An aqueous solution is made 1.000 M in AgNO3 and 1.000 M in Fe(NO3)2 and allowed to come to equilibrium. What are the concentrations of the ions present when equilibrium is established

This is an incomplete question, here is a complete question.

An aqueous solution is made 1.000 M in AgNO₃ and 1.000 M in Fe(NO₃)₂ and allowed to come to equilibrium. What are the concentrations of the ions present when equilibrium is established.

; K = 2.89

Answer : The concentration of , and is, 0.565 M, 0.435 M and 0.435 M respectively.

Explanation :

The balanced chemical reaction is:

Initial:             1.000      1.000                0        0

At eqllm:       (1.000-x)   (1.000-x)           x         x

The equilibrium expression is:

Now put all the given values in this expression, we get:

x = 0.565 M and x = 1.771 M

We are neglecting value of x = 1.771 because equilibrium concentration can not be more than initial concentration.

Thus, the value of x = 0.565 M

The concentration of = x = 0.565 M

The concentration of = (1.000-x) = (1.000-0.565) = 0.435 M

The concentration of = (1.000-x) = (1.000-0.565) = 0.435 M

its mg hope this

i'm assuming that the correct answer is indeed the first one/ "a"..