What is the molarity of a solution that contains 0.00372 moles hydrochloric acid in $2.39 \times 10^{2}$ $2.39 times 10^2$ liters of solution?

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What is the molarity of a solution that contains 0.00372 moles hydrochloric acid in $2.39 \times 10^{2}$ $2.39 times 10^2$ liters of solution?

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Answer 1 · 2017-05-17T01:19:01

$1.56 \times 10^{- 5} M$ $1.56xx10^-5 M"$

Explanation:

To find the molarity of this solution, we have to use the equation below:
![https://www.bing.com/images/search?view=detailV2&ccid=xdOyDgVa&id=81912BA1AAF426EB0252A2EDCBDD4DDA43CD1CA6&thid=OIP.xdOyDgVaJhHGXUoFSo8lhwEsA6&q=molarity+equation&simid=607989739330404602&selectedIndex=46&ajaxhist=0]( useruploads.socratic.org )

Let's list our known and unknown values:

$Knowns:$ $color(magenta)"Knowns:"$
- Moles of solute (0.00372 mol)
- Volume of solution (239 L)

$Unknowns:$ $color(brown)"Unknowns:"$
- Molarity of Solution M or $\frac{mol}{L}$ $"mol"/"L"$

Since we know the moles of solute and volume of solution, all we have to do is divide the moles of solute by the volume of solution to obtain the molarity:

Molarity = $\frac{0.00372 mol}{239L}$ $"0.00372 mol"/"239L"$

$Molarity$ $color(red) "Molarity"$ = $1.56 \times 10^{- 5} M$ $1.56xx10^-5 M"$

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What is the molarity of a solution that contains 0.00372 moles hydrochloric acid in $2.39 \times 10^{2}$ $2.39 times 10^2$ liters of solution?

1 Answer

Explanation:

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What is the molarity of a solution that contains 0.00372 moles hydrochloric acid in $2.39 \times 10^{2}$ $2.39 times 10^2$ liters of solution?