1.20 L of a solution that is 15.0 % of Pb(NO3)2 by mass (the density of the solution is 1.16 g/mL), starting with solid solute. how would you prepare this?

You want 1.2L or 1200 mL.

mass = volume x density = 1200 x 1.15 = approx 1400 grams. Remember to redo these calculations with more accuracy than my estimates.
To make 15% solution you need 15 g Pb(NO3)2 in 100 g solution. So for 1400 g solution you will need
15 g x 1400/100 = approx 210 g Pb(NO3)2.
Weigh out approx 210 g Pb(NO3)2 and add enough water to make a total of approx 1400 g.

Well, preparing this solution requires a little bit of math and a little bit of clown magic.

First, let's calculate how much lead nitrate (Pb(NO3)2) we need. We want a solution that is 15% Pb(NO3)2 by mass, and we know we want a total of 1.20 L of solution. So, we can calculate the mass of Pb(NO3)2 needed as:

Mass of Pb(NO3)2 = 15% of 1.20 L = 0.15 * 1.20 L = 0.18 L

Now, it's important to note that the density of the solution is 1.16 g/mL. Since we need to convert liters to grams, we can use this density to help us out. One liter of the solution will weigh 1.16 * 1000 g = 1160 g.

So, if we need 0.18 L of Pb(NO3)2, it would weigh 0.18 * 1160 g = 208.8 g.

Now, all that's left is to mix exactly 208.8 grams of solid Pb(NO3)2 with enough water to make 1.20 L of solution. And voila, your 15% Pb(NO3)2 solution is ready! Just be careful not to spill any, or it might rain clowns!

To prepare a solution of 1.20 L that is 15.0% Pb(NO3)2 by mass, you can follow these steps:

1. Determine the mass of Pb(NO3)2 needed:
Mass of Pb(NO3)2 = (15.0%)(1.20 L)(1.16 g/mL)

2. Calculate the volume of Pb(NO3)2 solution needed:
Volume of Pb(NO3)2 solution = (Mass of Pb(NO3)2)/(Density of Pb(NO3)2 solution)

3. Dissolve the calculated mass of Pb(NO3)2 in the calculated volume of solution. Add distilled water if necessary to achieve the final volume of 1.20 L.

It is important to note that these calculations are based on the assumption that the density of the Pb(NO3)2 solution is the same as water. If the density is different, you would need to adjust the calculations accordingly.

To prepare a 1.20 L solution of Pb(NO3)2 with a 15.0% concentration by mass, you can follow these steps:

Step 1: Calculate the mass of Pb(NO3)2 needed
To determine the mass of Pb(NO3)2 required, you need to know the desired volume of the solution and its concentration. In this case, the volume is given as 1.20 L, and the concentration is 15.0%.
Mass = Volume x Concentration
Mass = 1.20 L x 15.0% = 0.18 L

Step 2: Find the number of moles of Pb(NO3)2
To find the number of moles of Pb(NO3)2, you need to know the molar mass of Pb(NO3)2, which can be calculated by adding the atomic masses of lead (Pb), nitrogen (N), and oxygen (O).
Molar mass of Pb(NO3)2 = (1 x atomic mass of Pb) + (2 x atomic mass of N) + (6 x atomic mass of O)
Molar mass of Pb(NO3)2 = (1 x 207.2 g/mol) + (2 x 14.0 g/mol) + (6 x 16.0 g/mol) = 331.2 g/mol

Next, convert the mass of Pb(NO3)2 to moles using the molar mass:
Moles = Mass / Molar mass
Moles = 0.18 g / 331.2 g/mol = 0.000543 mol

Step 3: Convert moles to grams
To convert moles to grams, multiply the number of moles by the molar mass.
Mass = Moles x Molar mass
Mass = 0.000543 mol * 331.2 g/mol = 0.1796 g

Step 4: Calculate the volume of the solution
The density of the solution is given as 1.16 g/mL. Since the mass of the solute (Pb(NO3)2) is known, divide its mass by the density to find the volume of the solution.
Volume of solution = Mass of solute / Density of solution
Volume of solution = 0.1796 g / 1.16 g/mL ≈ 0.155 L

Step 5: Prepare the solution
Take the calculated mass of Pb(NO3)2 (0.1796 g) and dissolve it in a container. Gradually add distilled water while stirring until the solution reaches a final volume of 1.20 L.

Note: It is important to accurately measure both the mass of the solute and the volume of the solution to ensure the desired concentration is achieved. Additionally, be cautious when handling chemicals and always follow proper safety procedures.