To what volume should you dilute 30mL of a 12.0 M H2SO4 solution to obtain a 0.170 M H2SO4 solution?

M1 x V2 = M2 x V2

0.03L* 12 = 0.170 * VmL

V = 2.1L

First, convert your mL to L: 22.5 mL x 1L/1000mL = 0.0225 L H2SO4 answer next, be certain what share moles of H2SO4 you have on your unique answer: 11 mol/L x 0.0225 L = 0.2475 mol H2SO4 This tells you which you have 0.2475 mol H2SO4 on your answer. finally, you already know which you fairly choose the terrific molarity to be 0.a hundred and sixty mol/L, so which you would be able to desire to multiply the quantity of H2SO4 you have from the previous step via the inverse of the molarity you go with (so your contraptions artwork out precise). 0.2475 mol x 1L/0.160mol = a million.fifty 4 L you need an entire quantity of a million.fifty 4 liters.

Dilution problems are readily solved using

M1V1 = M2V2

M1 = initial molarity of acid = 12.0 M

V1 = initial volume of acid = 30 mL

M2 = molarity of diluted acid = 0.170 M

V2 = volume of diluted acid = ?

(12.0 M)(30 mL) = (0.170 M)(V2)

V2 = (12.0) M)(30 mL) / (0.170 M) = 2100 mL = 2.1 L