As part of the reading on equilibrium, I came across a description of the dynamic equilibrium that occurs when ethanoic acid is dissolved in water, so I now understand more about the difference between strong and weak acids, that I didn't understand before.
Here are just a few questions:
Given that pH is the negative logarithm of the number of H+ ions in solution, is that related to the strength, rather than the concentration of the acid? Also, how does this change with a diprotic acid with two H+ ions (eg for each mole of H2SO4, there will be two moles of dissociate H+ ions and one mole of SO4 2- ions). When H2SO4 reacts halfway to form HSO4, will that have a different pH?
Also, when we've learnt about a metal reacting with an acid, it always says with an excess of acid. What happens if the metal is in excess?
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