In: Chemistry
i mix 500ml of 0.250 M HCNO with 250ml of 0.333 M NaCNO. i then add 25ml of 1.00 M NaOH. A) how many moles of CNO- are in the beaker before the reaction takes place. B) what is the limiting reactant for the neutralization reaction
A )
The question relates to ' common ion effect ' ( ie. the degree of dissociation of
a soluble electrolyte is supressed due to addition of a common ion ' ) . HCNO is
a weak acid with Ka = 3.5 x 10-4 hence its degree of dissociation ( ie. number of
moles of the acid dissociated out of one mole ) is calculated using Ostwald's dilution
law. Accordingly
= SQRT ( Ka / C ) , where represents degree of dissociation of the acid
..............& C = concentration in moles
calculated* as =( 0.250 x 500 ) / 750
....................... = 0.166 M
.......... So , = SQRT {( 3.5 x 10-4 ) / 0.166 }
........................= 0.0459 x 10-2
...................or, = 4.59 x 10-4 M
This represents concentrations of H+ ion & also NCO- ion yielded by ionization of
HCNO in solution , which is much much less than unity ( <<< 1.0 ) and is therefore
insignificant. However , the total [ NCO- ] = [ NCO- ] produced by ionization of the salt
NaCNO + [ NCO- ]yielded by ionization of HCNO
NaCNO is a strong electrolyte and therefore gets completely ionized
The [ NaCNO] in 750 ml of solution is = (0.333 x 250 ) / 750
..............................................................= 0.111 M
therefore[ NCO- ] ion produced...........= ( 0.111 + 4.59 x 10-4 ) / L
again since( 4.59 x 10-4 ) is <<< 1.0 , it can be ignored
& the total NCO- in 750 ml of solution = ( 0.111 x 750 ) /1000
................................................................= 8.325 x 10-2 moles
B)
H+ has to partcipate in neutralization reaction with a base its concentration decides the
limiting reagent ,and a limiting reagent is one which gets consumed first, Therefore on addition of 25 ml of 1M NaOH solution HCNO should be considered as the limiting reagent.
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* strength or concentrations of HCNO ,& NaCNO are calculated using relation,
M1V1 = M2V2