Answer:
the difference in hydrogen ion concentration between these two solution is :\(3.9809\times 10^{-3} mol/L\)
Explanation:
Concentration of hydrogen ions when pH of the solution is 11.2(alkaline)
\(pH=-\log[H^+]\)
\(11.2=-\log[H^+]\)
\([H^+]=6.3095\times 10^{-12} mol/L\)
Concentration of hydrogen ions when pH of the solution is 2.4 (acidic).
\(pH=-\log[H^+]'\)
\(2.4=-\log[H^+]'\)
\([H^+]'=0.39810 mol/L\)
In an acidic solution hydrogen ion s concentration always larger than that of of the alkaline solution.
\([H^+]'>[H^+]\)
The approximate difference in the concentration of hydrogen ions between the two solutions:
\([H^+]'-[H^+]=0.39810 mol/L-6.3095\times 10^{-12} mol/L=0.0039809 mol/L=3.9809\times 10^{-3} mol/L\)
