Question #fe604

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Question #fe604

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Answer 1 · 2017-03-03T23:03:24

$0.336 moles$ $"0.336 moles"$

Explanation:

The trick here is to realize that magnesium chloride is soluble in water, which implies that it dissociates completely to produce magnesium cations and chloride anions.

${MgCl}_{2 (a q)} \to {Mg}_{(a q)}^{2 +} + 2 {Cl}_{(a q)}^{-}$ $"MgCl"_ (color(red)(2)(aq)) -> "Mg"_ ((aq))^(2+) + color(red)(2)"Cl"_ ((aq))^(-)$

Notice that every $1$ $1$ mole of magnesium chloride that dissolves in water produces

one mole of magnesium cations, $1 \times {Mg}^{2 +}$ $1 xx "Mg"^(2+)$

two moles of chloride anions, $2 \times {Cl}^{-}$ $color(red)(2) xx "Cl"^(-)$

This tells you that for every mole of magnesium chloride that you dissolve in water, you get

${1 mole Mg}^{2 +} + 2 . {moles Cl}^{-} = 3 moles ions$ $"1 mole Mg"^(2+) + color(red)(2)color(white)(.)"moles Cl"^(-) = "3 moles ions"$

in the resulting solution. In your case, $0.112$ $0.112$ moles of magnesium chloride will dissociate to produce

$0.112 color(red)(cancel(color(black)("moles MgCl"_2))) * "3 moles ions"/(1color(red)(cancel(color(black)("mole MgCl"_2)))) = color(darkgreen)(ul(color(black)("0.336 moles ions")))$

The answer is rounded to three sig figs.

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Question #fe604

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