The pK, values for the dibasic base B are pKbl = 2.10 and pKb2 = 7.38. Calculate the pH at each of the points in the titration of 50.0 mL of a 0.95 M B(aq) solution with 0.95 M HCl(aq). What is the pH before addition of any HCI? What is the pH after addition of 25.0 mL HCI? pH = pH =

Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 2.00 ✕ 102 mL of solution and then titrate the solution with 0.148 M NaOH. C6H5CO2H(aq) + OH-(aq)  C6H5CO2-(aq) + H2O(ℓ) What are the concentrations of the following ions at the equivalence point? Na+, H3O+, OH-C6H5CO2-   M Na+  M H3O+  M OH-  M C6H5CO2-What is the pH of the solution?

Consider the titration of 80.0 mL of 0.100 M Ba (OH), by 0.400 M HCI. Calculate the pH of the resulting solution after the following volumes of HCl have been added. а. 0.0 mL pH = b. 20.0 mL pH = c. 30.0 mL pH = d. 40.0 ml pH = e. 90.0 ml pH =

The pK, values for the dibasic base B are pKi = 2.10 and pk2 = 7.49. %3! Calculate the pH at each of the points in the titration of 50.0 ml. of a 0.55 M B(aq) solution with 0.55 M HCI(aq). What is the pH before addition of any HCI? pH What is the pH after addition of 25.0 ml. HCI? pH = What is the pH after addition of 50.0 mL HC? pH What is the pH after addition of 75.0 mlL HCI? pH = What is the pH after addition of 100.0 ml. HCI? pH =

In the titration of a solution of weak monoprotic acid with a O.1450 M solution of NaOH, the pH half way to the equivalence point was 4.38. In the titration of a second solution of the same acid, exactly twice as much of a 0.1450 M solution of NaOH was needed to reach the equivalence point. What was the pH half way to the equivalence point in this titration?

Calculate the pH for each point in the titration of 25.0 mL of 0.250 M pyridine, C,H,N(aq), with 0.250 M HBr(aq). pH before the addition of any HBr: pH after the addition of 12.5 mL HBr: pH after the addition of 24.0 mL HBr: pH after the addition of 25.0 mL HBr: pH after the addition of 32.0 mL HBr:

The pKa of hypochlorous acid is 7.530. A 51.0 mL solution of 0.122 M sodium hypochlorite (NaOCI) is titrated with 0.323 M HCI. Calculate the pH of the solution after the addition of 7.44 mL of 0.323 M HCl. pH = Calculate the pH of the solution after the addition of 20.0 mL of 0.323 M HCl. pH = 7.73 pH = 2.475 Calculate the pH of the solution at the equivalence point with 0.323 M HCI. & TOOLS

Consider the titration of 25.00 mL of 0.250 M NaOH by 0.355 M HCl. Calculate the pH of the solution before the titration and after 5.00 mL of the acid has been added. What volume of the acid is necessary to reach the equivalence point? What is the pH of the solution at the equivalence point?

Calculate the pH for each of the cases in the titration of 25.0 mL of 1.25 M pyridine, C5H5N(aq) with 0.250 M HBr(aq) at 25°C. The Kb of pyridine is 1.7×10−9. Report all your answers to 2 decimal places.  Before the addition of any HBr: After the addition of 10.0 mL of HBr:  After the addition of 62.5 mL of HBr:  After the addition of 125.0 mL of HBr: After the addition of 135.0 mL of HBr:

0 The pK, values for the dibasic base B are pKb1 = 2.10 and pKb2 = 7.67. Calculate the pH at each of the points in the titration of 50.0 mL of a 0.60 M B(aq) solution with 0.60 M HCl(aq). What is the pH before addition of any HCI? What is the pH after addition of 25.0 mL HC1? What is the pH after addition of 50.0 mL HC1? What is the pH after addition of 75.0 mL HC1? What is the pH after addition of 100.0 mL HC1? pH = pH pH = pH = pH = 12.76 11.9 9.2 6.33 1.4 Incorrect