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2 years ago

What is the molarity of solution that is 5.50 percentage by mass oxalic acid and has a density of 1.024 g/ml

Chemistry

1 answer:

Y_Kistochka [10]2 years ago

6 0

Answer:

0.6257 M is the molarity of solution that is 5.50 percentage by mass oxalic acid.

Explanation:

Mass percentage of oxalic acid = 5.50%

This means that in 100 grams of solution there are 5.50 grams of oxalic acid.

Mass of solution , m = 100

Volume of the solution = V

Density of the solution = d = 1.024 g/mL

$V=\frac{m}{d}=\frac{100 g}{1.024 g/mL}=97.66mL$

V = 97.66 mL = 0.09766 L

(1 mL = 0.001 L)

Moles of oxalic acid = $\frac{5.50 g}{90 g/mol}=0.06111 mol$

$Molarity=\frac{\text{Moles of solute}}{\text{Volume of solution in L}}$

The molarity of the solution :

$=\frac{0.06111 mol}{0.09766 L}=0.6257M$

0.6257 M is the molarity of solution that is 5.50 percentage by mass oxalic acid.

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1 year ago

Starting with the stock solution of 6.0 M, how many milliliters of 6.0 M sulfuric acid are needed to make 450 mL of 1.2 M soluti

Lina20 [59]

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Explanation:

To calculate the molarity of the diluted solution, we use the equation:

$M_1V_1=M_2V_2$

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$M_1\text{ and }V_1$ are the molarity and volume of the stock sulfuric acid solution

$M_2\text{ and }V_2$ are the molarity and volume of diluted sulfuric acid solution

We are given:

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2 years ago

Which row in the table shows how many electrons there could be in the outer shell of an atom of V?

Amanda [17]

Answer:

Explanation:

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