Final answer:
To find the volume of solution needed for 0.42 grams of silver nitrate, the molarity of the solution is required. With an assumed molarity of 1.00 M, Lisa would pour out 2.47 mL of the solution to get the desired mass of silver nitrate.
Step-by-step explanation:
To determine how much solution Lisa should pour out to get 0.42 grams of silver nitrate, one would need the concentration of the silver nitrate solution she is using. Without this information, it's impossible to provide an exact answer. However, if we assume a hypothetical concentration, we could use the formula Molarity (M) = moles of solute / liters of solution to calculate the volume required to get 0.42 grams of the substance.
For example, if the solution has a molarity of 1.00 M (silver nitrate solution of 1.00 molar), first convert the mass of silver nitrate to moles (given that the molar mass of AgNO3 is approximately 169.87 g/mol). Then divide the moles of solute by the molarity to find the volume in liters.
Calculating volume for the silver nitrate can be demonstrated as follows:
- Calculate moles: 0.42 g / 169.87 g/mol = 0.00247 mol of AgNO3.
- Calculate volume: 0.00247 mol / 1.00 M = 0.00247 L of the solution.
- Convert to milliliters: 0.00247 L x 1000 mL/L = 2.47 mL.
Lisa would need to pour out 2.47 mL of a 1.00 M silver nitrate solution to obtain 0.42 grams of silver nitrate.