What is the molar concentration of nitric acid?

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

By diluting the concentration of nitric acid (and the concentration of H+). ...

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

preparation of 0.1 molar nitric acid

Nitric acid (followed by a grade or concentration description)

They are different acids. They are also different by acid strength and the concentration of them. (Vinegar is 5% acetic acid in water, while a normal concentration of 70-78% nitric acid is stronger) ...

Not necessarily or even usually. The term "one molar" refers to the concentration of the acid added and does not have anything to do with the concentration of ferrous ions. ...

Hydrochloric acid and nitric acid have comparable degrees of acidity; the strength of either acid will depend upon the concentration. ...

1) What is the initial pH of the nitric acid solution? Nitric acid is a strong acid and therefore dissociates almost completely in water. The concentration of the hydronium ions must be .2M as well. This concentration yields a pH of (4) pH = -log[H3O+] = -log(.2) = .7 ...

Lynsie Clark should know.

As adjective to concentration or mass: The molar concentration of concentrated sulfuric acid is about 18.0 (mol/L) The molar mass of H2SO4 is about 100 g (per mole) ...

HCl is a stronger acid and will dissolve more of the shell than an equivalent concentration of nitric acid. ...

The pH of an acid depends on its concentration. pH stands for the -log of the concentration of H+ ions. Nitric acid is a strong acid, so it completely dissociates in water. You can tell if an acid is strong or not by the number of Hs and Os. If it has at least 2 more Hs than Os, it is a strong acid. The chemical formula of Nitric acid is HNO3, so it is strong. Because HNO3 is a strong...

For a weak acid (or base), as the concentration increases, the % ionization/dissociation decreases. This leads to fewer ions in solution, and hence the molar conductivity decreases. ...

The principle of dilution should be used here. The procedure should be to reduce the concentration of nitric acid by 65 times. Therefore, it should be diluted with the ratio of 1:64 between 65% nitric acid and distilled water respectively. ...

pH depends on the concentration of the acid as much as the strength. As HCl is a strong monoprotic acid the pH will be equal to the negative logarithm of its molar concentration. (a 1M solution will have a pH of 0, a .1 molar solution will have a pH of 1, etc.) ...

Nitric acid (HNO3), also known as aqua fortis and spirit of nitre, is a highly corrosive and toxic strong mineral acid which is normally colorless but tends to acquire a yellow cast due to the accumulation of oxides of nitrogen if long-stored. Ordinary nitric acid has a concentration of 68%. When the solution contains more than 86% of it, it is referred to as fuming nitric acid. Depending on the amount of nitrogen dioxide present, fuming nitric acid is further characterized as white...

Gastric fluid is about 0.1 molar hydrochloric acid (0.1M HCl).

This may due to Magnesium metal has high reactivity and concentration of nitric acid is dilute, thus magnesium reacts with H+ in water/ in nitric acid to give hydrogen ...

write a equation in words to show the relation between mass concentration,molar concentration and molar mass and give a short explanation of this? ...

add 8 molar solution of nitric acid and stir it with our hand. works everytime. ...

Nitric acid is a strong oxidizing acid.

Nitric Acid is HNO3 The chemical formula for nitric acid is HNO3

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

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