We're asked to find the pH of 50mL of .1 M of a weak acid (labeled HX), before we add any .1 M NaOH. The Ka is 1.5e-5. The pH I found was 4.00 (feel free to fact check me). Here's the part I need help with:
-We are also asked to find the pH of the solution at the "endpoint". Not sure what this means. Do they mean equilibrium? If so, how would I calculate this? Thanks.
We're asked to find the pH of 50mL of .1 M of a weak acid (labeled...
A) The Ka of a monoprotic weak acid is 2.29 × 10-3. What is the percent ionization of a 0.129 M solution of this acid? I got 104.8% which I know is impossible. B) The Ka value for acetic acid, CH3COOH(aq), is 1.8× 10–5. Calculate the pH of a 2.40 M acetic acid solution. C) Calculate the pH of the resulting solution when 4.00 mL of the 2.40 M acetic acid is diluted to make a 250.0 mL solution. I...
A) Find the pH of a 0.120 M solution of a weak monoprotic acid having Ka= 1.5×10−5. B) Find the percent dissociation of this solution. C) Find the pH of a 0.120 M solution of a weak monoprotic acid having Ka= 2.0×10−3. D) Find the percent dissociation of this solution. E) Find the pH of a 0.120 M solution of a weak monoprotic acid having Ka= 0.14. F ) Find the percent dissociation of this solution.
a.) Find the pH of a 0.130 M solution of a weak monoprotic acid having Ka= 1.0×10−3. b.) Find the percent dissociation of this solution c.) Find the pH of a 0.130 M solution of a weak monoprotic acid having Ka= 0.11. d.) Find the percent dissociation of this solution.
Part E Find the pH of a 0.140 M solution of a weak monoprotic acid having Ka= 0.12. Part F Find the percent ionization of a 0.140 M solution of a weak monoprotic acid having Ka= 0.12.
Part A A 0.150 M weak acid solution has a pH of 2.97. Find Ka for the acid. Part B Find the percent ionization of a 0.195 M HC2H3O2 solution. (The value of Ka for HC2H3O2 is 1.8×10−5.) Part C Find the pH of a 0.0191 M solution of hypochlorous acid. (The value of Ka for hypochlorous acid is 2.9×10−8.) Part D Find the pH of a 0.014 M solution of HF. (The value of Ka for HF is 3.5×10−4.) Part...
Find the pH and percent ionization of a 0.100 M solution of a weak monoprotic acid having the given Ka values. (a) Ka = 1.9 10-5 (b) Ka = 1.9 10-3 (c) Ka = 1.9 10-1
A 0.135 M weak acid solution has a pH of 3.60. Find Ka for the acid. Express your answer using two significant figures.
Part C Find the pH of a 0.140 M solution of a weak monoprotic acid having Ka= 1.9×10−3. Part D Find the percent ionization of a 0.140 M solution of a weak monoprotic acid having KKa= 1.9×10−3.
1. A 0.100 M solution of the weak acid HB has a pH of 3.00. What are the [H+], [B-], and Ka for this acid? 2. A solid acid is dissolved in water. Half the solution is titrated to a phenolphthalein end point with NaOH solution. The neutralized and acid solutions are then mixed and the pH of the resulting solution is found to be 4.60. Find Ka of the solid acid. 3. Assuming your buffered solution contains acetic acid,...
Post-Lab Assignment: pH and Buffers 1. A buffer is prepared from a weak acid with a Ka - 7.1 x 104 and its conjugate base. a. What pH would provide maximum buffer capacity? b. What would be the buffer range for this acid? (Your answer should show the lowest and the highest pH that would provide a reasonably effective buffer.) 2. If you were provided with a 0.1 M solution of an unknown weak acid and a 0.1 M solution...