The $pH$ of human blood is $7.4$. The $[H^{+}]$ concentration will be:
- A$4 \times 10^{-8} \ M$
- B$2 \times 10^{-8} \ M$
- C$4 \times 10^{-4} \ M$
- D$2 \times 10^{-4} \ M$
Explore More
Similar Questions
At a certain temperature,if $pK_w = 12.60$,then which of the following is correct for an acidic solution?
Medium
View SolutionThe concentration of hydrogen ions in a given solution is $6 \times 10^{-4} \ M$. The $pH$ of the solution is:
Medium
View SolutionThe number of $OH^{-}$ ions in $1 \ mL$ of solution having $pH = 4$ is :-
Medium
View SolutionAt $90\,^{\circ}C$ pure water has $[H_3O^{+}] = 10^{-6}\,M$. The value of $K_w$ at this temperature will be:
MediumAIPMT 1993
View SolutionCalculate $[OH^{-}]$ and $pH$ of a solution containing $[H^{+}] = 0.001 \ M$.
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