we know that
moles = molarity x volume (L)
so
moles of acid = 0.31 x 15 x 10-3
moles of acid (HCl) = 4.65 x 10-3
now
moles of base = 0.90 x 58 x 10-3
moles of base (CH3NH2) = 52.2 x 10-3
now
the reaction is
HCl + CH3NH2 ---> CH3NH3Cl
we can see that
moles of HCl required = moles of CH3NH2 = 52.2 x 10-3
but only 4.65 x 10-3 moles of HCl is present
so
HCl is the limiting reagent
and
CH3NH2 is the excess reactant
now
moles of CH3NH2 remaining = 52.2 x 10-3 - 4.65 x 10-3
moles of CH3Nh2 remaining = 47.55 x 10-3
so
moles of excess reactant after reaction is 47.55 x 10-3
now
final volume = 15 + 58 = 73 ml
now
Concentration = moles / volume (L)
so
conc of excess CH3NH2 = 47.55 x 10-3 / 73 x 10-3
conc of excess CH3NH2 = 0.65 M
now
the prodcut is CH3NH3Cl
now
moles of CH3NH3Cl formed = moles of HCl added = 4.65 x 10-3
conc of CH3NH3Cl = 4.65 x 10-3 / 73 x 10-3
conc of CH3NH3Cl = 0.0637 M
so
the concentration of pH active product is 0.0637 M
The reaction of the strong acid HCl with the weak base CH_3NH_2 is: HCl(aq) + CH_3NH_2(aq)...
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The extent of this reaction is: Below 50%, 50%, Above 50%,
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