Question
How much of each of the following substances would you add to water to prepare 1.90 L of a 0.15 M solution?
(a) H2SO4 from "concentrated" (18 M) sulfuric acid
mL
(b) HCl from "concentrated" (12 M) reagent
mL
(c) NiCl2 from the salt NiCl2ยท6 H2O
g
(d) HNO3 from "concentrated" (16 M) reagent
mL
(e) sodium carbonate from the pure solid
g
If u explained how to do one of them I should be able to do the rest. Thanks!
(a) H2SO4 from "concentrated" (18 M) sulfuric acid
mL
(b) HCl from "concentrated" (12 M) reagent
mL
(c) NiCl2 from the salt NiCl2ยท6 H2O
g
(d) HNO3 from "concentrated" (16 M) reagent
mL
(e) sodium carbonate from the pure solid
g
If u explained how to do one of them I should be able to do the rest. Thanks!
Answers
DrBob222
For solutions use the dilution formula of mL1 x M1 = mL2 x M2
For solids, calculate how many moles you need which is mols = M x L = 0.15 x 1.90 = ?
Then mols = grams/molar mass. You know mols and you have molar mass, solvel for grams.
Note that c wants Nicl2 but weighs NiCl2.6H2O. Since 1 mol NiCl2 is contained in 1 mol NiCl2.6H2O, use molar mass NiCl2.6H2O for this problem.
For solids, calculate how many moles you need which is mols = M x L = 0.15 x 1.90 = ?
Then mols = grams/molar mass. You know mols and you have molar mass, solvel for grams.
Note that c wants Nicl2 but weighs NiCl2.6H2O. Since 1 mol NiCl2 is contained in 1 mol NiCl2.6H2O, use molar mass NiCl2.6H2O for this problem.