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AIIMS AIIMS Solved Paper-2006

  • question_answer
    40 mL of 0.1 M ammonia solution is mixed, with 20 Ml of \[0.1\,HCl\].What is the pH of the mixture? (\[p{{K}_{b}}\] of ammonia solution is 4.74):

    A)  \[4.74\]   

    B)                                         \[2.26\]              

    C)         \[9.26\]              

    D)         \[5.00\]

    Correct Answer: C

    Solution :

    Handerson- Hasselbalch equation \[pOH=p{{K}_{b}}+\log \frac{[salt]}{[base]}\] At half stage of titration [salt] = [base] as          \[pOH=p{{K}_{b}}=4.74\] \[pH=14-pOH=14-4.74=9.26\]


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