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What is the poh of a solution with oh 2.0 10-2?
1.70
Is the concentration of H plus in solution given the OH equals 2.54 x 10-4?
[H+] = Kw / [OH-] = 1.0*10-14 / 2.5*10-4 = 4.0*10-11 mol/L
What is the pH of a solution withOH equals 1 10-4?
-log[1 X 10^-4 M OH(-)] = 4 14 - 4 = 10 pH ----------------
Which of these solutions are acidic a solution with OH equals 2.5 10-9 H plus equals 1.2 10 -4 H plus equals 3.4 10-8 pH equals 4.5 OH equals 1.0 10-4?
solution with [OH-] = 2.5 x 10-9 , A solution with [H+] = 1.2 x 10-4, A solution with pH = 4.5
What is the h3O concentration in 0.45 m hcn ka of hcn 4.0 10-10?
HCN + H20 => CN- + H3O+ 0.45 X X Solve for X (4.0*10^-10) = x^2/0.45M x=1.34e-5= [OH] Find pOH= -log of the above number then 14-4.87=pH= 9.13
What is the pH of a solution with a oh of 3.31 00000000 M?
[OH-] = 3.31 log[OH-] = pOH = .51982 14-pOH = pH = 13.48
OH- of a solution which has a pH equals 10.95?
pH + pOH = 14. So pOH = 14 - 10.95 = 3.05 pOH = -log[OH-] [OH-] = 8.91 x 10-4 M
If the pH of a solution is 10.7, what would the pOH be?
The pOH is 6,4.
What is the pOH range of bases?
An acidic solution will have a pOH ranging from 7 to 14
What is the OH- of a solution with pH 5.75?
pOH = -log[OH-] = -log(5*10^-3) = 2.3 pH = 14 - pOH = 14.0 - 2.3 = 11.7 (at 25 oC)
What is the solution's pH and pOH?
pH and pOH are a measure of the concentration of the hydronium ions and hydroxyl ions respectively in the solution. pH = -log[H+] pOH = -log[OH-] and they are related: pH + pOH = 14
How do you calculate OH- with a ph of 1.12?
pH + pOH = 14. So pOH = 14 - 1.12 = 12.88 pOH = -log[OH-] [OH-] = 1.31 x 10-13 M
What is the pOH of a solution with OH 2.0 x 10-2?
1.7
What is the pH of a 0.0110 M solution of Ba OH2?
pOH= -log(0.0220M OH) pH=14-pOH pH=12.34242268
What is the pOH of a solution whos OH- is 9.31 x 10-2 M?
pH + pOH = 14pH = -log 3.60x10^-10 = 9.44pOH = 14 - 9.44 = 4.56
If pH is 6 What is is OH?
pH + pOH = 14. So pOH = 14 - 6 = 8 pOH = -log[OH-] [OH-] = 10-8 M
What is the pOH of a solution with OH?
1.70
