Hydrogen and hydroxyl ion concentration in aqueous solutions of acids and bases: The ionic product is very important quantity in aqueous solutions because it controls the relative concentrations of H+…
0.561 g of KOH dissolved in 200 mL of solution will have: Moles of KOH = 0.561 / 56 = 1.0 x 10-2 As molar mass of KOH = 56…
1 mL of 13.6 M HCl is diluted with water to give 1 L of solution: Molarity of the diluted solution is given as: M1 V1 = M2 V2 13.6…
H3O+] = 3.8 x 10-3 pH = – log = – log (3.8 x 10-3) = – (log 3.8 – 3 log 10) = – log 3.8 + 3.0 =…
If we use the relation, pH = – log , we get pH equal to 8. But this is not correct because an acidic solution cannot have pH greater than…
Conjugate acid and base are related as: Base + H+ <—————> acid Acid <—————–> H+ + base Let us consider a weak acid, HA HA (aq) + H2O < —————>…
Sorensen in 1909 discovered a new tern for expressing the concentration of hydrogen ions known as pH or pH scale. The pH of a solution is defined as: The negative…
We know that HF < ———–> H+ + F– Ka (acid) x Kb (conjugate base) = Kw = 1.0 x 10-14 Ka = 6.8 x 10-4 (given) Kb (F–) =…
Bronsted acids which can donate more than one proton are called Polytrophic acids or polybasic acids. For example, oxalic acid and sulphuric acid have two ionizable protons per molecule of…
The second dissociation constant is very small than the first dissociation constant and therefore, the concentration of H3O+ is obtained only from the first dissociation constant: H2S + H2O <…
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