1) Calculate the pH of the buffer solution based on the known Ka value for acetic acid. pH = %3D

A buffer solution has a pH value of 9.8. Which value in the set of pH values 8.79.79.89.910.9 is the most likely value for the buffer solution pH after a. a small amount of strong acid has been added? b. a small amount of strong base has been added?

Calculate the pH of solutions that are 0.25 M formic acid and 0.40 M sodium formate. 0.50 M benzoic acid and 0.15 M sodium benzoate.

a.Calculate the pH of a buffer that is 0.1M in lactic acid, C2H4(OH)COOH, and 0.1M in sodium lactate, C2H4(OH)COONa. b.What is the pH of a buffer that is 1M in lactic acid and 1M in sodium lactate? c.What is the difference between the buffers described in parts a and b?

Which of these combinations is the best to buffer the pH at approximately 9? Explain your choice. CH3COOH/NaCH3COO HCl/NaCl NH3/NH4Cl

Explain why barium fluoride dissolves in dilute hydrochloric acid but is insoluble in water.

Vitamin C is ascorbic acid (HC6H7O6), for which Ka is 8.0105. Calculate the pH of a solution made by dissolvinga 500-mg tablet of pure vitamin C in water anddiluting to 100 mL.

A buffer solution is prepared by adding 0.125 mol ammonium chloride to 500. mL of 0.500-M aqueous ammonia. Calculate the pH of the buffer. If 0.0100 mol HCl gas is bubbled into 500. mL buffer and all of the gas dissolves, calculate the new pH of the solution.

Which of the following is true of a buffer solution that contains equivalent amounts of acid and conjugate base? O The pH of the solution will be equal to Kw. The pH will be equal to the concentration of the conjugate base. O The pH of the solution will be equal to the pka of the acid. O The pH will always be greater than 7, regardless of the acid and conjugate base. The pH will be equal to the concentration of the acid.

You have chosen Methylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.48 M in this salt. The desired pH of the buffer should be equal to 9.75. To prepare the buffer, a total volume of 550 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 0.98 M. (Remember the lesson on dilution: C1V1=C2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (round off final answer to 1 decimal place)