Using V * M = constant at dilution = amount of H2SO4 [mol] in both of the solutions
V= volume [L] of the solution
M= molarity [mol/L] of the solution
So: V *18.0 = 24.9 * 0.195 gives V = ( 24.9 * 0.195 ) / 18.0 = 0.270 L
Find by multiplication how many mMol H2SO4 you will need:
0.126 (Mol/L) * 19.6 (L) = 2.470 Mol = 2470 mMol H2SO4
Divide this by the concentration H2SO4 in the concentrated acid, being: 18.0 mol/L = 18.0 mMol/mL
then you'll get:
2470 (mMol H2SO4) / 18.0 (mMol/mL) = 137.2 = 137 mL concentrated H2SO4
(X Volume)(18.4 M H2SO4) = (250 ml)(3.00 M H2SO4)
18.4X = 750
X = 40.8 milliliters concentrated H2SO4
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7n h2so4
h
You need 49,8 mL H2SO4 6,4M.
H2SO4 is sulfuric acid. So the answer is 100%
H2SO4 is a strong acid known as sulfuric acid
202.44
7n h2so4
Mix 120 g sulfuric acid with water to 1000 mL.
You need 252 g sulfuric acid.
h
You need 49,8 mL H2SO4 6,4M.
H2SO4 is sulfuric acid. So the answer is 100%
H2SO4 is a strong acid known as sulfuric acid
Yes. H2SO4 is sulfuric acid.
Yes, sulfuric acid is a molecule with the formula H2SO4
0.1 N means you have a hydronium ion concentration of 0.1 mole/L. Since sulfuric acid is a diprotic acid, you get 2 moles of ionizable protons per mole a sulfuric acid. Meaning, you only need a concentration of 0.05 M sulfuric acid to obtain 0.1 N sulfuric acid. [10 L] * [0.1 mole H+/L] * [1 mole H2SO4/2 mole H+] * [98.08 g/mole H2SO4] * [1 mL/1.84 g H2SO4] = 26.65 mL H2SO4 required to make 10 L 0.1 N H2SO4.
Molarity = moles of solute/volume of solution 0.324 M H2SO4 = moles H2SO4/500 ml 162 millimoles, or, more precisely to the question 0.162 moles H2SO4