Describe how you would prepare each of the following aqueous solutions: (c) 1.20 L of a solution that is 15.0% Pb(NO 3 ) 2 by mass (the density of the solution is 1.16 g/mL), starting with solid solute;

Hey everyone today, we're being asked to find the mass of toxin present in a 3. liter water sample that has 0.025% toxin by mass. So to do this, the very first thing we can do is convert our volume, Our 3.4 L in two ml. And this is because the density given for this solution is in g per milliliter. This will help us with our calculations. So 3.4 L of water Can be converted to ml by remembering that we have 1000 ml for every one liter of water. So our leaders will cancel out and we will be left with 3400 ml of water from here. Taking this value. R 30 400 ml can then be multiplied by the density 1.01 g per one millimeter. In order to yield us A math of 34, 34 g of water. So now, since we know that this value is 0.025% toxin by mass, then that means we can take this mass 3434 g and that can be multiplied by the percentage 0.025 toxin For every 100 g of the sample of the water. So our grams will cancel out and simplifying this And solving it were left to the value of 0. 85 grams of toxin. Therefore there are Or there is 0.8585 g of toxin In a 3.4 liter water sample. I hope this helps, and I look forward to seeing you on the next one.

Ch.13 - Properties of Solutions

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Brown 14th Edition

Ch.13 - Properties of Solutions

Problem 54c

Chapter 13, Problem 54c

Describe how you would prepare each of the following aqueous solutions: (c) 1.20 L of a solution that is 15.0% Pb(NO₃)₂ by mass (the density of the solution is 1.16 g/mL), starting with solid solute;

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Calculate the total mass of the solution using the volume and density. Use the formula: \( \text{mass} = \text{volume} \times \text{density} \). Convert the volume from liters to milliliters first, since the density is given in g/mL.

Determine the mass of Pb(NO3)2 required for the solution. Since the solution is 15.0% Pb(NO3)2 by mass, use the formula: \( \text{mass of Pb(NO3)}_2 = \text{total mass of solution} \times 0.15 \).

Weigh out the calculated mass of solid Pb(NO3)2 using a balance.

Calculate the mass of water needed to make the solution. Subtract the mass of Pb(NO3)2 from the total mass of the solution to find the mass of water.

Dissolve the weighed Pb(NO3)2 in the calculated mass of water. Stir the mixture until the solute is completely dissolved, ensuring the solution is homogeneous.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Mass Percent Concentration

Mass percent concentration is a way to express the concentration of a solute in a solution, calculated as the mass of the solute divided by the total mass of the solution, multiplied by 100. In this case, a 15.0% mass concentration of Pb(NO3)2 means that there are 15 grams of lead(II) nitrate for every 100 grams of the solution.

Density and Volume Relationship

Density is defined as mass per unit volume and is crucial for converting between mass and volume in solution preparation. Given the density of the solution (1.16 g/mL), you can calculate the total mass of the solution by multiplying the volume (1.20 L or 1200 mL) by the density, which helps in determining how much solute is needed.

Stoichiometry in Solution Preparation

Stoichiometry involves the calculation of reactants and products in chemical reactions, and it is essential for preparing solutions. In this context, once the mass of Pb(NO3)2 needed is determined, stoichiometric principles can be applied to ensure the correct amount of solid solute is measured and dissolved in the appropriate volume of solvent to achieve the desired concentration.

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Describe how you would prepare each of the following aqueous solutions, starting with solid KBr: (d) a 0.150 M solution of KBr that contains just enough KBr to precipitate 16.0 g of AgBr from a solution containing 0.480 mol of AgNO3.

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Textbook Question

Commercial concentrated aqueous ammonia is 28% NH₃ by mass and has a density of 0.90 g/mL. What is the molarity of this solution?

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Describe how you would prepare each of the following aqueous solutions: (c) 1.20 L of a solution that is 15.0% Pb(NO3)2 by mass (the density of the solution is 1.16 g/mL), starting with solid solute;

Verified video answer for a similar problem:

Key Concepts

Mass Percent Concentration

Density and Volume Relationship

Stoichiometry in Solution Preparation

Describe how you would prepare each of the following aqueous solutions: (c) 1.20 L of a solution that is 15.0% Pb(NO₃)₂ by mass (the density of the solution is 1.16 g/mL), starting with solid solute;