Given the following experimental data, calculate the molarity and the pKa of the acid analyte (HA) in the titration, with the following data: HA + NaOH à NaA + H2O. -A pH reading of 3.65 is obtained when 13.0 mL of 0.413 M NaOH is added to the 25.0 mL analyte. -The endpoint of the titration is achieved when 31.25 mL of NaOH have been added. Show all your calculations.

Given the following experimental data, calculate the molarity and the pKa of the acid analyte (HA) in the titration, with the following data: HA + NaOH à NaA + H2O. -A pH reading of 3.65 is obtained when 13.0 mL of 0.413 M NaOH is added to the 25.0 mL analyte. -The endpoint of the titration is achieved when 31.25 mL of NaOH have been added. Show all your calculations.

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)...

See similar textbooks

Similar questions

Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
Malonic acid is a dicarboxylic acid with structure CH2(COOH)2 with Ka1 and Ka2 = 2.0 × 106. Consider the titration of 50.0 mL of 0.2 M disodium malonate = 1.5 x 10-3 (N22CH2(COO)2) by 0.2 M HCI and answer the following questions. Calculate the pH after the following total volumes of HCI have been added. a) 0.0 mL b) 25.0 mL c) 50.0 mL d) 75.0 mL e) 100.0 mL f) 110.0 mL
A 15.0 mL sample of 0.20 M of an unknown weak acid is titrated with 0.15 M NaOH at 25 oC. At 25 oC, the pKa of the weak acid is 4.06. What is the pH when 20.0 mL of titrant has been added to the analyte? Enter the answer to two decimal places.
A sample of vinegar weighing 10.52 g is titrated with NaOH. The end point is overstepped, and the solution is titrated back with HCl. From the following data, calculate the acidity of the vinegar in terms of percentage of acetic acid, CH3COOH Standardization Data:1.050 mL HCl ≡ 1.000 mL NaOH1.000 mL NaOH ≡ 0.06050 g benzoic acid, C6H5COOH (122.12 g/mol) Analysis Data:Volume NaOH used = 19.03 mLVolume HCl used for back titration = 1.50 mL
Determine the pH at the equivalence point in the titration of 50.0 mL of 0.300 M CH₃COOH with 0.300 M NaOH. The value of Ka for CH₃COOH is 1.8 × 10⁻⁵. Use a BCA table to detrmine the moles of reactant and product after the reaction of the acid and base. Ignore the amount of liquid water. Then, set up an ICE table to identify the unknown. Then figure the pH.
Malonic acid is a dicarboxylic acid with structure CH2(COOH)2 with Ka1 = 1.5 × 10-3 and Ka2 = 2.0 × 10-6. Consider the titration of 50.0 mL of 0.2 M disodium malonate (Na2CH2(COO)2) by 0.2 M HCl and answer the following questions. Calculate the pH after the following total volumes of HCl have been added.
The pKa of a weak acid acid HA is 4.47. Consider the titration of 100 mL of 200 mM HA (aq.) with 200 mM NaOH (aq). Draw a graph representing this titration that includes the following labeled points/regions, which are deliberately out of order. (A) pH=7| (B) Starting point (0 mL NaOH added)' (C) Region where the pH approaches 13.30 (D) Equivalence point| (E) Buffered region" (F) Halfway point And determine the pH and mL NaOH added for points B, D, and F
(a) What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant Ka of ha IS 5.66 X 10-7. Express the pH numericall to three decimal places (b) What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. Express the pH numerically to three decimal places. (c) What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of the base. Express the pH numerically to three decimal places
A 105.2 mL sample of 0.100 M methylamine ( CH3NH2; Kb = 3.7 x 10-4) is titrated with 0.270 M HNO3. Calculate the pH after the addition of each of the following volumes of acid. 39.0 mL Express the pH to two decimal places. pH =
In a titration, 25.00 mL of 0.1000 M triethyl amine ((CH3CH2)3N) is titrated with 0.0500 M hydrochloric acid (HCl). The following data was obtained: mL HCl added pH 0.00 11.86 25.00 10.71 50.00 6.79 What is pKa for the triethylammonium ion? 3.29 10.71 11.86 6.79
For the titration of 75 mL of 0.10 M acetic acid with 0.10 M NaOH, calculate the pH. For acetic acid, HC2H302, Ka = 1.8 x 105. (a) before the addition of any NaOH solution. Use correct number of significant digits; (b) after 25 mL of the base has been added. Use correct number of significant digits; (c) after half of the HC2H302 has been neutralized. Use correct number of significant digits; (d) at the equivalence point. Use correct number of significant digits;
You are going to titrate 29.0 mL of 0.294 M cyanic acid (HCNO) with 0.15 M NaOH. What is the pH of the solution after 5.684 mL of the NaOH has been added? The Ka of cyanic acid at the temperature of the experiment is 2.3 x 10-4. Report your answer to the hundredths place and do not include units