molecular weight of sulphuric acid=98g/mol. solution that contains 1 mole of compound in 1L solvent. take 1L volumetric flask and add 500ml of water and add 98g of sulphuric acid in flask. we get 1M OF sulphuric acid.
How much does sulfuric acid cost?
Sulphuric Acid 98% at Rs 15/kg | Sulphuric Acid | ID: 13075049212.
What is m of H2SO4?
98.08 grams of H2SO4 is equal to 1 mole. Therefore, we can say that 1 liter of Sulfuric acid contains 17.822 moles or in other words molarity of 95% (w/w) Sulfuric acid is equal to 17.822 M.
What is the pH of 98% sulfuric acid?
Products
| Physicochemical Information | |
|---|---|
| Density | 1.80 – 1.84 g/cm3 |
| Melting Point | 10.31 °C |
| pH value | 0.3 (49 g/l, H₂O, 25 °C) |
| Vapor pressure | 1.33 hPa (145.8 °C) |
How do you make 1M nitric acid?
1L contains 15.6 moles, therefore 1 mole is contained within = 1L / 15.6 moles. Add 64.1mL, or 90.4g, of SEASTAR™’s Nitric Acid to water up to 1L to make a 1 Molar Solution of Nitric Acid.
Is sulfuric acid expensive?
Over 100 billion lb (45 billion kg) of sulfuric acid are produced each year. It is also one of the least expensive acids, which makes it a favorite of industries around the world.
Why is sulfuric acid so cheap?
All Answers (3) Contact the local chemical suppliers in your area for a quote. Sulfuric acid is traded internationally in huge quantities so it is surprisingly cheap.
How do you make H2SO4 formula?
H₂SO₄
Sulfuric acid/Formula
What is the pH of a 1m sulfuric acid solution?
The pH of 1M sulfuric acid is 0. for a pH of 4, a 0.0001M solution. You do not need a base, this can be done simply by diluting with water. 8 clever moves when you have $1,000 in the bank.
How can I prepare 1m sulphuric acid from concentrated sulphuric acid?
To prepare 1M sulphuric acid from concentrated sulphuric acid: First consider the molecular weight of H2SO4 = 98 g/mol, so you have to add 98g of conc. acid and make up to 1 liter of water (as pointed out at the 4thpoint).
Is sulphuric acid a monobasic acid?
This means that at 1.0 M sulphuric acid behaves more or less as a monobasic acid (releasing just one proton, where the pH would = 0), however if you do the same calculation for 0.001M sulphuric acid the pH calculation = 2.73, which is not far from the pH = 2.70 that full dissociation of both protons would give; i.e. at low concentrations sulphuric
What is the pH of a 5m H2SO4?
OK, so it probably is a homework question (the what is the pH of a 5M H2SO4) and yes, using the standard definition for pH (pH = -log [H+]) a diprotic acid, fully dissociated (e.g., H2SO4) at a concentration of 5 M will give 10 M H+ concentration (though perhaps a different activity) and leads to a negative pH (= -1 here).
