What's the pH of a solution of $1.5 M H N O_{3}$ $1.5M HNO_3$ ?

Question

What's the pH of a solution of $1.5 M H N O_{3}$ $1.5M HNO_3$ ?

1 Answer

Impact of this question

1239 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2018-02-11T22:07:04

$p H = - 0.18$ $pH=-0.18$

Explanation:

By definition, $p H = - {log}_{10} [H_{3} O^{+}]$ $pH=-log_10[H_3O^+]$ ..

and here... $H N O_{3} (a q) + H_{2} O (l) \to H_{3} O^{+} + N O_{3}^{-}$ $HNO_3(aq) + H_2O(l) rarr H_3O^+ +NO_3^(-)$

....the equilibrium LIES strongly to the right....and we presume that the solution is stoichiometric in $H_{3} O^{+}$ $H_3O^+$ , i.e. $1.50 \cdot m o l \cdot L^{- 1}$ $1.50*mol*L^-1$

And so $p H = - {log}_{10} (1.50) = - (0.176) = - 0.18$ $pH=-log_10(1.50)=-(0.176)=-0.18$

Science

Math

Humanities

... and beyond

What's the pH of a solution of $1.5 M H N O_{3}$ $1.5M HNO_3$ ?