Home
Class 11
CHEMISTRY
The number of moles of NH(3), that must ...

The number of moles of `NH_(3)`, that must be added to 2L of 0.80M `AgNO_(3)` in order to reduce the concentration of `Ag^(+)` ions to `5.0xx10^(-8)M` (`K_("formation")` for `[Ag(NH_(3))_(2)]^(+)=1.0xx10^(8)`) is ______________.(Nearest integer)
[Assume no volume change on adding `NH_(3)`]

Text Solution

Verified by Experts

The correct Answer is:
4
Let no. Moles of `NH_(3)` added = x
`Ag^(+)(aq) + 2NH_(3)(aq) `K_(eq) = ([[Ag(NH_(3))_(2)]^(+)])/([Ag^(+)][NH_(3)]^(2))`
`x/2 - 1.6 = 0.4`
`x = 4`
Promotional Banner

Similar Questions

Explore conceptually related problems

How many moles of NH_(3) must be added to 1.0L of 0.75M AgNO_(3) in order to reduce the [Ag^(o+)] to 5.0 xx 10^(-8)M. K_(f) Ag (NH_(3))_(2)^(o+) = 1 xx 10^(8) .

How many moles of NH_(3) must be added to 1 litre of 0.1 M AgNO_(3) solution to reduce Ag^(+) concentration to 2xx10^(-7) " M "K_(d) [Ag (NH_(3))_(2)^(+)] = 6.8 xx10^(-8) .

1 mole of AgNO_(3) is added to 10 litre of 1 M NH_(3) . What is the concentration of Ag(NH_(3))^(+) in solution? [Given : For Ag(NH_(3))_(2)^(+),K_(f_(1))=2.0xx10^(3),K_(f_(2))=10^(3) ]

Calculated the minimum amount of Nh_(3) which must be added to 1.0L of solution in order to dissolve 0.1mol AgC1 by forming [Ag(NH_(3))_(2)]^(o+)? K_(sp) of AgC1 = 1 xx 10^(-10), K_(f) (NH_(3))_(2)^(o+) = 1 xx 10^(8) .

Calculate how much AgBR could dissolves in 1.0L of 0.4M NH_(3). K_(f) Ag(NH_(3))_(2)^(o+) = 1.0 xx 10^(8) .

What is the molar solubility of AgCl(s) in 0.1 M NH_(3)(aq)?K_(sp)(AgCl)=1.8xx10^(-10), K_(f)[Ag(NH_(3))_(2)]^(+)=1.6xx10^(7).