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Chemistry

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    $\begingroup$ pH will change all right, only way less than it would change in pure water. $\endgroup$
    – Ivan Neretin
    Commented Aug 12, 2017 at 16:40
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    $\begingroup$ we can't ignore the forward reaction in the second case as the net equilibrium(of water formation and decompostion of CH3COOH) would be around 10^10.(10^15 of water and 10^(-5) of acetic acid) $\endgroup$
    – Ayushmaan
    Commented Aug 12, 2017 at 16:51
  • $\begingroup$ @Ayushmaan and we can ignore it in the first casE? $\endgroup$
    – Arishta
    Commented Aug 12, 2017 at 16:52
  • $\begingroup$ yes, because in the first case the equilibrium constant would only be 1. ( 10^5*10^(-5)). So, if initial concentration of acetic acid is large in comparison to H+ we have put, the pH would be approx. same. $\endgroup$
    – Ayushmaan
    Commented Aug 12, 2017 at 16:59