If a 0.01 M Mn(NO3)2 solution has an ammonia concentration of 6.0 M, should a precipitate...

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If a 0.01 M Mn(NO3)2 solution has an ammonia concentration of 6.0 M, should a precipitate...

If a 0.01 M Mn(NO3)2 solution has an ammonia concentration of 6.0 M, should a precipitate of Mn(OH)2 form? Calculate the ion product (reaction quotient) and compare it to Ksp to support your answer.

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Answer 1

Answer #1

NH3 concentration = 6.0 M

Kb = 1.8 x 10^-5

[OH-] = sqrt (Kb x C )

= sqrt (1.8 x 10^-5 x 6.0)

= 0.0104 M

Q = [Mn2+][OH-]^2

Q = (0.01 ) (0.0104)^2

ionic product = Q = 1.08 x 10^-6

Ksp of Mn(OH)2 = 4.6 x 10^-14

Q > Ksp

so precipitate will be formed

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Answer 2

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