Consider a 2.0000 g sample containing MgSO4 (FW 120.366). The sample is dissolved and the sulfate...
Consider a 2.0000 g sample containing MgSO4 (FW 120.366). The sample is dissolved and the sulfate is precipitated as BaSO4 (FW 233.39). If the BaSO4 precipitate weighs 1.4900 g, what is the mass % of MgSO4 in the sample?
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Consider a 2.0000 g sample containing MgSO4 (FW
120.366). The sample is dissolved and the sulfate...
4) A sample of 0.870 g of an unknown compound containing barium ions (Ba2+) is dissolved...
4) A sample of 0.870 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and treated with an excess of Na2SO4. If the mass of the BaSO4 precipitate formed is 0.4105 g, what is the percent by mass of Ba in the original compound?
A sample containing phosphorus weighs 1.342 g. The phosphorus containing compound in this sample is P4010....
A sample containing phosphorus weighs 1.342 g. The phosphorus containing compound in this sample is P4010. A gravimetric experiment was performed and phosphorus in the sample was precipitated as Ca3(PO4)2. The mass of the isolated precipitate is 0.752 g. Find the mass % of phosphorus in the sample.
Metal Sulfate Hydrate lab (12 points) 4) An unknown metal sulfate hydrate (MSO XHO) sample with...
Metal Sulfate Hydrate lab (12 points) 4) An unknown metal sulfate hydrate (MSO XHO) sample with the recorded mass below is dissolved in water, and the sulfate ions from the sample precipitated with Ba2+ ions as BaSO4. A pre-massed filter paper is then used to collect the solid BaSO4. Experimental data was recorded below following same procedure in MSH lab. 0.6939 96.06 g/mol Molar mass of SO42- PARTA Mass of unknown metal sulfate hydrate (MSH) Mass of unknown sample sulfate...
A 1.546g sample containing a mixture of only k2So4 and kno3 was dissolved in water an...
A 1.546g sample containing a mixture of only k2So4 and kno3 was dissolved in water an treated with BaCl2, precipitating the So42- as Baso4(pksp=9.96) the resulting precipitate was isolated and yielded 863.5mg of baso4. What is % in mass of K2So4 and Kno3
In the analysis of 0.8503 g of impure chloride containing sample, 1.250 g of AgCl were...
In the analysis of 0.8503 g of impure chloride containing sample, 1.250 g of AgCl were precipitated out. What is the percent of mass of chlorine in the sample. (FW of AgCl = 143.32 g/mol, FW of Cl =35.453) a.29.09% b.30.92% c.36.37% d.72.74% explain
1. A 0.7336-g sample of an alloy containing copper and zinc is dissolved in 8 M...
1. A 0.7336-g sample of an alloy containing copper and zinc is dissolved in 8 M HCl and diluted to 100 mL in a volumetric flask. In one analysis, the zinc in a 25.00-mL portion of the solution is precipitated as ZnNH4PO4, and subsequently isolated as Zn2P2O7, yielding 0.1163 g. The copper in a separate 25.00-mL portion of the solution is treated to precipitate CuSCN, yielding 0.1931 g. Calculate the %w/w Zn and the %w/w Cu in the sample.
A sample of 0.7360 g of an unknown compound containing barium ions (Ba2+) is dissolved in...
A sample of 0.7360 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and treated with an excess of Na2CO3. If the mass of the BaCO3 precipitate formed is 0.7578 g, what is the percent by mass of Ba in the original unknown compound?
4) A sample of 0.670 g of an unknown compound containing barium ions (Ba2*) is dissolved in water and treated with...
4) A sample of 0.670 g of an unknown compound containing barium ions (Ba2*) is dissolved in water and treated with an excess of NA2SO4. If the mass of the BaS04 precipitate formed is 0.4105 g, what is the percent by mass of Ba in the original compound?
3. A1.22 g solid sample of impure lead (11) nitrate was dissolved in 40.0 mL of...
3. A1.22 g solid sample of impure lead (11) nitrate was dissolved in 40.0 mL of distilled water and analyzed by gravimetric analysis. Sodium sulfate was delivered from a burette to precipitate the lead ions as lead sulfate. Sodium sulfate was added until no more precipitate was seen to form. The precipitate was filtered, washed an dried before been weighed. When weighed, the precipitate had a mass of 1.44 g. What is the mass percent of lead in the original...
A 3.00- g sample of an alloy of Pb Lead was dissolved in nitric acid (HNO)....
A 3.00- g sample of an alloy of Pb Lead was dissolved in nitric acid (HNO). Sulfuric acid was added to this solution, which precipitated 1.69 g of lead sulfate (PbSO.). What is the percentage of lead (Pb) in the sample? (Given the atomic mass of Pb - 207, S =32,0 - 16 gram/mole)
4) A sample of 0.870 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and treated with an excess of Na2SO4. If the mass of the BaSO4 precipitate formed is 0.4105 g, what is the percent by mass of Ba in the original compound?
A sample containing phosphorus weighs 1.342 g. The phosphorus containing compound in this sample is P4010. A gravimetric experiment was performed and phosphorus in the sample was precipitated as Ca3(PO4)2. The mass of the isolated precipitate is 0.752 g. Find the mass % of phosphorus in the sample.
Metal Sulfate Hydrate lab (12 points) 4) An unknown metal sulfate hydrate (MSO XHO) sample with the recorded mass below is dissolved in water, and the sulfate ions from the sample precipitated with Ba2+ ions as BaSO4. A pre-massed filter paper is then used to collect the solid BaSO4. Experimental data was recorded below following same procedure in MSH lab. 0.6939 96.06 g/mol Molar mass of SO42- PARTA Mass of unknown metal sulfate hydrate (MSH) Mass of unknown sample sulfate...
4) A sample of 0.670 g of an unknown compound containing barium ions (Ba2*) is dissolved in water and treated with an excess of NA2SO4. If the mass of the BaS04 precipitate formed is 0.4105 g, what is the percent by mass of Ba in the original compound?
3. A1.22 g solid sample of impure lead (11) nitrate was dissolved in 40.0 mL of distilled water and analyzed by gravimetric analysis. Sodium sulfate was delivered from a burette to precipitate the lead ions as lead sulfate. Sodium sulfate was added until no more precipitate was seen to form. The precipitate was filtered, washed an dried before been weighed. When weighed, the precipitate had a mass of 1.44 g. What is the mass percent of lead in the original...
A 3.00- g sample of an alloy of Pb Lead was dissolved in nitric acid (HNO). Sulfuric acid was added to this solution, which precipitated 1.69 g of lead sulfate (PbSO.). What is the percentage of lead (Pb) in the sample? (Given the atomic mass of Pb - 207, S =32,0 - 16 gram/mole)
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