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
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A chloride unknown sample weighing 0.4213 g is dissolved in
acidic solution and is treated with...
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 2.31 g sample of a mixture of AgNO3 and NaNO3 is treated with excess Na2S(aq)....
A 2.31 g sample of a mixture of AgNO3 and NaNO3 is treated with excess Na2S(aq). The precipitate is filtered off, dried and weighed. The dried precipitate weighs 0.47 g. What is the percentage by mass of NaNO3 in the original mixture? Your answer must be accurate to two significant digits. Keep several extra digits in your calculations and round off only at the end. Do not include the percent sign (%) as part of your answer! Molar masses (in...
A 1.59-g sample of a metal chloride, MCl_2, is dissolved in water and treated with excess...
A 1.59-g sample of a metal chloride, MCl_2, is dissolved in water and treated with excess aqueous silver nitrate. The silver chloride that formed weighed 3.60 g. Calculate the molar mass of M. 70.9 g/mol 28 g/mol 55.9 g/mol 63 g/mol 72.4 g/mol
QUESTION 1 A 20.0 mL sample solution contains unknown amount of bromide ion (Br). To this...
QUESTION 1 A 20.0 mL sample solution contains unknown amount of bromide ion (Br). To this solution was added the solution that contains plenty of AgNO3. AgBr precipitates were formed. The precipitate were filtered and measured to be is 0.6964 g. What is the molarity of bromide ion in the original sample solution? The molar mass of Br = 80.0 g; the molar mass of AgBr = 188 g. (Solution) AgNO, is soluble and thus exists Ag+ ion and NO3-ion....
16. A solid sample contains only NaCl and KCI. A 0.5623 g sample of this material...
16. A solid sample contains only NaCl and KCI. A 0.5623 g sample of this material was dissolved in water. An excess of 0.10 M AgNO3 solution was added to precipitate out AgCl: Agt(aq) + Cl(aq) → AgCl(s) The AgCl was filtered, dried, and weighed. 1.2691 g of AgCl was obtained. What was the wt% of NaCl and the wt% of KCl in the sample?
Question A 20.0 mL sample solution contains unknown amount of bromide ion (Br). To this solution...
Question
A 20.0 mL sample solution contains unknown amount of bromide ion (Br). To this solution was added the solution that contains plenty of AgNO3. AgBr precipitates were formed. The precipitate were filtered and measured to be is 0.6964 g. What is the molarity of bromide ion in the original sample solution? The molar mass of Br = 80.0 g; the molar mass of AgBr = 188 g. (Solution) AgNO, is soluble and thus exists Ag+ ion and NO3-ion. Ag+...
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 0.6407 g sample containing chloride and iodide ions gave a silver halide precipitate weighing 0.4430...
A 0.6407 g sample containing chloride and iodide ions gave a silver halide precipitate weighing 0.4430 g. This precipitate was then strongly heated in a stream of Cl2 gas to convert the AgI to AgCl; on completion of this treatment, the precipitate weighed 0.3181 g. Calculate the percentage of chloride and iodide in the sample separately.
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 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)
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 1.59-g sample of a metal chloride, MCl_2, is dissolved in water and treated with excess aqueous silver nitrate. The silver chloride that formed weighed 3.60 g. Calculate the molar mass of M. 70.9 g/mol 28 g/mol 55.9 g/mol 63 g/mol 72.4 g/mol
QUESTION 1 A 20.0 mL sample solution contains unknown amount of bromide ion (Br). To this solution was added the solution that contains plenty of AgNO3. AgBr precipitates were formed. The precipitate were filtered and measured to be is 0.6964 g. What is the molarity of bromide ion in the original sample solution? The molar mass of Br = 80.0 g; the molar mass of AgBr = 188 g. (Solution) AgNO, is soluble and thus exists Ag+ ion and NO3-ion....
16. A solid sample contains only NaCl and KCI. A 0.5623 g sample of this material was dissolved in water. An excess of 0.10 M AgNO3 solution was added to precipitate out AgCl: Agt(aq) + Cl(aq) → AgCl(s) The AgCl was filtered, dried, and weighed. 1.2691 g of AgCl was obtained. What was the wt% of NaCl and the wt% of KCl in the sample?
Question
A 20.0 mL sample solution contains unknown amount of bromide ion (Br). To this solution was added the solution that contains plenty of AgNO3. AgBr precipitates were formed. The precipitate were filtered and measured to be is 0.6964 g. What is the molarity of bromide ion in the original sample solution? The molar mass of Br = 80.0 g; the molar mass of AgBr = 188 g. (Solution) AgNO, is soluble and thus exists Ag+ ion and NO3-ion. Ag+...
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 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)
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