## How do you make 1M sulfuric acid solution?

To prepare 1M of sulphuric acid​ we have add 54.3 ml of Sulphuric Acid.

1. The Molecular weight of is 98 g/mol.
2. Next we add 98g of conc.
3. As Acid is a liquid,density should be taken into account.
4. Density =Mass/volume.
5. Density given on the bottle of Sulphuric acid is 1.84 g/ml.

## What is the concentration of 1M sulfuric acid?

Dilutions to Make a 1 Molar Solution

Concentrated Reagent Formula Weight1 Molarity (M)
Sulfuric Acid (H2SO4) 98.073 18
Ammonium Hydroxide (NH4OH) 35.046 14.5
Sodium Hydroxide (NaOH) 39.997 19.4
Potassium Hydroxide (KOH) 56.105 11.7

How do you make 1 M 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.

### What is the molarity of 1 N H2SO4 solution?

2M
The molarity of 1N SULPHURIC ACID = 2M.

### How do you make a 1M solution?

Molar solutions To prepare a 1 M solution, slowly add 1 formula weight of compound to a clean 1-L volumetric flask half filled with distilled or deionized water. Allow the compound to dissolve completely, swirling the flask gently if necessary.

How do you make 1M orthophosphoric acid?

This solution is infinitely soluble in water or alcohol; it is soluble at 1 part in 8 of a 3:1 (v/v) ether:alcohol mixture. 2 The pH of a 0.1 N aqueous solution is approximately 1.5. 2 Approximately 67.8 mL are required to prepare 1 L of 1.0 M phosphoric acid.

## What is the concentration of nitric acid?

Commercially available nitric acid is an azeotrope with water at a concentration of 68% HNO3. This solution has a boiling temperature of 120.5 °C (249 °F) at 1 atm. It is known as “concentrated nitric acid”.

## How do you make 6M nitric acid?

For example, to make 500 mL of 6M HCl, use 250 mL of concentrated acid and slowly dilute to 500 mL with water.

How do you make 5% HNO3?

The volume of 7.14 g of concentrated HNO3 can be obtained from the density V = 7.14 g / 1.42 = 5.03 mL. If you then measure 5.03 mL of the concentrated HNO3 and dilute to 100 mL with water, you would have the required 5% solution.

### How will you prepare 1N H2SO4 from concentrated H2SO4?

If you took 6.9 mL of concentrated sulfuric acid and diluted it to 250 mL, you would have a 1 N H2SO4 solution. (Important note: Always add the acid (or base) to water, in that order. Pour slowly with constant mixing.

### Which is more concentrated 1M H2SO4 or 1N H2SO4?

1 M H2SO4 solution is more concentrated than 1 N acid solution. Since 1M solution has a greater amount of solute dissolved in it, this solution is more concentrated than 1N solution of the acid.

Why is sulfuric acid used as a nitrating agent?

Sulphuric acid is necessary as it helps in the generation of nitronium ion from nitric acid which is the actual nitrating agent. Nitronium ion is not easily generated when we use only nitric acid. What happens when sulfuric acid reacts with nitric acid?

## 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).

## What is the concentration of 70% nitric acid?

Using 70% concentrated nitric acid as an example: 70% nitric acid means that 100 grams of this acid contains 70 grams of HNO 3. The concentration is expressed at 70% wt./wt. or 70 wt. % HNO 3. Some chemists and analysts prefer to work in acid concentration units of Molarity (moles/liter).

What is the molecular formula of nitnitric acid?

Nitric acid PubChem CID 944 Structure Find Similar Structures Chemical Safety Laboratory Chemical Safety Summary (LCSS Molecular Formula HNO3 Synonyms NITRIC ACID 7697-37-2 Hydrogen nitrate A