What is the $pH$ of a solution in which $25.0 \ mL$ of $0.1 \ M \ NaOH$ is added to $25 \ mL$ of $0.08 \ M \ HCl$ and the final solution is diluted to $500 \ mL$?
- A$3$
- B$11$
- C$12$
- D$13$
Explore More
Similar Questions
$10^{-6} \ M \ NaOH$ is diluted $100$ times. The $pH$ of the diluted base is
Calculate the $pH$ of a $1.0 \times 10^{-8} \ M$ solution of $HCl$.
Difficult
View SolutionWhat is the $pH$ of $10^{-9} \ M$ aqueous $HCl$ solution?
Medium
View SolutionThe $pH$ of $0.0001 \ N$ solution of $KOH$ will be
Medium
View SolutionHow many litres of water must be added to $1 \ L$ of an aqueous solution of $HCl$ with a $pH$ of $1$ to create an aqueous solution with $pH$ of $2$?
Medium
View SolutionVedclass 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