1- Identify buffer solutions from the following list.
Choose all that apply.
0.39 M sodium iodide + 0.25 M sodium bromide
0.14 M sodium hydroxide + 0.22 M sodium bromide
0.24 M hydrobromic acid + 0.21 M potassium bromide
0.17 M hypochlorous acid + 0.16 M potassium hypochlorite
0.29 M ammonia + 0.40 M ammonium bromide
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NDTAPMindTap – Cengage LearningHomework Help – Q&A fror SolutionsQ Search this courseBuffer SolutionsSubmit for GradingCurrent score:AutoTutored Practice Problem 17.2.7 COUNTS TOWARDS GRADEPrepare a buffer by acid-base reactions.Close ProblemConsider how to prepare a buffer solution with pH – 7.23 (using one of the weak acid/conjugate base systems shown here) by combining 1.00 L of a0.483-M solution of weak acid with 0.399 M potassium hydroxide.Weak Acid Conjugate BaseKapkaHNO2NO24.5 x 10-43.35HCIOCIO3.5 x 10-87.46HCNCN4.0 x 10-109.40How many L of the potassium hydroxide solution would have to be added to the acid solution of your choice?Check & Submit AnswerShow ApproachAlpha PlotsAs shown in the preceding example problems, the pH of a buffer solution is controlled by the relative amounts of weak acid and conjugate basepresent and by the weak acid pKa . That is, buffer pH is independent of solution volume. If a buffer solution is diluted, the pH does not change.Regardless of the amounts of weak acid and conjugate base that are present in the solution, however, the relative amounts can change if the pH is
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