An experiment calls for you to use 100. mL of 0.91 M HNO3 solution. All you have available is a bottle of 5.00 M HNO3. How would you prepare the desired solution
Available is a 5 M/liter solution. You need 100 mL of a 0.91 M solution.
In units of moles, you need 0.91 mol/liter * 0.1 liter = 0.091 moles of HNO3
0.091 moles / (5moles/liter) = 0.0182 liters of the 5 M solution.
Take 0.0182 liters of the 5 M solution, and dilute to 100 mL = 0.1 L (add 0.1 - 0.0182 = 0.0818 L = 81.8 mL of water to this solution.
To prepare the desired solution, you can use the formula for dilution:
C1V1 = C2V2
Where:
C1 = initial concentration of the stock solution
V1 = volume of the stock solution to be used
C2 = final concentration of the desired solution
V2 = final volume of the desired solution
Let's use this formula to find out how much of the 5.00 M HNO3 solution you need to make 100. mL of 0.91 M HNO3 solution.
First, rearrange the formula to solve for V1:
V1 = (C2V2) / C1
Now, plug in the values:
V1 = (0.91 M × 0.100 L) / 5.00 M
V1 ≈ 0.0182 L or 18.2 mL
So, you would need to measure 18.2 mL of the 5.00 M HNO3 solution and then dilute it to a final volume of 100. mL with water, in order to prepare the desired solution of 0.91 M HNO3.