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Chemistry · Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes

Predict if there will be any precipitate by mixing of NaCl and 50 mL of solution

Predict if there will be any precipitate by mixing \( 50 \mathrm{mL} \) of \( 0.01 \mathrm{M} \) NaCl and 50 mL of \( 0.01 \mathrm{M} A g N O_{3} \) solution. The solubility product of \( A g C l \) is \( 1.5 \times \) \( 10^{-10} \)

  • A. since ionic product is greater than solubility product no precipitate will be formed
  • B. since ionic product is lesser than solubility product. precipitation will occur
  • C. since ionic product is greater than solubility product. precipitation will occur.
  • D. since ionic product and solubility product are same, precipitation will not occur

Step-by-step solution

After mixing, the concentrations of Ag+ and Cl- are both 0.005 M. The ionic product [Ag+][Cl-] = (0.005)(0.005) = 2.5 × 10^-5, which is greater than the solubility product (1.5 × 10^-10). Hence, precipitation occurs.
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