Question

What is the pH of nitric acid?

Answer 1

Hint: We know that Nitric acid (\[HN{O_3}\]), otherwise called water fortis (Latin for "solid water") and soul of niter, is a profoundly destructive mineral acid. The unadulterated compound is dull, yet more seasoned examples will in general obtain a yellow cast because of decay into oxides of nitrogen and water. Most industrially accessible nitric acid has a grouping of \[68\% \] in water. At the point when the solution contains over \[86\% \] \[HN{O_3}\], it is alluded to as seething nitric acid. Contingent upon the measure of nitrogen dioxide present, seething nitric acid is additionally portrayed as red smoldering nitric acid at focuses above\[86\% \], or white raging nitric acid at fixations above \[95\% \].

Complete answer:
For a \[70\% \]solution of \[HN{O_3}\] at \[1.513g/ml\] thickness you have:
One liter of \[70\% \]\[HN{O_3}\]solution\[ = 1513g\].
Out of that:
\[0.700 \times 1513 = 1059.1 = \] Grams of unadulterated \[HN{O_3}\] per liter of \[70\% \]solution.
The molar mass of \[HN{O_3}\] is \[63.1\] g/mole which thusly implies:
\[\dfrac{{1059.1}}{{63.1}} = 16.78M\]
So our molarity is $16.78$ 16.78 for this fixation.
\[ - {\text{ }}log\left[ {16.78} \right] = - 1.22\]
Typically \[HN{O_3}\] concentrated is around \[68\% - 70\% \] however can go higher (fumans acid). Generally you can recollect that \[16M\] \[HN{O_3}\] is \[68\% \] with a \[1.2\] pH.

Note:
Economically accessible nitric acid is an azeotrope with water at a centralization of \[68\% \] \[HN{O_3}\]. This arrangement has a bubbling temperature of \[120.5^\circ C\] at \[1\] atm. It is known as "concentrated nitric acid". Unadulterated concentrated nitric acid is a vapid fluid at room temperature. Nitric acid is the essential reagent utilized for nitration – the expansion of a nitro bunch, commonly to a neutral atom. While some subsequent nitro compounds are stun and thermally-touchy explosives, a couple are adequately steady to be utilized in weapons and destruction, while others are even more steady and utilized as shades in inks and colors. Nitric acid is additionally regularly utilized as a solid oxidizing specialist.