A sample of mixture of FeSO4.(NH4)2So4.6H2O and inert material is dissolved in water, and the Fe...

A sample of mixture of FeSO4.(NH4)2So4.6H2O and inert material is dissolved in water, and the Fe is oxidized with bromine water. The excess Br2 is boiled out and NH4OH is added to precipitate the Fe(III). This precipitate, after ignition, weighs 0.160 g. Calculate a) the volume of the NH4OH (specific gravity 0.960, containing 10.0% Nh3 by weight) theoretically required in the above preecipitaion? b) The volume of 0.100 N BaCl2 solution required to precipitate the sulfate from the filtrate of the NH4OH precipitation.

Expert Solution

queen_honey_blossom answered 4 months ago

A mixture contains only and . A 4.51-g sample of the mixture is dissolved in water...

A mixture contains only and . A 4.51-g sample of the mixture is dissolved in water and an excess of is added, producing a precipitate of . The precipitate is filtered, dried, and weighed. The mass of the precipitate is 1.06 g. What is the mass percent of in the sample? %

A 0.9140 g sample of a mixture of NaCl and KCl is dissolved in water, and...

A 0.9140 g sample of a mixture of NaCl and KCl is dissolved in water, and the solution is then treated with an excess of AgNO3 to yield 1.943 g of AgCl. Calculate the percent by mass of each compound in the mixture.

A 0.9000 g sample of a mixture of NaCl and KCl is dissolved in water, and...

A 0.9000 g sample of a mixture of NaCl and KCl is dissolved in water, and the solution is then treated with an excess of AgNO3 to yield 1.923 g of AgCl. Calculate the percent by mass of each compound in the mixture. ____% mass of NaCl ____% mass of KCl

A mixture of MgBr2 and inert material is analyzed to determine the Mg content. First the...

A mixture of MgBr2 and inert material is analyzed to determine the Mg content. First the mixture is dissolved in water. Then all of the bromide ion is precipitated as AgBr by the addition of an excess of silver nitrate. MgBr2(aq) + 2AgNO3(aq) 2AgBr(s) + Mg(NO3)2(aq) In one experiment, a 0.8107 g sample of the mixture resulted in 1.1739 g of AgBr. Determine the percent (by mass) of Mg in the mixture.

A 0.3146-g sample of a mixture of NaCl(s) and KBr(s) was dissolved in water. The resulting...

A 0.3146-g sample of a mixture of NaCl(s) and KBr(s) was dissolved in water. The resulting solution required 36.00 mL of 0.08765 M AgNO3(aq) to precipitate the Cl–(aq) and Br–(aq) as AgCl(s) and AgBr(s). Calculate the mass percentage of NaCl(s) in the mixture.

a 0.5153g solid sample containing only a mixture of LaCl3 & Ce(NO3)3 was dissolved in water....

a 0.5153g solid sample containing only a mixture of LaCl3 & Ce(NO3)3 was dissolved in water. Potassium iodate was then added to the obtained solution producing the precipitates La(IO3)3 molar mass 663.61 g/mol & Ce(IO3)3 molar mass 664.82 g/mol. the total mass of the precipitates was found to be equal to 1.1650g. Calc the % of LaCl3 and Ce(NO3)3 in the sample. i have to where there are two equations and two unknowns. I just don't know how to solve...

The ionic compound, (NH4)2SO4, will fully dissolve in water. If 19.90 g is dissolved in 482.0...

The ionic compound, (NH4)2SO4, will fully dissolve in water. If 19.90 g is dissolved in 482.0 mL water, find the following ion concentrations. The concentration of the NH4+ is: The concentration of the SO42- is:

A mass of 14.22g of (NH4)2SO4 (molar mass = 132.06g/mol) is dissolved in water. After the...

A mass of 14.22g of (NH4)2SO4 (molar mass = 132.06g/mol) is dissolved in water. After the solution is heated, 30.19g of Al2(SO4)3•18H2O (molar mass = 666.36g/mol) is added. calculate the theoretical yield of the resulting alum. Hint: This is a limiting reactant problem.

A 0.500 g sample containing Ag2O and inert material is heated, causing the silver oxide to...

A 0.500 g sample containing Ag2O and inert material is heated, causing the silver oxide to decompose according to the following equation: 2 Ag2O(s) → 4 Ag(s) + O2(g) If 13.8 mL of gas are collected over water at 27°C and 1.00 atm external pressure, what is the percentage of silver oxide in the sample? The partial pressure of water is 26.7 mm Hg at 27°C. a.) 25.1% b.) 51.9% c.)12.5% d.) 50.1%

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...

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