Aqueous ammonia is commercially available at a concentration of 16.0 M.
Part A
How much of the concentrated solution would you use to prepare 500.0mL of a 1.30M solution?
mL1 x M1 = mL2 x M2
To determine the amount of concentrated solution required, we can use the dilution formula:
C1V1 = C2V2
Where:
C1 = initial concentration of the concentrated solution
V1 = volume of the concentrated solution used
C2 = final concentration of the diluted solution
V2 = final volume of the diluted solution
Given:
C1 = 16.0 M
C2 = 1.30 M
V2 = 500.0 mL
Now, we can plug these values into the formula and solve for V1:
C1V1 = C2V2
(16.0 M)(V1) = (1.30 M)(500.0 mL)
Next, we need to convert the final volume from milliliters to liters:
V2 = 500.0 mL = 500.0 mL * (1 L / 1000 mL) = 0.500 L
Now we can solve for V1:
(16.0 M)(V1) = (1.30 M)(0.500 L)
V1 = (1.30 M)(0.500 L) / 16.0 M
V1 ≈ 0.0406 L
Therefore, you would use approximately 0.0406 liters (or 40.6 mL) of the concentrated 16.0 M aqueous ammonia solution to prepare 500.0 mL of a 1.30 M solution.
To calculate the amount of concentrated solution needed to prepare a desired concentration, you can use the concept of dilution. Dilution is the process of adding a concentrated solution or solvent to create a solution with a lower concentration.
To solve this problem, you can use the dilution formula:
C1V1 = C2V2
Where:
C1 = concentration of the concentrated solution
V1 = volume of the concentrated solution used
C2 = desired concentration of the final solution
V2 = desired volume of the final solution
Let's plug in the values given in the problem:
C1 = 16.0 M (concentration of the concentrated solution)
V1 = ? (volume of the concentrated solution used)
C2 = 1.30 M (desired concentration of the final solution)
V2 = 500.0 mL (desired volume of the final solution)
Now rearrange the formula to solve for V1:
V1 = (C2V2) / C1
V1 = (1.30 M * 500.0 mL) / 16.0 M
V1 = 40.625 mL
Therefore, you would need to measure and use 40.625 mL of the concentrated solution to prepare 500.0 mL of a 1.30 M solution.