Final answer:
To find the pH of a 0.110 M ammonia solution, we can use the Kb expression for ammonia and calculate the concentration of hydroxide ions (OH-). The concentration of OH- is equal to Kb divided by the concentration of ammonia (NH3). Using this information, we find that the pH of the solution is 3.8.
Step-by-step explanation:
The pH of a 0.110 M ammonia solution can be determined by using the Kb value for ammonia, which is 1.76 x 10-5. Ammonia is a weak base, so we can assume that it partially ionizes in water. To calculate the pH, we need to find the concentration of hydroxide ions (OH-) in the solution. We can use the Kb expression for ammonia: Kb = [NH4+][OH-]/[NH3]. By assuming that the concentration of [OH-] is unknown and [NH4+] is negligible compared to [NH3], we can simplify the expression to Kb = [OH-][NH3]. Rearranging the expression, we get [OH-] = Kb/[NH3]. Substituting the values, we find [OH-] = (1.76 x 10-5)/(0.110), which equals 1.60 x 10-4 M. To find the pH, we use the equation pH = -log[H3O+]. Since water acts as an acid in this case, the concentration of [H3O+] is equal to [OH-]. Therefore, the pH of a 0.110 M ammonia solution is 3.8.