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Lesson: Balancing Ionic Half-Equations in Acidic or Basic Conditions

Worksheet • 13 Questions

Q1:

Manganate ions ( M n O 4 2 ) react under basic aqueous conditions to produce permanganate ( M n O 4 ) and solid manganese dioxide.

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

  • A M n O ( ) + 2 H O ( ) + 2 e M n O ( ) + 4 O H ( ) 4 2 2 2 a q l s a q
  • B M n O ( ) + 2 H O ( ) + 6 e M n O ( ) + 4 O H ( ) 4 2 2 2 a q l s a q
  • C M n O ( ) + 2 H O ( ) + 4 e M n O ( ) + 4 O H ( ) 4 2 2 2 a q l s a q
  • D M n O ( ) + 4 H O ( ) + 6 e M n O ( ) + 4 O H ( ) 4 2 2 2 a q l s a q
  • E M n O ( ) + 4 H O ( ) + 2 e M n O ( ) + 8 O H ( ) 4 2 2 2 a q l s a q

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

  • A 3 M n O ( ) + 2 H O ( ) M n O ( ) + 2 M n O ( ) + 4 O H ( ) 4 2 2 2 4 a q l s a q a q
  • B 5 M n O ( ) + 6 H O ( ) 3 M n O ( ) + 2 M n O ( ) + 1 2 O H ( ) 4 2 2 2 4 a q l s a q a q
  • C 2 M n O ( ) + 2 H O ( ) M n O ( ) + M n O ( ) + 4 O H ( ) 4 2 2 2 4 a q l s a q a q
  • D 3 M n O ( ) + 4 H O ( ) 2 M n O ( ) + M n O ( ) + 8 O H ( ) 4 2 2 2 4 a q l s a q a q
  • E 5 M n O ( ) + 2 H O ( ) M n O ( ) + 4 M n O ( ) + 4 O H ( ) 4 2 2 2 4 a q l s a q a q

Q2:

Which of the following is a properly balanced half reaction under acidic conditions?

  • A C r O + 8 H + 3 H C O 2 C r + 7 H O + 6 C O 2 7 2 + 2 2 4 3 + 2 2
  • B 2 A u + 6 I 2 A u + 3 I 3 + 2
  • C 1 2 H + 5 I + I O 3 I + 6 H O + 3 2 2
  • D 3 C d + 8 H + 2 N O 3 C d + 2 N O + 8 H O + 3 2 + 2
  • E 2 F e ( O H ) + H O 2 F e ( O H ) 2 2 2 3

Q3:

Write the oxidation half-equation, including state symbols, for the conversion of chloride to chlorate(V) ions under basic aqueous conditions.

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

Q4:

When liquid bromine reacts with sulfur dioxide gas under acidic aqueous conditions, bromide and sulfate ions are produced.

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

  • A S O ( ) + 2 H O ( ) S O ( ) + 4 H ( ) + 2 e 2 2 4 2 + g l a q a q
  • B S O ( ) + H O ( ) S O ( ) + 2 H ( ) + 4 e 3 2 4 2 + g l a q a q
  • C S O ( ) + 2 H O ( ) S O ( ) + 4 H ( ) + 6 e 2 2 4 2 + g l a q a q
  • D S O ( ) + 2 H O ( ) S O ( ) + 4 H ( ) + 4 e 2 2 4 2 + g l a q a q
  • E S O ( ) + H O ( ) S O ( ) + 2 H ( ) + 2 e 3 2 4 2 + g l a q a q

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

  • A B r ( ) + S O ( ) + 2 H O ( ) 2 B r ( ) + S O ( ) + 4 H ( ) 2 2 2 4 2 + l g l a q a q a q
  • B 3 B r ( ) + 2 S O ( ) + 2 H O ( ) 6 B r ( ) + 2 S O ( ) + 4 H ( ) 2 3 2 4 2 + l g l a q a q a q
  • C 2 B r ( ) + S O ( ) + 2 H O ( ) 4 B r ( ) + S O ( ) + 4 H ( ) 2 2 2 4 2 + l g l a q a q a q
  • D 3 B r ( ) + 2 S O ( ) + 4 H O ( ) 6 B r ( ) + 2 S O ( ) + 8 H ( ) 2 2 2 4 2 + l g l a q a q a q
  • E B r ( ) + S O ( ) + H O ( ) 2 B r ( ) + S O ( ) + 2 H ( ) 2 3 2 4 2 + l g l a q a q a q

Q5:

When cyanide ions react with chlorine dioxide under acidic aqueous conditions, cyanate ( C N O ) and chloride ions are produced.

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

  • A C l O ( ) + 4 H ( ) + 5 e C l ( ) + 2 H O ( ) 2 + 2 a q a q a q l
  • B C l O ( ) + 4 H ( ) + 6 e C l ( ) + 2 H O ( ) 2 + 2 a q a q a q l
  • C C l O ( ) + 4 H ( ) + 4 e C l ( ) + 2 H O ( ) 2 + 2 a q a q a q l
  • D C l O ( ) + 2 H O ( ) + 4 e C l ( ) + 4 O H ( ) 2 2 a q l a q a q
  • E C l O ( ) + 2 H O ( ) + 6 e C l ( ) + 4 O H ( ) 2 2 a q l a q a q

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

  • A 5 C N ( ) + 2 C l O ( ) + H O ( ) 5 C N O ( ) + 2 C l ( ) + 2 H ( ) 2 2 + a q a q l a q a q a q
  • B 5 C N ( ) + C l O ( ) + 3 H O ( ) 5 C N O ( ) + C l ( ) + 6 H ( ) 2 2 + a q a q l a q a q a q
  • C C N ( ) + C l O ( ) + 2 H ( ) C N O ( ) + C l ( ) + H O ( ) 2 + 2 a q a q a q a q a q l
  • D C N ( ) + 2 C l O ( ) + 6 H ( ) C N O ( ) + 2 C l ( ) + 3 H O ( ) 2 + 2 a q a q a q a q a q l
  • E 3 C N ( ) + C l O ( ) + H O ( ) 3 C N O ( ) + C l ( ) + 2 H ( ) 2 2 + a q a q l a q a q a q

Q6:

Write the reduction half-equation, including state symbols, for the conversion of aqueous iodate(V) ions to solid elemental iodine under basic conditions.

  • A 2 I O ( ) + 6 H O ( ) + 1 0 e I ( ) + 1 2 O H ( ) 3 2 2 a q l s a q
  • B 2 I O ( ) + 4 H O ( ) + 6 e I ( ) + 8 O H ( ) 2 2 2 a q l s a q
  • C 2 I O ( ) + 1 2 H ( ) + 1 0 e I ( ) + 6 H O ( ) 3 + 2 2 a q a q s l
  • D 2 I O ( ) + 4 H O ( ) + 4 e I ( ) + 8 O H ( ) 2 2 2 2 a q l s a q
  • E 2 I O ( ) + 8 H ( ) + 4 e I ( ) + 4 H O ( ) 2 2 + 2 2 a q a q s l

Q7:

When permanganate ( M n O 4 ) ions react with nitrite ions under basic aqueous conditions, solid manganese(IV) dioxide and nitrate ions are produced.

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

  • A M n O ( ) + 2 H O ( ) + 3 e M n O ( ) + 4 O H ( ) 4 2 2 a q l s a q
  • B M n O ( ) + 4 H O ( ) + 5 e M n O ( ) + 8 O H ( ) 4 2 2 a q l s a q
  • C M n O ( ) + 2 H O ( ) + 3 e M n O ( ) + 2 O H ( ) 4 2 2 a q l s a q
  • D M n O ( ) + 2 H O ( ) + 4 e M n O ( ) + 4 O H ( ) 4 2 2 a q l s a q
  • E M n O ( ) + 4 H O ( ) + 4 e M n O ( ) + 4 O H ( ) 4 2 2 a q l s a q

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

  • A 2 M n O ( ) + 3 N O ( ) + H O ( ) 2 M n O ( ) + 3 N O ( ) + 2 O H ( ) 4 2 2 2 3 a q a q l s a q a q
  • B 3 M n O ( ) + 2 N O ( ) + 4 H O ( ) 3 M n O ( ) + 2 N O ( ) + 8 O H ( ) 4 2 2 2 3 a q a q l s a q a q
  • C M n O ( ) + 2 N O ( ) M n O ( ) + 2 N O ( ) 4 2 2 3 a q a q s a q
  • D 2 M n O ( ) + 5 N O ( ) + 2 O H ( ) 2 M n O ( ) + 5 N O ( ) + H O ( ) 4 2 2 3 2 a q a q a q s a q l
  • E M n O ( ) + 3 N O ( ) + 2 O H ( ) M n O ( ) + 3 N O ( ) + H O ( ) 4 2 2 3 2 a q a q a q s a q l

Q8:

Write the oxidation half-equation, including state symbols, for the conversion of sulfite to sulfate ions under acidic aqueous conditions.

  • A S O ( ) + H O ( ) S O ( ) + 2 H ( ) + 2 e 3 2 2 4 2 + a q l a q a q
  • B S O ( ) + 2 O H ( ) S O ( ) + H O ( ) + e 3 4 2 2 a q a q a q l
  • C S O ( ) + H O ( ) S O ( ) + 2 H ( ) + 2 e 3 2 4 + a q l a q a q
  • D S O ( ) + 2 O H ( ) S O ( ) + H O ( ) + e 3 2 4 2 2 a q a q a q l
  • E S O ( ) + 2 O H ( ) S O ( ) + H O ( ) + 2 e 3 4 2 a q a q a q l

Q9:

When tin(II) ions react with copper(II) ions in water, tin(IV) and copper(I) ions are produced.

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

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

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

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

Q10:

Under acidic aqueous conditions, the permanganate ion dissociates and forms M n 2 + and 4 molecules of water. In this reaction, how many moles of electrons are transferred per mole of permanganate ions?

Q11:

Write the oxidation half-equation, including state symbols, for the conversion of water to oxygen under acidic conditions.

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

Q12:

Write the reduction half-equation, including state symbols, for the conversion of manganate(VII) to manganese(II) ions under acidic aqueous conditions.

  • A M n O ( ) + 8 H ( ) + 5 e M n ( ) + 4 H O ( ) 4 + 2 + 2 a q a q a q l
  • B M n O ( ) + 4 H O ( ) + 7 e M n ( ) + 8 O H ( ) 4 2 2 + a q l a q a q
  • C M n O ( ) + 1 0 H ( ) + 5 e M n ( ) + 5 H O ( ) 5 3 + 2 + 2 a q a q a q l
  • D M n O ( ) + 4 H O ( ) + 3 e M n ( ) + 8 O H ( ) 4 3 2 2 + a q l a q a q
  • E M n O ( ) + 1 0 H O ( ) + 5 e M n ( ) + 2 0 O H ( ) 5 3 2 2 + a q l a q a q

Q13:

When hydrogen sulfide gas reacts with H g 2 2 + ions in solution, liquid mercury and solid elemental sulfur are produced.

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

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

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

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