What mass of nitric acid is present in 5000mL, 1.24 molar solution?. Created by azraelknightsschneid. Chemistry

]Step 1: Calculate the number of moles of solute.Note that the volume of solution must be expressed in liters (L) and one molar (M) solution is equal to one mole per liter (mol/L).Note that 5000 mL = 5.00 LFinal Step: Calculate the mass of solute.Note that the molar mass of nitric acid is 63.02 g/mol.Hence, the mass of nitric acid present in 5000 mL of 1.24 molar solution is 391 g.#CarryOnLearning.

What mass of nitric acid is present in 5000mL, 1.24 molar solution?...

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azraelknightsschneid @azraelknightsschneid

August 2022 1 6 Report

What mass of nitric acid is present in 5000mL, 1.24 molar solution?

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Tokamak

$\tt{\huge{\red{Solution:}}}$ ]

Step 1: Calculate the number of moles of solute.

Note that the volume of solution must be expressed in liters (L) and one molar (M) solution is equal to one mole per liter (mol/L).

Note that 5000 mL = 5.00 L

$\begin{aligned} \text{moles of solute} & = \text{molarity} \times \text{volume of solution} \\ & = 1.24 \: M \times \text{5.00 L} \\ & = \text{1.24 mol/L} \times \text{5.00 L} \\ & = \text{6.20 mol} \end{aligned}$

Final Step: Calculate the mass of solute.

Note that the molar mass of nitric acid is 63.02 g/mol.

$\begin{aligned} \text{mass of solute} & = \text{moles of solute} \times \text{molar mass of solute} \\ & = \text{6.20 mol} \times \text{63.02 g/mol} \\ & = \boxed{\text{391 g}} \end{aligned}$

Hence, the mass of nitric acid present in 5000 mL of 1.24 molar solution is 391 g.

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