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Phantasy [73]
3 years ago
7

A solution contains an unknown mass of dissolved barium ions. When sodium sulfate is added to the solution, a white precipitate

forms. The precipitate is filtered and dried and then found to have a mass of 236 mg. What mass of barium was in the original solution? (Assume that all of the barium was precipitated out of solution by the reaction.)
Chemistry
1 answer:
AVprozaik [17]3 years ago
4 0

Answer:

0.1388 g

Explanation:

The mass of BaSO_4 obtained on precipitation = 236 mg

1 mg = 0.001 g

Thus, Mass of BaSO_4 = 0.236 g

Molar mass of BaSO_4 = 233.43 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

Moles= \frac{0.236\ g}{233.43\ g/mol}

Moles of BaSO_4 = 0.001011 moles

According to the reaction,

Ba^{2+}+SO_4{2-}\rightarrow BaSO_4

Thus, moles of barium = 0.001011 moles

Molar mass of barium = 137.327 g/mol

Thus, Mass = Moles * Molar mass = 0.001011*137.327 g = 0.1388 g

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<h3>The answer is 8.29 %</h3>

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