A student has 600.0 mL of a 0.30M solution of HNO3. How much water must she add in order to make it a 0.15 M solution? Be careful how this question is answered.
half the concentration means twice the volume.
so, add another 600.0 mL of H2O
a solution is prepared by dissolving 22.0g of NaOH in 117.0g of water. The NaOH solution has a density of 1.15 g/mL. what is the Molarity(M) of the solution.
To solve this problem, we need to use the formula for dilution:
(C1)(V1) = (C2)(V2)
where:
C1 is the initial concentration of the solution (0.30 M),
V1 is the initial volume of the solution (600.0 mL),
C2 is the final desired concentration (0.15 M), and
V2 is the final volume of the solution we want to find.
First, let's rearrange the formula to solve for V2:
V2 = (C1)(V1) / C2
Substituting the given values into the formula, we get:
V2 = (0.30 M)(600.0 mL) / 0.15 M
Now, let's calculate the final volume of the solution:
V2 = 1800 mL
So, the student needs to add 1800 mL of water to the 600.0 mL solution in order to make it a 0.15 M solution.