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Worksheet: Henderson–Hasselbalch Equation

Q1:

What concentration of N a F is required to make [ H O ] 3 + = 2 . 5 × 1 0 4 in a 0.320 M solution of H F ? 𝐾 a of hydrofluoric acid is 3 . 5 × 1 0 4 .

Q2:

Consider the equilibrium

What is [ O H ] in a solution of 0 . 1 2 5 M C H N H 3 2 and 0 . 1 3 0 M C H N H C l 3 3 at 2 5 C ?

  • A 2 . 2 × 1 0 5 M
  • B 4 . 6 × 1 0 4 M
  • C 8 . 4 × 1 0 5 M
  • D 4 . 2 × 1 0 4 M
  • E 9 . 7 × 1 0 6 M

Q3:

To 2 significant figures, what mass of N H C l 4 must be added to 0.650 L of a 0.120 M solution of N H 3 to give a buffer solution with a pH of 9.08? Assume a negligible change in volume as the solid is added. The 𝐾 b of N H 3 is 1 . 8 × 1 0 5 .

Q4:

A 1.00 L aqueous buffer solution is prepared from 0 . 2 0 m o l N H 3 and 0 . 4 0 m o l N H N O 4 3 . The 𝐾 b of N H 3 is 1 . 8 × 1 0 5 and the self-ionization constant of water, 𝐾 w , is 1 . 0 × 1 0 1 4 . Calculate to 1 decimal place the pH of the buffer solution.

Q5:

What concentration of N H N O 4 3 is required to make [ O H ] = 1 . 0 × 1 0 5 in a 0.200 M solution of N H 3 ? 𝐾 b of N H 3 is 1 . 8 × 1 0 5 .

  • A 0.14 M
  • B 0.52 M
  • C 1.6 M
  • D 0.36 M
  • E 0.58 M

Q6:

Consider the equilibrium

What is [ O H ] in a solution of 1 . 3 5 M N H 3 and 0 . 8 2 M N H N O 4 3 ?

  • A 9 . 1 × 1 0 M
  • B 1 . 1 × 1 0 M
  • C 3 . 4 × 1 0 M
  • D 3 . 0 × 1 0 M
  • E 7 . 2 × 1 0 M

Q7:

Consider the equilibrium

What is [ H O ] 3 + in a solution of 0 . 0 6 5 M H N O 2 and 0 . 0 4 0 M N a N O 2 ?

  • A 2 . 8 × 1 0
  • B 4 . 5 × 1 0
  • C 1 . 7 × 1 0
  • D 7 . 3 × 1 0
  • E 1 . 1 × 1 0