Question

we wish to determine the mass of baso₄ formed when 200. ml of 0.10 m bacl₂ reacts with excess na₂so₄ according to the equation below. bacl₂(aq) + na₂so₄(aq) → baso₄(s) + 2nacl(aq) in the previous step, you determined 0.020 mol bacl₂ reacts. the molar mass of baso₄ is 233.39 g/mol. what mass of baso₄ forms during the reaction?

Explanation:

Step1: Determine mole ratio

From the reaction equation \( \text{BaCl}_2(\text{aq}) + \text{Na}_2\text{SO}_4(\text{aq})
ightarrow \text{BaSO}_4(\text{s}) + 2\text{NaCl}(\text{aq}) \), the mole ratio of \( \text{BaCl}_2 \) to \( \text{BaSO}_4 \) is \( 1:1 \). So moles of \( \text{BaSO}_4 \) = moles of \( \text{BaCl}_2 \) = \( 0.020 \, \text{mol} \).

Step2: Calculate mass of \( \text{BaSO}_4 \)

Use the formula \( \text{mass} = \text{moles} \times \text{molar mass} \). Molar mass of \( \text{BaSO}_4 \) is \( 233.39 \, \text{g/mol} \), moles = \( 0.020 \, \text{mol} \). So mass = \( 0.020 \, \text{mol} \times 233.39 \, \text{g/mol} = 4.6678 \, \text{g} \approx 4.7 \, \text{g} \) (or keep more decimals as needed).

Answer:

The mass of \( \text{BaSO}_4 \) formed is \( \boldsymbol{4.67 \, \text{g}} \) (or \( 4.7 \, \text{g} \), depending on significant figures; precise calculation gives \( 0.020 \times 233.39 = 4.6678 \approx 4.67 \, \text{g} \))