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JEE Main & Advanced Chemistry Equilibrium / साम्यावस्था Question Bank Self Evaluation Test - Equilibrium

  • question_answer
    The dissociation constant of 0.1 M acetic acid solution is\[1.8\times {{10}^{-5}}\]. If 1 L of this solution is mixed with 0.05 mole of\[HCl\], what will be pH of mixture? \[\left[ log5=0.7 \right]\]

    A) 1.3                   

    B) 2.6   

    C) 1.9                   

    D) 3.4

    Correct Answer: A

    Solution :

    [a] The pH of mixture is due to the \[HCl\] only, because \[C{{H}_{3}}COOH\] is negligibly ionised due to common ion effect. Thus, \[[{{H}^{+}}]=0.05M=5\times {{10}^{-2}}M\] \[pH=-log\left( 5\times {{10}^{-2}} \right)=-\left[ log5+log{{10}^{-2}} \right]\] \[pH=1.3\]


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