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    I'm in the middle of my lab report for this reaction and I can't really get my head around why this reaction works the way it does, can somebody help me out and explain it? Also, what happens when you repeat the experiment and add Sodium Hydroxide and an indicator to the solution? I can't figure it out - thanks!
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    Sorry you've not had any responses about this. Are you sure you've posted in the right place? Here's a link to our subject forum which should help get you more responses if you post there.

    You can also find the Exam Thread list for A-levels here and GCSE here. :dumbells:


    Just quoting in Fox Corner so she can move the thread if needed
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    (Original post by Jessinoch)
    I'm in the middle of my lab report for this reaction and I can't really get my head around why this reaction works the way it does, can somebody help me out and explain it? Also, what happens when you repeat the experiment and add Sodium Hydroxide and an indicator to the solution? I can't figure it out - thanks!
    Nitric acid is a good oxidising agent (as the nitrate ions can be easily reduced in the presence of an acid) and oxidises the copper to copper(II) ions.

    The products depend on the concentration of the nitric acid.

    Concentrated nitric acid reacts with copper in a 4:1 ratio and produces copper(II) ions and nitrogen(IV) oxide and water.

    Dilute nitric acid reacts with copper in a ratio of 8:3 and produces copper(II) ions and nitrogen(II) oxide and water.
 
 
 
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