Concentrated hydrochloric acid is a 38% solution of hcl in water and has a density of 1.18g/ml. How many milliliters of concentrated hydrochloric acid are needed to prepare 500ml of a 1:200 hcl solution?

My calculation
500ml x 1:200 =2.5 1:200 means 1gm/200ml
2.5 x 36.5 = 91.25
91.25/0.38=240.13
240.13/1.18 = 204ml This is my answer. I am not sure. Pls helps me .

dude that's very messed up

solution:-
first calculate the molarity from % concentration and take volume to be 1L
==>
d=m/v
m=d*v
m=1000ml*1.18g/ml=1180g.
molarity=(1180/36.5)/1L=32.32M
using c1v1=c2v2
v1=c2v2/c1
v1=((1/200)*500)/32.32=0.077ml

To find the number of milliliters of concentrated hydrochloric acid needed to prepare a 1:200 HCl solution, you have to follow these steps:

1. Calculate the amount of HCl needed for the desired concentration:
500 ml x (1/200) = 2.5 ml
This tells you that you need 2.5 ml of HCl for a 1:200 HCl solution.

2. Convert the volume of HCl to grams using the density of the concentrated hydrochloric acid:
Density = mass/volume
rearranging the equation, mass = density x volume
mass = 1.18 g/ml x 2.5 ml = 2.95 g
This means you need 2.95 grams of concentrated HCl for a 1:200 HCl solution.

3. Determine the amount of concentrated hydrochloric acid solution needed:
Concentration = 38% = 38 g/100 ml
Using the equation, concentration = mass of solute/volume of solution,
Rearranging the equation, volume of solution = mass of solute/concentration.
volume of solution = 2.95 g / (38 g/100 ml) = 7.76 ml

Therefore, you would need approximately 7.76 ml of the concentrated hydrochloric acid to prepare 500 ml of a 1:200 HCl solution.