Home
Class 11
CHEMISTRY
a. Calculate [Ag^(o+)] in a solution of ...

a. Calculate `[Ag^(o+)]` in a solution of `[Ag^(o+)]` in a solution of `[Ag(NH_(3))_(2)^(o+)]` prepared by adding `1.0 xx 10^(-3)mol AgNO_(3)` to `1.0L of 1.0M NH_(3)` solution `K_(f) Ag(NH_(3))_(2)^(o+) = 10^(8)`.
b. Calculate `[Ag^(o+)]` which is in equilibrium with `0.15M [Ag(NH_(3))_(2)]^(o+)` and `1.5 NH_(3)`.

Text Solution

Verified by Experts

The correct Answer is:
A, B
i.Since `K_(f)` is so large, most of `Ag^(o+)` will form complex ions.
`{:("Initial mol"),("Reacted"),("At equilibrium")]{:(Ag^(o+)+,2NH_(3)hArr,Ag(NH_(3))_(2)^(o+),,,),(10^(-3),0.1,0,,),(-x,-2x,0,,),(10^(-3)-x~~10^(-3),0.1-2x,10^(-3)-x~~10^(-3),,),(,0.1-2(10^(-3)),,,),(,~~0.098,,,):}`
`K_(f) =([Ag(NH_(3))_(2)^(o+)])/([Ag^(o+)][NH_(3)]^(2))`
`10^(8) = (10^(-3))/((x)(0.098)^(2)) :. x = [Ag^(o+)] = 1 xx 10^(-9)M`
ii. `10^(8) = (0.15)/((x)(1.5)^(2)) :. x = [Ag^(o+)] = 7 xx 10^(-10)M`.
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    CENGAGE CHEMISTRY|Exercise Exercises Subjective (Weak Acid And Weak Bases)|15 Videos

  • IONIC EQUILIBRIUM

    CENGAGE CHEMISTRY|Exercise Exercises Subjective (Buffer Solutions)|2 Videos

  • IONIC EQUILIBRIUM

    CENGAGE CHEMISTRY|Exercise Ex 8.4|39 Videos

  • HYDROGEN, WATER AND HYDROGEN PEROXIDE

    CENGAGE CHEMISTRY|Exercise Subjective Archive (Subjective)|3 Videos

  • ISOMERISM

    CENGAGE CHEMISTRY|Exercise Assertion-Reasoning Type|1 Videos

Similar Questions

Explore conceptually related problems

The hybridization of Ag in the linear complex [Ag(NH_(3))_(2)]^(+) is

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) .

Calculate [OH^(-)] in 0.20M solution of NH_(3) , if K_(b) for NH_(3) is 1.8xx10^(-5) .

What is the concentration of Ag^(+) ion in a 1 L solution containing 0.02 mol of AgNO_(3) and 0.14 mol of NH_(3) ? For [Ag(NH_(3))_(2)]^(+), K_(I nstab)=10^(8)

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) .

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) .