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chemistry question

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  • 05-06-2010 3:43pm
    #1
    s0ur_cherry
    Registered Users Posts: 29 ✭


    hey just wondering how to solve the second part of hl 2007 #7 (b):

    Calculate the pH of 0.1M HNO2; the value of Ka is 5 x 10^4.

    I can get that bit fine, it's this next part here I don't understand:

    What is the pH of of a HNO3 solution of the same concentration?

    I checked the marking scheme which gives an answer but doesn't explain where it comes from.. Thanks in advance!


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    #2
    lc2010
    Registered Users Posts: 241 ✭✭lc2010


    s0ur_cherry wrote: »
    hey just wondering how to solve the second part of hl 2007 #7 (b):

    Calculate the pH of 0.1M HNO2; the value of Ka is 5 x 10^4.

    I can get that bit fine, it's this next part here I don't understand:

    What is the pH of of a HNO3 solution of the same concentration?

    I checked the marking scheme which gives an answer but doesn't explain where it comes from.. Thanks in advance!
    HNO3 is a strong acid therefore the PH of 0.1m HNO3 =

    -log[0.1]=1

    Hope this helps:D


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