You make 250 mL of a 75 mM CHES buffer (pKa=9.3) and adjust the pH to 9.0. Determine what volume (in mL) of 0.85M NaOH you would have to add to this buffer to exceed its buffer capacity.

2. What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium chloride (NH4CI) in enough water to form 2.50L of solution. The Kb of ammonia is 1.76 x 10-5.

a) Determine the mass (in grams) of sodium formate that must be added to 1.00 L of 0.180 M formic acid to prepare a buffer with a pH = 3.50. Assume there is no change in volume upon addition of the sodium formate. b) Write the predominant chemical reaction that occurs when 0.050 mol of HClO4 is added to 1.00 L of the buffer prepared in part a and calculate the pH of the solution.

Calculate the pH of solution after the addition of 0.010 mol NaOH to 1.00L of a 0.100 M acetic acid / 0.100 M sodium acetate buffer solution. (Ka = 1.8 x 10*) What is the neutralization reaction that happens? Is the system still a buffer after neutralization?