1.70
12.85
solution with [OH-] = 2.5 x 10-9 , A solution with [H+] = 1.2 x 10-4, A solution with pH = 4.5
0.20 X 420.00 = 84.00
CH3-C=O-NH2 +HCl----> CH3-C=O-OH+ NH4Cl
[H+] = Kw / [OH-] = 1.0*10-14 / 2.5*10-4 = 4.0*10-11 mol/L
1.70
12.85 is the pOH.
1.70
[OH-] = 3.31 log[OH-] = pOH = .51982 14-pOH = pH = 13.48
1.70
The pOH is the negative log of the OH- concentration. Thus, pOH = -log 2.0x10^-2pOH = 1.699 = 1.7
The pOH is 6,4.
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
1.70
12.85
12.85
12.85