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Acid -Base theories

By jschemistrytelugu@gmail.comPosted on January 5, 2026Posted in IONIC EQUILIBRIUMNo Comments

Arrhenius Theory of Acids and Bases It was proposed by Arrhenius to explainthe behaviour of acids and bases in aqueous solutions. Arrhenius acids:— A substance that produces hydrogenions (H⁺) when dissolved in water. ex:(i) HCl (aq) → H⁺ (aq) + Cl⁻ (aq)(ii) H₂SO₄ (aq) → 2H⁺ (aq) + SO₄²⁻ (aq)(iii) HNO₃ (aq) → H⁺ (aq) […]

Calculate the pH of an aqueous solution of 1.0M ammonium formate assuming complete dissociation. ([ pK_a ] of formic acid = 3.8, [ pK_b ] of ammonia = 4.8)

By jschemistrytelugu@gmail.comPosted on October 16, 2025Posted in IONIC EQUILIBRIUMNo Comments

The hydrolysis reaction is a reversible reaction.The process of hydrolysis is a reverse reaction of neutralization. hydrolysis constant (𝐾ℎ):The equilibrium constant for the hydrolysis reaction multiplied by concentration of water is known as hydrolysis constant. it is represented by Kh. degree of hydrolysis (h): The fraction of the total salt which is hydrolysed it […]

The hydrolysis constant [ K_h ] of a salt of NaOH and a weak acid (HX) if the [ K_a ] of the acid is]

By jschemistrytelugu@gmail.comPosted on October 16, 2025Posted in IONIC EQUILIBRIUMNo Comments

Question : Which pair will show common ion effect? 1) AgNO₃ + KNO₃ 2) NaCl + HCl 3) NH₄OH + NH₄Cl 4) BaCl₂ + Ba(NO₃)₂

By jschemistrytelugu@gmail.comPosted on October 15, 2025Posted in IONIC EQUILIBRIUMNo Comments

Correct answer: 3 A mixture of NH₄OH (ammonium hydroxide) and NH₄Cl (ammonium chloride) forms a basic buffer solution. It contains a weak base and a salt of its strong conjugate acid. It is widely used in qualitative inorganic analysis. Buffer Solutions: The solution which resists the change in its pH when some […]

The pH of a solution obtained by mixing 50 mL of 0.4 N HCl and 50 mL of 0.2 N NaOH is 1)–log 2 2)–log 0.2 3)1.0 4)2.0

By jschemistrytelugu@gmail.comPosted on October 14, 2025Posted in IONIC EQUILIBRIUMNo Comments

Correct answer:(3) * The final pH depends on the difference in milliequivalents of acid and base present in the mixed solution…

A 0.01 M ammonia solution is 5% ionized, the concentration of OH⁻ ions is 1) 0.005 M 2) 0.0001 M 3) 0.0005 M 4) 0.05 M

By jschemistrytelugu@gmail.comPosted on October 14, 2025Posted in IONIC EQUILIBRIUMNo Comments

Degree of dissociation is defined as the ratio of number of molecules dissociated as ions to total number of molecules of electrolyte dissolved. Degree of association of strong electrolytes is unity(1). But,for weak electrolytes is less than Unity. The extent of dissociation for weak electrolytes increases upon the dilution.

The equilibrium constant for the reaction A ⇌ B is K. The equilibrium constant for the reaction mA ⇌ mB is 1) mK 2)K/m 3) Kᵐ 4) K⁻ᵐ

By jschemistrytelugu@gmail.comPosted on October 14, 2025Posted in IONIC EQUILIBRIUMNo Comments

Equilibrium constant depends on, 1. Temperature 2)Stoichiometric Coefficient 3) direction of reaction.. 1. Temperature : * For an exothermic reaction ( H < 0), equilibrium constant is inversly proportional to temperature. Increasing temperature decreases Kcd. Decreasing the temperature increases Kc. * For an endothermic reaction ( H > 0). Equilibrium constant is directly proportional to […]

Question : The ionic product of water is 10⁻¹⁴. The H⁺ ion concentration in 0.01 M NaOH solution is 1)10⁻¹¹ M 2)10⁻¹² M 3)10⁻¹ M 4) 10⁻⁴ M

By jschemistrytelugu@gmail.comPosted on October 12, 2025Posted in IONIC EQUILIBRIUMNo Comments

Question : The Kₐ of a weak acid is 10⁻⁵, pKb value of its conjugate base is 1)7 2)5 3)9 4)6

By jschemistrytelugu@gmail.comPosted on October 12, 2025Posted in IONIC EQUILIBRIUMNo Comments

Video solution: dissociation constant of acid (Ka) : It is a measure of the extent to which an acid dissociates in solution. The less an acid dissociates, the smaller the value of Ka. The stronger the acid, higher will be the value of Ka. What is a Conjugate Acid-Base Pair? Every […]