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Name: 1. 40.0mL of 0.120M benzoic acid (CHiCH CH,CO,H, K, 1.52 x 10) is being titrated...
20. A 50.00-mL solution of 0.0350 M benzoic acid (Ka 6.4 x 10) is titrated with a 0.0134 M solution of sodium hydroxide as the titrant. What is the pH of the acid solution after 15.00 mL of titrant have been added? (Kw 1.00 x 10-14) A) 2.83 B) 9 C) 4.19 D) 3.37 E) 1.46 9.6
Assume you dissolve 0.367 g of the weak acid benzoic acid, CH3CO2H, in enough water to make 1.00 x 102 mL of solution and then titrate the solution with 0.101 M NaOH. K, for benzoic acid = 6.3 x 10-5) CH, CO,H(aq) + OH- (aq) = CH,CO, - (aq) + H20(0) a. What was the pH of the original benzoic acid solution? pt pl pH = pt b. What are the concentrations of all of the following ions at the...
сн. A 75.0 mL solution of 0.146 M potassium alaninate (H, NC,H,CO,K) is titrated with 0.146 M HCl. The pK values for the amino acid alanine are 2.344 (PK) and 9.868 (pK22), which correspond to the carboxylic acid and amino groups, respectively. H2N- CH-C- Calculate the pH at the first equivalence point. Potassium Alaninate pH = Calculate the pH at the second equivalence point. pH =
2. 20.00 mL of 0.270 M HA (K. = 7.2 x 10-4) was titrated with 0.300 M sodium hydroxide (3 + 3 + 2 + 3 + 3 + 3 + 12 = 29 points) a) Write the titration equation and calculate volume of NaOH needed to reach the equivalence point. ml b) At what volume of the titrant would pH=pKa? Why? c) pH at the equivalence point when the acid and base are neutralized will be ..choose one of...
1. A weak acid (benzoic acid) is titrated with a strong base such as sodium hydroxide. Determine the pH at the half equivalence point of the titration. The Ka of the weak acid is 6.3 x 10-5. 2.Calculate the pH of a buffer made from 0.6 M HNO2 and 0.5 M NaNO2. Ka = 4.5 x 10-5 pKa = 4.3 Answer with one digit after the decimal place (e.g. 2.1) Hint: HNO2 is a weak acid. NaNO2 forms the conjugate...
A buffer containing acetic acid and sodium acetate has a pH of 5.55. The K, value for CH3CO,H is 1.80 x 10. What is the ratio of the concentration of CH3CO H to CH3CO,t? [CH,CO,H1 CH2C0, 1 = Calculate the pH of a solution that has an ammonium chloride concentration of 0.054 M and an ammonia concentration of 0.053 M. Kb = 1.8 x 10-5 pH = What is the pH of 0.35 M acetic acid to 1.00 L of...
Assume you dissolve 0.132 g of the weak acid benzoic acid, C6H; CO2H, in enough water to make 1.00 x 102 mL of solution and then titrate the solution with 0.184 M NaOH.( K, for benzoic acid = 6.3 x 10-5.) CoH; CO, H(aq) + OH (aq) = C, H; CO2 (aq) + H20(4) a. What wasythe pH of the original benzoic acid solution? pH = b. What are the concentrations of all of the following ions at the equivalence...
CH3 A 60.0 mL solution of 0.183 M potassium alaninate (H2NC,H,CO,K) is titrated with 0.183 M HCl. The pKa values for the amino acid alanine are 2.344 (pKal) and 9.868 (pKa2), which correspond to the carboxylic acid and amino groups, respectively. H2NCH——0 Calculate the pH at the first equivalence point. Potassium Alaninate pH = Calculate the pH at the second equivalence point. pH = ||
15. (25 pts) If 50 mL of 0.20 M benzoic acid (K, = 6.5 x 10) is titrated with 0.25 M NaOH, what is the pH after 0 ml, 10 ml, 20 ml, 40 ml and 50 ml of base have been added? (You may use the approximation.). BE SURE TO SHOW ALL CALCULATIONS.
3. Pyruvic acid, C- , is a monoprotic acid with K. = 3.3 x 10-3 and pk, = 2.48. In H. C OH a titration experiment, pyruvic acid (0.090 M, 50.00 mL) was titrated with NaOH (0.108 M). Find the pH (a) Before any NaOH is added. (b) After 5, 10, 20, 30 and 40 mL of NaOH are added. (c) At the equivalence point. (d) And after 10 mL excess NaOH is added.