Questions: According to the following reaction, what volume of 0.305 M AgNO3 is required to react with 155.0 mL of 0.274 M Na2SO4 solution? 2 AgNO3(aq) + Na2SO4(aq) → Ag2SO 4(s) + 2 NaNO3(aq) 139 mL 345 mL 278 mL 173 mL 581 mL

According to the following reaction, what volume of 0.305 M AgNO3 is required to react with 155.0 mL of 0.274 M Na2SO4 solution?

2 AgNO3(aq) + Na2SO4(aq) → Ag2SO 4(s) + 2 NaNO3(aq)

139 mL
345 mL
278 mL
173 mL
581 mL

Transcript text: According to the following reaction, what volume of $0.305 \mathrm{M} \mathrm{AgNO}_{3}$ is required to react with 155.0 mL of $0.274 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}$ solution? \[ 2 \mathrm{AgNO}_{3}(\mathrm{aq})+\mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow \mathrm{Ag}_{2} \mathrm{SO} 4(\mathrm{~s})+2 \mathrm{NaNO}_{3}(\mathrm{aq}) \] 139 mL 345 mL 278 mL 173 mL 581 mL

Solution

Solution Steps

Step 1: Determine Moles of $\text{Na}_{2} \text{SO}_{4}$

Calculate the moles of $\text{Na}_{2} \text{SO}_{4}$ using its concentration and volume: \[ \text{Moles of } \text{Na}_{2} \text{SO}_{4} = 0.274 \, \text{M} \times 0.155 \, \text{L} = 0.04247 \, \text{mol} \]

Step 2: Use Stoichiometry to Find Moles of $\text{AgNO}_{3}$

From the balanced chemical equation, the stoichiometric ratio between $\text{AgNO}_{3}$ and $\text{Na}_{2} \text{SO}_{4}$ is 2:1. Therefore, calculate the moles of $\text{AgNO}_{3}$ needed: \[ \text{Moles of } \text{AgNO}_{3} = 2 \times 0.04247 \, \text{mol} = 0.08494 \, \text{mol} \]

Step 3: Calculate Volume of $\text{AgNO}_{3}$ Solution

Use the concentration of $\text{AgNO}_{3}$ to find the required volume: \[ \text{Volume of } \text{AgNO}_{3} = \frac{0.08494 \, \text{mol}}{0.305 \, \text{M}} = 0.278 \, \text{L} = 278 \, \text{mL} \]

Final Answer

$\boxed{278 \, \text{mL}}$

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