Recent content by Kqwert

Something like the H+ ions will "force" Pb2+ ions into solution as it wants to form HSO4-? (and therefore needs the SO42- from PbSO4)..??

Solubility of SO4^2- goes up and not down?

Sorry - cation and anion! I mean if we have the following equation: NaOH(aq) + HCl(aq) <--> Na+(aq) + Cl-(aq) + H2O (l) we can simply write it as H+(aq) + OH-(aq) <--> H2O(l) and calculate deltaH for that equation, as no further reaction happens with the Na+ and Cl- cation/anion?

I did it now, and it seems like we simply ignore the cations in our deltaH calculations if they do not react after dissociation..?

I assume it's something like [H^+] from the acid reacting with [SO4^2-] from the dissolution of our compound (which reduces the total concentration of [SO4^2-] in solution), which again will increase the amount of [Pb^2+] in solution..?

Ok, so we have the equilibrium eq. : 10^-2 = [10^-1][SO4^2-] / [HSO4^-]. This results in: 0.1 = [SO4^2-] / [HSO4^-] I.e. concentration of HSO4^- is significantly higher than SO4^2-. But what exactly does this tell us?

1 mole of water, correct? And then the rest of it must come from the fact that it's a 1L solution? What about my first question, that relating to the deltaH calculations?

What do you mean by "what part"? I don't understand what this is leading to, and why exactly pH 1?

It's 10^-1.99? I.e. high? What does that tell us?

I don't quite understand this. When solving PbSO4(s) we get the equilibrium equation: PbSO4(s) <--> Pb2+ + SO42-. I know H2SO4 is a strong acid, that will dissociate completely (or almost completely), Like this: H2SO4 -> H+ + HSO4- HSO4- -> H+ + SO42-So as far as I can see, the concentration...

I have a couple of questions related to this task. The reaction that I proposed was this: NaOH(aq) + HCl(aq) <--> Na+ + Cl- + H2O (l) where as the solution manual have this net reaction, as nothing will happen with the Na+ and Cl- ions: H+ + OH- <--> H2O. I assume these reactions will...

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Ok, so if we have the following reaction: HA <--> H+ + A- Then if we decrease the pH - concentration of [H+] will increase, reaction will be shifted towards the left => less products. If we increase the pH - concentration of [H+] will decrease, reaction will be shifted towards the right =>...

Anyone..?

Thank you! I edited my post, is it correct now?