Question

The equation for the pH of a substance is pH = –log[H+], where H+ is the concentration of hydrogen ions. A basic solution has a pH of 11.2. An acidic solution has a pH of 2.4. What is the approximate difference in the concentration of hydrogen ions between the two solutions?

Answer 1

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:

$[H^+]'-[H^+]=0.39810 mol/L-6.3095\times 10^{-12} mol/L=0.0039809 mol/L=3.9809\times 10^{-3} mol/L$

Answer 2

[H+] of basic solution = 10⁻¹¹·² = 6.31x10⁻¹² moldm³

[H+] of acidic solution = 10⁻²·⁴  = 3.98x10⁻³ moldm³

the diffrence is 3.9799x10⁻³ moldm³

hope that helps