1) A 200.0 ML solution of 1.3 x 10 -3M AgNO3 is mixed with 100mL of a 4.5 x 10-5

Question

1) A 200.0 ML solution of 1.3 x 10 -3M AgNO3 is mixed with 100mL of a 4.5 x 10-5M Na2S solution. Assume that both of these are completely soluble. Given Ksp for AgS(s) = 1.6x10^-49 .
a) Write the reaction showing the precipitate which might form in this mixture. include states of matter
b) Calculate Qsp for the above concentrations
c) State whether or not a precipitate will form. explain how you know. 1) A 200.0 ML solution of 1.3 x 10 -3M AgNO3 is mixed with 100mL of a 4.5 x 10-5M Na2S solution. Assume that both of these are completely soluble. Given Ksp for AgS(s) = 1.6x10^-49 .
a) Write the reaction showing the precipitate which might form in this mixture. include states of matter
b) Calculate Qsp for the above concentrations
c) State whether or not a precipitate will form. explain how you know.
a) Write the reaction showing the precipitate which might form in this mixture. include states of matter
b) Calculate Qsp for the above concentrations
c) State whether or not a precipitate will form. explain how you know.

Explanation / Answer

moles of AgNO3 = 200 x 1.3 x 10^-3 / 1000 = 2.6 x 10^-4

moles of Na2S = 100 x 4.5 x 10^-5 / 1000 = 4.5 x 10^-6

a)

AgNO3 (aq) + Na2S(aq) -----------------> Ag2S (s) + NaNO3 (aq)

b)

Ag2S   --------------> 2 Ag+     + S^-2

                                 2.6 x 10^-3 4.5 x 10^-5

Qsp = [Ag+]^2[S-2]

        = (2.6 x 10^-3)^2 x (4.5 x 10^-5)

        = 3.04 x 10^-10

Qsp = 3.04 x 10^-10

c)

here Qsp is greater than Ksp .

Qsp > Ksp . so precipitate will form

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