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Lesson: Acid–Base Reaction Equations

In this lesson, we will learn how to write balanced chemical equations for acid–base reactions and how to describe common patterns of reactivity.

Worksheet • 3 Questions

Q1:

Write a balanced molecular equation for the acid-base reaction between barium hydroxide and nitric acid, including state symbols.

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

Q2:

In dilute aqueous solutions, H F acts as a weak acid. However, pure liquid H F (boiling point = 1 9 . 5 ∘ C ) is a strong acid. In liquid H F , H N O 3 acts like a base and accepts protons. The acidity of liquid H F can be increased by adding one of several inorganic fluorides that are Lewis acids and accept F – ions (i.e., B F 3 or S b F 5 ).

Give a balanced chemical equation for the reaction of H N O 3 with pure H F .

  • A H N O + H F H N O + F 3 2 3 + –
  • B H N O + H F H N O + F 3 2 3
  • C H N O + H F H F + N O 3 2 3
  • D H N O + H F H F + N O 3 2 + 3 –

Give a balanced chemical equation for the reaction of B F 3 with pure H F .

  • A B F + H F B F + H 3 4 – +
  • B B F + H F B F + H 3 4
  • C B F + H F H B F + F 3 3 + –
  • D B F + H F H B F + F 3 3

Q3:

Write a balanced molecular equation for the acid-base reaction between hydrogen hypochlorite ( H O C l ) and water, including state symbols.

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