Using the information in the data table, calculate the molarity of the permangan

Question

Using the information in the data table, calculate the molarity of the permanganate solution. (Note that 1 mole of As2O3 solid becomes 2 moles of H3AsO3 when dissolved in water.)

Trial

mass As2O3 (g)

volume KMnO4 (mL)

molarity KMnO4 (mole/L)

1

0.1(g)

47.27 (mL)

0.0106mol/L

2

0.1(g)

46.79 (mL)

0.0108mol/L

3

0.1(g)

46.61 (mL)

0.0108mol/L

4

5

(Note that the molecular weight of As2O3 is 197.84 g/mol.)

Trial

mass As2O3 (g)

volume KMnO4 (mL)

molarity KMnO4 (mole/L)

1

0.1(g)

47.27 (mL)

0.0106mol/L

2

0.1(g)

46.79 (mL)

0.0108mol/L

3

0.1(g)

46.61 (mL)

0.0108mol/L

4

5

Explanation / Answer

2As2O3 +6H2O===4H3AsO3

2 H3ASO3 + KMnO4 + 2 H2SO4 = 2 H3ASO4 + MnSO4 + KSO4 + 2 H2O

Trial

mass As2O3 (g)

volume KMnO4 (mL)

molarity KMnO4 (mole/L)

1

0.1(g)

47.27 (mL)

0.0106mol/L

2

0.1(g)

46.79 (mL)

0.0108mol/L

3

0.1(g)

46.61 (mL)

0.0108mol/L

47.27mL*0.0106moles/L=0.501mmoles

46.79mL*0.0108moles/L=0.505mmoles

46.79mL*0.0108moles/L=0.503mmoles

Moles of KMnO4=0.505mmoles=0.000505moles

Trial

mass As2O3 (g)

volume KMnO4 (mL)

molarity KMnO4 (mole/L)

1

0.1(g)

47.27 (mL)

0.0106mol/L

2

0.1(g)

46.79 (mL)

0.0108mol/L

3

0.1(g)

46.61 (mL)

0.0108mol/L

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