3. A1.22 g solid sample of impure lead (11) nitrate was dissolved in 40.0 mL of...
Complete each question with the best for math questions, the proper number of dicanture 1. You've inherited an 18 karat gold ring that weighs 9.0 grams. Puregold is 24 karats, which means your ring is 75 pure godowany atoms of old are in your 2. It takes 38 ml of 0.75 M NaOH solution to completely neutralize 155 ml of a sulfuric acid solution ( HSO). What is the concentration of the HSO solution? 3. A1.22 g solid sample of...
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 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 18.88-g sample consisting of a mixture of sodium chloride and potassium sulfate is dissolved in water. This aqueous mixture then reacts with excess aqueous lead(II) nitrate to form 36.80 g of solid. Determine the mass percent of sodium chloride in the original mixture.
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?
The concentration of lead ions (Pb2+) in a sample of polluted water that also contains nitrate ions (NO3−) is determined by adding solid sodium sulfate (Na2SO4) to exactly 500 mL of the water. Calculate the molar concentration of Pb2+ if 0.00230 g of Na2SO4 was needed for the complete precipitation of lead ions as PbSO4.
A salt contains only strontium and one of the halide ions. A 0.0910-g sample of the salt was dissolved in water, and an excess of sulfuric acid was added to form strontium sulfate (SrSO4), which was filtered, dried, and weighed. Its mass was found to be 0.133 g. What is the formula of the strontium halide? (Omit states-of-matter from your answer.)
A 6.04 g sample of a solid containing Ni is dissolved in 20.0 mL water. A 5.00 mL aliquot of this solution is diluted to 100.0 mL and analyzed in the lab. The analyzed solution was determined to contain 6.88 ppm Ni . Determine the molar concentration of Ni in the 20.0 mL solution. *concentration= ? M Determine the mass, in grams, of Ni in the original sample. *mass= ? g Determine the weight percent of Ni in the sample....
Enter your answer in the provided box. The concentration of lead ions (Pb2) in a sample of polluted water that also contains nitrate ions (NO3 ) is determined by adding solid sodium sulfate (Na2SO4) to exactly 500 mL of the water. Calculate the molar concentration of Pb2* if 0.00275 g of NazSO4 was needed for the complete precipitation of lead ions as Pbso4 Enter your answer in the provided box. The concentration of lead ions (Pb2) in a sample of...
5. A 2.600 g sample of limestone was dissolved in excess 0.200 M HCl(aą): CaCO(s) 2 HCa)Ca (a2 CT(a)CO (g)HO) Excess 0.10 M (NH C20(a) was added to the resulting solution to precipitate the calcium ions as calcium oxalate, CaC204(s). Ca (aq) (NH).CO(a)CaC,04(s)2 NH (aq) The precipitate was filtered and dried three times to a constant mass of I 036 g. Determine the mass% Ca in the limestone sample.