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How many grams of Milk of Magnesia, $\mathrm{Mg}(\mathrm{OH})_{2}(s)(58.3 \mathrm{g} / \mathrm{mol})$ , would be soluble in 200 $\mathrm{mL}$ of water. $K_{\mathrm{sp}}=$ $7.1 \times 10^{-12} .$ Include the ionic reaction and the expression for $K_{\mathrm{sp}}$ in your answer. $\left(K_{\mathrm{w}}=1 \times 10^{-14}=\right.$ $\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\left[\mathrm{OH}^{-}\right] )$
$1.14 \times 10^{-3} g$, 10.38
Chemistry 102
Chapter 15
Equilibria of Other Reaction Classes
Chemical Equilibrium
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I've won. This is Ricky. And today we're working on problem 57. So we want to calculate the grams of milk of magnesia justice, magnesium hydroxide. Um, that would be soluble in 200 milliliters. All right, this is our disassociation of waging. Um, our initial mass for milk of magnesia is or rather, the molar masses for she ate 13 grams. Ramon. And we have a case, Pete given just 71 times 10. All right, So GSP is equal to you like museum times hydroxide squared. So we have female. A mass of magnesium. We're also giving a volume wait 200 leaders. All right, so we can now calculate the Moler saw you ability. Um So look, in case piece of one times 10 to 12 is equal to x. Times two X squared is there's twice as many eye drops that I owns. Me missing. My owns, we got that X is equal to 1.21 times 10 to the negative for, um, and X is equal to the concentration of magnesium ions. Willis's in malls, print leader. And so we want to calculate actual mass, which is soluble. So what? We're going to do is multiply first by, um So what we're gonna do first, Isn't it supplied by volume 200 meters. So now that we have moles of magnesium, I and then we wantto multiply by the molar ratio of milk of magnesia to man using my owns, which is a 1 to 1 ratio. So and then, lastly, you want to multiply by the mole Nash, so we could get the mass. And what we see is that 1.14 times 10 to the negative third grams of milk of magnesia will be dissolved.
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