What do you mean by solubility product and sparingly soluble salts?
admin The solubility of ionic solids in water differs to a great extent. Some of the ionic solids are so soluble that they are hygroscopoic in nature and absorb even water…
What is the importance of Solubility Product?
The concept of solubility product is very useful in explaining many phenomenons. Various fields in which it can be used are:- 1. Calculation of solubility: If we know the solubility…
What are the differences between solubility product and ionic product?
The main differences between solubility product and ionic product are given as under: Solubility product Ionic product Solubility product is the concentration of ions of electrolyte, each raised to the…
Define buffer solution with example. Also discuss its types.
The solution which resists changes in the hydrogen ion concentration on the addition of small amount of acid or base is known as buffer solution. Many medical and cosmetic formulations…
What do you mean by common ion effect?
We know that weak acids and weak bases slightly ionize in water and equilibrium is established in their solutions. The phenomenon of suppression of the degree of dissociation of a…
Define Buffer Action?
Buffer action: the ability of the buffer solution to resist the changes in pH value on the addition of small amount of an acid or a base is known as…
Derive Henderson – Hasselbalch equation?
We can derive a general equation for calculating the pH of any buffer solution. Consider a mixture of weak acid (HX) and its conjugate base. HX + H2O ⇌ H3O+…
The salt of strong acid and strong base does not undergo hydrolysis. Explain.
In this case, neither the cations nor the anion undergoes hydrolysis. Therefore, the solution remains neutral. For example: in the aqueous solution of NaCl, its ions Na+ and Cl– ions…
The ionization constant of formic acid is 1.8 x 10-4. Around what pH will its mixture with sodium formate give buffer solution of higher capacity? Calculate the ratio of sodium formate and formic acid in a buffer of pH 4.25.
Buffer capacity is defined as the rate of change of pH with number of moles of acid or base added. Buffer capacity = dpH / dn acid or base dpH…
Calculate the pH of a buffer solution containing 0.2 mole of NH4Cl and 0.1 mole of NH4OH per litre. Kb for NH4OH = 1.85 x 10-5.
According to Henderson – Hasselbalch equation: pOH = pKb + log (/ ) pKb = – log Kb = – log .85 x 10-5 = 4.733 Therefore, pOH = 4.733…