bored of sc
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I only put the chart for monoprotic and only for 1st ionisation Not the second one as you can't really get an exact degree of ionisation for Sulfuric acid's 2nd partial ionisation.For a monoprotic acid:
say the height was 2x starting
e.g. HCl --> H+ + Cl-
wouldn't the height of the products be x respectively
For a diprotic acid:
let height be 3x starting
e.g. H2SO4 --> 2H+ + SO42-
wouldn't height be 2x for H ions and x for SO4 ions
That is true. Since the 2nd ionisation of Sufluric Acid is reversible. Anyway the qn only asked for a monoprotic acid.I only put the chart for monoprotic and only for 1st ionisation Not the second one as you can't really get an exact degree of ionisation for Sulfuric acid's 2nd partial ionisation.
In response to the acid qn:Hi
For the acid model, say you did HCL
This goes HCL--> H+ + Cl-, the mole ratio is still 1:1:1, so the bars should be the same size, not half the original, I think..
I didn't really find that ionisation one weird. The one with the table? We did one just like that in our half yearlies, and its in the syllabus.
Less concentration of HCl (i think that was the strong acid) is needed to get the same pH as as a higher concontration of acetic acid, because HCl is strong and completely disassociates whereas acetic acid is weak (since pH is based on concentration of H+)i completely stuffed that one, what was the answer... i went blank!!
Less concentration of HCl (i think that was the strong acid) is needed to get the same pH as as a higher concontration of acetic acid, because HCl is strong and completely disassociates whereas acetic acid is weak (since pH is based on concentration of H+)
The pH for the acetic acid solution went up when the sodium acetate was added because the sodium acetate further reacts with water for form hydroxide ions, causing the solution to become more basic. On the other hand, sodium chloride is a completely neutral salt which does not react further with water so the pH for the HCl solution did not change when HCl was added