What is the equivalent number for H2SO4?

sulfuric acid has a molar mass of 98.078(5) g mol−1, and supplies two moles of hydrogen ions per mole of sulfuric acid, so its equivalent weight is 98.078(5) g mol−1/2 eq mol−1 = 49.039(3) g eq−1.

What is the pH of 0.1 m of H2SO4?

And so 0.1⋅mol⋅L−1 is 0.2⋅mol⋅L−1 with respect to H3O+ . And thus pH=−log10(0.2)=−(−0.699)=0.699 . And on the other hand, 0.1⋅N sulfuric acid is in fact 0.05⋅mol⋅L−1 with respect to sulfuric acid….the acid STILL requires TWO equivs of base for stoichiometric equivalence.

What is equivalent weight of sulphuric acid?

49u
Sulphuric acid contains two replaceable hydrogen. Hence, the equivalent weight of sulphuric acid is 49u.

What is 2m H2SO4?

2 M sulfuric acid means that it has 2 x the molecular weight of sulfuric acid as expressed in grams is dissolved in one liter of water. So the molecular weight of sulfuric acid is 98: that’s 2 for Hydrogen, 32 for sulfur, and 4 x 16 or 64 for oxygen. Therefore you would mix 196 g.

How do you find the normality of H2SO4?

If you know the Molarity of an acid or base solution, you can easily convert it to Normality by multiplying Molarity by the number of hydrogen (or hydroxide) ions in the acid (or base). For example, a 2 M H2SO4 solution will have a Normality of 4N (2 M x 2 hydrogen ions).

What is the equivalent weight of H2SO4 in the reaction H2SO4 Nai?

The answer is 49+12.25=61.25 but I don’t know,how?

What is the difference between HCl and H2SO4?

1 normal HCl would have 1 gm-equivalent of H+ ions in one liter (equivalent to 1 M of HCl) and 1 normal H2SO4 would have 1 gm-equivalent of H+ ions in one liter (equivalent to 0.5 M of H2SO4)

How much H2SO4 is required to make 1 n solution?

For 1N we need to take 1 gram equivalent of H2SO4 i.e. 49 grams, add sufficient water to get 1000 ml dilute solution. For 0.1. N we need to take 4.9 grams of H2SO4 and make up to 1000 ml with water.

How do you calculate the equivalent mass of H2SO4 in water?

= mass of solute (in gram) ( volume of solvent in Liter) × ( equivalent mass of solute (in gram)) Hence, dissolve 0.1 g m equivalent of H 2 S O 4 in 1 Litre of water i.e. dissolve 0.1 × 98.079 2 = 4.90395 g m of H 2 S O 4 in 1 Litre of water to obtain 0.1 N H 2 S O 4 8 clever moves when you have $1,000 in the bank.

Is the normality of H2SO4 the same as molarity?

Some compounds, however, will not have the same normality as molarity, as in the case of H 2 SO 4: The normality of a 1.0 liter solution of H 2 SO 4 containing 1.0 gram-equivalent weight will be the molecular weight of H 2 SO 4 divided by the valence of H 2 SO 4: