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Question 1 4 points 0.200 moles of HA (Ka=1.00x10-8) is mixed with 0.300 moles NaA. Calculate...
1. A solution has [HC7H5O2] = 0.100 M and [Ca(C7H5O2)2] = 0.200 M. Ka = 6.3 × 10-5 for HC7H5O2. The solution volume is 5.00 L. What is the pH of this solution after 5.00 mL 10.0 M HCl is added? 2. Which of the following solution(s) is a buffer? 100 mL of 0.1 M acetic acid mixed with 25 mL of 0.5 M NaOH 50 mL of 0.1 M acetic acid mixed with 25 mL of 0.05 M sodium...
8. 25.00mL of 0.100M of a weak acid HA is titrated with 0.100M sodium hydroxide: Ka = 1.8 x 10-5 Calculate the pH of the solution after the following: a) Prior to titration (no NaOH added yet) b) 7.50mL of NaOH added c) 12.50mL of NaOH added d) 25.00mL of NaOH added e) 32.50mL of NaOH added
Ka for hypochlorous acid, HClO, is 3.0 x 10^-8. Calculate the pH after 10.0, 20.0, 30.0, and 40.0 ml of 0.100M NaOH have been added to 40.0ml of 0.100M HClO. Expert Answer GoldenApple6699 GoldenApple6699 answered this Was this answer helpful? 8 0 766 answers At any point between 0 and 40 mL of NaOH added, you will have a solution containing both HClO and ClO- ... that's a buffer system (a weak acid and its conjugate base) and the pH...
NH4+ salt is confirmed 8/24 points Previous Answers My Note Calculate the change in pH to 0.01 pH units caused by adding 10. mL of 2.82-M NaOH is added to 390. mL of each of the following solutions. a) water pH before mixing = 7.00 pH after mixing= 12.85 pH change = 5.85 b) 0.127 M NH41+ > pH before mixing = 5.07 pH after mixing= 9.50 X pH change = X c) 0.127 M NH3 pH before mixing =...
please help!! calculate pH of solutions on second page a-c!! 1. (4 points) A buffer solution is created with C;H,NH, and 0.012 M C;HsNH2. The K, for C,H,NH2 is 4.7 х 104. What is the concentration of C,HNH, in the buffer solution that has a pH of 11.50? а. What is the concentration of the buffer solution if 0.0011 M HC is added to the buffer in part a.? b. Why is the buffer a basic solution? Could this weak...