1) Calculate the masses of Ca(NO 3 ) 2 x4H 2 O (s) and KIO 3(s) required tomake
ID: 690408 • Letter: 1
Question
1) Calculate the masses of Ca(NO3)2 x4H2O(s) and KIO3(s) required tomake 10 g of Ca(IO3)2(s). Calculate theamount of Ca(NO3)2 x4H2O(s) needed so that the Ca2+ isin excess of the iodate ion concentration by 20% (i.e., calculate aweight of calcium nitrate that is 20% higher than the minumumrequired to produce 10 g of calcium iodate). 2) Calculate the mass of Ca(NO3)2 x4H2O(s) required to generate a 0.1XX MCa2+ solution in a 100 mL volumetric flask. (It iswritten as 0.1XX M because you don't know the actual concentrationof calcium needed until you weigh the solid and generate thesolution, but here is what you need to know: a) It should beclose to 0.1 M; b) the final concentration should be known out to 3significant figures; and c) you should use the actually generatedconcentration for all of your subsequent calculations (not just 0.1M) 1) Calculate the masses of Ca(NO3)2 x4H2O(s) and KIO3(s) required tomake 10 g of Ca(IO3)2(s). Calculate theamount of Ca(NO3)2 x4H2O(s) needed so that the Ca2+ isin excess of the iodate ion concentration by 20% (i.e., calculate aweight of calcium nitrate that is 20% higher than the minumumrequired to produce 10 g of calcium iodate). 2) Calculate the mass of Ca(NO3)2 x4H2O(s) required to generate a 0.1XX MCa2+ solution in a 100 mL volumetric flask. (It iswritten as 0.1XX M because you don't know the actual concentrationof calcium needed until you weigh the solid and generate thesolution, but here is what you need to know: a) It should beclose to 0.1 M; b) the final concentration should be known out to 3significant figures; and c) you should use the actually generatedconcentration for all of your subsequent calculations (not just 0.1M)Explanation / Answer
Ca(NO3)2 .4H2O(s) + 2KIO3(s) ------>Ca(IO3)2(s) + 2KNO3 + 4H2OMolar mass of Ca(NO3)2 .4H2O = 40 + 2 ( 14 + 3 * 16 ) + 4 ( 2 * 1 +16 ) = 236 g Molar mass of KIO3 = 39 + 127 + 3 * 16= 214 g Molar mass of Ca(IO3)2 is = 40 + 2 (127 + 3 * 16 ) = 390 g 236 g of Ca(NO3)2 .4H2O react with 2 * 214 g ofKIO3 produces 390 g ofCa(IO3)2 236 g of Ca(NO3)2 .4H2O produces 390 g ofCa(IO3)2 X g of Ca(NO3)2 .4H2O produces 10 g ofCa(IO3)2 X = ( 10 * 236 ) / 390 = 6.0513 g ofCa(NO3)2 .4H2O 2 * 214g of KIO3 produces 390 g of Ca(IO3)2 Y g of KIO3 produces 10g of Ca(IO3)2 Y = ( 2*214 * 10 ) / 390 = 10.9743 g of KIO3 calculate a weight of calcium nitrate that is 20% higherthan the minumum required to produce 10 g of calciumiodate for the production of 10 g of calcium iodate weight ofcalcium nitrate required is 6.0513 g
20% of 6.0513 g = 6.0513 * (20 / 100 ) = 1.2103 g So the required weight of calcium nitrate = 6.0513 +1.2103 = 7.2616g 2) Calculate the mass of Ca(NO3)2 x4H2O(s) required to generate a 0.1XX MCa2+ solution in a 100 mL volumetric flask. Molarity , M = ( mass / Molar mass ) / Volume in L 0.1 M =( m / 236 ) / 0.1 L === > m = 2.36 g ofCa(NO3)2 x 4H2O Y g of KIO3 produces 10g of Ca(IO3)2 Y = ( 2*214 * 10 ) / 390 = 10.9743 g of KIO3 calculate a weight of calcium nitrate that is 20% higherthan the minumum required to produce 10 g of calciumiodate calculate a weight of calcium nitrate that is 20% higherthan the minumum required to produce 10 g of calciumiodate for the production of 10 g of calcium iodate weight ofcalcium nitrate required is 6.0513 g
20% of 6.0513 g = 6.0513 * (20 / 100 ) = 1.2103 g So the required weight of calcium nitrate = 6.0513 +1.2103 = 7.2616g 2) Calculate the mass of Ca(NO3)2 x4H2O(s) required to generate a 0.1XX MCa2+ solution in a 100 mL volumetric flask. Molarity , M = ( mass / Molar mass ) / Volume in L 0.1 M =( m / 236 ) / 0.1 L === > m = 2.36 g ofCa(NO3)2 x 4H2O
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.