Does any solid Ag2CrO4 form when 2.7×10−5 g of AgNO3 is dissolved in 15.0 ml of 4.0×10−4 K2CrO4?

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Does any solid Ag2CrO4 form when 2.7×10−5 g of AgNO3 is dissolved in 15.0 ml of 4.0×10−4 K2CrO4?

Talisha · Accepted Answer

Balanced reaction-:  2AgNO3(aq)+K2CrO4(aq)→Ag2CrO4(s)+2KNO3(aq)  Moles of AgNO3=mass(g)molar mass (g/mol)=2.7×10−5g169.86 gmol  =1.589⋅10−7 mol  Molarity of Ag+=moles of soluteV(L)=1.589⋅10−7 mol0.015 L=1.059⋅10−5M  Ksp of Ag2CrO4  =[Ag+]2[CrO42−]  1.2⋅10−12=[2s]2[s]  4s3=1.2⋅10−12  s=6.69⋅10−5 M  Molarity of Ag+ is less than the molar solubility thus ppt will not occur

Does any solid Ag2CrO4 form when 2.7×10−5 g of AgNO3 is dissolved in 15.0 ml...

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