How do you lower your acidity pH?

1 Answer
Jul 10, 2018

Answer:

Do you not simply add an acid?

Explanation:

In water, we invoke the following equilibrium...

#2H_2O(l) rightleftharpoonsH_3O^+ + HO^-#

And we can write an equilibrium expression, to quantify this dissociation.......

#underbrace(K_w=[HO^-][H_3O^+]=10^-14)_"specified under standard conditions of 298 K and near 1 atm"#

And we take #log_10# OF BOTH SIDES....

#log_10K_w=log_10[HO^-]+log_10[H_3O^+]=log_(10)10^-14#

But #log_(10)10^-14=-14#

And so #+14=underbrace(-log_10[H_3O^+])_"pH by definition"underbrace(-log_10[HO^-])_"pOH by definition"#

And thus our working relationship...#14=pH+pOH#

And thus if we gots #0.5*mol*L^-1# #HCl(aq)#, we gots #[H_3O^+]=0.50*mol*L^-1#...#pH=-log_10(0.50)=-(-0.301)=+0.301#..

And so #pOH=14-0.301=13.7#...

Conc. #HCl(aq)# is #10.6*mol*L^-1# out of the bottle. What is #pH# here?