A buffer solution was prepared by adding 4.96 g of sodium acetate,NaCH3CO2, to 2.50x 10^2  mL of 0.170 M acetic acid, CH3CO2H  (Ka=1.8 x 10^-5).  What is the pH of the system if you add 72 mg of NaOH to the 1.00x 10^2 mL of the prepared buffer solution?

A solution is prepared by dissolving 0.350 g of benzoic acid, HC7H5O2, in water to make 100.0 mL of solution. A 30.00-mL sample of the solution is titrated with 0.272 M KOH. Calculate the pH of the solution (a) before titration. (b) halfway to the equivalence point. (c) at the equivalence point.

A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.

A 5.36-g sample of NH4Cl was added to 25.0 mL of 1.00 M NaOH and the resulting solution diluted to 0.100 L.. (a) What is the pH of this buffer solution?. (b) Is the solution acidic or basic?. (c) What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to the solution?

The composition diagram, or alpha plot, for the important acid-base system of carbonic acid, H2CO3, is illustrated. (See Study Question 1.7 for more information on such diagrams.) (a) Explain why the fraction of bicarbonate ion, HCO3, rises and then falls as the pH increases. (b) What is the composition of the solution when the pH is 6.0? When the pH is 10.0? (c) If you wanted to buffer a solution at a pH of 11.0, what should be the ratio of HCO3 to CO32?

Acrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’. What is the pH of a 0.11 M solution of acrylic acid, CH2CHCOOH?

A buffer solution is prepared from 5.15 g NH4NO3 and 0.10 L of 0.15-M NH3; calculate the pH of the solution.

A buffer solution was prepared by adding 4.92 g of sodium acetate, NaCH3CO2, to 2.50 x 10^2 mL of 0.170 M acetic acid, CH3CO2H (Ka= 1.8 x 10^-5).  What is the pH of the system if you add 72 mg of NaOH to the 1.00 x 10^2 mL of the prepared buffer solution?

A buffer solution is prepared by dissolving 1.000 g of sodium acetate (CH3COONa) into 100.00 mL of a 0.100 M solution of acetic acid. Then 3.00 mL of a 2.00 M solution of sodium hydroxide is added to the acetic acid/sodium acetate buffer solution. The Ka of acetic acid is 1.8 × 10−5.   What is the pH of the solution after adding NaOH?

If a buffer solution is made of 12.2 g of benzoic acid (C6H5COOH) and 7.20 g of sodium benzoate (C6H5COONa) in exactly 250 mL of solution, what is the pH of the buffer?  If the solution is diluted to exactly 500 mL with pure water, what is the new pH of the solution?