The unknown sample from Part (a) was found to have a mass of 0.7041 g. The mass of silver chloride that precipitated was 0.8717 g. What is the percentage chloride in the unknown?
The unknown sample from Part (a) was found to have a mass of 0.7041 g. The...
A 0.5711 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated as AgCI by the addition of an excess of silver nitrate. The mass of the resulting AgCl is found to be 1.2913 g. What is the mass percentage of chlorine in the original compound? 9 more group attempts remaining Submit Answer Retry Entire Group
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 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
A sample of an unknown gas is found to have a density of 1.53 g/L at a pressure of 0.612 atm and a temperature of 48 °C. Assume ideal behavior. The molar mass of the unknown gas is ? g/mol.
A sample of an unknown gas is found to have a density of 2.53 g/L at a pressure of 1.04 atm and a temperature of 49 °C. Assume ideal behavior. The molar mass of the unknown gas is ___________g/mol.
An organic pesticide (MW 183.7) is 8.43% Cl in mass. A 0.627 g sample containing the pesticide plus inert material containing no chloride was decomposed with metallic sodium in alcohol. The liberated chloride ion was precipitated as 0.0831 g AgCl(s). Calculate the percentage of pesticide in the sample. (1)
5. Given the following balanced chemical reaction, find the mass of silver chloride formed from 8.00 g of silver nitrate using the following steps: AgNO3 (aq) + NaCl (aq) → NaNO3 (aq) + AgCl (s) a. Given 8.00 g of silver nitrate (AgNO3), how many moles are there? b. What is the molar ratio of silver chloride (AgCl) to silver nitrate? C. How many moles of silver chloride are formed from the number of moles of silver nitrate found in...
11. The bromide impurity in a 2.00 g sample of a metal nitrate is precipitated as silver bromide. If 6.40 mL of 0.200 M AgNO, solution is required, what is the mass percentage of bromide in the sample? (A) 1.28 (B) 2.56 (C) 5.11 (D) 9.15
A mixture consisting of only iron(III) chloride (FeCl3) and aluminum chloride (AlCl3) weighs 1.0397 g. When the mixture is dissolved in water and an excess of silver nitrate is added, all the chloride ions associated with the original mixture are precipitated as insoluble silver chloride (AgCl). The mass of the silver chloride is found to be 3.0178 g. Calculate the mass percentages of iron(III) chloride and aluminum chloride in the original mixture. Mass percent FeCl3 = % Mass percent AlCl3...
A chloride of an unknown metal is believed to have the formula MCl3. A 1.603g sample of the compound is found to contain 3.606 x 10^-2 mol Cl. Find the atomic mass of M.