exercise 1 - solution
1) -log(4·10-3) = -(-3+0.60) = 2.40
2) pH = -log [H+] -log [H+] = 4.60 log[H+] = -4.60 [H+] = 10-4,60 = 2.5·10-5 mol/L.
3) pH+pOH = 14 pOH = 14-pH = 14-10.8 = 3.20 -log[OH-] = 3.20 log[OH-] = -3.20 [OH-] = 10-3.20 = 6.31·10-4 mol/L.
exercise 2 - solution
1) The hydrogen ion (H+) concentration in solution if defined as:
-log[H+] = 4,18 log[H+] = - 4,18 [H+] = 6,61·10-5 mol/L.
The value of the ion-product constant (K1) is determined in Table 1.
The concentration of [HCO3-] ions is determined as: [HCO3-] = 4,45·10-7·10-7/ (6,61·10-5) = 6,67·10-5 mol/L.
In the same way the value of the ion - product (K2) is determined in Table 1.
The concentration of [CO32-] ions is determined as: [CO32-] = 4,69·10-11·6,73·10-5/(6,61·10-5) = 4,8·10-11 mol/L