Worksheet: Stability Constants

In this worksheet, we will practice calculating formation constants for Lewis acid–base adducts based on their concentrations.

Q1:

The 𝐾 f value of [ Z n ( C N ) ] 4 2 is 2 . 1 × 1 0 . What is the equilibrium concentration of Z n 2 + in a solution with initial concentrations [ Z n ] = 0 . 1 5 0 M 2 + and [ C N ] = 3 . 0 0 M ?

  • A 2 . 2 × 1 0 M
  • B 7 . 4 × 1 0 M
  • C 3 . 0 × 1 0 M
  • D 4 . 8 × 1 0 M
  • E 9 . 8 × 1 0 M

Q2:

The formation constant, 𝐾 f , of [ F e ( C N ) ] 6 3 is 2 . 0 × 1 0 . What is the equilibrium concentration of F e 3 + when 0.0888 moles of K [ F e ( C N ) ] 3 6 are added to 0.100 L of a 1 . 0 0 × 1 0 M N a C N solution?

  • A 7 . 0 × 1 0 M
  • B 5 . 5 × 1 0 M
  • C 5 . 0 × 1 0 M
  • D 4 . 4 × 1 0 M
  • E 4 . 4 × 1 0 M

Q3:

What is the C o 2 + equilibrium concentration when 0.080 moles of [ C o ( N H ) ] ( N O ) 3 6 3 2 is added to 1.00 L of a solution with 0.025 M N H 3 ? Take 𝐾 = 1 . 3 × 1 0 f 3 6 2 + [ C o ( N H ) ] .

Q4:

What is the equilibrium concentration of C u 2 + in a solution initially with 0 . 0 5 0 M C u 2 + and 1 . 0 0 M N H 3 ? Take 𝐾 = 1 . 7 × 1 0 f 3 4 2 + [ C u ( N H ) ] .

  • A 1 . 8 × 1 0 M
  • B 5 . 9 × 1 0 M
  • C 7 . 2 × 1 0 M
  • D 6 . 2 × 1 0 M
  • E 3 . 7 × 1 0 M

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