Your Online "Ionic Equilibria" Teacher


Home » Chemistry » Ionic Equilibria »

Conjugate acid and base are related as: Base + H+ acid Acid H+ + base Let us consider a weak acid, HA HA (aq) + H2O < ---------------> H3O+ (aq) + A- (aq) Ka (HA) = [H3O+] [A-] / [HA]...................... (1) The conjugate base, A- behaves as ...

Continue Comments Off on Derive the relationship between Ka and Kb for an acid and its conjugate base.

If we use the relation, pH = - log [H3O+], we get pH equal to 8. But this is not correct because an acidic solution cannot have pH greater than 7. It may be noted that in very dilute acidic solution, when H+ concentrations from ...

H3O+] = 3.8 x 10-3 pH = - log [H3O+] = - log (3.8 x 10-3) = - (log 3.8 – 3 log 10) = - log 3.8 + 3.0 = - 0.589 + 3 = 2.42 The pH of a sample of soft drink whose hydronium ion concentration ...

Continue Comments Off on Calculate the pH of a sample of soft drink whose hydronium ion concentration is 3.8 x 10-3 M.

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 M x 1 mL = M2 x 1000 mL Therefore, M2 = 113.6 / 1000 = 1.36 x 10-2 ...

Continue Comments Off on Calculate the pH if 1 mL of 13.6 M HCl is diluted with water to give 1 L of solution.

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 u Concentration of solution = (moles of KOH / vol. of solution) x 1000 = (1.0 x 10-2 / ...

Continue Comments Off on Calculate the pH of the 0.561 g of KOH dissolved in 200 mL of solution.

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+ and OH- ions because their product is constant. In pure water, the concentrations of [H3O+] and ...

Continue Comments Off on Derive the hydrogen and hydroxyl ion concentration in aqueous solutions of acids and bases.

Ionization of water – ionic product of water Water is a weak electrolyte and undergoes self dissociation to a small extent as: H2O (l) + H2O (l) < --------------> H3O+ (aq) + OH- The dissociation constant foe the ionization of water is: K = [H3O+] [OH-] / H3O+] Since the ...

Continue Comments Off on Discuss the ionization of water.

Ka for acetic acid is 1.8 x 10-5. Acetic acid, CH3COOH is a weak acid which ionizes partially and sodium acetate is a strong electrolyte which ionizes completely in the solution. Let x be the number of moles of acetic acid ionized. Then, the concentrations of various ...

Continue Comments Off on Calculate the concentration of H3O+ ions in a mixture of 0.02 M acetic acid and 0.1 M sodium acetate.
Page 4 of 623456
Copyright © All rights reserved. TheBigger.com | Privacy Policy | Contact Us | Copyright Policy | Useful Resources