Molecular Mass

# What is the molecular mass of nitric acid?

###### Wiki User

63.08 g/mol I got that by adding the molar mass of one atom of hydrogen, 1.01 g/mol, one atom of nitrogen, 14.07 g/mol, and 3 atoms of oxygen, 16 g/mol each.

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## Related Questions

the molar mass of nitric acid is the molar mass of nitic acid! :)

A nitric acid molecule has 1 hydrogen atom, 1 nitrogen atom and 3 oxygen atoms. Their atomic masses are 1, 14 and 16. So, the atomic mass of nitric acid is 1x1+14x1+16x3=63g.

The correct molecular equation of, calcium carbonate-CaCO3 nitric acid-HNO3

No, it is FAR TO toxic to be used as such. Nitric acid is having molecular formula HNO3

Nitric acid has the molecular formula of HNO3. With a molar mass of 63.0128 grams per mole and a density of 1.5129 grams per cubic centimeter, one gallon has a mass of 5.73 kg.

Nitric acid has molecular formula HNO3, so its elements are Hydrogen, Nitrogen and Oxygen.

The problem for nitric acid (HNO3). Molar mass would be 63.02g/mol

The molecular weight of nitric acid is 63 and it's n-factor is 1, therefore by dividing the molecular weight by n-factor, we get equivalent weight =63.

10 mL of nitric acid has a mass of 15.1 grams.

Molecular mass of sulfuric acid is 98 u. Molecular mass of potassium and nitrate ions are 39 and 62 respectively. The molar mass of potassium nitrate is 101u.

Molar mass of lauric acid is 200.32g/mol.

The molecular maass of sulfuric acid (98,08) is greater than the molecular mass of water (18).

The molecular mass of carbonate ion is 60u. Carbonic acid molecule has two protons attached to it. Therefore, its molecular mass is 62u.

Ethylenediaminetetraacetic acid, widely abbreviated as EDTA, has a molecular mass of 292.24 g/mol

Nitric acid is a strong oxidizing acid.

Molar mass of butanoic acid, CH3CH2CH2COOH, is 88.11 g.mol&minus;1

To solve this problem, we basically have 2 equations and 2 unknowns. The unknowns are the (volume of water) &amp; the (volume of 70 wt%) nitric acid to add. * This problem will assume that you are interested in making 1 L (or 1000 mL) of 5 wt% nitric acid solution. Equation 1: (volume of water) + (volume of 70 wt% nitric acid) = 1000 mL Equation 2: mass of nitric acid / [mass of water + mass of 70 wt% nitric acid solution] = 0.05 (0.05 is 5 wt%) * Remember that mass = density * volume * Remember that 70 wt% nitric acid solution mean that for 100 grams (gm) of this acid, then there's 70 grams of HNO3 * Remember that density of 70 wt% nitric acid solution is 1.413 gm/cm^3 * Remember that density of water is 1 gm/cm^3 Equation 2 is now re-written as: [(density of 70 wt% nitric acid soln)*(volume of 70 wt% nitric acid)*0.70] / [(volume water)*(1gm*cm^3) + (volume of 70 wt% nitric acid)*(1.413gm/cm^3)] = 0.05 Solving for the 2 equations gives answer to the 2 unknowns: Answer: To make 1000 mL of 5 wt% nitric acid solution, add 1) 51.63 mL of 70 wt% nitric acid solution 2) 948.37 mL of water

how to prepare 10% nitric acid from 55% nitric acid

Nitric acid is just nitric acid. At room temperature, it is a liquid.

Nitric Acid is HNO3The chemical formula for nitric acid is HNO3

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