Answer to Question #122927 in General Chemistry for Istyanti

Question #122927
What mass of H2C2O4 is present in a sample if it is titrated to its equivalence point with
18.09 mL of 0.2235 M NaOH? The balanced chemical reaction is as follows:
H2C2O4+2NaOH→Na2C2O4+2H2O
1
Expert's answer
2020-06-18T14:42:01-0400

Solution.

"V(NaOH)=18.09mL=18.09\\sdot10^{-3}L;"

Concentration of NaOH ="0.2235 mol\/L;"

Amount of NaOH (mol) = Concentration of NaOH (mol/L) • Volume of NaOH consumed (L);

Amount of NaOH="0.2235mol\/L\\sdot18.09\\sdot10^{-3}L=4.043\\sdot10^{-3}mol;"

x mol "4.043\\sdot10^{-3}mol"

"H_2C_2O_4+2NaOH\u2192Na_2C_2O_4+2H_2O;"

1 2

Amount of "H_2C_2O_4=\\dfrac{1\\sdot4.043\\sdot10^{-3}mol}{2}=2.0215\\sdot10^{-3}mol;"

"\\nu(H_2C_2O_4)=\\dfrac{m(H_2C_2O_4)}{M(H_2C_2O_4)}\\implies"

"m(H_2C_2O_4)=\\nu(H_2C_2O_4)M(H_2C_2O_4);"

"M(H_2C_2O_4)=90g\/mol;"

"m(H_2C_2O_4)=2.0215\\sdot10^{-3}mol\\sdot90g\/mol=0.182g;"

Answer: "m(H_2C_2O_4)=0.182g."



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