At $100\, ^oC$,the $K_w$ of water is $55$ times its value at $25\, ^oC$. What will be the $pH$ of a neutral solution at this temperature? $(\log 55 = 1.74)$
- A$7$
- B$7.87$
- C$5.13$
- D$6.13$
Explore More
Similar Questions
The ionic product of water increases if....
Easy
View SolutionGiven that $K_w$ for water is $10^{-13} \ M^2$ at $62 \ ^\circ C$,compute the sum of $pOH$ and $pH$ for a neutral aqueous solution at $62 \ ^\circ C$.
Medium
View SolutionIf $20 \ mL$ of an acidic solution of $pH$ $3$ is diluted to $100 \ mL$,the $H^{+}$ ion concentration will be
DifficultMHT CET 2009
View SolutionAt $25 \, ^\circ C$,the ionic product of water $(K_w)$ is equal to .......
Easy
View SolutionWhen $KBr$ is dissolved in water,$K^{+}$ ions are
Vedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo