 2 + 3 3 2 2 4 a q a q a q a q s s
  • D B a ( ) + S O ( ) B a S O ( ) 2 + 4 2 4 a q a q s
  • E 2 K ( ) + S O ( ) K S O ( ) + 4 2 2 4 a q a q s

Q12:

Write the reduction half-equation, including state symbols, for the conversion of solid H g C l 2 2 to liquid mercury in water.

  • A H g C l ( ) + 4 e 2 H g ( ) + C l ( ) 2 2 2 s l a q
  • B H g ( ) + e H g ( ) + a q l
  • C 2 C l ( ) + 2 e C l ( ) 2 a q a q
  • D H g C l ( ) + 2 e 2 H g ( ) + 2 C l ( ) 2 2 s l a q
  • E H g ( ) + 2 e H g ( ) 2 + a q l