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JEE Mains · Chemistry · STD 11 - 6.1. Equilibrium - 1 (chemical Equilibrium)

The number of moles of \(\mathrm{NH}_{3}\), that must be added to \(2 \,\mathrm{~L}\) of \(0.80\, \mathrm{M}\, \mathrm{AgNO}_{3}\) in order to reduce the concentration of \(\mathrm{Ag}^{+}\)ions to \(5.0 \times 10^{-8}\, \mathrm{M}\left(\mathrm{K}_{\text {formation }}\right.\) for \(\left.\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}=1.0 \times 10^{8}\right)\) is ...... . (Nearest integer) [Assume no volume change on adding \(\mathrm{NH}_{3}\) ]

  1. A \(16\)
  2. B \(5\)
  3. C \(4\)
  4. D \(2\)
Verified Solution

Answer & Solution

Correct Answer

(C) \(4\)

Step-by-step Solution

Detailed explanation

Let moles added \(=\mathrm{a}\) \(\mathrm{Ag}_{(\mathrm{ag} .)}^{+}+2 \mathrm{NH}_{3(\mathrm{ag} .)} \rightleftharpoons \mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2(\mathrm{aq} .)}^{+}\) \(t=0 \quad \quad 0.8 \quad\quad\quad \left(\frac{a}{2}\right)\)…
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