1. If the statement ph=-log([H+] is true, then how come a solution can be acidic when carbonate is present? I have been told that even if carbonate does not accept H+ the solution will still be basic just by the presence of CO3(2-)? The confusion is this: ph only depends on [H+] then how come the presence of negative ions change the acidity level, even if they don’t actually accept hydrons? I thought acidity levels change ONLY because CO3(-2) ----> H2CO3 H+ is taken away.