The correct option is
2.35 %
Question 6 (1 point) A weak base has an initial concentration of 0.588 M. After undergoing...
A weak base has an initial concentration of 0.287 M. After undergoing dissociation the pH is 12.23. A- + H2O ⇌ OH- + HA What is the percent ionization of the base? Options: A 5.92% B 12.3% C 1.68% D 0.0123% E 0.995%
A weak acid has an initial concentration of 0.0415 M. After undergoing dissociation the pH is 5.31. HA + H2O ⇌ H3O+ + A- What is the percent ionization of the acid?
A weak acid has an initial concentration of 0.0415 M. After undergoing dissociation the pH is 5.31. HA + H20 = H30* + A What is the percent ionization of the acid? 0.155% 2.34% 0.0993% 0.782% O 0.0118%
The degree to which a weak base dissociates is given by the base-ionization constant, Kb. For the generic weak base, B B(aq)+H2O(l)⇌BH+(aq)+OH−(aq) this constant is given by Kb=[BH+][OH−][B] Strong bases will have a higher Kb value. Similarly, strong bases will have a higher percent ionization value. Percent ionization=[OH−] equilibrium[B] initial×100% Strong bases, for which Kb 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....
A weak acid, HF, is prepared with an initial concentration of 1.20 M. After reaching equilibrium, it has a pH of 1.551. What is the percent ionization of this acid? Select one: 4.2% 0.84% 2.4% None of these 0.082%
percent ionization of a weak base pH and Percent lonization of a Weak Base Ammonia, NH, is a weak base with a Ky, value of 1.8 x 105 The degree to which a weak base dissociates is given by the base ionization content K) For the generic weak base, B B(aq) + H2O(1) BH(aq) + OH (!) this constant is given by Pan A KDO What is the pH of a 0.165 Mammonia solution? Express your answer numerically to two...
Question HA is a weak acid. Its ionization constant, K, is 3.0 x 10) Calculate the pH of an aqueous solution with an initial NaA concentration of 0.060 M. Question 2 We place 0.150 mol of a weak acid, HA, in enough water to produce 100L of solution. The final pH of the solution is 1.18. Calculate the ionization contant, K., HA. Question We place 0.607 mol of a weak acid, HA, and 13.9 g of NaOH in enough water...
14. A weak acid, (HA), has an acid dissociation constant of 2.50 . 10-6. A 25.00 ml sample with a concentration of 0.250 M is titrated with 0.150 M NaOH. a. Write the equation for the acid dissociation equilibrium. b. What is the pH of the original 0.250 M sample of HA? c. What is the percent ionization of the 0.250 M acid? d. Write the equation for the neutralization reaction. e. What is the pH after 12.00 ml 0.150M...
A weak acid, (HA), has an acid dissociation constant of 4.60∙10–6. A 25.00 ml sample with a concentration of 0.1200 M is titrated with 0.1500 M NaOH. a. Write the equation for the acid dissociation equilibrium. b. What is the pH of the original 0.1200 M sample of HA? c. What is the percent ionization of the 0.1200 M acid? d. Write the equation for the neutralization reaction. e. What is the pH after 8.00 ml NaOH have been added?
30 QUESTIONS FOR WEAK ACIDS & BASES EXP. 1. Examine the data for acetic acid and discuss the effects of dilution on the percent dissociation of this weak acid. a. What immediate effect did dilution have on Q? b. Did K change? Should it have changed? Why or why not? c. Which way did any changes cause the equilibrium to shift? Why? d. How did the shift affect the percent dissociation? Should the effects of dilution on % dissociation for...