Calculate the pH of a buffer solution that contains 0.76 M NaH2PO4 and 0.28M Na2HPO4.   Calculate the change in pH if 0.090 g of solid NaOH is added to 150 mL of the solution in the problem above.

1. A buffer solution contains 0.419 M of ammonium chloride and 0.221 M of ammonia.If 0.0293 moles of sodium hydroxide are added to 150 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume does not change upon adding sodium hydroxide.) 2. A buffer solution contains 0.286 M of ammonium chloride and 0.472 M of ammonia. If 0.0620 moles of nitric acid are added to 250 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume does not change upon adding nitric acid.)

A buffer solution contains 0.235 M ammonium bromide and 0.314 M ammonia. If 0.0164 moles of hydrobromic acid are added to 125 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume change does not change upon adding hydrobromic acid) pH =

A buffer is made by adding 0.300 mol HC:H:Oz and 0.300 mol NaC:H»O2 to enough water to make 1.00 L of solution. Ka for acetic acid is 1.8 × 105. 3. Calculate the pH after 5.0 ml of 4.0 M NaOH is added. 4. Calculate the pH after 5.0 mL of 4.0 M HCl is added.