The initial pH of a 250.0 mL buffer that consists of 0.15 M nitrous acid and 0.13 M sodium nitrite is 3.41.  Calculate the pH of the buffer after 10.00 mL of 0.50 M HNO3 is added to the buffer. (Ka for nitrous acid = 4.5 x 10-4)

Calculate the pH (to 2 decimal points) of 0.175 M HC5H10O2 (pentanoic acid; Ka = 1.4 x 10-5)

Calculate the pH (to 2 decimal points) of 0.250 M HC4H7O2 (butanoic acid; Ka = 1.5 x 10-5)

Calculate the pH (to 2 decimal points) of 0.175 M HC3H4O2Cl (3-Chloropropanoic acid; Ka = 7.8 x 10-5)

Calculate the pH (to 2 decimal points) of 0.175 M HC5H10O2 (pentanoic acid; Ka = 1.4 x 10-5)

Consider the following endothermic reaction that is at equilibrium. Determine whether each of the following scenarios will shift the reaction to favor the products, the reactants, or neither. 

Calculate the pH (to 2 decimal points) of 0.520 M HBr (Bromic acid)

Calculate the pH (to 2 decimal points) of 0.250 M HClO3 (chloric acid) 

Calculate the pH (to 2 decimals) of 0.500 M acetic acid (Ka = 1.8 x 10-5). You can avoid using the quadratic equation.

Which acidic/basic salt is needed to create a buffer when mixed with pentanoic acid?