A 40.00 mL solution of 0.3550 M AgNO3 was added to a solution of AsO43–. Ag3AsO4

Question

A 40.00 mL solution of 0.3550 M AgNO3 was added to a solution of AsO43–. Ag3AsO4 precipitated and was filtered off. Fe3 was added and the solution was titrated with 0.2700 M KSCN. After 30.00 mL of KSCN solution had been added, the solution turned red. What mass of AsO43– was in the original solution?

A 40.00 mL solution of 0.3550 M AgNO3 was added to a solution of Aso4AgAso4 precipitated and was filtered off. Fe was added and the solution was titrated with 02700 M KSCN. After 30.00 mL of KSCN solution had been added, the solution tumed red. What mass of Aso was in the original solution? Number mg AsO

Explanation / Answer

3AgNO3(aq) + AsO43-(aq) -----------> Ag3AsO4(s) + 3NO3-

Moles of AgNO3 used = molarity*volume of solution in litres = 0.355*0.04 = 0.0142

Thus, moles of AsO43-(aq) present = (1/3)*moles of AgNO3 = 4.734*10-3

Molar mass of AsO43-(aq) = 138.92 g/mole

Thus, mass of AsO43-(aq) present in the solution = moles*molar mass = 0.658 g

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