Practice Problem: Consider The Titration of 100.0 mL of 0.250 M HA (K = 5.0 x 104, pKa = 3.30) With 0.250 M NaOH. Determine The pH At The Equivalence Point: a. 7.00. b. 5.80. c. 11.59. d. 8.20. e. 9.86.
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Q: What quantity in moles of CH3NH3CI need to be added to 200.0 mL of a 0.500 M solution of CH3NH₂ (Kb…
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- How would you determine the pKa1 and Ka1 from graph. Please show calculation steps to finding the KaHow much 5.60 M NaOH must be added to 530.0 mL of a buffer that is 0.0205 Macetic acid and 0.0255 M sodium acetate to raise the pH to 5.75? Answer should be in mLPROBLEM 1. What will be the pH when 50.0 ml of 2.00M carbonic acid is mixed 20.0 ml of 3.00 M sodium bicarbonate? The Ka of carbonic is 4.30 x 10-7. PROBLEM 2. For the buffer in Problem no. 1, what will be the pH when (a) 15.0 ml of 0.500 M HCl and (b) when 15.0 ml of 0.750 M NaOH is added to the buffer separately? PROBLEM 3. How will you prepare 500 ml of 0.750 M citrate buffer with pH of 4.25 from solid citric acid (C6H8O7) and solid sodium citrate (Na3 C6H5O7)? The Ka of citric acid is 7.40 x 10-4.