Suppose you wanted to produce 1.17 L of a 3.41 M aqueous solution of H2SO4.
How many grams of solute are needed to make this solution? (H2SO4)
To determine the number of grams of solute (H2SO4) needed to make the solution, we need to use the molarity (M) and the volume (V) of the solution. The formula to calculate the amount of solute is as follows:
Amount of solute (in moles) = Molarity (in moles per liter) × Volume of solution (in liters)
First, let's convert the volume of the solution from liters to milliliters since the molarity is given in moles per liter:
Volume of solution = 1.17 L × 1000 mL/L = 1170 mL
Next, rearrange the formula to solve for the moles of solute:
Amount of solute (in moles) = Molarity (in moles per liter) × Volume of solution (in liters)
Now substitute the given values into the equation:
Amount of solute = 3.41 mol/L × 1.17 L = 3.9877 moles
Finally, we can convert the moles of solute to grams using the molar mass of H2SO4. The molecular mass of H2SO4 is calculated as follows:
H2 = 2(1.008) = 2.016 g/mol
S = 32.07 g/mol
O4 = 4(16.00) = 64.00 g/mol
Total molecular mass of H2SO4 = 2.016 + 32.07 + 64.00 = 98.086 g/mol
To calculate the grams of solute, multiply the moles by the molar mass:
Grams of solute = 3.9877 moles × 98.086 g/mol = 391.786 grams
Therefore, you would need approximately 391.786 grams of H2SO4 to produce 1.17 L of a 3.41 M aqueous solution.