NEETChemistryIonic Equilibrium
Which of the following best explains why the pH of a 10 –8 mol dm –3 solution of HCl is observed to be less than 7.0, even though pH = – log [H + ] suggests it should be 8?
Options
- AThe solution is contaminated with impurities, causing a decrease in pH.
- BHCl undergoes partial dissociation in the solution, resulting in a higher concentration of H + ions.
- CThe pH scale is not applicable to such dilute solutions, as the contribution of H 3 O + from water is signific
- DThere is a measurement error in determining the pH of the solution.
Correct answer
C. The pH scale is not applicable to such dilute solutions, as the contribution of H 3 O + from water is signific
Step-by-step solution
Correct Option is : (C) The pH scale is not applicable to such dilute solutions, as the contribution of H 3 O + from water is significant.