What is the pH of a 500 mL solution that is 0.40 M H2PO4-  and 0.20 M HPO42-? pKa values for H3PO4 are 2.14, 7.20, and 12.14. What will be the new pH if 0.02 mole of KOH is added to the above buffer?

1. What would be the pH of buffer containing 137ml of 3.50M boric acid and 228ml of 1.90M lithium borate. The pKa of buffer system is 13.80.  solved answer pH= 13.76 2. What would be the pH of the buffer from question 1, after adding 84.5ml of 0.71 M KOH (strong base) to buffer? ??

A buffer solution is made that is 0.452 M in HC10 and 0.452 M in KC10. If K, for HC10 is 3.50 x 10-8, what is the pH of the buffer solution? pH : Write the net ionic equation for the reaction that occurs when 0.100 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) +

The pK, values for the dibasic base B are pKi = 2.10 and pk2 = 7.49. %3! Calculate the pH at each of the points in the titration of 50.0 ml. of a 0.55 M B(aq) solution with 0.55 M HCI(aq). What is the pH before addition of any HCI? pH What is the pH after addition of 25.0 ml. HCI? pH = What is the pH after addition of 50.0 mL HC? pH What is the pH after addition of 75.0 mlL HCI? pH = What is the pH after addition of 100.0 ml. HCI? pH =

3. A buffer is prepared by adding 0.50 mol of acetic acid (HC₂H3O₂) and 0.75 mol of sodium acetate (NaC₂H302) to enough water to form 2.00L solution. (pKa for acetic acid is 4.74) Calculate the pH of the buffer.

Solutions for question 3 (a) and (b) please

What will be the resulting pH if we add 0.010 mole of HCl to 1 L of the acetate buffer solution in the previous example? 0.10 M CH3COOH, 0.15 M CH3COO-, pH = 4.92, pKa = 4.74(HINT: the pH should decrease but only slightly)