It is desired to prepare 4.0 M nitric acid from the available acid solution of strength 1.4 M & 6.8 M respectively. If the total volume of the 4.0 M nitric acid required to be prepared is 4 #dm^3#, calculate the volume of the 2 acid solutions to be mixed?
First we find the total moles of
Let volume of the 1.4M solution =
Let volume of the 6.8M solution =
So we can write:
and since the total volume =
These are called simultaneous equations. There are 2 equations and 2 unknowns which we can easily solve:
We can then substitute this for
The idea behind this problem is that you need to use two equations, one that describes the number of moles needed for the target solution, and one that describes the total volume of the target solution.
The target solution must have a concentration of 4.0 M and a volume of 4 L (
Now, let's label the volume of the 1.4-M solution
The total volume of the solution must be 4 L, so you know that
Use the molarities and volumes of the stock solutions to find a relationship between the number of moles of nitric acid each solution adds to the total.
This is your second equation
Use this value in equation
This means that
I rounded the answer to two sig figs, despite the fact that you only gave one sig fig for the volume of the target solution.