Calculate #[H_3O^+]# for a solution that has #pH = 1.76#?

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A well-explained, easy-to-follow and neat answer will be highly appreciated because I am still not quite sure how we can find the concentration of #H_3O^+# when we are given the #pH# of the solution. Please also understand that I'm not using this website to teach (cos somebody accused me of using Socratic to cheat). Thanks in advance!

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Answer 1 · 2018-02-09T05:02:53

#H_3O^+=0.01737800828M~~0.02M#

#pH# is calculated using the expression

#pH=-log[H_3O^+]#

#:.H_3O^+=10^(-pH)#

#:.H_3O^+=10^-1.76~~0.02M#

So, there exists #0.02# moles of hydronium #(H_3O^+)# ions per liter of the solution.

In fact, the solution's concentration is around #0.02M#.