Question

A 25.00 mL pipetful of 0.250 M K,CrO, is added to an excess of AgNO,(aq). What mass of Ag,CrO, will precipitate from the solution? K,CrO.(aq) 2AgNO,(aq) → Ag:CrO.(s) 2KNO(aq)

Answer 1

To determine the mass of Ag₂Cr₂O7 that will precipitate, calculate the moles of K₂Cr₂O7 and use the mole ratio from the balanced equation to find the moles of Ag₂Cr₂O7. Convert the moles of Ag₂Cr₂O7 to mass using its molar mass.

To determine the mass of Ag₂Cr₂O7 that will precipitate from the solution, we need to first identify the limiting reactant. Given that we have an excess of AgNO3, K₂Cr₂O7 will be the limiting reactant.

From the balanced chemical equation, we know that 2 moles of AgNO3 react with 1 mole of K₂Cr₂O7 to form 1 mole of Ag₂Cr₂O7.

Using the volume and concentration of K₂Cr₂O7 given in the question, we can calculate the moles of K₂Cr₂O7.

Then, using the mole ratio from the balanced equation, we can determine the moles of Ag₂Cr₂O7 formed.

Finally, we can convert the moles of Ag₂Cr₂O7 to mass using its molar mass.