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Ionic Equilibrum question

2015 · Q90
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Ionic Equilibrum question

2015 · Q90

NEETChemistryIonic EquilibrumMCQ+4 / −1
What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
  1. A
    2.0
  2. B
    7.0
  3. C
    1.04
  4. D
    12.65
View written solutionFree

Correct answer: D

            HCl + NaOH →\to→ NaCl + H2O
Initial  0.01       0.1            0          0
Final     0         0.09          0.01     0.01

As equal volumes of HCl and NaOH are added so the volume of resulting solution becomes double and the concentration of the solution becomes half.

∴\therefore∴ [OH-] = 0.092{{0.09} \over 2}20.09​ = 0.045 M

∴\therefore∴ pOH = – log[OH– ] = –log [0.045] = 1.35

∴\therefore∴ pH = 14 – pOH = 14 – 1.35 = 12.65

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