18. Aqueous Equilibrium

Calculate the pH of the solution resulting from the mixing of 75.0 mL of 0.100 M NaC₂H₃O₂ and 75.0 mL of 0.30 M HC₂H₃O₂ with 0.0040 moles of HBr.

In order to create a buffer 7.321 g of potassium lactate is mix with 550.0 mL of 0.328 M lactic acid, HC₃H₅O₃. What is the pH of the buffer solution after the addition of 300.0 mL of 0.100 M hydrobromic acid, HBr? The K_a of HC₃H₅O₃ is 1.4 × 10⁻⁴.

Consider the titration of 100.0 mL of 0.100 M CH₃NH₂ with 0.250 M HNO₃ at the equivalence point. What would be the pH of the solution at the equivalence point? The K_b of CH₃NH₂ is 4.4 × 10⁻⁴.

A solution contains 100.0 mL of 0.550 M sodium nitrite, NaNO₂. Find the pH after the addition of 180.0 mL of 0.400 M HClO₄. The K_a of HNO₂ is 4.6 × 10⁻⁴.

A 1.0-L buffer solution is 0.125 M in HNO2 and 0.145 M in NaNO2. Determine the concentrations of HNO2 and NaNO2 after the addition of each substance: a. 1.5 g HCl

Consider the titration of a 25.0-mL sample of 0.175 M CH3NH2 with 0.150 M HBr. Determine each quantity. c. the pH at 5.0 mL of added acid