The indicator constant for an acidic indicator, HIn is 5×10-6M. The indicator appears only in the colour of acidic form when [In−HIn]⩽120 and it appears only in the colour of basic form when [HInIn]⩽140 . The pH range of indicator is [Given: log 5 = 0.7]

pkxn=5×10−6;HIn⇌H++In− KIN=[H+][In−][HIn] [H+]=KIn[HIn][In];pH=pkIn+log[In][HIn] pH=6−log5+log120=6−0.7−1.3=6−2=4.0 pH=6−log5+log40=6−0.7+1.6=6.9 Range in 4.0 to 6.9

The indicator constant for an acidic indicator, HIn is 5×10-6M. The indicator appears only in the colour of acidic form when [In−HIn]⩽120 and it appears only in the colour of basic form when [HInIn]⩽140 . The pH range of indicator is [Given: log 5 = 0.7]

pkxn=5×10−6;HIn⇌H++In− KIN=[H+][In−][HIn] [H+]=KIn[HIn][In];pH=pkIn+log[In][HIn] pH=6−log5+log120=6−0.7−1.3=6−2=4.0 pH=6−log5+log40=6−0.7+1.6=6.9 Range in 4.0 to 6.9

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The indicator constant for an acidic indicator, HIn is ${5×10}^{-6} M$ . The indicator appears only in the colour of acidic form when $[\frac{{In}^{-}}{HIn}] ⩽ \frac{1}{20}$ and it appears only in the colour of basic form when $[\frac{HIn}{In}] ⩽ \frac{1}{40}$ . The pH range of indicator is [Given: log 5 = 0.7]

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4.0 – 6.9

4.3 – 6.3

3.7 – 6.6

6.0 – 6.9

answer is B.

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Detailed Solution

$p k x n = 5 \times 10^{- 6}; H I n ⇌ H^{+} + I n^{-} K_{I N} = \frac{[H^{+}] [I n^{-}]}{[H I n]} [H^{+}] = K_{I n} \frac{[H_{I n}]}{[I n]}; p H = p^{k I n} + \log \frac{[I n]}{[H I n]} p H = 6 - \log 5 + \log \frac{1}{20} = 6 - 0.7 - 1.3 = 6 - 2 = 4.0 p H = 6 - \log 5 + \log 40 = 6 - 0.7 + 1.6 = 6.9$