The pOH is the negative log of the OH- concentration. Thus, pOH = -log 2.0x10^-2pOH = 1.699 = 1.7
pH =2.4
H+ = 10^-2.4 = 0.00398107171
OH- = 1X10^-14/H+
OH- = 2.51188643 x 10^-12
Much like calculating pH, you can calculate pOH. pOH = -log[OH-]
After that pH + pOH = 14. All you need to do is subtract and that will give the pH.
pH + pOH = 14.0 pH = 6.2 means pOH = 7.8 [OH-] = 10^-pOH = 10^-7.8 = 1.6 x 10^-8 M
pH=8
pH is -log[H+] and can be found using pH meter.
The higher the pH, the greater the concentration of Hydroxide (OH-) ions. So, the solution with the pH of 9 is your answer.
HCl is a strong acid, so we assume that it completely breaks up into ions in solution. HCl ----> H+ & Cl- if we have 0.01m of HCl, it will give 0.01m of H+ and 0.01m Cl- pH = -log [H+] pH = -log 0.01 pH = 2
Depends on the pH, at low pH (below pH 7), the H+ ion concentration is greater, and high pH the OH- ion concentration is greater
pH=8
The pH is the negative log of [H+].
pH is -log[H+] and can be found using pH meter.
[OH-] = 3.31 log[OH-] = pOH = .51982 14-pOH = pH = 13.48
The concentration of H+ or OH-.
The higher the pH, the greater the concentration of Hydroxide (OH-) ions. So, the solution with the pH of 9 is your answer.
HCl is a strong acid, so we assume that it completely breaks up into ions in solution. HCl ----> H+ & Cl- if we have 0.01m of HCl, it will give 0.01m of H+ and 0.01m Cl- pH = -log [H+] pH = -log 0.01 pH = 2
little amount concentration of OH-...must afect the pH of this solution......so first u must calculate the concentration of oH-......& u must aply this fomula to culculate pOH(-log(oh-)......then pH+pOh is equal to 14 if temparature is 25 digree.....
the concentration of OH ions in solutions
Adding a base will make the pH go up (increasing of OH- ions concentration).
A solution with a pH greater than 7
Depends on the pH, at low pH (below pH 7), the H+ ion concentration is greater, and high pH the OH- ion concentration is greater