A beaker with 175 mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 7.60 mL of a 0.330 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.760.
At 25 degrees C phosphoric acid, H3PO4, has the following equilibrium constants:
Ka1 = 7.5 X 10-3
Ka2 = 6.2 X 10-8
Ka3 = 4.2 X 10-13
What is the pH of a solution of 0.700 M K2HO4, potassium hydrogen phosphate?
What is the pH of a solution of 0.750 M KH2PO4, potassium dihydrogen phosphate?