Final answer:
There are 1.25 moles of ammonia in 0.250 L of a 5.00 M solution. If this solution is diluted to 1.000 L, the resulting solution will have a molarity of 1.25 M.
Step-by-step explanation:
The question asks how many moles of ammonia are in a 0.250 L of a 5.00 M aqueous ammonia solution and what would be the molarity of the solution if it were diluted to 1.000 L.
To find the moles of ammonia in the initial 0.250 L of the 5.00 M solution, we use the molarity equation:
Molarity (M) = moles of solute / volume of solution in liters
By rearranging this equation, we get:
moles of ammonia = Molarity (M) × volume of solution (L)
So, moles of ammonia = 5.00 M × 0.250 L = 1.25 moles
Now, when the solution is diluted to 1.000 L, according to the dilution equation:
M1V1 = M2V2
Where M1 and V1 are the initial molarity and volume, and M2 and V2 are the final molarity and volume. Using the information given:
M1 = 5.00 M
V1 = 0.250 L
V2 = 1.000 L
We need to find M2.
5.00 M × 0.250 L = M2 × 1.000 L
Therefore, M2 = (5.00 M × 0.250 L) / 1.000 L = 1.25 M