How is the concentration of hydronium ions $(H_3O^+)$ affected when a solution of an acid is diluted ?
How is the concentration of hydronium ions $(H_3O^+)$ affected when a solution of an acid is diluted ?
When an acid is diluted, the concentration of hydronium ions $(H_3O^+)$ per unit volume decreases. This means that the strength of the acid decreases.
Similar Questions
A milkman adds a very small amount of baking soda to fresh milk.
$(a)$ Why does he shift the $pH$ of the fresh milk from $6$ to slightly alkaline ?
$(b)$ Why does this milk take a long time to set as curd ?
A milkman adds a very small amount of baking soda to fresh milk.
$(a)$ Why does he shift the $pH$ of the fresh milk from $6$ to slightly alkaline ?
$(b)$ Why does this milk take a long time to set as curd ?
What effect does the concentration of $H^+_{(aq)}$ ions have on the nature of the solution ?
What effect does the concentration of $H^+_{(aq)}$ ions have on the nature of the solution ?
Why do $HCl$, $HNO_3$, etc., show acidic characters in aqueous solutions while solutions of compounds like alcohol and glucose do not show acidic character ?
Why do $HCl$, $HNO_3$, etc., show acidic characters in aqueous solutions while solutions of compounds like alcohol and glucose do not show acidic character ?
Write word equations and then balanced equations for the reaction taking place when -
$(a)$ dilute sulphuric acid reacts with aluminium powder.
$(b)$ dilute hydrochloric acid reacts with iron filings.
Write word equations and then balanced equations for the reaction taking place when -
$(a)$ dilute sulphuric acid reacts with aluminium powder.
$(b)$ dilute hydrochloric acid reacts with iron filings.
Do basic solutions also have $H^+_{(aq)}$ ions ? If yes, then why are these basic ?
Do basic solutions also have $H^+_{(aq)}$ ions ? If yes, then why are these basic ?