If 1 mol L of 2.0 mol L hydrochloric acid is diluted to form a solution with concentration 0.2 mol L,
A. What is the final volume?
B. how much water must be added to the original acid?
Use C1V1= C2V2, thanks in advance
To find the final volume and the amount of water to be added, we can use the formula C1V1 = C2V2, also known as the dilution formula. Let's break it down step by step:
A. Final Volume (V2):
Given:
C1 = 2.0 mol/L (initial concentration)
V1 = 1 mol/L (initial volume)
C2 = 0.2 mol/L (final concentration)
Using the dilution formula: C1V1 = C2V2
Plugging in the values: (2.0 mol/L)(1 L) = (0.2 mol/L)(V2)
Now we can solve for V2:
2.0 L = (0.2 mol/L)(V2)
V2 = 2.0 L / 0.2 mol/L
V2 = 10 L
So, the final volume (V2) is 10 liters.
B. Amount of Water to be Added:
To determine how much water needs to be added, we subtract the initial volume (V1) from the final volume (V2).
Water Volume = V2 - V1
Water Volume = 10 L - 1 L
Water Volume = 9 L
Therefore, 9 liters of water must be added to the original 1 liter of hydrochloric acid to obtain a final solution with a concentration of 0.2 mol/L.