Analysis of Aspirin Tablets, Lab Report Example

Abstract

The Brønstead Lowry paradigm of protons which donate electrons and protons which accept electrons in the acid- based chemical reactions is a substantial improvement over the theories of their predecessors. The Arrhenius theory suggested those base chemicals which have a pH higher than 7 were restricted to the hydroxyl collection. The primary implication of the Brønstead- Lowry theory is to classify the transfer of electrons by protons in the reactions between acids and bases. The ionic element which is a residue subsequent to the reaction is designated as the acid’s conjugated base. The compound and the reaction are classified as:

Base + acid ? conjugated acid + conjugated base

The acid becomes a giver of the H⁺ (Hydronium) ion to become the conjugated base. The base receives the proton and converts into a conjugated acid. The proposed experiment will demonstrate the reaction in the titration of acetylsalicylic acid with a sodium hydroxide base. This will occur during the analysis of five different brands of aspirin. These brands are: Bayer Aspirine, Contra- Schmerz Plus, Alcacyl, Asperger and Alka- Seltzer. The goal of this experiment is to apply the theories proposed by Lewis and Brønstead- Lowry in assessing the quantity of acetylsalicylic acid contained in the samples.

Introduction

The aim of this experiment is to ascertain the number of moles of aspirin (acetylsalicylic acid) which is manifest in five distinct tablets providing titration for the compound with a sodium hydroxide solution 0.100 dm^-3 as a base. The determination will be conducted if the acid possesses a robust of feeble aspect in accordance with the Lewis and Brønstead – Lowry theories. The formula of the reaction which occurs between the acid and the base will be ascertained (Burgot, 1997; Chou &Lai, 2004; Gris et al., 2004; Dejaegher et al, 2006; Görög, 2008).

The dependent variable is the proportion of aspirin (acetylsalicylic acid which is contained in each base. Theautonomous variable is the quantity ofbase evaluated in moles of NaOHwhich are required to provide a neutralizingeffect to the solution.

Materials

The materials which will be applied in this experiment are:

1. Scale
2. 5 aspirin samples which are from distinctmanufacturers
3. 50 cm³
4. Alcohol 95% 10.00 cm³.
5. NaOH (sodium hydroxide) in a 0.100 mole dm^-3
6. Hydronium ion (pH) tester.

The aspirin samples are titrated with 0.00 mole dm^-3 solution by the application of pH tester in order to assess the hydronium ion (pH) content to see if the solution possesses a neutralhydronium ion concentration (pH)

The data was recorded with the number of ml which was applied in order to neutralize the aspirin samples during each trial.

Bayer Aspirine

Contra- Schmerz Plus

Alcacyl

Aspégic

Alka- Seltzer

Empirical Data

1. Bayer Asperine possesses 500 mg of acetylsalicylic acid. The cost is Fr.6.55.
2. Contra- Schmerz Plus possesses 500 mg of acetylsalicylic acid. The cost is Fr.6.50.
3. Alcacyl possesses 415 mg of acetylsalicylic acid. The cost is Fr. 7.50.
4. Aspégic possesses 500 mg of acetylsalicylic acid. The cost is Fr. 7.50.
5. Alka- Seltzer possesses 500 mg of acetylsalicylic acid. The cost is Fr. 13.15.

The number of moles (molarity) of sodium hydroxide (NaOH) in a solution of 0.000 ml/L is +0.01 M. The number of grams per mole of acetylsalicylic acid (C₉H₈O₄) is 180.157 grams per mole.

The solution initiated the acquisition of a pink hue. This inferred that the compounds were engaged in a reaction. The 50 ml flask provides an error of ± 0.05 ml. The evaluations of the mass of the aspirin tablets have an error of ± 0.001 g.  The materials were rinsed thoroughly in order to minimize errors in the hydronium ion (pH) evaluation.

Data Analysis

Bayer Aspirine

Bayer Aspirine Trial # 1-The quantity of sodium hydroxide which was required to provide a neutralization was 24.5 ml NaOH/ 0.10 NaOH mole= 0.00245 mole of NaOH ± 0.11 ml / NaOH L.The number of grams of acetylsalicylic acid is calculated by considering 0.00245 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylicacid (C₉H₈O₄) (Burgot et al., 1997). The proportion of aspirin in the solutionis 0.00245 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is .45759 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100%and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Chou & Lai, 2004). The proportion of acetylsalicylic acid in the solution is 457.59% C₉H₈O₄. The degree of error can be calculated by 0.1 ml X 100%/ 24.5 ml = ±0.41 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Bayer Asperine trial 1 is 0.001g x 100%/.319g = 0.31%.

Bayer Aspirine Trial # 2- The quantity of sodium hydroxide which was required to provide a neutralization was 23.6 ml NaOH/ 0.10 NaOH mole= 0.00236 mole of NaOH ± 0.11 ml / NaOH L.The number of grams of acetylsalicylic acid is calculated by considering0.00236 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄). The proportion of aspirin in the solution is 0.0236 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is .4252 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Chou & Lai, 2004). The proportion of acetylsalicylic acid in the solution is 425.52% C₉H₈O₄. The degree of error can be calculated by 0.1 ml X 100%/ 23.6 ml = ±0.424 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Bayer Asperine trial 2 is 0.001g x 100%/.319g = ±0.218%.

Bayer Aspirine Trial # 3- The quantity of sodium hydroxide which was required to provide a neutralization was 25.8 ml NaOH/ 0.10 NaOH mole= 0.00258 mole of NaOH ± 0.11 ml / NaOH L.The number of grams of acetylsalicylic acid is calculated by considering 0.00258 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Burgot et al., 1997). The proportion of aspirin in the solution is 0.00258 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 0.4648 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Chou & Lai, 2004). The proportion of acetylsalicylic acid in the solution is 464.8% C₉H₈O₄. The degree of error can be calculated by 0.1 ml X 100%/ 25.8 ml = ±0.3876 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Bayer Asperine trial 3 is 0.001g x 100%/.319g = ±0.179%.

Bayer Aspirine Trial # 4-  The quantity of sodium hydroxide which was required to provide a neutralization was 26.2 ml NaOH/ 0.10 NaOH mole= 0.00262 mole of NaOH ± 0.11 ml / NaOH L. The number of grams of acetylsalicylic acid is calculated by considering 0.00262 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Burgot et al., 1997). The proportion of aspirin in the solution is 0.00258 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 0.4720 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Chou & Lai, 2004). The proportion of acetylsalicylic acid in the solution is 472.0% C₉H₈O₄. The degree of error can be calculated by 0.1 ml X 100%/ 26.2 ml = ±0.3817 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Bayer Asperine trial 4 is 0.001g x 100%/.319g = ±0.1876%. The average percentage of aspirin in each tablet of Bayer Aspirine is 97.28% ± .212%

Contra- Schmerz Plus

Contra- Schmerz Plus Trial # 1- The quantity of sodium hydroxide which was required to provide a neutralization was 26.1 ml NaOH/ 0.10 NaOH mole= 0.00261 mole of NaOH ± 0.11 ml / NaOH L.The number of grams of acetylsalicylic acid is calculated by considering 0.00261 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Burgot et al., 1997). The proportion of aspirin in the solution is 0.00261 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 0.4702 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Chou & Lai, 2004). The proportion of acetylsalicylic acid in the solution is 470.2% C₉H₈O₄. The degree of error can be calculated by 0.1 ml X 100%/ 26.1 ml = ±0.3831 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Contra- Schmerz Plus trial 1 is 0.001g x 100%/0.780g = ±0.128%.

Contra- Schmerz Plus Trial 2- The quantity of sodium hydroxide which was required to provide a neutralization was 26.2 ml NaOH/ 0.10 NaOH mole= 0.00262 mole of NaOH ± 0.11 ml / NaOH L. The number of grams of acetylsalicylic acid is calculated by considering 0.00262 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Burgot et al., 1997). The proportion of aspirin in the solution is 0.00258 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 0.4720 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Chou & Lai, 2004). The proportion of acetylsalicylic acid (C₉H₈O₄) in the solution is 472% .The degree of error can be calculated by 0.1 ml x100%/ 26.2 ml = ±0.3817 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Contra- Schmerz Plus Trial 2 is 0.001g x 100%/.319g = ±0.13%.

Contra- Schmerz PlusTrial # 3- The quantity of sodium hydroxide which was required to provide a neutralization was 26.0 ml NaOH/ 0.10 NaOH mole= 0.00261 mole of NaOH ± 0.11 ml / NaOH L.The number of grams of acetylsalicylic acid is calculated by considering 0.00260 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Burgot et al., 1997). The proportion of aspirin in the solution is 0.00260 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 0.4684 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Chou & Lai, 2004). The proportion of acetylsalicylic acid in the solution is 468.4% C₉H₈O₄. The degree of error can be calculated by 0.1 ml X 100%/ 26.0 ml = ±0.3846 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Contra- Schmerz Plus trial 3 is 0.001g x 100%/0.780g = ±0.128%.

Contra- Schmerz  PlusTrial # 4- The quantity of sodium hydroxide which was required to provide a neutralization was 26.4 ml NaOH/ 0.10 NaOH mole= 0.00264 mole of NaOH ± 0.11 ml / NaOH L. The number of grams of acetylsalicylic acid is calculated by considering 0.00264 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Burgot et al., 1997). The proportion of aspirin in the solution is 0.00264 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 0.4756 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Chou & Lai, 2004). The proportion of acetylsalicylic acid in the solution is 475.6% C₉H₈O₄. The degree of error can be calculated by 0.1 ml x 100%/ 26.4 ml = ±0.3787 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Contra- Schmerz Plus trial 4 is 0.001g x 100%/0.770g = ±0.1298%. The average percentage of aspirin in each tablet of Contra – Schmerz Plus is 60.96% ± .210%.

Alcacyl

Alcacyl Trial # 1- The quantity of sodium hydroxide which was required to provide a neutralization was 1.6 ml NaOH/ 0.10 NaOH mole= 0.00016 mole of NaOH ± 0.11 ml / NaOH L.The number of grams of acetylsalicylic acid is calculated by considering 0.00016 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Burgot et al., 1997). The proportion of aspirin in the solution is 0.00016 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 0.02889 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Burgot et al., 1997). The proportion of acetylsalicylic acid in the solution is 28.89% C₉H₈O₄. The degree of error can be calculated by 0.1 ml X 100%/ 1.6 ml = ±6.25 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Alcacyltrial 1 is 0.001g x 100%/0.770g = ±0.099%.

Alcacyl Trial # 2- The quantity of sodium hydroxide which was required to provide a neutralization was 1.1 ml NaOH/ 0.10 NaOH mole= 0.00016 mole of NaOH ± 0.11 ml / NaOH L.The number of grams of acetylsalicylic acid is calculated by considering 0.00011 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Chou & Lai, 2004). The proportion of aspirin in the solution is 0.00011 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 0.01982 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Burgot et al., 1997). The proportion of acetylsalicylic acid in the solution is 19.82% C₉H₈O₄. The degree of error can be calculated by 0.1 ml X 100%/ 1.1 ml = ±9.09 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Alcacyl trial 2 is 0.001g x 100%/0.770g = ±0.091%.

Alcacyl Trial # 3- The quantity of sodium hydroxide which was required to provide a neutralization was 1.3 ml NaOH/ 0.10 NaOH mole= 0.00013 mole of NaOH ± 0.11 ml / NaOH L.The number of grams of acetylsalicylic acid is calculated by considering 0.00013 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Chou & Lai, 2004). The proportion of aspirin in the solution is 0.00013 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 0.02342 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Burgot et al., 1997). The proportion of acetylsalicylic acid in the solution is 23.42% C₉H₈O₄. The degree of error can be calculated by 0.1 ml x 100%/ 1.3 ml = ±7.69 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Alcacyl trial 2 is 0.001g x 100%/1.051g = ±0.095%.

Alcacyl Trial # 4- The quantity of sodium hydroxide which was required to provide a neutralization was 1.6 ml NaOH/ 0.10 NaOH mole= 0.00016 mole of NaOH ± 0.11 ml / NaOH L.The number of grams of acetylsalicylic acid is calculated by considering 0.00016 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Burgot et al., 1997). The proportion of aspirin in the solution is 0.00016 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 0.02889 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Burgot et al., 1997). The proportion of acetylsalicylic acid in the solution is 28.89% C₉H₈O₄. The degree of error can be calculated by 0.1 ml x 100%/ 1.6 ml = ±6.25 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Alcacyl trial 1 is 0.001g x 100%/1.027g = ±0.097%. The average percentage of aspirin in each tablet of Alcacyl is 2.4465% ± 3.96%.

Aspégic

Aspégic # 1- The quantity of sodium hydroxide which was required to provide a neutralization was 22.4 ml NaOH/ 0.10 NaOH mole= 0.00224 mole of NaOH ± 0.11 ml / NaOH L.The number of grams of acetylsalicylic acid is calculated by considering 0.00224 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Chou & Lai, 2004). The proportion of aspirin in the solution is 0.00016 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 0.4045 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Burgot et al., 1997). The proportion of acetylsalicylic acid in the solution is 404.5% C₉H₈O₄. The degree of error can be calculated by 0.1 ml X 100%/ 22.4 ml = ±0.446 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Aspégic trial 1 is 0.001g x 100%/0.924g = ±0.1082%.

Aspégic # 2- The quantity of sodium hydroxide which was required to provide a neutralization was 23.6 ml NaOH/ 0.10 NaOH mole= 0.00236 mole of NaOH ± 0.11 ml / NaOH L.The number of grams of acetylsalicylic acid is calculated by considering 0.00236 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Chou & Lai, 2004). The proportion of aspirin in the solution is 0.00236 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 0.4252 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3NaOH (Burgot et al., 1997).The proportion of acetylsalicylic acid in the solution is 404.5% C₉H₈O₄. The degree of error can be calculated by 0.1 ml X 100%/23.6 ml = ±0.4237 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Aspégic trial 2 is 0.001g x 100%/0.970g = ±0.1031%.

Aspégic # 3- The quantity of sodium hydroxide which was required to provide a neutralization was 23.0 ml NaOH/ 0.10 NaOH mole= 0.00230 mole of NaOH ± 0.11 ml / NaOH L. The number of grams of acetylsalicylic acid is calculated by considering 0.00230 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) (Chou & Lai, 2004) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄). The proportion of aspirin in the solution is 0.00230 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 0.4045 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Burgot et al., 1997). The proportion of acetylsalicylic acid in the solution is 404.5% C₉H₈O₄. The degree of error can be calculated by 0.1 ml X 100%/ 22.4 ml = ±0.414 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Aspégic trial 3 is 0.001g x 100%/0.865g = ±0.116%.

Aspégic # 4- The quantity of sodium hydroxide which was required to provide a neutralization was 23.5 ml NaOH/ 0.10 NaOH mole= 0.00235 mole of NaOH ± 0.11 ml / NaOH L.The number of grams of acetylsalicylic acid is calculated by considering 0.00235 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Chou & Lai, 2004). The proportion of aspirin in the solution is 0.00235 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 0.4234 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Burgot et al., 1997). The proportion of acetylsalicylic acid in the solution is 423.4% C₉H₈O₄. The degree of error can be calculated by 0.1 ml X 100%/ 23.5 ml = ±0.426 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Aspégic trial 4 is 0.001g x 100%/0.906g = ±0.11%. The average percentage of aspirin in each tablet of Aspégic is 45.23% ± .241%.

Alka- Seltzer

Alka- Seltzer # 1- The quantity of sodium hydroxide which was required to provide a neutralization was 74.3 ml NaOH/ 0.10 NaOH mole= 0.00743 mole of NaOH ± 0.11 ml / NaOH L.The number of grams of acetylsalicylic acid is calculated by considering 0.00743 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Chou & Lai, 2004). The proportion of aspirin in the solution is 0.00743 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 1.3385 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Burgot et al., 1997). The proportion of acetylsalicylic acid in the solution is 1,338.5% C₉H₈O₄. The degree of error can be calculated by 0.1 ml X 100%/74.3 ml = ±0.1346 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Alka- Seltzer trial 1 is 0.001g x 100%/ 2.881g = ±0.0347%.

Alka- Seltzer # 2- The quantity of sodium hydroxide which was required to provide a neutralization was 72.3 ml NaOH/ 0.10 NaOH mole= 0.00723 mole of NaOH ± 0.11 ml / NaOH L.The number of grams of acetylsalicylic acid is calculated by considering 0.00743 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Chou & Lai, 2004). The proportion of aspirin in the solution is 0.00235 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 1.3025 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Burgot et al., 1997). The proportion of acetylsalicylic acid (C₉H₈O₄)in the solution is 1,302.5%. The degree of error can be calculated by 0.1 ml X 100%/ 72.3 ml = ±0.13831 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Alka- Seltzer trial 2 is 0.001g x 100%/ 2.752 g = ±0.0363%.

Alka- Seltzer # 3- The quantity of sodium hydroxide which was required to provide a neutralization was 71.5 ml NaOH/ 0.10 NaOH mole= 0.00715 mole of NaOH ± 0.11 ml / NaOH L.The number of grams of acetylsalicylic acid is calculated by considering 0.00715 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Chou & Lai, 2004). The proportion of aspirin in the solution is 0.00715 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 1.2881 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Burgot et al., 1997). The proportion of acetylsalicylic acid (C₉H₈O₄) in the solution is 1,288.1%. The degree of error can be calculated by 0.1 ml x 100%/71.5 ml = ±0.1399 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Alka- Seltzer trial 3 is 0.001g x 100%/2.780g = ±0.036%.

Alka- Seltzer # 4- The quantity of sodium hydroxide which was required to provide a neutralization was 70.9 ml NaOH/ 0.10 NaOH mole= 0.00709 mole of NaOH ± 0.11 ml / NaOH L.The number of grams of acetylsalicylic acid is calculated by considering 0.00709 moles of NaOH per mole of acetylsalicylic acid (C₉H₈O₄) with a molar weight of 180.157 grams per mole. One mole of sodium hydroxide (NaOH) is required to neutralize one mole of acetylsalicylic acid (C₉H₈O₄) (Chou & Lai, 2004). The proportion of aspirin in the solution is 0.00709 moles x 180.157 grams / mole. The amount of acetylsalicylic acid is 1.277.3 g.

The proportion of acetylsalicylic acid in the solution is determined by multiplying the number of grams of solute by 100% and dividing by 0.100 grams which is the mass of a mole of 0.01 ml dm^-3 NaOH (Burgot et al., 1997). The proportion of acetylsalicylic acid (C₉H₈O₄) in the solution is 1,277.3.1%. The degree of error can be calculated by 0.1 ml x 100%/ 71.5 ml = ±0.1410 % is the percentage error for the NaOH 0.100 ml dm^-3.  The error for the Alka- Seltzer trial 4 is 0.001g x 100%/2.860 g = ±0.035%. The average percentage of aspirin in each tablet of Alka- Seltzer is 46.19% ± .077%.

Discussion

The medication of the five which had been evaluated which had been proven to have the highest aspirin content is Alka- Seltzer. Alka -Seltzer was proven to have almost 195% of the average content of aspirin in comparison to the other three. The lowest percentage of experimental error was shown by the Alka- Seltzer trials. This may be attributed to experimental error. The sodium bicarbonate content in the Alka- Seltzer tablet could have led to a larger assessment of the aspirin content. The medication which possessed the second largest content of aspirin was Contra- Schmerz Plus. The amount of aspirin content was followed by Bayer Aspirine and Aspégic. The medication with the least aspirin content was shown to be Alcacyl (Gris et al., 2004; Dejaegher et al., 2006; Görög, 2008). The experimental error could have occurred during the titration process. Humidity and improperly prepared flasks could have attributed to experimental error.In this experiment the theories of acid and base electron transfer which were proposed by Lewis and   Brønstead- Lowry .The acid converted into a donor of the H⁺ (Hydronium) ion to transform into the conjugated base. The base received the proton and converted into a conjugated acid.

References

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