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    I just finished learning how to find either pH of strong acid or concentration of H+ ions. However I'm stuck on a question.

    Calculate the pH of the solution formed when 250 cm3 of water is added to 50cm3 of 0.200 moldm-3 HNO3.

    I worked out the new H+ concentration to be 0.0333moldm-3.
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    -log10([H+])
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    Looks good so far.
    What's the next step?
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    (Original post by TutorsChemistry)
    Looks good so far.
    What's the next step?
    300/1000 * [H+] = 50/1000 x 0.200
    [H+] = 0.0333 moldm-3 (monoprotic acid so no need to multiply anything?)

    pH = -log10(0.0333)
    = 1.48

    Does this look right? I'm not confident I got the concentration bit right
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    That's what i got too.
    Your method looks fine.
 
 
 
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