a. A 1.500 g sample of a mixture of solid Na3PO4 - 12H2O and BaCl2 -...

a. A 1.500 g sample of a mixture of solid Na3PO4 - 12H2O and BaCl2 - 2H2O was dissolved in water and formed 0.520g of Ba3(PO4)2 precipitate. If reagent tests demonstrated that Na3PO4 - 12H2O was the limiting reactant in the precipitation reaction, calculate the mass percent of each reactant in the original sample. b. Clearly demonstrate which reactant salt would be limiting if the experiment was performed with equal masses of each salt. Assume 0.500g of each salt, for instance.

Expert Solution

queen_honey_blossom answered 1 year ago

A mixture contains 58.50 % BaCl2 and 41.50 % Na3PO4 by weight. When dissolved in water,...

A mixture contains 58.50 % BaCl2 and 41.50 % Na3PO4 by weight. When dissolved in water, the following double displacement reaction forms the barium phosphate precipitate. If you start with 6.00 grams of the mixture, how many grams of barium phosphate precipitate should form? 3 BaCl2 (aq) + 2 Na3PO4 (aq) --> 6 NaCl (aq) + Ba3(PO4)2 (s) Use the following molar masses: BaCl2 = 208.23 g/mol Na3PO4 = 163.91 g/mol NaCl = 58.44 g/mol Ba3(PO4)2 = 601.93 g/mol Enter...

A 8.40-g sample of solid BaCl2·2H2O was heated such that the water turned to steam and...

A 8.40-g sample of solid BaCl2·2H2O was heated such that the water turned to steam and was driven off. Assuming ideal behavior, what volume would that steam occupy at 1.00 atm and 100.0 °C?

A 1.500 L flask is filled with a mixture of 1.20 g H2 and 8.40 g...

A 1.500 L flask is filled with a mixture of 1.20 g H2 and 8.40 g O2, at 25°C. The mixture is ignited, and hydrogen and oxygen combine to form water. What is the total pressure inside the flask before the reaction? (Report your answer in units of atmospheres.) What is the total pressure after the reaction, once the flask is returned to 25°C? (Vapour pressure of water at 25°C is 23.8 mm Hg.)

A 0.5065 g solid sample containing a mixture of LaCl3 (molar mass = 245.26 g/mol) and...

A 0.5065 g solid sample containing a mixture of LaCl3 (molar mass = 245.26 g/mol) and Ce(NO3)3 (molar mass = 326.13 g/mol) was dissolved in water. The solution was titrated with KIO3, producing the precipitates La(IO3)3(s) and Ce(IO3)3(s). For the complete titration of both La3 and Ce3 , 44.81 mL of 0.1252 M KIO3 was required. Calculate the mass fraction of La and Ce in the sample.

A 0.5072 g solid sample containing a mixture of LaCl3 (molar mass = 245.26 g/mol) and...

A 0.5072 g solid sample containing a mixture of LaCl3 (molar mass = 245.26 g/mol) and Ce(NO3)3 (molar mass = 326.13 g/mol) was dissolved in water. The solution was titrated with KIO3, producing the precipitates La(IO3)3(s) and Ce(IO3)3(s). For the complete titration of both La3 and Ce3 , 44.01 mL of 0.1289 M KIO3 was required. Calculate the mass fraction of La and Ce in the sample.

A 0.5070 g solid sample containing a mixture of LaCl3 (molar mass = 245.26 g/mol) and...

A 0.5070 g solid sample containing a mixture of LaCl3 (molar mass = 245.26 g/mol) and Ce(NO3)3 (molar mass = 326.13 g/mol) was dissolved in water. The solution was titrated with KIO3, producing the precipitates La(IO3)3 and Ce(IO3)3. For the complete titration of both La3+ and Ce3+, 42.10 mL of 0.1204 M KIO3 was required. Calculate the mass fraction of La and Ce in the sample. mass fraction La: g Lag sample mass fraction Ce: g Ceg sample

A 0.5206 g solid sample containing a mixture of LaCl3 (molar mass = 245.26 g/mol) and...

A 0.5206 g solid sample containing a mixture of LaCl3 (molar mass = 245.26 g/mol) and Ce(NO3)3 (molar mass = 326.13 g/mol) was dissolved in water. The solution was titrated with KIO3, producing the precipitates La(IO3)3(s) and Ce(IO3)3(s). For the complete titration of both La3 and Ce3 , 43.38 mL of 0.1236 M KIO3 was required. Calculate the mass fraction of La and Ce in the sample.

Balance these equations: HCl+CaCO3= HCl+Na2CO3= HCl+NaOH= NaOH+FeCl3= CoCl2+AgNO3= CuSO4+Na2CO3= CuSO4+BaCl2= Na3PO4+CuSO4= Na3PO4+NiCl2= Na3PO4+BaCl2= NH4Cl+AgNO3=

Combustion analysis of 1.500 g of a sample produced 0.0468 moles of CO2(g) and 0.0936 moles...

Combustion analysis of 1.500 g of a sample produced 0.0468 moles of CO2(g) and 0.0936 moles of H2O(g). Which substance is consistent with this analysis?

A solid mixture consists of 39.1 g of KNO3 (potassium nitrate) and 6.9 g of K2SO4...

A solid mixture consists of 39.1 g of KNO3 (potassium nitrate) and 6.9 g of K2SO4 (potassium sulfate). The mixture is added to 130. g of water. A. Consider the mixture described in the introduction. At 60 ∘C , to what extent will each solute be dissolved? (Totally dissolved, partially dissolved, not dissolved) B. If the solution is cooled to 0 degrees Celsius, what mass, in grams, would KNO3 crystallize?

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