`color{green}(★)` Strength of acids and bases depends on the no. of `color{red}(H^+)` ions and `color{red}(OH^–)` ions produced respectively.
`color{green}(★)` With the help of a universal indicator we can find the strength of an acid or base. The universal indicator shows different colours at different concentrations of hydrogen ions in a solution.
`color{green}(★)` A scale for measuring hydrogen ion concentration in a solution, called pH scale has been developed. The p in pH stands for ‘potenz’ in German, meaning power. On the pH scale we can measure pH generally from 0 (very acidic) to 14 (very alkaline).
`color{green}(★)` pH should be thought of simply as a number which indicates the acidic or basic nature of a solution. Higher the hydronium ion concentration, lower is the pH value.
`color{green}(★)` The pH of a neutral solution is 7. Values less than 7 on the pH scale represent an acidic solution. As the pH value increases from 7 to 14, it represents an increase in `color{red}(OH^–)` ion concentration in the solution, that is, increase in the strength of alkali (Fig. 2.6). Generally paper impregnated with the universal indicator is used for measuring pH.
Strong Acids give rise to more `color{red}(H^(+))` ions .
`color{red}(Eg. \ \ HCl , H_2SO_4 )` and `color{red}(HNO_3)`.
Weak Acids give rise to less `color{red}(H^(+))` ions.
`color{red}(Eg. \ \ CH_3COOH , H_2CO_3 ("Carbonic acid"))`
Strong Bases - Strong bases give rise to more `color{red}(OH^(-)) ` ions .
`color{red}(Eg.\ \ NaOH , KOH , Ca(OH)_2)`
Weak Bases ; gives rise to less `color{red}(OH^(-))` ions .
`color{red}(Eg. \ \ NH_4OH)`
`color{green}(★)` Strength of acids and bases depends on the no. of `color{red}(H^+)` ions and `color{red}(OH^–)` ions produced respectively.
`color{green}(★)` With the help of a universal indicator we can find the strength of an acid or base. The universal indicator shows different colours at different concentrations of hydrogen ions in a solution.
`color{green}(★)` A scale for measuring hydrogen ion concentration in a solution, called pH scale has been developed. The p in pH stands for ‘potenz’ in German, meaning power. On the pH scale we can measure pH generally from 0 (very acidic) to 14 (very alkaline).
`color{green}(★)` pH should be thought of simply as a number which indicates the acidic or basic nature of a solution. Higher the hydronium ion concentration, lower is the pH value.
`color{green}(★)` The pH of a neutral solution is 7. Values less than 7 on the pH scale represent an acidic solution. As the pH value increases from 7 to 14, it represents an increase in `color{red}(OH^–)` ion concentration in the solution, that is, increase in the strength of alkali (Fig. 2.6). Generally paper impregnated with the universal indicator is used for measuring pH.
Strong Acids give rise to more `color{red}(H^(+))` ions .
`color{red}(Eg. \ \ HCl , H_2SO_4 )` and `color{red}(HNO_3)`.
Weak Acids give rise to less `color{red}(H^(+))` ions.
`color{red}(Eg. \ \ CH_3COOH , H_2CO_3 ("Carbonic acid"))`
Strong Bases - Strong bases give rise to more `color{red}(OH^(-)) ` ions .
`color{red}(Eg.\ \ NaOH , KOH , Ca(OH)_2)`
Weak Bases ; gives rise to less `color{red}(OH^(-))` ions .
`color{red}(Eg. \ \ NH_4OH)`