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    If we use the same molarity when standarising HCL what is the difference to the results and why?


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    NaCl is a salt and won't change the pH of the solution in the conical flask.

    You need the pH change to determine the end point of the titration.

    I think. Someone else should back be up. But adding NaCl to hydroxide won't do much
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    Sorry I was doing two things at once, I meant to say Sulphuric acid.

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    Please quote me so I can refer back to this thread.

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    (Original post by Liverpool's Number 9)
    Sorry I was doing two things at once, I meant to say Sulphuric acid.

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    Please quote me so I can refer back to this thread.

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    There are two potential H+ ions that can come from one molecule of sulfuric acid, compared to just one H+ from a HCl
 
 
 
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