a) What is the pH of a solution that consist of 0.20 M ammonia, NH3, and 0.20 M ammonium choride, NH4Cl? (Kb for ammonia is 1.8 x 10-5) b) 1.25 g of benzoic acid (C6H5CO2H) and 1.25 g of sodium benzoate (NaC6H5CO2) are dissolved in enough water to make 250 mL solution. Calculate the pH of the solution using the Handerson-Hasselbach equation (Ka for benzoic acid is 6.3 x 10-5). c) What is the pH after adding 82 mg of...
calculate the pH of the solution at the equivalence point when 25.0 mL of .10 M benzoic acid is titrated with 0.10 M potassium hydroxide. The Ka for benzoic acid is 6.3 x 10^-5
a) Calculate the pH of 0.500 L of a buffer solution that contains 0.200 M of benzoic acid C6H5CO2H and 0.100 M sodium benzoate NaC6H5CO2. Ka = 6.3 x 10-5. b) Calculate the pH after .10 mL of 1.00 M H+ has been added. c) Calculate the pH after 10 mL of 1.00 M OH- has been added.
How many milliliters of 1.0 M NaOH should be added to a 100 mL solution containing 12.212g of benzoic acid (F.W. 122.12g ; Ka = 6.28 x 10-5) to get a pH of 4.8?
What mass of sodium benzoate should you add to 150.0 mL of a 0.14 molL−1 benzoic acid solution to obtain a buffer with a pH of 4.25? For benzoic acid, Ka=6.3×10−5.
Calculate the pH of a buffer solution that results from combining 37.5 mL of a 0.450 M in benzoic acid (HC7H5O2) and 82.5 mL of a 0.250 M in sodium benzoate (NaC7H5O2). For benzoic acid, Ka = 6.5 × 10–5 .
#3. - Determine the pH, [H3O+], pOH and [OH‾] for each of the following. Be sure to write balanced chemical equation and the set-up for solving the problem. a. 1.5 M HNO3 b. 0.25 M Sr(OH)2 c. 0.035 M HNO2 d. 0.0048 M Mn(OH)2 #1 - What are the [H3O+] and the pH of a solution that consists of 0.33 M C6H5COOH (benzoic acid) and 0.28 M C6H5COONa (sodium benzoate)? The Ka of benzoic acid is 6.3 x 10-5. #8-...
What mass of sodium benzoate should you add to 140.0 mL of a 0.15 mol/L benzoic acid solution to obtain a buffer with a pH of 4.25? For benzoic acid, Ka= 6.3 • 10^-5
What is the pH of a solution prepared by mixing 25.0 mL of 0.100 M benzoic acid and 50.0 mL of 0.050 M KOH ? (Ka benzoic acid = 6.4 x 10-5) A. 8.36 B. 5.19 C. 8.81 D. 9.04 E. 5.64
Calculate the hydroxide ion concentration and the POH in an aqueous solution with a pH = 2.3 at 25°C. a. [OH 1 - 2.0 * 10-12M : POH - 2.30 b. [OH 7 -2.0 * 10-11M: POH = 11.70 C[OH 7 -5.0 x 10-3 M : POH = 11.70 d. [OH ) - 2.0 x 10-12 M : POH = 11.70 e.[OH ) - 2.0*10-12M : POH -8.50 Which of the following solutions is a good buffer system? a. A...