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Calculated the minimum amount of NH(3) w...

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

A

0.5 mol

B

1.0 mol

C

1.1 mol

D

1.2 mol

Text Solution

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The correct Answer is:
D
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Knowledge Check

  • The solubility of AgSCN in 0.002 M NH_(3) is ( K_(sp) for AgSCN=1.0xx10^(-12),K_(d) for Af(NH_(3))_(2)^(+)=1.0xx10^(-8) )

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    `3xx10^(-5)M`
    B
    `4xx10^(-4)M`
    C
    `4xx10^(-5)M`
    D
    `2xx10^(-5)M`

  • The molar solubility of AgCl in 1.8 M AgNO_(3) solution is ( K_(sp) of AgCl = 1.8 xx 10^(-10) )

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    `10^(-5)`
    B
    `10^(-10)`
    C
    `1.8 xx 10^(-5)`
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    `1.8 xx 10^(-10)`

  • The solubility of AgCl in 0.1 M NaCl is ( K_(sp) of AgCl = 1.2 xx 10^(-10) )

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    `0.05 M`
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    `1.2 xx 10^(-6)`
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    `2 xx 10^(-5)`
    D
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