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A $0.125-M$ solution of $\mathrm{Mn}\left(\mathrm{NO}_{3}\right)_{2}$ is saturated with $\mathrm{H}_{2} \mathrm{S}\left(\left[\mathrm{H}_{2} \mathrm{S}\right]=0.10 \mathrm{M}\right) .$ At what pH does MnS begin to precipitate? $$\operatorname{Mn} S(s) \rightleftharpoons \operatorname{Mn}^{2+}(a q)+S^{2-}(a q) \quad K_{\mathrm{sp}}=4.3 \times 10^{-22}$$$$\mathrm{H}_{2} \mathrm{S}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons 2 \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{S}^{2-(a q)} \qquad K=1.0 \times 10^{-26}$$

3.27

Chemistry 102

Chapter 15

Equilibria of Other Reaction Classes

Chemical Equilibrium

Carolin M.

September 7, 2020

The book states an the correct solution is 7.66. Is the book wrong?

University of Central Florida

Brown University

University of Toronto

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Hello, everyone, this is Ricky. And they were working on a problem number 99. So we have to calculate the pH at which, um, magnesium, so, so far, so fied, um will begin to precipitate when it is in a solution. That ISS 0.1 to 5 Moeller minis nitrate And when it itself has a concentration point where, mother. And so we know the concentration of manganese nitrate because or of manganese? I own because making these nitrate completely, completely dissociates and in solution. All right, so I've written down the chaos pay expressions, um, for the precipitation. And if my agonies sulfide and the K expression four room, it's to us reacting with with water. And now what we're going to be doing iss solving for the sulfide. I own concentration. So let's rewrite our expression, men. Plus my apologies, I'll be sulfur or sulfide. So what? I don't know. Just went on. There is a monkey. Okay, here we go. And so sulfide ion concentrations equal to Casspi. Hope for manganese, iron concentration. Plug in chuck and we get a concentration of one point. Oh, I mean, sorry. Get a concentration of 3.44 comes into the negative 21st. Smaller. All right, now that we know are sulfur concentration, we're gonna flip down here and solve for each plus. So let's rewrite this. H plus is equal to the square root of K A times each to us. Oh, there s minus two. All right now, we can just plug in all of our values to solve for the H plus concentration. When we get 5.39 times 10 to the fourth more and some pH equals negative log each plus plug in our age plus concentration. And we get that MNS will begin to precipitate that 3.27 right up each of 3.7.

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