A.   The starting solution would be more acidic as such it would consume more base to achieve the equivalence point

        B.   the student cannot get an equivalence point owing to the fact that tap water was used not distilled water

        C.   The solution would require more of indicator at the beginning of the experiment

        D.   the starting solution would be more alkaline therefore it would require more volume of acid than expected

        A.   50 mol

        B.   0.125 mol

        C.   0.25 mol

        D.   0.5 mol

        A.   To determine the concentration of a substance that is in excess after a chemical reaction.

        B.   To determine the base in excess.

        C.   To determine the acid in excess.

        D.   To determine the average value of acid base titration.

        A.   The end point will appear when only half of Na2CO3 has been used

        B.   The end point will appear at the first drop of the acid.

        C.   The end point will appear when half of the HCl has been used.

        D.   The indicator will be sensitive to the acid alone

        A.   Any indicator

        B.   Phenolphthalein

        C.   Methyl orange

        D.   No suitable indicator

        A.   Phenolphthalein

        B.   Methyl orange

        C.   Any indicator

        D.   No suitable indicator

        A.   Pressure filtration

        B.   Simple filtration

        C.   Ordinary filtration

        D.   Suction filtration

        A.   Any acid that ionizes completely in solution

        B.   Any acid which turns blue litmus paper red

        C.   Any acid that is highly corrosive and can cause burn to the skin

        D.   Any acid whose pH is less than 3

        A.   Methyl orange

        B.   Bromothymol

        C.   Phenolphthalein

        D.   Litmus paper

        A.   Blue

        B.   Red

        C.   Yellow

        D.   Colourless

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