To a 250.0 mL volumetric flask are added 1.00 mL volumes of three solutions: 0.0

Question

To a 250.0 mL volumetric flask are added 1.00 mL volumes of three solutions: 0.0100M AgNO3, 0.150M NaBr, and 0.100M NaCN. The mixture is diluted with deionized water to the mark and shaken vigorously. What mass of AgBr would precipitate from this mixture? (The Ksp of AgBr is 5.4x10^-13 and the Kf of Ag(CN)2- is 1,0x10^21). To a 250.0 mL volumetric flask are added 1.00 mL volumes of three solutions: 0.0100M AgNO3, 0.150M NaBr, and 0.100M NaCN. The mixture is diluted with deionized water to the mark and shaken vigorously. What mass of AgBr would precipitate from this mixture? (The Ksp of AgBr is 5.4x10^-13 and the Kf of Ag(CN)2- is 1,0x10^21).

Explanation / Answer

concentration of Ag+ in solution = 0.01 M x 1ml/250 ml = 0.00004 M

concentration of Br- in solution = 0.150 M x 1 ml/250 ml = 0.0006 M

moles of Ag+ = 0.00004 M x 250 ml = 0.01 mmols

moles of Br- = 0.0006 M x 250 ml = 0.15 mmols

1 mole of AgBr with combine with 1 mole of NaBr to form 1 mole of AgBr

moles of AgBr formed = 0.01 mmols

mass of AgBr formed = 0.01 mmol x 187.77 g/mol/1000 = 1.88 mg

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