ana chem lab 3b

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    in digestion and also kill bacteria the acid is highly corrosive and may cause ulceration or heart

    burn. There is a mucus barrier which protects the lining of the stomach, if this mucus membrane

    is damaged the stomach lining will be exposed to the acid and this results in ulcers. The antacid

    works by neutralizing the acid so as to make it less corrosive, this helps to prevent the ulcers and

    gastritis and heart burn. The reach reaction between the antacid and the stomach acid HCL is a

    acid base reaction. Majority of antacids contain weak bases, true a chemical reaction they

    neutralize the stomach acid the most common bases which antacid contains include: magnesium

    hydroxide, aluminium hydroxide, sodium bicarbonate and calcium carbonate. Acid and bases

    react to produce salt and water, example of the chemical reaction is magnesium hydroxide plus

    hydrochloric acid produces magnesium choride and water. Antacids are insoluble and in the case

    that carbon dioxide is produced they are analysed by a method known as back titration. The

    antacid is allowed to react with a known amount of HCL and the excess HCL is titrated with

    excess sodium hydroxide. The amount neutralized by the antacid is determined by the excess

    moles minus the initial moles to give moles neutralized. If there is carbon dioxide production in a

    reaction of an antacid, the carbon dioxide must be removed before titration this gas can be

    removed by boiling which will shift the equilibrium in the reaction below to the left:

    CO2+ H2O HCO1-

    3(aq) + H1+

    (aq)

    If CO2is left dissolve, the H+ produced would be titrated by sodium hydroxide.

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    Results:

    TABLE 1- SHOWING MASS FOR KHP

    1 2 3

    Mass of beaker

    +solid(g)

    33.8645 33.7434 32.7501

    Mass of beaker(g) 33.3042 33.2211 32.1985

    Mass of solid(g) 0.5603 0.5223 0.5516

    TABLE 2-SHOWING BURETTE READINGS FOR STANDARDISATION OF NAOH

    Mass of KHP(g) 0.5603 0.5223 0.5516

    Initial vol of

    NaOH(ml)

    4.46 4.08 2.51

    Final vol ofNaOH(ml)

    33.48 31.21 30.81

    Titre vol ofNaOH(ml)

    29.02 27.13 28.30

    Observation: Solution changed from colourless to pink

    TABLE 3- SHOWING MASS FOR ANTACID TABLETS

    Mass of watch glass + tablets(g) 39.8185

    Mass of watch glass(g) 37.3309

    Mass of tablets(g) 2.4876

    Avg mass of one tablet(g) 0.8292

    TABLE 4- SHOWING MASS FOR CRUSHED ANTACID TABLETS

    1 2 3

    Mass ofbeaker+antacid(g) 34.4648 33.8068 33.7431

    Mass of beaker(g) 33.9211 33.2854 33.2014

    Mass of antacid(g) 0.5437 0.5214 0.5417

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    TABLE 5- SHOWING BURETTE READINGS FOR STANDARDISATION OF HCL

    Volume of HCL(ml) 25 25 25

    Initial vol of

    NaOH(ml)

    4.22 2.78 4.21

    Final vol ofNaOH(ml) 29.96 28.61 30.09

    Titre vol of

    NaOH(ml)

    25.74 25.83 25.88

    Avg titre vol of

    NaOH(ml)

    25.82

    Observation: Solution changed from colourless to pink

    ANALYSIS OF ANTACID

    TABLE 6- SHOWING BACK TITRATION WITH NaOH

    Mass of antacid(g) 0.5437 0.5214 0.5417

    Vol of HCL used(ml) 50 50 50

    Initial vol of

    NaOH(ml)

    2.92 2.13 2.51

    Final vol of NaOH

    (ml)

    42.89 41.51 42.52

    Titre vol of

    NaOH(ml)

    39.97 39.38 40.01

    Observation: Solution changed from cloudy to pink

    Discussion: In this experiment the boiling of the antacid solution wasnt necessary because

    there was no carbonate present in the sample hence, carbon dioxide was absent. A limtitation

    could be that the antacid was not fully dissolved if the solution was boiled the antacid would

    have dissolved.

    In order to know the effectiveness of antacid, the amount of hydrochloric acid neutralized was

    normalized to the mass of tablet. The larger the normalized value, the more effective the antacid.

    Conclusion: