JEE MAIN - Chemistry (2021 - 27th August Morning Shift - No. 21)
The number of moles 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 $$\times$$ 10$$-$$8 M (Kformation for [Ag(NH3)2]+ = 1.0 $$\times$$ 108) is ____________. (Nearest integer)
[Assume no volume change on adding NH3]
[Assume no volume change on adding NH3]
Answer
4
Explanation
Let moles added = a
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$${{0.8} \over {(5 \times {{10}^{ - 8}})\left( {{a \over 2} - 1.6} \right)}} = {10^8}$$
$$\Rightarrow$$ $${{a \over 2}}$$ $$-$$ 1.6 = 0.4 $$\Rightarrow$$ a = 4
$${{0.8} \over {(5 \times {{10}^{ - 8}})\left( {{a \over 2} - 1.6} \right)}} = {10^8}$$
$$\Rightarrow$$ $${{a \over 2}}$$ $$-$$ 1.6 = 0.4 $$\Rightarrow$$ a = 4
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