what is the ph of the solution 0.15 M nho3 And 0.62M NAOH and 0.36M HCL
Answers
Problem :
What is the pH of a solution of 0.36 M HCl, 0.62 M NaOH, and 0.15 M HNO3?
Hydrochloric acid and nitric acid are strong acids, and sodium hydroxide is a strong base; these all dissociate completely. The total [H+] from the two acids is 0.51 M and [OH-] from NaOH is 0.62 M. Therefore, 0.51 moles per liter of H+ will react with 0.51 moles per liter of OH- to form water. That leaves a 0.11 M NaOH solution. The pOH of a 0.11 M NaOH solution is 0.96 pOH units, and the pH is 13.04 pH units.
What percent of formic acid (HCOOH) is dissociated in a 0.1 M solution of formic acid? The Ka of formic acid is 1.77 x 10-4.
Problem :
What happens to the pH of a 0.1 M solution of formic acid when enough HCl (g) is added to make the solution 0.01 M in HCl?
Note that in this problem the volume of the solution does not change so you do not have to recalculate the concentration of formic acid. The only change to the problem is that there is now an initial concentration of H+ in solution:
As you can see, the addition of a strong acid can, by Le Chatlier's principle, cause a weak acid not to dissociate. An exact solution for this problem does show a small dissociation of formic acid that is insignificant.