4) A sample of 0.670 g of an unknown compound containing barium ions (Ba2*) is dissolved in water and treated with...

Question

Question

Answer 1

Answer #1

Amount of Bajet polt = 0.41054 su in 0 41059 Balla Ba?t present - : In 233.38 g Basoa , Ba2l paesert 137.327 So, in 0.4105 a

Answer 2

Similar Homework Help Questions

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 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?
A 0.649-g sample containing only K_2SO_4 and (NH_4)2SO_4 was dissolved in water and treated with Ba...

A 0.649-g sample containing only K_2SO_4 and (NH_4)2SO_4 was dissolved in water and treated with Ba (NO_3)_2 to precipitate all SO^2-_4 as BaSO_4. Find the weight percent of K_2SO_4 in the sample if 0.977 g of precipitate was formed.

A 21.524 g paint sample was analyzed for barium (Ba2+, MW = 137.327 g/mole) by an...

A 21.524 g paint sample was analyzed for barium (Ba2+, MW = 137.327 g/mole) by an EDTA back titration: Ba2+(aq) + Y4–(aq) à BaY2–(aq). The sample was dissolved in acid and sufficient water was added to produce a volume of 100 mL. 10.00 mL of this concentrated solution was diluted to a volume of 50.00 mL. 25.00 mL of the diluted solution was treated with 33.95 mL of excess 0.09456 M EDTA. The excess EDTA was titrated to the endpoint...
A 1.42 g sample of a pure compound, with formula M_2SO_4, was dissolved in water and...

A 1.42 g sample of a pure compound, with formula M_2SO_4, was dissolved in water and treated with an excess of aqueous barium chloride, resulting in the precipitation of all the sulfate ion as barium sulfate. The precipitate was collected, dried, and found to weigh 2.3.3 g. Determine the atomic mass of M, and identify M.
A 0.2150 g sample is dissolved and treated with excess AgNO3. The precipitate is filtered, washed,...

A 0.2150 g sample is dissolved and treated with excess AgNO3. The precipitate is filtered, washed, dried, and weighed. The mass of the product (AgCl) is 0.4587 g. What is the wt% of Cl in the original sample? The molecular weight of AgCl is 143.32 g/mol.

A 12.5855 g sample of an unknown compound (X) is dissolved in 32.0000 g of water....

A 12.5855 g sample of an unknown compound (X) is dissolved in 32.0000 g of water. The resulting solution has a freezing point of – 4.3oC. What is the molar mass of X? Kf = 1.858 oC/m.
A 2.018-g sample of a metal bromide. MBr2, is dissolved in water and treated with excess...

A 2.018-g sample of a metal bromide. MBr2, is dissolved in water and treated with excess aqueous silver nitrate. The silver bromide (AgBr) that formed weighed 2.721 g. Calculate the atomic mass of Mand identify M. (molar mass of AgBr - 187.80 g/mol)
1. A 0.4187 g sample of a pure soluble chloride compound is dissolved in water, and...

1. A 0.4187 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated as AgCl by the addition of an excess of silver nitrate. The mass of the resulting AgCl is found to be 0.9536 g. What is the mass percentage of chlorine in the original compound? ________% 2. A student determines the calcium content of a solution by first precipitating it as calcium hydroxide, and then decomposing the hydroxide...

A chloride unknown sample weighing 0.4213 g is dissolved in acidic solution and is treated with...

A chloride unknown sample weighing 0.4213 g is dissolved in acidic solution and is treated with the precipitating solution. The silver chloride precipitate that forms is filtered, washed, dried and weighed. The mass of the silver chloride obtained is 0.5915 g. Calculate the % Cl in this unknown sample. Molar Masses: AgCl = 143.35 g/mol, Cl– = 35.45 g/mol