1.250 g of H2C2O4 are dissolved into 100.0 ml of water which is then titrated with...

1.250 g of H2C2O4 are dissolved into 100.0 ml of water which is then titrated with 28.56 ml of NaOH solution. What is the molarity of the NaOH solution? H2C2O4 + NaOH arrow Na2C2O4 + H2O (not balanced) Select one: a. 0.6942 M b. 2.957 M c. 0.4862 M d. 1.945 M e. The correct answer is not given as an option.

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Expert Solution

H2C2O4 + 2NaOH --------------> Na2C2O4 + 2H2O

Oxalic acid exists as H2C2O4.2H2O

Molar mass = 126 g/mol

H2C2O4

molarity of H2C2O4 M1 = (mass/ molar mass) x (1/ volume in Lires)

= (1.25 g/ 126 g/mol) x (1/ 0.1 L)

= 0.099 M

Volume of H2C2O4, V1 = 100 mL

no of moles of H2C2O4 in the balanced equation , n1 = 1

NaOH

M2 = ?

V2 = 28.56 mL

no of moles of NaOH in the balanced equation , n2 = 2

At equivalence point,

M1V1/n1 = M2V2/n2

M2 = ( M1V1/n1 ) (n2/V2)

= (0.099 M X 100 ml /1 ) (2 /28.56 ml)

= 0.6942 M

M2 = 0.6942 M

Therefore,

molarity of the NaOH solution = 0.6942 M

queen_honey_blossom answered 1 year ago

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