Calculate the volume of 0.660-M NaOH solution needed to completely neutralize 49.6 mL of a 0.460-M solution of the diprotic acid H2C2O4.
Balanced chemical equation is:
H2C2O4 + 2 NaOH ---> Na2C2O4 + 2 H2O
Here:
M(H2C2O4)=0.46 M
M(NaOH)=0.66 M
V(H2C2O4)=49.6 mL
According to balanced reaction:
2*number of mol of H2C2O4 =1*number of mol of NaOH
2*M(H2C2O4)*V(H2C2O4) =1*M(NaOH)*V(NaOH)
2*0.46 M *49.6 mL = 1*0.66M *V(NaOH)
V(NaOH) = 69.1 mL
Answer: 69.1 mL
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