2.1 The correct indicator was added to 25.00 mL of a 0.1345 M solution of propanoic acid (CH3CH2COOH) (Ka = 1.3 x 10-5 ) in a flask, and this was titrated with a 0.1895 M solution of sodium hydroxide from a burette. 2.1.1 Write the net ionic balanced equation for the reaction taking place (include all phases) 2.1.2 Determine the final concentrations of the acid-base conjugate pair present after the titration, and show that the ratio of these species' concentrations is 1:1 at half the equivalence point. Hint: Firstly, determine the volume of base (in mL) that is required to reach the equivalence point for this titration. You may make use of a table to determine the amounts of species present. 2.1.3 Using the Henderson-Hasselbalch equation, determine the pH of the solution in the flask at this point.

2.1 The correct indicator was added to 25.00 mL of a 0.1345 M solution of propanoic acid (CH3CH2COOH) (Ka = 1.3 x 10-5 ) in a flask, and this was titrated with a 0.1895 M solution of sodium hydroxide from a burette. 2.1.1 Write the net ionic balanced equation for the reaction taking place (include all phases) 2.1.2 Determine the final concentrations of the acid-base conjugate pair present after the titration, and show that the ratio of these species' concentrations is 1:1 at half the equivalence point. Hint: Firstly, determine the volume of base (in mL) that is required to reach the equivalence point for this titration. You may make use of a table to determine the amounts of species present. 2.1.3 Using the Henderson-Hasselbalch equation, determine the pH of the solution in the flask at this point.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 98AP

See similar textbooks

Similar questions

4.51 What is the role of an indicator in a titration?
Carminic acid, a naturally occurring red pigment extracted from the cochineal insect, contains only carbon, hydrogen, and oxygen. It was commonly used as a dye in the first half of the nineteenth century. It is 53.66% C and 4.09% H by mass. A titration required 18.02 mL of 0.0406 M NaOH to neutralize 0.3602 g carminic acid. Assuming that there is only one acidic hydrogen per molecule, what is the molecular formula of carminic acid?
Hydrochloric acid. HCl, with a concentration of 0.100 M can be purchased from chemical supply houses, and this solution can be used to standardize the solution of a base. If titrating 25.00 mL of a sodium hydroxide solution to the equivalence point requires 29.67 mL of 0.100 M HCI, what is the concentration of the base?
Calcium in blood or urine can be determined by precipitation as calcium oxalate, CaC2O4. The precipitate is dissolved in strong acid and titrated with potassium permanganate. The equation for reaction is 2MnO4(aq)+6H+(aq)+5H2C2O4(aq)2Mn2+(aq)+10CO2(g)+8H2O A 24-hour urine sample is collected from an adult patient, reduced to a small volume, and titrated with 26.2 mL of 0.0946 M KMnO4. How many grams of calcium oxalate are in the sample? Normal range for Ca2+ output for an adult is 100 to 300 mg per 24 hour. Is the sample within the normal range?
A sample of solid calcium hydroxide, Ca(OH)2, is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00102M HCl requires 36.6 mL of the acid to reach the end point. Ca(OH)2(aq)+2HCl(aq)CaCl2(aq)+2H2O(l) What is the molarity?
Copper has compounds with copper(I) ion or copper(II) ion. A compound of copper and chlorine was treated with a solution of silver nitrate, AgNO3, to convert the chloride ion in the compound to a precipitate of AgCl. A 59.40-mg sample of the copper compound gave 86.00 mg AgCl. a Calculate the percentage of chlorine in the copper compound. b Decide whether the formula of the compound is CuCl or CuCl2.
In most of its ionic compounds, cobalt is either Co(II) or Co(III). One such compound, containing chloride ion and waters of hydration, was analyzed, and the following results were obtained. A 0.256-g sample of the compound was dissolved in water, and excess silver nitrate was added. The silver chloride was filtered, dried, and weighed, and it bad a mass of 0.308 g. A second sample of 0.416 g of the compound was dissolved in water, and an excess of sodium hydroxide was added. The hydroxide salt was filtered and heated in a flame, forming cobalt(III) oxide. The mass of cobalt(III) oxide formed was 0.145 g. a. What is the percent composition, by mass, of the compound? b. Assuming the compound contains one cobalt ion per formula unit, what is the formula? c. Write balanced equations for the three reactions described.
The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing small water-soluble ions and molecules. The iron in the aqueous solution is reduced to iron(II) ion and then titrated against potassium permanganate. In the titration, iron(ll) is oxidized to iron(III) and permanganate is reduced to manganese(II) ion. A 5.00-g sample of hemoglobin requires 32.3 mL of a 0.002100 M solution of potassium permanganate. The reaction with permanganate ion is MnO4(aq)+8H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+(aq)+4H2O What is the mass percent of iron in hemoglobin?
What is the concentration of NaCl in a solution if titration of 15.00 mL of the solution with 0.2503 M AgNO3 requires 20.22 mL of the AgNO3 solution to reach the end point? AgNO3(aq)+NaCl(aq)AgCl(s)+NaNO3(aq)
Citric acid, which can be obtained from lemon juice, has the molecular formula C6H8O7. A 0.250-g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?