The $pH$ of a solution is $4$. The hydroxide ion concentration of the solution would be:
- A$10^{-4} \ M$
- B$10^{-10} \ M$
- C$10^{-2} \ M$
- D$10^{-12} \ M$
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If the ionic product of water $(K_w)$ is $1.96 \times 10^{-14}$ at $35^{\circ} C$, what is its value at $10^{\circ} C$?
If the $pH$ of a soft drink is $3.7$,what is the concentration of hydrogen ions?
Medium
View SolutionThe $pH$ of a solution having $[OH^{-}] = 10^{-7} \ M$ is
MediumAIIMS 1996
View SolutionWhat will be the hydrogen ion concentration in moles $L^{-1}$ of a solution whose $pH$ is $4.58$?
Difficult
View SolutionFor the following Assertion and Reason,the correct option is
Assertion : The $pH$ of water increases with increase in temperature.
Reason : The dissociation of water into $H^{+}$ and $OH^{-}$ is an exothermic reaction.
Assertion : The $pH$ of water increases with increase in temperature.
Reason : The dissociation of water into $H^{+}$ and $OH^{-}$ is an exothermic reaction.
DifficultJEE MAIN 2020
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