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3 years ago

Calculate the mass, in grams, of the solvent present in a 32.2% solution that contains 14.7 g of NaBr.

Chemistry

1 answer:

emmasim [6.3K]3 years ago

4 0

Answer:

32g

Explanation:

We have to remember that for percent (w/w) concentration we usually write;

Percent concentration= mass of solute/mass of solution ×100

Since mass of solute= 14.7 g and percent concentration = 32.2%

Then

Mass of solution= mass of solute × 100/ percent concentration

Mass of solution= 14.7 ×100/32.2

Mass of solution= 46.7 g

Since mass of solution = mass of solute + mass of solvent

Mass of solute= 14.7 g

Mass of solution = 46.7g

Mass of solvent = 46.7g -14.7g = 32g

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Answer: The identity of the unknown acid is butanoic acid or ascorbic acid.

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$\text{Molarity of the solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (in L)}}$

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Volume of solution = 39.55 mL

Putting values in above equation, we get:

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1 mole of NaOH reacts with 1 mole of HX

So, moles of monoprotic acid = 0.0225 moles

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$2NaOH+H_2X\rightarrow 2NaX+2H_2O$

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Putting values in above equation, we get:

$\text{Moles of butanoic acid}=\frac{2.002g}{88g/mol}=0.02275mol$

For L-tartaric acid:

Mass of L-tartaric acid = 2.002 g

Molar mass of L-tartaric acid = 150 g/mol

Putting values in above equation, we get:

$\text{Moles of L-tartaric acid}=\frac{2.002g}{150g/mol}=0.0133mol$

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Mass of ascorbic acid = 2.002 g

Molar mass of ascorbic acid = 176 g/mol

Putting values in above equation, we get:

$\text{Moles of ascorbic acid}=\frac{2.002g}{176g/mol}=0.01137mol$

As, the number of moles of butanoic acid and ascorbic acid is equal to the number of moles of acid getting neutralized.

Hence, the identity of the unknown acid is butanoic acid or ascorbic acid.

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