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A 1.475-g sample containing NH4Cl (FM 53.492), K2CO3 (FM 138.21), and inert ingredients
Chapter 26, Problem 26-21(choose chapter or problem)
A 1.475-g sample containing NH4Cl (FM 53.492), K2CO3 (FM 138.21), and inert ingredients was dissolved to give 0.100 L of solution. A 25.0-mL aliquot was acidified and treated with excess sodium tetraphenylborate, NaB(C6H5)4 , to precipitate K and NH4 ions completely: FM 358.33 FM 337.27 The resulting precipitate amounted to 0.617 g. A fresh 50.0-mL aliquot of the original solution was made alkaline and heated to drive off all the NH3: It was then acidified and treated with sodium tetraphenylborate to give 0.554 g of precipitate. Find the weight percent of NH4Cl and K2CO3 in the original solid. 26-
Questions & Answers
QUESTION:
A 1.475-g sample containing NH4Cl (FM 53.492), K2CO3 (FM 138.21), and inert ingredients was dissolved to give 0.100 L of solution. A 25.0-mL aliquot was acidified and treated with excess sodium tetraphenylborate, NaB(C6H5)4 , to precipitate K and NH4 ions completely: FM 358.33 FM 337.27 The resulting precipitate amounted to 0.617 g. A fresh 50.0-mL aliquot of the original solution was made alkaline and heated to drive off all the NH3: It was then acidified and treated with sodium tetraphenylborate to give 0.554 g of precipitate. Find the weight percent of NH4Cl and K2CO3 in the original solid. 26-
ANSWER:The mass of NH4Cl in the original solid = (0.617g/358.33)*53.492 = 0.046 g
The mass of K2CO3 in