Determination of the Concentration of Acetic Acid in Vinegar

Determination of the Absorption of Acerb Acerbic in Alkali Lab Exercise 4 CHEM 1106 9/19/12 Purpose: Standardize a sodium hydroxide band-aid application a primary accepted acid. Actuate the molarity and the percent by accumulation of acerb acerbic in alkali by titration with the connected sodium hydroxide solution. Introduction: Alkali is a adulterate band-aid absolute acerb acid. Since alkali has a low pH, it can be titrated with a base. Titration is a adjustment acclimated in adjustment to ascertain the bulk of a basic in a band-aid by barometer the aggregate of a accepted absorption of a reagent appropriate to complete a acknowledgment with it, about application a burette. The adequation point of a titration occurs back chemically agnate amounts of acerbic and abject are present. In this experiment, the adequation point occurs back the moles of acerbic in the band-aid equals the moles of abject added in the titration. A accelerated change in pH with the baby accession of acerbic or abject is the indicator of acid-base equivalency. Accompanying material: Alkali Battery Statement of the Problem Using a pH beat and a blueprint of pH advised against the aggregate of abject added, the adequation point can be accurately begin by award the point that is in the average of the vertical allotment of the curve. Once the adequation point of the titration is known, the absorption of the sodium hydroxide can be determined. Sodium hydroxide is acclimated to titrate alkali so that the absorption of the alkali is determined. The allotment of acerb acerbic in the band-aid can be bent from the absorption of the vinegar.  Part A – Standardization of a Sodium Hydroxide Solution: Prepare 150 mL of about 0. M sodium hydroxide band-aid from solid NaOH. The band-aid can be able in a beaker, it is not all-important to use a accelerating butt or a volumetric alembic because the NaOH band-aid will be standardized. Weigh a 150-mL alembic and almanac the accumulation to the abutting 0. 001 g. Add about 0.5 grams of potassium hydrogen phthalate (KHP) to the beaker. Almanac the accumulation of the alembic and KHP to the abutting 0. 001 g. Calculate the accumulation of KHP by aberration and almanac it. Add about 50 mL of distilled baptize to the beaker. Stir the band-aid until the KHP has attenuated completely. Record a titration ambit application the MeasureNet pH delving and bead counter. (See Appendix F) Repeat accomplish 2 and 3. From the plots, actuate the aggregate of NaOH appropriate to abrogate the KHP band-aid in anniversary titration. Almanac the volumes. Calculate the molarity of sodium hydroxide. Allotment B – Determination of Acerb Acerbic Absorption in Vinegar Transfer 2. 0 mL of alkali to a clean, dry 150 mL alembic application a 10-mL volumetric pipet. Add acceptable water, 50 mL, to awning the pH electrode tip during the titration. Record a titration ambit application the MeasureNet pH delving and bead counter. See Appendix F)  From the plots, actuate the aggregate of NaOH appropriate to abrogate alkali in anniversary titration. Almanac the volumes. Calculate the molarity of acerb acerbic in vinegar. Calculate the percent by accumulation of acerb acerbic in vinegar. Data: Allotment A - Standardization of a Sodium Hydroxide Band-aid Accumulation of beaker97. 47 g Accumulation of alembic + KHP97. 99 g Accumulation of KHP0. 52 g Aggregate of NaOH to abrogate the KHP solution7. 755 mL Molarity of sodium hydroxide 0. 535 M NaOH Allotment B – Determination of the Absorption of Acerb Acerbic in Alkali Aggregate of NaOH appropriate to abrogate vinegar3. 18 mL Molarity of acerb acerbic in vinegar0. 8515 M CH3COOH Percent by accumulation of acerb acerbic in vinegar5. 115%. Equations: (1) Molarity (M) = moles of solute/liter of band-aid (2) Percent solute= (grams of solute/grams of solution) x 100% (3) NaOH (aq) + CH3COOH (aq) NaCH3CO2 (aq) + H2O (l) (4) pH = -log[H3O+] (5) KHC8H4O4 (aq) + NaOH (aq) KNaC8H4O (aq) + H2O (l) Calculations: Allotment A - Standardization of a Sodium Hydroxide Band-aid Calculate the accumulation of KHP: (Mass of Alembic + KHP) – Accumulation of Alembic = Accumulation of KHP 97. 99g – 97. 47g = 0. 52g Calculate the molarity of sodium hydroxide: Moles of KHP = g/MW = 0. 52g/204. 22g = 0. 002546 mol KHP Equation 5 = 1:1 arrangement 0. 002546 mol KHP x 1 mol NaOH/1mol KHP = 0. 002546 mol NaOH Equation 1 = 0. 002546 mol/0. 004755 L = 0. 535 M NaOH Part B – Determination of the Absorption of Acerb Acerbic in Alkali Calculate the molarity of acerb acerbic in vinegar: 3. 318 mL/1000 = 0. 00318 L NaOH 0. 00318 L NaOH x 0. 535 mol/1L NaOH = 0. 001703 mol NaOH Equation 3 = 1:1 arrangement 0. 001703 mol NaOH x 1 mol CH3COOH/1 mol NaOH = 0. 001703 mol CH3COOH 2. 0 mL CH3COOH/1000 = 0. 0020 L CH3COOH Equation 1 = 0. 01703 mol CH3COOH/0. 0020 L soln. = 0. 8515 M CH3COOH Calculate the percent by accumulation of acerb acerbic in vinegar: 0. 0020 L CH3COOH x 0. 8515/1 L soln. = 0. 001703 mol CH3COOH 0. 001703 mol CH3COOH x (60. 06g CH3COOH/1 mol CH3COOH) = 0. 1023g CH3COOH 2. 0 mL CH3COOH x (1g CH3COOH/1 mol CH3COOH) = 2. 0 mL CH3COOH soln. Equation 2 of CH3COOH = (0. 1023 g CH3COOH/2. 0g CH3COOH) x 100% = 5. 115% Final Answer: Molarity of vinegar:0. 8515 M CH3COOH Percent mass: 5. 115% CH3COOH From the plots actuate the aggregate of NaOH appropriate to abrogate the KHP band-aid in anniversary titration.

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