0.275gAgNO3 is dissolved in 500mL of solution.
a. What is the molarity of this solution.
b. If 10.0 mL of this solution are transferred to a flask and diluted to 500mL, what is the concentration of the resulting solution?
c. If 10.0mL of the solution in (b) are transferred to a flask and diluted to 250mL, what is the concentration of the resulting solution?
I got the molarity = .00162moleAgNO3 / .5L = .00324
I do not know how to do concentrations. I know it's the amount of solute / amount of solvent or solution but I do not know how to determine these. Can you please explain this to me? Thanks
a is right.
b and c. There is more than one way to do these. The easiest, I think, is to see what the factor is; i.e., you are diluting 10 mL to 500 so the new concn is
0.0324 x (10/500) = ?
Then c is answer from a x (10/250) = ?
Another way is to use the definition of molarity or M = mols/L.
How many mols do you have in the 10 mL of part a? That's mols = M x L.
Then the molarity of that solution in 500 mL is mols/0.5 L = ? Actually the numbers inserted are exactly the same but the thought process is different.
Sure! To calculate concentration, you need to know the amount of solute (the substance being dissolved) and the amount of solvent or solution in which it is dissolved.
a. Molarity is defined as the number of moles of solute per liter of solution. In this case, you have 0.275 grams of AgNO3 dissolved in 500 mL of solution. To calculate the molarity, you need to convert the mass of AgNO3 to moles and the volume of the solution to liters.
First, you need to convert grams to moles. The molar mass of AgNO3 is 169.87 g/mol. So, to convert 0.275 grams of AgNO3 to moles, you divide the mass by the molar mass:
0.275 g / 169.87 g/mol = 0.00162 mol
Next, you need to convert the volume of the solution to liters. There are 1000 mL in 1 L, so 500 mL is 0.5 L.
Now you can calculate the molarity:
Molarity = moles of solute / volume of solution in liters
Molarity = 0.00162 mol / 0.5 L = 0.00324 M
b. In part (b), 10.0 mL of the solution from part (a) is transferred to a flask and diluted to 500 mL. To find the concentration of the resulting solution, you can use the equation:
M1V1 = M2V2
In this case, M1 is the molarity of the original solution, V1 is the volume of the original solution taken (10 mL), M2 is the molarity of the resulting solution, and V2 is the volume of the resulting solution (500 mL).
Rearranging the equation to solve for M2, we have:
M2 = (M1 * V1) / V2
Substituting the given values:
M2 = (0.00324 M * 10 mL) / 500 mL
M2 = 0.0000648 M
So, the concentration of the resulting solution is 0.0000648 M.
c. For part (c), 10.0 mL of the resulting solution from part (b) is transferred to a flask and diluted to 250 mL. You can use the same equation as before:
M1V1 = M2V2
In this case, M1 is the molarity of the solution from part (b) (0.0000648 M), V1 is the volume of the solution taken (10 mL), M2 is the molarity of the resulting solution, and V2 is the volume of the resulting solution (250 mL).
Again, rearranging the equation to solve for M2:
M2 = (M1 * V1) / V2
Substituting the given values:
M2 = (0.0000648 M * 10 mL) / 250 mL
M2 = 0.000002592 M
So, the concentration of the resulting solution in part (c) is 0.000002592 M.