Explain a simple and practical way to make

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Reference no: EM13181611

A) What combination of a molecular base (compound must be neutral and not contain a cation) and a salt (must be composed of a cation and anion) of the conjugate acid of the molecular base (don't forget to specify a common spectator ion as the anion in the salt) should you select to prepare a buffer solution that would maintain a pH of 9.00? Explain how you came to that answer.

B)What ratio of concentrations of the molecular base you chose in part A and its conjugate acid would be necessary to achieve a pH of exactly 9.00?

C) Describe a simple and practical way to make 1.00 L of this buffer solution, assuming a 1.0 M solution of the molecular base is available and that the chloride salt of the conjugate acid is available as a solid. (Note: Lab balances are calibrated to measure in grams and pipettes in mL, neither of these are calibrated in moles hint hint!)

Reference no: EM13181611

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