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Calculate the ph of an aqueous solution

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Reference no: EM132363059

Question

A. Select and justify (through solving) which will be the more acidic solution and which will have the lower pH.

  1. 0.10M aspirin (pKa = 3.47) or 0.10M acetic acid (pKa = 4.74)
  2. Beer with [H3O+] = 3.16 x 10-5 or wine with [H3O+] = 5.01 x 10-4
  • How do you especially solve for the [H3O+]? I don't really get what the purpose of this when with pH and pOH.

B. If the [OH-] = 1 x 10-14 M what is the [H3O+] and pH of the solution?

C. Blood plasma had a pH range of 7.35 - 7.45. From the midpoint of this range calculate the following:

  1. [H3O+]
  2. [OH-]
  3. pOH

D. Find the pH of a 400.0 mL solution with a concentration of 0.75 M NaOH.

E. Calculate the pH of an aqueous solution containing 0.80 M lactic acid and 0.40 M lactate acid.

Reference no: EM132363059

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