Question

Calculate the percent ionization of HA in a 0.10 M solution. Express your answer as a percent using two significant figures. View Available Hint(s) nothing % Part B Calculate the percent ionization of HA in a 0.010 M solution. Express your answer as a percent using two significant figures. View Available Hint(s)

pH and Percent Ionization of a Weak Base 20 of 22 > A Review Constants Periodic Table The degree to which a weak base dissociates is given by the base-ionization constant, kb. For the generic weak base, B Part A B(aq) + H2O(1) = BH(aq) + OH(aq) this constant is given by What is the pH of a 0.205 M ammonia solution? Express your answer numerically to two decimal places. K, = BHOH) View Available Hint(s) Strong bases will have a higher Kb value. Similarly, strong bases will have a higher percent ionization value. pH = 11.28 Percent ionization - OH equilibrium x 100% Submit Previous Answers B initial Correct Strong bases, for which K, is very large, ionize completely (100%). For weak bases, the percent ionization changes with concentration. The more dilute the solution, the greater the percent ionization. Part B What is the percent ionization of ammonia at this concentration? Express your answer with the appropriate units. View Available Hint(s) I! A R O 21 ? Units % ionization = Value

Answer 1

Part B:

pH = 11.28

pH + pOH = 14.00

pOH = 14.00 -pH

pOH = 14.00 - 11.28

pOH = 2.72

pOH = -log[OH-]

[OH-] = 10^-pOH

[OH-] = 10^-2.72

[OH-] = 0.001905 M

Percent ionization =( [OH-] equilibrium / [NH3]intial ) × 100@%

=( 0.001905 / 0.205) × 100%

= 0.929 %

Hence the percent ionization is 0.929 %

for acid,

percent ionization = ([H3O+] equilibrium / [HA] initial ) × 100%

Actual here Ka of weak acid HA is not given.so unable to calculate the [H3O+] equilibrium