You are a workstudy for the chemistry department. Your supervisor has just asked you to prepare 500mL of 3M HCl for tomorrow's undergraduate experiment. In the stockroom explorer, you will find a cabinet called "Stock Solutions". Open this cabinet to find a 2.0L bottle labeled "11.6M HCl". The concentration of the HCl is 11.6M. Please prepare a flask containing 500 ml of a 3 M (+/- 0.005M) solution and relabel it with its precise molarity. Note that you must use realistic transfer mode, a buret, and a volumetric flask for this problem.
As a reminder, to calculate the volume needed to make a solution of a given molarity, you may use the following formula:
C1V1 = C2V2
C[mol/l], v[mL]
C[mol/l] X v/1000 [L] = CV/1000 [mol]
11.6M HCI c2=3M V2= 500 mL
C1=11.6 M V1(mL)
the answer is Volume of HCl used 500ml
129.31 ml
500mL of 3M HCl contains 1.5 moles of HCl
so 129.31 mL of the 11.6 M acid is needed
acid is added to water (NOT vice versa)
using a volumetric cylinder, add the necessary acid to 350 ml of water
... then add more water to make the 500 mL of solution required
2.25
use the following formula:
C1V1 = C2V2
11.6M HCI
c2=3M
V2= 500 mL
v1=129.31
C1=11.6 M V1(mL)
the answer is 2.25 ml
what is the percentage error % error = (experimental concentration – 3.0 M) / 3.0 M * 100, in absolute value.
one of the people answered and said it is 129.31 ml is that the correct answer