Reference no: EM13898012

Calculate the ratio of ethyl amine (CH3CH2NH2) to the ethyl ammonium ion (CH3CH2NH3+) in a solution with a pH of 11.0. pKa for CH3CH2NH3+ = 10.636.

A buffer solution was prepared by mixing 50.0 mL of a 0.100 M solution of CH3COOH with 0.500 grams of NaCH3COO. The resulting mixture is diluted to 100.0 mL. What is the pH of the solution? Ka for acetic acid is 1.75 x 10-5.

How many grams of NaCH3COO must be added to 150.0 mL of a 0.150 M solution of CH3COOH to produce a buffer of pH 4.75? Assume that the volume will remain constant, pKa for CH3COOH = 4.757

A buffer solution was prepared by dissolving 5.00 grams of sodium propanate (NaCH3CH2CO2) in a solution containing 0.100 moles of propanoic acid (CH3CH2CO2H) and diluting the mixture to 500.0 mL. To this solution was added 5.00 mL of 1.00 M HCl. Calculate the pH of the resulting solution. pKa for propanoic acid is 4.874.

A beaker containing 500.0 mL was determined to contain 0.150 M ammonia (NH3) and 0.150 M ammonium chloride NH4Cl. To this solution was added 50.0 mL of 0.15 M HCl. What was the change in pH of the ammonia-ammonium ion solution? pKa for NH4+ = 9.244.

What weight of sodium lactate (CH3CHOHCOONa; MW = 112.05) must be added to 500 mL of 0.200 M lactic acid (CH3CHOHCOOH, MW= 90.07; Ka = 1.4 x 10-4) in order to produce a buffered solution with a pH = 4.50?