Carbonate and bicarbonate can be combined to form a buffer system.  How many grams of magnesium carbonate would have to be dissolved in 750.0 mL of a 0.1330 M bicarbonate solution to prepare a solution with a pH of 9.33? (Ka of bicarbonate is 4.7 X 10 -11)

Which weak acid would be best to use when preparing a buffer solution with a pH of 6.2? An acid with K, = 2.5 x 10-3 An acid with K, = 3.2 x 10-7 An acid with K, = 2.5 x 10* An acid with K, = 1.7 x 10-10 An acid with K, = 1.0 x 10-"

A buffer solution is made that is 0.417 M in HC1O and 0.417 M in KC1O. If K, for HC1O is 3.50 × 10-8, what is the pH of the buffer solution? PH = Write the net ionic equation for the reaction that occurs when 0.110 mol HNO3 is added to 1.00L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H30* instead of H*)

The acid HZ has a pKa of 7.03.  If 25.00 mL of a 0.111 M solution of HZ are titrated with 0.100 M NaOH solution, what's the pH before any base is added?