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NEETChemistryIonic Equilibrium

Arrange the solubility of AgCl in the following four different solvents in decreasing order: I. 0.1 M AgNO ₃ II. 0.1 M NaCl III. 0.1 M BaCl ₂ IV. Pure water

Options

  1. AIV > I = II > III
  2. BIV > I = II = III
  3. CIII > I = II > IV
  4. DIV > I > II > III

Correct answer

A. IV > I = II > III

Step-by-step solution

The solubility of a sparingly soluble salt like AgCl is inversely proportional to the concentration of the common ion due to the common ion effect. In pure water (IV), there is no common ion effect, so the solubility is maximum. In 0.1 M AgNO ₃ (I), the common ion is Ag ^+ and its concentration is 0.1 M . In 0.1 M NaCl (II), the common ion is Cl ^- and its concentration is 0.1 M . In 0.1 M BaCl ₂ (III), the common ion is Cl ^- . Since one mole of BaCl ₂ provides two moles of Cl ^- , the concentration is [ Cl ^-] =

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