The graph here shows the pH curve for the titration of 25.00 mL of a 0.100-M monoprotic acid solution, HA(aq), with a 0.1 M solution of a monoprotic base. 14 Hd 12 8 2. 10 15 20 25 30 35 40 45 50 Volume of 0.100-M base added (mL) (1) The pH curve represents the titration of a acid with a O base. (2) Choose a suitable indicator for the endpoint of the titration from the following pulldown lis v to the table of indicators in the Approach. Refer Bromocresol green Methyl red Bromothymol blue Submit Show Approach Show Tutor Steps Cresol red Thymol blue Phenolphthalein

The graph here shows the pH curve for the titration of 25.00 mL of a 0.100-M monoprotic acid solution, HA(aq), with a 0.1 M solution of a monoprotic base. 14 Hd 12 8 2. 10 15 20 25 30 35 40 45 50 Volume of 0.100-M base added (mL) (1) The pH curve represents the titration of a acid with a O base. (2) Choose a suitable indicator for the endpoint of the titration from the following pulldown lis v to the table of indicators in the Approach. Refer Bromocresol green Methyl red Bromothymol blue Submit Show Approach Show Tutor Steps Cresol red Thymol blue Phenolphthalein

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 74QAP: Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a)...

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Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
A 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was added
Calculate the pH at the equivalence point of 65 ml solution containing a weak acid, AH, for instance CH3COOH, titrated with 30 ml of a strong base, B OH, like KOH, with a concetration of 0.91 M. The acid dissociation constant, Ka , is 2.15e-7. pH ← please insert your value
Similar to acetic acid, benzoic acid is a weak acid (HA) and is a commonly used as antimicrobial preservative in food and beverages, especially in carbonated beverages Suppose 10.00-mL of 0.5000 M benzoic acid (C6H5COOH) is titrated with 0.2000M NaOH. Ka for benzoic acid is 6.3 x 10-5 . What is the pH after addition of 35.00 mL of NaOH to the benzoic acid solution?
Aspirin (Acetylsalicylic acid, C9H8O4) is a monoprotic weak acid with Ka= 3.16e-4. One way to verify the quanitity of this medication in a given tablet is through titration. Consider a titration of 50.00 mL of a 0.5000 M solution of acetylsalicylic acid with a 0.1000 M solutionn of NaOH. Calculate the volume of the titrant needed to reach the center of the buffer region.
Calculate the pH of a 1.07 M solution of a weak acid, AH, for instance CH3COOH, and 0.62 M of a salt derived by its conjugate base, ANa, like CH3COONa. The acid dissociation constant, Ka , is 2.27e-6. What is the pH if 38 mL of 0.149 M of a strong acid, like HCl, is added to 100 mL of the buffer solution? What if a strong base, like NaOH, is added with the same ammount instead ? pH ← please insert your values Add acid = _______ Add base = _________
1 Calculate the pH at the equivalence point in titrating 0.069 M solutions of each of the following with 0.056 M NaOH. (a) periodic acid (HIO4) pH = (b) ascorbic acid (HC6H7O6), Ka = 8e-05 pH = (c) hydrocyanic acid (HCN), Ka = 4.9e-10 pH
Calculate the pH at the equivalence point in titrating 0.077 M solutions of each of the following with 0.068 M NaOH. (a) hydrochloric acid (HCl) pH = (b) arsenous acid (H3AsO3), Ka = 5.1e-10 pH = (c) hydrazoic acid (HN3), Ka = 1.9e-05 pH =
A sample of 50.00 mL of 0.1000 M aqueous solution of chloroacetic acid, CH2ClCOOH (K1= 1.4 × 10-3), is titrated with a 0.1000 M NaOH solution. Calculate the pH at the following stages in the titration, and plot thetitration curve: 0, 5.00, 25.00, 49.00, 49.90, 50.00, 50.10, and 55.00 mL NaOH.
A weak base, ammonia, is to be titrated with hydrochloric acid. A volume of 30.0 mL of the 0.75 M NH3 (weak base) whose Kb = 5.25 x10^-6 is titrated with 0.96 M HCl (strong monoprotic acid). Assuming that the stoichiometry for this neutralization titration is 1:1 , calculate the ff: A. pH of the resulting solution when the volume of the added strong acid titrant neutralizes 70% of the analyte. B. pH of the resulting solution at the equivalence point. C. pH of the resulting solution at 5.0 ml added titrant beyond the equivalence point.
The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. 1. what is the pH when the volume of base added equals half the volume of the equivalence point? 2. what is the pH of the titration when 20.00 mL of base have been added? 3. what is the pH of the titration when 30.00 mL of base have been added?
Calculate the pH at each point in the titration of 20.0 mL of 0.125 M weak acid, HA, with a Ka value = 5.20x10-4with 0.100 M NaOH after the following increments of base: 0 mL, 20.0 mL, 25.0 mL and 30.0 mL.