What is the pH at the equivalence point if 25.0 ml of 0.015 M benzoic acid (HC7H5O2 , pKa=4.19) is titrated with 0.025 M NaOH?
What is the pH at the equivalence point if 25.0 ml of 0.015 M benzoic acid...
Calculate the pH at the equivalence point when 40.0 mL of 0.100 M benzoic acid is titrated with 40.0 mL 0.100 M NaOH. HC7H5O2(aq) + H2O (l) C7H5O2-(aq) + H3O+(aq) Ka = 6.3 x 10 -5 A. 9.17 B. 3.22 C. 4.97 D. 10.1 E. 8.45 F. 9.00 G. 7.96 H. 6.07
25.00 mL of 0.150M benzoic acid HC7H5O2 was titrated with 0.200 M NaOH. Calculate the pH at the following points. Ka for benzoic acid is 6.3x10-5 a. Before adding any NaOH b. Halfway to equivalence c. After adding 12.2 mL of the NaOH d. At the equivalence point Please answer all the parts!
8) A 25.0 mL sample of 0.150 M benzoic acid is titrated with a 0.150 M NaOH solution. What is the pH at the eq. point? pka= 4.20
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 25.0 mL sample of 0.150 M benzoic acid is titrated with a 0.150 M NaOH solution. What is the pH after the addition of 13.0 mL of NaOH? The Ka of benzoic acid is 6.3x10-5.
Calculate the pH at the halfway point and at the equivalence point for each of the following titrations a. 100.0 ml of 0.70M HC7H5O2 (Ka= 6.4x10^-5) titrated by 0.10 M NaOH pH at the halfway point = ______? pH at the equivalence point = _____? b. 100.0ml of 0.70M C2H5NH2 (Kb= 5.6x10^-4) titrated by 0.60M HN03 pH at the halfway point = ______? pH at the equivalence point = _____? c. 100.0 ml of 0.70M HCL titrated by 0.15m NaOH...
A sample of 0.2140 g of an unknown monoprotic acid was dissolved in 25.0 mL of water and titrated with 0.0950 M NaOH. The titration required 30.0 mL of base to reach the equivalence point, at which point the pH was 8.68. a) What is the molecular weight of the acid? b) What is the pKa of the acid?
Calculate the pH at the equivalence point in titrating 0.047 M solutions of each of the following with 0.055 M NaOH. (a) nitric acid (HNO3) pH = (b) acetic acid (HC2H3O2), Ka = 1.8e-05 pH = (c) benzoic acid (HC7H5O2), Ka = 6.3e-05 pH = Calculate the pH at the equivalence point in titrating 0.047 M solutions of each of the following with 0.055 M NaOH. (a) nitric acid (HNO3) pH = (b) acetic acid (HC2H302), Ka = 1.84-05...
Calculate the pH at the equivalence point in titrating 0.047 M solutions of each of the following with 0.055 M NaOH. (a) nitric acid (HNO3) pH = (b) acetic acid (HC2H3O2), Ka = 1.8e-05 pH = (c) benzoic acid (HC7H5O2), Ka = 6.3e-05 pH = Calculate the pH at the equivalence point in titrating 0.047 M solutions of each of the following with 0.055 M NaOH (a) nitric acid (HNO3) pH= (b) аcetic acid (HC2H302), ка = 1.8e-05 pH =...
A 25.0 mL sample of 0.150 M chloroacetic acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The of chloroacetic acid is 1.4 ×10-3.