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Ionic Equilibrium question

2005 · Shift 0 · Q10
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Ionic Equilibrium question

2005 · Shift 0 · Q10

JEE MainChemistryIonic EquilibriumMCQ+4 / −1
Hydrogen ion concentration in mol / L in a solution of pH = 5.4 will be :
  1. A
    3.98 ×\times× 10-6
  2. B
    3.68 ×\times× 10-6
  3. C
    3.88 ×\times× 106
  4. D
    3.98 ×\times× 108
View written solutionFree

Correct answer: A

  1. Use the definition of pH

    pH=−log⁡10[H+]\text{pH} = -\log_{10}[H^+]pH=−log10​[H+]

    Given:

    pH=5.4\text{pH} = 5.4pH=5.4

    So,

    [H+]=10−5.4[H^+] = 10^{-5.4}[H+]=10−5.4

  2. Simplify the expression

    10−5.4=10−5×10−0.410^{-5.4} = 10^{-5} \times 10^{-0.4}10−5.4=10−5×10−0.4

    Now,

    10−0.4=1100.4≈12.512≈0.39810^{-0.4} = \frac{1}{10^{0.4}} \approx \frac{1}{2.512} \approx 0.39810−0.4=100.41​≈2.5121​≈0.398

    Therefore,

    [H+]=10−5×0.398=3.98×10−6 mol L−1[H^+] = 10^{-5} \times 0.398 = 3.98 \times 10^{-6}\,\text{mol L}^{-1}[H+]=10−5×0.398=3.98×10−6mol L−1

  3. Match with the options

    [H+]=3.98×10−6 mol/L[H^+] = 3.98 \times 10^{-6}\,\text{mol/L}[H+]=3.98×10−6mol/L

    This corresponds to Option A.

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