The number of miles of NH₃, that must be added to 2L of 0.80 M AgNO₃ in order to reduce the concentration of Ag⁺ions to 5.0 × 10^-8 M (K_formation for [Ag(NH₃)₂]⁺ = 1.0 × 10⁸) is_________.

(Nearest integer)

[Assume no volume change on adding NH₃]

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Answered by

Vishal Baghel | Contributor-Level 10

2 months ago

$A g^{+} (a q) + 2 N H_{3} (a q) ? A g {(N H_{3})}_{2}^{+} (a q)$

t = 00.8 M $(\frac{a}{2}) M$

0 $= \infty$ 5 × 10^-8 M $(\frac{a}{2} - 1.6) M$ 0.8M

$k_{f} = \frac{[A g {(N H_{3})}_{2}^{+}]}{[A g^{+}] {[N H_{3}]}^{2}}$

$1 0^{8} = \frac{0.8}{(5 \times 1 0^{- 8}) {(\frac{a}{2} - 1.6)}^{2}}$

$\frac{a}{2} = 2$

Concentration of NH₃ added = $\frac{a}{2} = 2 M$

Volume of solution = 2L

Moles of NH₃ added = 2 × 2 mol = 4 mol.

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The number of miles of NH₃, that must be added to 2L of 0.80 M AgNO₃ in order to reduce the concentration of Ag⁺ions to 5.0 × 10^-8 M (K_formation for [Ag(NH₃)₂]⁺ = 1.0 × 10⁸) is_________.

(Nearest integer)

[Assume no volume change on adding NH₃]

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The number of miles of NH3, that must be added to 2L of 0.80 M AgNO3 in order to reduce the concentration of Ag+ ions to 5.0 × 10-8 M (Kformation for [Ag(NH3)2]+ = 1.0 × 108) is_________. (Nearest integer) [Assume no volume change on adding NH3]

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The number of miles of NH₃, that must be added to 2L of 0.80 M AgNO₃ in order to reduce the concentration of Ag⁺ions to 5.0 × 10^-8 M (K_formation for [Ag(NH₃)₂]⁺ = 1.0 × 10⁸) is_________.

(Nearest integer)

[Assume no volume change on adding NH₃]