We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
A 2.018-g sample of a metal bromide. MBr2, 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
1. A l64-g sample of HF is dissolved in water to give 2.0 x 10' ml of solution. The concentration of solution is: A) 0.82 M B) 0.16 M C) 0.08 M D) 4.1 M E) 8.2 M 2. You have 75.0 mL of a 2.50 M solution of Na,CrO(ag). You also have 125 mL of a 2.01 M solution of AgNOs(ag), Calculate the concentration of Cro. after the two solutions are mixed together. A) 0.00 M B) 0.309 M...
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 21.5 g sample of nickel was treated with excess silver nitrate solution to produce silver metal and nickel(II) nitrate. The reaction was stopped before all the nickel reacted, and 36.5 g of solid metal (nickel and silver) is present. Calculate the mass of solid silver metal present.
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, 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.
What is the mass of insoluble silver bromide (187.77 g/mol) produced from 2.96 g of iron(III) bromide (295.55 g/mol) and aqueous silver nitrate? FeBr3(s) + AgNO3(aq) → AgBr(s) + Fe(NO3)3(aq)
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
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...
Impure sample of table salt that weighed 0.8421g, when dissolved in water and treated with excess AgNO3, formed 2.044g of AgCl. What is the percentage of NaCl in the impure sample? Do I need the molecular weight to start this equation? Where do I start?