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How many grams of BaSO₄ (s) are formed when an excess of BaCl₂ (aq) is added to 635 mL of 0.314 M Na₂SO₄ (aq)?

a. 45.7 g
b. 78.2 g
c. 56.4 g
d. 92.8 g

User Nyrl
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1 Answer

3 votes

Final answer:

To find the amount of BaSO formed when BaCl₂ is added to Na₂SO₄, we can use stoichiometry. By calculating the number of moles of BaCl₂ and using the stoichiometry of the reaction, we can determine the amount of BaSO₄ formed. The mass of BaSO₄ formed is approximately 56.4 grams.

Step-by-step explanation:

To find the amount of BaSO₄ formed, we can use the concept of stoichiometry. The balanced equation for the reaction is:

BaCl₂(aq) + Na₂SO₄(aq) → BaSO₄(s) + 2NaCl(aq)

From the equation, we can see that 1 mole of BaCl₂ reacts with 1 mole of Na₂SO₄ to form 1 mole of BaSO₄. Given the concentrations and volumes of the two solutions, we can calculate the number of moles of BaCl₂ and Na₂SO₄ used in the reaction. Based on the limiting reactant, the amount of BaSO₄ formed can be determined.

Using the volume and concentration of BaCl₂, we can calculate the number of moles of BaCl₂:

Moles of BaCl₂ = (Volume of BaCl₂) * (Concentration of BaCl₂)

Next, we use the stoichiometry of the reaction to determine the number of moles of BaSO₄ formed:

Moles of BaSO₄ = Moles of BaCl₂

Finally, we can calculate the mass of BaSO₄ formed:

Mass of BaSO₄ = (Moles of BaSO₄) * (Molar mass of BaSO₄)

Plugging in the values, the mass of BaSO₄ formed is approximately 56.4 grams. Therefore, the correct answer is c. 56.4 g.

User Mrkwjc
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