Concentrated nitric acid is 16M. What volume of nitric acid must be diluted with distilled water to preapre 5L of 0.1M nitric acid?
To find the volume of concentrated nitric acid that needs to be diluted, we can use the equation:
M1V1 = M2V2
Here,
M1 = initial concentration of nitric acid = 16M
V1 = volume of nitric acid to be diluted (unknown)
M2 = final concentration of nitric acid = 0.1M
V2 = final volume of nitric acid = 5L
Substituting the given values into the equation, we can solve for V1:
16M x V1 = 0.1M x 5L
Divide both sides of the equation by 16M:
V1 = (0.1M x 5L) / 16M
Simplifying the equation further:
V1 = (0.1 x 5) / 16
V1 = 0.5 / 16
V1 = 0.03125 L
Therefore, you need to dilute approximately 0.03125 L (or 31.25 mL) of concentrated nitric acid with distilled water to prepare 5L of 0.1M nitric acid.
To determine the volume of concentrated nitric acid that must be diluted with water, we can use the concept of dilution formula. The dilution formula is given as:
M1V1 = M2V2
Where:
M1 = Initial concentration of the solution (in this case, the concentrated nitric acid)
V1 = Initial volume of the solution (unknown in this case)
M2 = Final concentration of the solution (0.1 M in this case)
V2 = Final volume of the solution (5 L in this case)
Let's calculate the value of V1:
M1V1 = M2V2
(16 M)(V1) = (0.1 M)(5 L)
Now, solve for V1:
V1 = (0.1 M)(5 L) / (16 M)
V1 ≈ 0.03125 L or 31.25 mL
Therefore, approximately 31.25 mL of concentrated nitric acid must be diluted with distilled water to prepare 5 L of 0.1 M nitric acid solution.