Molarity of hydrogen solution equals 2.3 X 10^-4 -log(2.3 X 10^-4) = 3.6 pH
2
- log(2.3 X 10 -12 ) = 11.6 pH -----------------very little H + concentration in this solution.
-log(9.40 X 10^-4) = 3 pH
solution with [OH-] = 2.5 x 10-9 , A solution with [H+] = 1.2 x 10-4, A solution with pH = 4.5
100 times. (10^2)
pH = 6.0 at 25 oC when water equilibrium is taken into account correctly.
2.5 x 10-2
OH - A base. - log(1.5 X 10 -6 M) 14 - 5.8 = 8.2 pH =======
the water is more alkaline than a soution with a ph of 10
100,000 times more acidic
The presence of an acid lowers the pH of the solution in water.
its 7!
The pH is under 7.
The pH of water increase.
...that solution is alkaline or basic.
The pH of a solution is defined as -log10[H+]. Thus a solution with a hydrogen ion concentration of 10-5M has a pH of 5. [H+] = 10-5 pH = -log[H+] pH = - log [10-5] pH = 5