![Pure water is netural in nature [H^(+)]=[OH^(-)]. When this condition is disturbed by changing the concentration of H^(+)or OH^(-), the natural solution changes to acidic {[H^(+)]gt[OH^(-)]} or basic {[H^(+)]lt[OH^(-)]}. This change occurs Pure water is netural in nature [H^(+)]=[OH^(-)]. When this condition is disturbed by changing the concentration of H^(+)or OH^(-), the natural solution changes to acidic {[H^(+)]gt[OH^(-)]} or basic {[H^(+)]lt[OH^(-)]}. This change occurs](https://d10lpgp6xz60nq.cloudfront.net/web-thumb/644354016_web.png)
Pure water is netural in nature [H^(+)]=[OH^(-)]. When this condition is disturbed by changing the concentration of H^(+)or OH^(-), the natural solution changes to acidic {[H^(+)]gt[OH^(-)]} or basic {[H^(+)]lt[OH^(-)]}. This change occurs
![Calculation of Hydrolysis Constant, Degree of Hydrolysis and pH of Salt Solution - Chemistry, Class 11, Ionic Equilibrium Calculation of Hydrolysis Constant, Degree of Hydrolysis and pH of Salt Solution - Chemistry, Class 11, Ionic Equilibrium](https://classnotes.org.in/wp-content/uploads/Relation-between-kh-Kw-Ka.png)
Calculation of Hydrolysis Constant, Degree of Hydrolysis and pH of Salt Solution - Chemistry, Class 11, Ionic Equilibrium
![Calculate pH of a solution of given mixture (0.1 mole CH3COOH + 0.2 mole CH3COONa ) in 100 ml 0f mixture. K = 2 × 10^-5 Calculate pH of a solution of given mixture (0.1 mole CH3COOH + 0.2 mole CH3COONa ) in 100 ml 0f mixture. K = 2 × 10^-5](https://dwes9vv9u0550.cloudfront.net/images/4773946/6d290db4-b4c2-4a08-a1ee-75bd2c7ff4d0.jpg)
Calculate pH of a solution of given mixture (0.1 mole CH3COOH + 0.2 mole CH3COONa ) in 100 ml 0f mixture. K = 2 × 10^-5
![aqueous solution - Accurate method to calculate the pH of a salt from a weak acid and weak base - Chemistry Stack Exchange aqueous solution - Accurate method to calculate the pH of a salt from a weak acid and weak base - Chemistry Stack Exchange](https://i.stack.imgur.com/9cPp3.png)
aqueous solution - Accurate method to calculate the pH of a salt from a weak acid and weak base - Chemistry Stack Exchange
![Calculate pH of a salt of weak monobasic acid and weak monoacidic base having concentration 0.1 M at 25^oC (Given : - pka = 4.8 pkb = 5.2 ) Calculate pH of a salt of weak monobasic acid and weak monoacidic base having concentration 0.1 M at 25^oC (Given : - pka = 4.8 pkb = 5.2 )](https://haygot.s3.amazonaws.com/questions/1937136_1337314_ans_f6b01bc763224f6c88fb7e4e1fbec6a8.jpg)
Calculate pH of a salt of weak monobasic acid and weak monoacidic base having concentration 0.1 M at 25^oC (Given : - pka = 4.8 pkb = 5.2 )
![SOLVED: A scientist prepared a 0.031 M NH4Cl salt solution by dissolving the solid salt in water. Calculate the pH at 25°C for the solution, given that the Kb of ammonia, NH3, SOLVED: A scientist prepared a 0.031 M NH4Cl salt solution by dissolving the solid salt in water. Calculate the pH at 25°C for the solution, given that the Kb of ammonia, NH3,](https://cdn.numerade.com/ask_previews/c2cd49a3-274d-4d7c-bb2b-4f0d27aa1d3b_large.jpg)