Consider the following equilibrium:
Ag + 1aq2 + Cl-1aq2 ∆ AgCl1s2...

Question

Consider the following equilibrium:
Ag + 1aq2 + Cl-1aq2 ∆ AgCl1s2
Use Le Châtelier’s principle to predict how the amount of solid silver chloride will change when the equilibrium is disturbed by: (c) Adding NO3, which reacts with Ag + to form the com- plex ion Ag1NH322+

Accepted Answer

Hello everyone in this problem. We're using le principle to determine the change in the amount of Zn C. L. When O. H minus is added to the solution to produce the complex ion here. So our chemical reaction then, since we're just basing it off of this equation here, So we're given that we have our Z. N. Two plus which is a chris dive reacts with H minus which is also Aquarius and it yields a complex iron C. N. O. H. 42 minus. And to bounce this reaction out we see that we have four um of these old age is so we can go ahead and put a coefficient of four on the left side. All right. And this complex sion is also Aquarius. Alright so when O. H. Which is a story material as you can see here, his attitude equation the amount of ZN two plus will decrease. So the reaction will have to shift to the left to produce this. Alright, let's go ahead and put this in writing. So according two left sharply A's principal when O. H. Is Adan the amount of our other agents, so ZN two plus will decrease. So the reaction I just simplify to our X shifts to the left. So basically what this means is that the amount of our complex ion. So that's or rather it's going to raise this or rather talking about the amount of Z. N. C. L. Two we'll go ahead and decrease. So this right here is going to be my final answer for this problem

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