Write the chemical equation involved in the reaction between the excess acid and NaHCO3. Given this, briefly explain why NaHCO3 is preferred over NaOH for the neutralization of excess acid.

An analytical chemist is titrating 239.3 mL of a 0.8400M solution of methylamine (CH, NH,) with a 0.3300M solution of HNO,. The p K, of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 257.2 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH =

Use the equation of the dissociation of the weak acid and a Le Schatelier principle to answer the following question: What change will be caused by the addition of a small amount of the weak base B to a solution containing weak acid HB? O pH increase; pOH increase O no change at all O pH slightly decrease; pOH slightly decrease O pH slightly increase; pOH slightly decrease O pH decrease; pOH decrease

3. Explain at the molecular level why the pH increases as NaOH is added to CH,COOH.