Which of the following aqueous solutions are good buffer systems? 0 0.27 M hydroiodic acid + 0.22 M potassium iodide ) 0.27 M ammonia + 0.31 M barium hydroxide O 0.12 M calcium hydroxide + 0.23 M calcium bromide | 0.31 M barium chloride + 0.27 M potassium chloride O 0.19 M hydrocyanic acid + 0.21 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

Which of the following aqueous solutions are good buffer systems? 0.10 M nitrous acid + 0.13 M sodium nitrite 0.31 M ammonium bromide + 0.31 M ammonia 0.29 M hydroiodic acid + 0.23 M potassium iodide 0.16 M potassium fluoride + 0.21 M hydrofluoric acid O 0.39 M acetic acid + 0.25 M potassium acetate

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

Which of the following are good buffer systems?

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

A student was required to prepare 250.0 mL of a cyanoacetic acid/sodium cyanoacetate buffer in which the concentration of the weak acid component was 0.06 M and the concentration of the conjugate base was 0.028 M. The student was supplied with 0.512 M cyanoacetic acid and 1.0M NaOH to perform this task. What volume (in mL) of the acid would the student need to prepare this buffer solution? Hint: assume that all of the conjugate base comes directly from the reaction of NaOH with the weak acid (in other words, there is negligible dissociation of the weak acid). Please enter answers with 2 decimal places.

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A student is making a titration curve. To do so, they added 25.00 mL of 0.1390 M HCl to a flask. They then added 36.78 mL of 0.1080 M KOH to the flask. What is the pH at this point in the titration curve?

Which of the following aqueous solutions are good buffer systems? O0.13 M hypochlorous acid + 0.12 M sodium hypochlorite O 0.10 M potassium fluoride + 0.30 M hydrofluoric acid 0.27 M hydrobromic acid + 0.23 M potassium bromide 0.39 M acetic acid + 0.28 M potassium acetate O 0.34 M ammonium nitrate + 0.38 M ammonia