Which solution is the most concentrated? 2.0 mL of 10 m H_(2)SO_(4) , where H_(2)SO_(4) has a molar mass of 98g/mol 5.0 mL of 1.0 M PbSO_(4) where PbSO_(4) has a molar mass of 303g/mol 2.0 mL of 105M H_(2)O_(2) where H_(2)O_(2) has a molar mass of 34g/mol 100 mL of 10 M NaCl, where NaCl has a molar mass of 58g/mol

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Which solution is the most concentrated? 2.0 mL of 10 m H_(2)SO_(4) , where H_(2)SO_(4) has a molar mass of 98g/mol 5.0 mL of 1.0 M PbSO_(4) where PbSO_(4) has a molar mass of 303g/mol 2.0 mL of 105M H_(2)O_(2) where H_(2)O_(2) has a molar mass of 34g/mol 100 mL of 10 M NaCl, where NaCl has a molar mass of 58g/mol

Answer 1

To find the most concentrated solution, we need to calculate the number of moles of solute per unit volume of solution for each option.Let's calculate the number of moles for each solution:1. For \(10 \, \text{M} \, \text{H}_2\text{SO}_4\), we have: \[\text{Number of moles} = \frac{\text{concentration} \times \text{volume}}{\text{molar mass}} = \frac{10 \, \text{M} \times 2.0 \, \text{mL}}{98 \, \text{g/mol}} \approx 0.204 \, \text{mol}\]2. For \(1.0 \, \text{M} \, \text{PbSO}_4\), we have: \[\text{Number of moles} = \frac{\text{concentration} \times \text{volume}}{\text{molar mass}} = \frac{1.0 \, \text{M} \times 5.0 \, \text{mL}}{303 \, \text{g/mol}} \approx 0.0165 \, \text{mol}\]3. For \(10.5 \, \text{M} \, \text{H}_2\text{O}_2\), we have: \[\text{Number of moles} = \frac{\text{concentration} \times \text{volume}}{\text{molar mass}} = \frac{10.5 \, \text{M} \times 2.0 \, \text{mL}}{34 \, \text{g/mol}} \approx 6.176 \, \text{mol}\]4. For \(10 \, \text{M} \, \text{NaCl}\), we have: \[\text{Number of moles} = \frac{\text{concentration} \times \text{volume}}{\text{molar mass}} = \frac{10 \, \text{M} \times 100 \, \text{mL}}{58 \, \text{g/mol}} \approx 17.24 \, \text{mol}\]Comparing the number of moles per unit volume for each solution:1. For \(10 \, \text{M} \, \text{H}_2\text{SO}_4\), we have approximately \(0.204 \, \text{mol/mL}\).2. For \(1.0 \, \text{M} \, \text{PbSO}_4\), we have approximately \(0.0165 \, \text{mol/mL}\).3. For \(10.5 \, \text{M} \, \text{H}_2\text{O}_2\), we have approximately \(6.176 \, \text{mol/mL}\).4. For \(10 \, \text{M} \, \text{NaCl}\), we have approximately \(0.1724 \, \text{mol/mL}\).So, the most concentrated solution is the \(10.5 \, \text{M} \, \text{H}_2\text{O}_2\) solution, with a concentration of approximately \(6.176 \, \text{mol/mL}\).Therefore, the most concentrated solution is \(2.0 \, \text{mL}\) of \(10.5 \, \text{M} \text{H}_2\text{O}_2\).**Answer:** \(2.0 \, \text{mL}\) of \(10.5 \, \text{M} \text{H}_2\text{O}_2\)

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