0.02M sulphuric acid= molar mass x M x 1 litre
= 98.08 x 0.02 x 1
=1.9616ml/l
You need 49,8 mL H2SO4 6,4M.
how 2.5N H2SO4 prepared from concentrated H2SO4
The answer is 0,526 mL.
To prepare a 200ml solution of 0.5M H2SO4, you need to add 12.5ml of 8M H2SO4 and then dilute it up to 200ml. Well, this is how to calculate it, I'll go straight to the equation. use the M1V1 = M2V2 equation, M1 = 8.0 M V1 = Volume needed M2 = 0.5 M V2 = 200 ml 8.0 M x V1 = 0.5 M x 200 ml V1 = (0.5 M x 200 ml)/ 8.0 M = 12.5 ml Cheers :)
con.H2SO4 is 98%(v/v)ie 980ml/litre.or 980X1.84(specific gravity of H2So4)ie wt/litre is 1803.2Normality= wt per litre/ Eq.wtie 1803.2/49=36.8 NHence con H2So4 is 36.8 NTo prepare 5 N , It has be diluted 7.36 times with water68
You need 49,8 mL H2SO4 6,4M.
how 2.5N H2SO4 prepared from concentrated H2SO4
The answer is 0,526 mL.
To prepare a 200ml solution of 0.5M H2SO4, you need to add 12.5ml of 8M H2SO4 and then dilute it up to 200ml. Well, this is how to calculate it, I'll go straight to the equation. use the M1V1 = M2V2 equation, M1 = 8.0 M V1 = Volume needed M2 = 0.5 M V2 = 200 ml 8.0 M x V1 = 0.5 M x 200 ml V1 = (0.5 M x 200 ml)/ 8.0 M = 12.5 ml Cheers :)
con.H2SO4 is 98%(v/v)ie 980ml/litre.or 980X1.84(specific gravity of H2So4)ie wt/litre is 1803.2Normality= wt per litre/ Eq.wtie 1803.2/49=36.8 NHence con H2So4 is 36.8 NTo prepare 5 N , It has be diluted 7.36 times with water68
h
- log(0.000626 M H2SO4) = 3.2 pH -----------
4.5m H2SO4 Solushen 25%
Using V * M = constant at dilution = amount of H2SO4 [mol] in both of the solutionsV= volume [L] of the solutionM= molarity [mol/L] of the solutionSo: V *18.0 = 24.9 * 0.195 gives V = ( 24.9 * 0.195 ) / 18.0 = 0.270 L
7n h2so4
Mix 120 g sulfuric acid with water to 1000 mL.
You need 252 g sulfuric acid.