Addition of an excess silver nitrate to a 0.5012 g sample yielded a mixture of AgCl and Agl thatweighed 0.4700 g. The precipitate was then heated in a stream of Cl2 to convert the Agl to AgCl.2 Agl (s) + Cl2 (g)2 AgCI (s) + 12(g)The precipitate was found to weigh 0.3900 g after this treatment. Calculate the percentages of NH4Iand NH4CI, respectively.19.71, 25.0725.07, 28.7228.72, 19.95O 25.07, 19.71O 19.95, 28.72

Excess silver nitrate was added to a mixture containing NH4I and NH4Cl.…

Answered: Addition of an excess silver nitrate to…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Excess solid Ni(OH)2 was added to water and the resulting solution was allowed to stand for several days. The solution was then filtered to remove excess solid Ni(OH)2. A 0.250 L aliquot of the solution was then titrated with 10.54 mL of a standardized 0.000500 M HCl solution. What is the Ksp of Ni(OH)2?
Suppose that the solubility of calcium iodate are 2.5 g/L at 20oC and 5.5 g/L at 60oC. What are the solubility in mol/L at 20oC and at 60oC? How many milliliters (mL) of 0.045 M Na2S2O3 will be required to titrate a 10.0-mL sample of saturated Ca(IO3)2 solution collected at 20oC and 60oC, respectively?
2. A 0.4912-g sample of a petroleum product was burned in a tube furnace, and the SO2 produced was collected in H2O2. SO2(g) + H2O2 → H2SO4 A 25.00-mL portion of 0.00873 M NaOH was introduced into the solution of H2SO4, following which the excess base was back-titrated with 15.17 mL of 0.01102 M HCl. Calculate the sulfur concentration in parts per million.
A 1.00 gram sample of anhydrous cerium sulfate was dissolved in water. Barium nitrate solution was then added until no further precipitation occurred. The precipitate was filtered from the solution then dried and was found to weigh 1.41 g. Determine the formula of the cerium sulfate. Encom calt is hydrated
Ksp for PbCl2(s) is 1.6 x 10-³. If you mix 200.0 mL of 0.010 M Pb(NO3)2(aq) with 400.0 mL of 0.010 M NaCI(aq), then sodium nitrate will precipitate. the concentration of CI will be 0.0033 M. no precipitate will form. PbCl2(s) will precipitate.
A 4.908-g sample of a petroleum product was burned in a tube furnace, and the SO2 produced was collected in 2% H2 O2. Reaction: SO2 (g) + H2O2 → H2SO4 A 27.00-mL portion of 0.00826 M NaOH was introduced into the solution of H2 SO4, following which the excess base was back-titrated with 15.15 mL of 0.01165 M HCl. Calculate the sulfur concentration in the sample in parts per million. Concentration ppm
A student weighs a sample of potassium hydrogen phthalate (KHP) to prepare a primary standard for a titration. She later discovers that the KHP was contaminated with sugar. To determine the amount of KHP in the mixture, she takes 4.678 g4.678 g of the mixture and make a 100.0 mL100.0 mL solution. The student then titrates 10.00 mL10.00 mL of this solution with a 0.1030 M0.1030 M sodium hydroxide solution. She finds that 15.15 mL15.15 mL of the NaOHNaOH solution is needed to reach the end point.
2. To standardize a solution of NaOH, a student measured 0.326 g of potassium hydrogen phthalate (KHC8H404 or KHP) and dissolved it in 50.0 mL of water. To the solution, two drops of phenolphthalein indicator was added. To reach the equivalence point as indicated by endpoint of the titration where the solution retained a pale pink color, a volume of 15.3 mL was required. What is the molarity of the NaH solution? (KHP is a monoprotic acid that furnishes one H* ion; at the equivalence point, mols OH (base) = mols H* (acid))
Write a formula for the following precipitate and write a balanced net ionic equation for the reaction that occured between this precipitate and 3 M HNO3(aq). CO32- and 0.2M Pb(NO3)2
The hardness of water (hardness count) is usually expressed in PPM (by mass) of CaCO3 which is equivalent to mg of CaCO3 per liter of water. What is the molar concentration of Ca2+ ions in a water sample with a hardness count of 185mg CaCO3/L
A 750. mL sample of 0.13 M K₂CO3(aq) is combined with 250. mL of 0.13 M CUNO3(aq). The Ksp for Cu₂CO3 = 1.4 x 10-10 and the Ksp for KNO3 = 1.4 x 10¹0. Which of the following statements is true? Both Cu₂CO3 and KNO3 will precipitate. KNO3 will precipitate. No precipitate forms. There is not enough information to make any of the above predictions. Cu₂CO3 will precipitate.
A 2.45 g mixture of BaCl2 and Ba(NO3)2 is dissolved in water. Excess AgNO3 is added and all of the dissolved chloride ion is precipitated. The resulting precipitate weighs 0.845 g. Use the following Molar Masses (in g mol−−1) as required: Ba: 137.3 Cl: 35.45 Ag: 107.9 N: 14.01 O: 16.00 What is the mass of Ba(NO3)2 in the original mixture? Enter a mass accurate to three significant figures.

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