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Standard X

Chemistry

Neutralisation Reaction

An unknown so...

Question

An unknown solution having a pH of $3.5$ was titrated with $0.1 M N a O H$ . Analysis of the resulting titration curve showed a single equivalence point at $p H 7$ . Therefore, which of the following could be the unknown solute in the initial solution?

H F

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H C l

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L i O H

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N H_{3}

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H_{2} S O_{4}

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Solution

The correct option is B $H C l$
Since $P^{H} = 7$ at equivalence point only occur for titration of strong acid and strong base. So since $N a O H$ is strong base strongest acid among them is $H C l$ (due to its fast ionisation as compared to $H_{2} {S O}_{4}$ which has weak ionisations)

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Similar questions

Q. Determine the unknown solute from the given observation.
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An unknown solution having a pH of 3.5 was titrated with 0.1 M NaOH. Analysis of the resulting titration curve showed a single equivalence point at pH 7. Therefore, which of the following could be the unknown solute in the initial solution?

The correct option is B HClSince PH=7 at equivalence point only occur for titration of strong acid and strong base. So since NaOH is strong base strongest acid among them is HCl (due to its fast ionisation as compared to H2SO4 which has weak ionisations)

An unknown solution having a pH of $3.5$ was titrated with $0.1 M N a O H$ . Analysis of the resulting titration curve showed a single equivalence point at $p H 7$ . Therefore, which of the following could be the unknown solute in the initial solution?

The correct option is B $H C l$
Since $P^{H} = 7$ at equivalence point only occur for titration of strong acid and strong base. So since $N a O H$ is strong base strongest acid among them is $H C l$ (due to its fast ionisation as compared to $H_{2} {S O}_{4}$ which has weak ionisations)