Question

Determine the molarity of a solution formed by dissolving 97.7 g libr in enough water to yield 750.0 ml of solution.

Answer 1

Hello!

Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 ml of solution.

We have the following data:

M (Molarity) =? (in mol / L)

m1 (mass of the solute) = 97.7 g

V (solution volume) = 750 ml → V (solution volume) = 0.75 L

MM (molar mass of LiBr)

Li = 6.941 u

Br = 79.904 u

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MM (molar mass of LiBr) = 6.941 + 79.904

MM (molar mass of LiBr) = 86.845 g/mol

Now, let's apply the data to the formula of Molarity, let's see:

`M = (m_1)/(MM*V)`

`M = (97.7)/(86.845*0.75)`

`M = (97.7)/(65.13375)`

`M = 1.49999... \to \boxed{\boxed{M \approx 1.5\:mol/L}}\:\:\:\:\:\:\bf\green{\checkmark}`

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*** Another way to solve is to find the number of moles (n1) and soon after finding the molarity (M), let's see:

`n_1 = (m_1\:(g))/(MM\:(g/mol))`

`n_1 = (97.7\:\diagup\!\!\!\!\!g)/(86.845\:\diagup\!\!\!\!\!g/mol)`

`n = 1.12499.. \to \boxed{n_1 \approx 1.125\:mol}`

`M = (n_1\:(mol))/(V\:(L))`

`M = (1.125\:mol)/(0.75\:L)`

`\boxed{\boxed{M = 1.5\:mol/L}}\:\:\:\:\:\:\bf\blue{\checkmark}`

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`\bf\purple{I\:Hope\:this\:helps,\:greetings ...\:Dexteright02!}\:\:\ddot{\smile}`

Answer 2

1.5 M.

Step-by-step explanation:

• Molarity (M) is defined as the no. of moles of solute dissolved in a 1.0 L of the solution.

M = (no. of moles of LiBr)/(Volume of the solution (L).

∵ no. of moles of LiBr = (mass/molar mass) of LiBr = (97.7 g)/(86.845 g/mol) = 1.125 mol.

Volume of the solution = 750.0 mL = 0.75 L.

∴ M = (no. of moles of luminol)/(Volume of the solution (L) = (1.125 mol)/(0.75 L) = 1.5 M.