What is the pH at the equivalence point in the titration of a 24.0 mL sample of a 0.391 M aqueous hypochlorous acid solution with a 0.468 M aqueous sodium hydroxide solution?

In an alkalinity titration of a 100.0 mL sample of water from a hot spring, 2.56 mL of a 0.0365 M  solution of HCl is needed to reach the first equivalence point (pH = 8.3) and another 10.42 mL is needed to reach the second equivalence point (pH = 4.0). If the alkalinity of the spring water is due only to the presence of carbonate and bicarbonate, what are the concentrations of each of them? What is the concentration of carbonate?     M        What is the concentration of bicarbonate?

Which of the following aqueous solutions are good buffer systems?. 0.34 M nitrous acid + 0.27 M potassium  nitrite 0.30 M ammonium  bromide + 0.31 M ammonia 0.15 M sodium  hypochlorite + 0.22 M hypochlorous acid 0.28 M nitric acid + 0.23 M sodium  nitrate 0.14 M hydrocyanic acid + 0.11 M potassium  cyanide   you can choose multiple choices if needed.

Which of the following aqueous solutions are good buffer systems? | 0.30 M ammonia + 0.39 M ammonium bromide O 0.12 M barium hydroxide + 0.21 M barium bromide | 0.23 M hydrochloric acid + 0.21 M potassium chloride O 0.16 M hydrocyanic acid + 0.11 M hydroiodic acid O 0.40 M calcium iodide + 0.29 M potassium iodide

Use the References to acces Which of the following aqueous solutions are good buffer systems? 0.27 M ammonium bromide + 0.37 M ammonia O 0.12 M acetic acid + 0.20 M sodium acetate 0.25 M hydrochloric acid + 0.24 M sodium chloride O 0.15 M sodium fluoride + 0.21 M hydrofluoric acid O 0.39 M hydrocyanic acid + 0.29 M sodium cyanide

When a 28.1 mL sample of a 0.465 M aqueous acetic acid solution is titrated with a 0.419 M aqueous potassium hydroxide solution, what is the pH at the midpoint in the titration? pH = 35.9 mL sample of a 0.576 M aqueous hypochlorous acid solution is titrated with a 0.329 M aqueous sodium hydroxide solution. What is the pH after 42.9 mL of base have been added? Ka for HC1O is 3.5 × 10-8. pH = A 26.3 mL sample of 0.296 M ethylamine, C₂H5NH₂, is titrated with 0.246 M perchloric acid. At the titration midpoint, the pH is A 20.0 mL sample of 0.369 M diethylamine, (C₂H5)₂NH, is titrated with 0.320 M perchloric acid. After adding 8.88 mL of perchloric acid, the pH is

I don’t understand

Which of the following aqueous solutions are good buffer systems? 0.28 M perchloric acid + 0.19 M sodium perchlorate 0.38 M sodium perchlorate + 0.29 M barium perchlorate 0.16 M potassium hydroxide + 0.20 M potassium chloride 0.30 M ammonia + 0.35 M sodium hydroxide 0.15 M acetic acid + 0.12 M sodium acetate

When a 18.3 mL sample of a 0.460 M aqueous hydrocyanic acid solution is titrated with a 0.330 M aqueous barium hydroxide solution, (1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 19.1 mL of barium hydroxide have been added?

Which of the following aqueous solutions are good buffer systems?   0.13 M acetic acid + 0.20 M sodium acetate 0.20 M nitric acid + 0.25 M sodium nitrate 0.28 M ammonium nitrate + 0.36 M ammonia 0.13 M potassium hydroxide + 0.22 M potassium chloride 0.32 M nitrous acid + 0.30 M sodium nitrite