Find the pH of the equivalence point and the volume (mL) of 0.0865 M KOH needed to reach the equivalence point in the titration of 23.4 mL of 0.0390 M HNO₂. Volume: pH = mL KOH

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 HC1. Calculate the pH of the solution after the addition of 7.44 mL of 0.323 M HC1. pH = Calculate the pH of the solution after the addition of 20.0 mL of 0.323 M HCl. pH = Calculate the pH of the solution at the equivalence point with 0.323 M HCI. pH =

Calculate the pH for each of the cases in the titration of 25.0 mL of 0.230 M pyridine, C₂H₂N(aq) with 0.230 M HBr(aq). The K of pyridine is 1.7 × 10-⁹. before addition of any HBr pH = after addition of 12.5 mL of HBr after addition of 18.0 mL of HBr after addition of 25.0 mL of HBr after addition of 30.0 mL of HBr x10 pH = pH = = pH = TOOLS 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?

15. How many grams of sodium acetate must be added to 0.100 L of 0.150 M acetic acid to obtain a buffer having a pH = 5.00. Ignore volume changes due to adding the sodium acetate. K, 1.8 x 10° for HC2H3O2 16. Determine the pH of a buffer made by adding 50.0 mL of 2.00 M acetic acid with 100.0 mL of 2.00 M sodium acetate. Ka = 1.8 x 10 for HC2H;O2

Calculate the pH at the equivalence point for the titration of 0.230 M methylamine (CH 3 NH 2 ) with 0.230 M HCI. The Kb of methylamine is 5.0 * 10 ^ - 4

Calculating the pH of a weak acid titrated with a strong base 0/5 Izabella An analytical chemist is titrating 127.4 mL of a 0.4200M solution of nitrous acid (HNO 2) with a 0.2400M solution of KOH. The pK of nitrous acid is 3.35. Calculate the pH of the acid solution after the chemist has added 260.9 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH = 0 ☑ G 000 18 Ar B

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

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:

A sample weighing 1.25 g of the diprotic acid potassium acid phthalate (KHP) is dissolved in 50.0 ml of water. Consider the titration of this solution with 0.100 M NaOH. The two Ka’s for KHP are 1.12 x 10-3 and 3.90 x 10-6   Calculate the pH of this solution before adding any NaOH. How many ml of NaOH must be added to reach the equivalence point? What is the pH at the equivalence point? Calculate the pH of the solution after 100. ml of NaOH have been added.