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oh yeh i got it now, damn

wait, how'd u get this? what values did you use for c1 and c1 3M hcl was diluted to 5M hcl

i got this too, hope its right

MEGaboner

re: HSC Chemistry Marathon Archive really? woo where'd u get the question from btw how do u know the answer

re: HSC Chemistry Marathon Archive this is what i got hope im right hahahaha a)CaCO3(s) + 2HCL(aq) ----> CaCl2(aq) + CO2(g) + H2O(l) b) n(NaOH)= 0.0112x1 =0.0112 moles of NaOH c) NaOH+HCL are in a 1:1 so no need to write equation since 10mL of the diluted sample required 11.2mL of 1mol/L NaOH...

this thread should have been locked and closed from page 1 i have no idea why its still up

its quite abit to remember and its rarely ever needed in the HSC so gay

the one, don't listen to these haters u can get high 60s easily i believe in u

Pb2+ + 2CL- ----> PbCl2(s) the dried precipitate is PbCl2 so we calculate the moles of it 0.595/(207+70.9) = approximately 0.002 moles then we find mass of Pb 0.002x207 =0.443g then to put it into g/L we divide by the volume 0.443/0.05 =8.86g/L just use exact values all the way until the...

re: HSC Chemistry Marathon Archive don't we have to take into account that H2SO4 is diprotic? H2SO4 ----> 2H+ + SO4-

is that u in ur dp

re: HSC Chemistry Marathon Archive carbon monoxide? lol

re: HSC Chemistry Marathon Archive yep

re: HSC Chemistry Marathon Archive look at the equation for every 1 mole of SO2 used, 2 moles of H2S is consumed, so in the end 4 moles of SO2 will be in excess

re: HSC Chemistry Marathon Archive this, since H2S is the limiting reagent

re: HSC Chemistry Marathon Archive ah thx for clearing that up

dont forget ur ppm calculations boyss

re: HSC Chemistry Marathon Archive i can't see where you got this from, i tested exact values and sig fig and still couldnt get this

a back titration in a multiple choice so smooth