The range of most suitable indicator which should be used...

The range of most suitable indicator which should be used for titration of $\mathrm{NaX}$ $(0.1 \mathrm{M}, 10 \mathrm{ml})$ with $0.1 \mathrm{M} \mathrm{HCl}$ should be
$\left(K_{\mathrm{b}}\right.$ of $\left.\mathrm{X}-=10^{-6}\right)$
(a) $2-3$
(b) $3-5$
(c) $6-8$
(d) $8-10$

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Key Concepts

Indicator Selection and Transition Range

Choosing a proper indicator is vital in titration experiments, as it must have a color change range that encompasses the pH at the equivalence point. An ideal indicator will show a noticeable color change right around the equivalence point, ensuring accurate determination of the titration endpoint.

Hydrolysis of Salts

When a salt derived from a weak base and a strong acid (or vice versa) dissolves in water, it typically undergoes hydrolysis, which affects the pH of the solution. Understanding the hydrolysis behavior is important for predicting the pH at the equivalence point, which in turn informs the indicator selection.

Acid-Base Titration

This concept involves the gradual addition of one reactant (the titrant) to another (the analyte) until the reaction reaches completion, known as the equivalence point. In acid-base titrations, the change in pH during the reaction is often used to determine the point of neutralization between an acid and a base.

Equivalence Point

The equivalence point in a titration is the stage at which the moles of acid equal the moles of base, leading to complete neutralization. Calculating the pH at the equivalence point is crucial because it determines the optimal range for an indicator to signal the endpoint of the titration.

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