What is the volume of the solution that would result by diluting 80.00 ml of 9.13×10−2 m naoh to a concentration of 1.60×10−2 m ?

The equation that we will use to solve this question is:
M1*V1 = M2*V2
where:
M1 is the initial concentration = 9.13*10^-2 M
V1 is the initial volume = 80 ml
M2 is the final concentration = 1.6*10^-2 M
V2 in the final volume that we need to find

Substitute with the values given in the equation to calculate the final volume as follows:
(9.13*10^-2*80) = (1.6*10^-2) * V2
V2 = 456.5 ml

456.5 ml When we dilute the solution, the total number of moles of NaOH won't change. And since the number of moles is volume multiplied by molarity, we can create the following equality. 80.00 * 9.13x10^-2 = V * 1.60x10^-2 Now solve for V 80.00 * 9.13x10^-2 = V * 1.60x10^-2 7.304 = V * 1.60x10^-2 456.5 = V So you need to dilute the 80.00 ml of solution to 456.5 ml in order to reach the desired molarity.

I’m pretty sure it’s false i’m not sure