How many mLs of 18.0 M H2SO4 must be added to 100mL H2O to give soln of 5.00M H2SO4?
I don't know how to set this up or solve, need some help.
- 7 years agoFavorite Answer
Seems like a trick question!!!!!
Volumes ARE NOT ADDITIVE, but assuming that they were, how many mLs of 18.0M H2SO4 must be ADDED to 100mL of H2O to give a solution of 5.00M H2SO4?
Use the following relationship:
Subtract 0.2778V1 from both sides of the equation to isolate V1's and mL's on opposite sides of the equation.
How many moles does 38.5mL of 18M H2SO4 contain?
38.5mL=38.5 x 10^-3L
moles=18M*38.5 x 10^-3L=0.6923 moles of H2SO4
However, if you meant how many mLs of 18M H2SO4 do you need to make a 100mL solution of 5.00M H2SO4 solution, then use the following relationship:
Solve for V1
Add 50mL of H2O followed by 27.8mL of 18M acid. Fill the rest of volumetric flask with H2O until the bottom of the meniscus touches the line and shake throughly.
- westlingLv 44 years ago
The response of SO3 with H2O produces a mist of H2SO4 which corrodes the containers as it is rather reactive . The response is violent and can exit of control.The mist is hard to isolate.The 2nd replacement procedure which is used more almost always is cheaper and more efficient.Additionally the acid can be diluted to the preferred awareness within the process.
- KennyBLv 77 years ago
M1V1 = M2V2
M1 = 5.00 M
V1 = 0.100 L
M2 = 18.0 M
solve for V2
V2 = M1V1/M2 = 5.00 * 0.100 / 18.0 = 0.0278 L or 27.8 mL