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For strong acid/strong base reactions: pH 7 is the equivalence point For titration of a weak base with strong acid : pH 6-3 is the equivalence point For titration of a weak acid with strong base : pH 8-11 is the equivalence point For weak acid/weak base reactions it is also around pH 7, but it happens so NON-sharply, vague, that titrations can't be used for these.
Iodine solution is an efficient indicator for starch. It will go from a light brown colour to a black colour if starch is present and will stay light brown if no starch is present. Hope this Helps!
A titration usually has an acid (pH 0-6) in the burette and an alkali (pH 8-14) in the conical flask below the burette. Your aim is to neutralise the two solutions by titrating them against each other.So the endpoint pH should be 7 (universal indicator/litmus paper will appear a greenish colour). The solution in the conical flask is neutral.Hope this Helps!
pH = 6 is the answer. For pH = 2, [H+] = 10-2 For pH = 6, [H+] = 10-6
pH of 6 is 5,
By titration with alkaline on methyl-red indicator (pH<6)
For strong acid/strong base reactions: pH 7 is the equivalence point For titration of a weak base with strong acid : pH 6-3 is the equivalence point For titration of a weak acid with strong base : pH 8-11 is the equivalence point For weak acid/weak base reactions it is also around pH 7, but it happens so NON-sharply, vague, that titrations can't be used for these.
Iodine solution is an efficient indicator for starch. It will go from a light brown colour to a black colour if starch is present and will stay light brown if no starch is present. Hope this Helps!
A titration usually has an acid (pH 0-6) in the burette and an alkali (pH 8-14) in the conical flask below the burette. Your aim is to neutralise the two solutions by titrating them against each other.So the endpoint pH should be 7 (universal indicator/litmus paper will appear a greenish colour). The solution in the conical flask is neutral.Hope this Helps!
At 'half way' point the pH is equal to the pKa value of the acid: pH = pKa - log[cA/cB] because at that point cA = cB . So pH = pKa = - log(5.2*10-6) = 5.3
Well, there really is no "exact" pH of an acid. An acid can be a certain pH, before it is considered a base, and to change an acid to a base would be called titration, but lets not get carried away. The pH of an acid can be anywhere between 0-6 on the pH scale, 7 would be neutral, and 8-14 would be considered a base.
Bromothymol blue is used as pH indicator: under pH=6 is yellow and above pH=7,6 is blue. For other applications see the link below.
pH = 6 is the answer. For pH = 2, [H+] = 10-2 For pH = 6, [H+] = 10-6
pH of 6 is 5,
Bromothymol blue (pH 6.0-7.6) Phenol red (pH 6.4-8.0) Neutral red (pH 6.8-8.0)
Natural rainwater (pH 5 - 6) Milk (pH 6 - 6.6)
A solution that has a pH of 6 is slightly acidic.