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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0.753-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting the evolved gases in a solution of NaOH. After neutralizing, the sample was treated with 25.74 mL of a 0.264 M AgNO3 solution. This precipitated the chloride (Cl-) out as AgCl and left an excess of AgNO3. The excess AgNO3 was titrated with 0.1 M KSCN and required 16.47 mL to reach the endpoint in a Volhard titration. Calculate the % w/w Cl– (35.45 g/mol) in the sample. Provide your answer to 2 places after the decimal point and without units. Reactions: Cl– + Ag+ → AgCl(s) Reaction 1 Ag+ + SCN– → AgSCN(s) Reaction 2 HINT: This is an example of a back-titration. Steps to success: First, calculate the TOTAL amount (in moles) of Ag+ added from the volume and molarity of the silver nitrate solution. Second, determine the EXCESS amount of Ag+ from the reaction with thiocyanate (Reaction 2 above). Third, calculate the…
A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 28.4 mL of HNO₃ was required. Given that 0.00966 mol of HNO₃ are used in the titration, how many moles of Ca(OH)₂ had to be present in the initial reaction?
A sample containing calcium was analyzed by gravimetry, converting all calcium to calcium oxalate monohydrate (CaC2O4 • H2O). The sample weighing 0.2654 g was dissolved by adding 6M HCl, and then ammonium oxalate solution was added to precipitate all the calcium. The precipitate was suction filtered and dried in an oven at 95 °C for one hour. The solid obtained weighed 0.3216 grams.Calculate:A) The percentage of CaCO3B) The percentage of Ca C) The percentage of CaO
The zinc content of a 1.03 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc. The excess HCI is then neutralized with with NaOH. The reaction of HCl with Zn is shown. Zn(s) + 2 HCl(aq) ->> ZnCl₂ (aq) + H₂(g) The ore was dissolved in 150 mL of 0.600 M HCl, and the resulting solution was diluted to a total volume of 300 mL. A 20.0 mL aliquot of the final solution required 8.94 mL of 0.530 M NaOH to neutralize the excess HCl. What is the mass percentage (%w/w) of Zn in the ore sample? %w/w = % Zn
A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 20.2 mL of HNO₃ was required. Write the balanced chemical equation for the reaction
16. A sample of seawater contains 400 g Ca? ions per m³. What must be the minimum concentration of PO to start the precipitation of Ca? ions as Ca3(PO4)2 for which K = 1.6 x 1025 Ca= 40 A) 3 x 10 ? D) 1 x 10 19 %3D B) 4 x 10 17 C) 2 x 10 23 E) 4 x 101 10
a Pb(NO;)2 + MgSO, The precipitate is Cu(NO3)2 + ZnBr2 The precipitate is Submit (NH4)2 CO3 + Bal, The precipitate is K2 CrO4 + Pb(NO3)2 The precipitate is
A quantitative analysis for ethanol, C2H60, is accomplished by a redox back titration. Ethanol is oxidized to acetic acid, C2H402, using excess dichromate, 3+ Cr207 2-, which is reduced to Cr3*. The excess dichromate is titrated with Fe2*, giving C and Fe+ as products. In a typical analysis, a 5.00-mL sample of a brandy is diluted to 500 mL in a volumetric flask. A 10.00-mL sample is taken and the ethanol is removed by distillation and collected in 50.00 mL of an 2- acidified solution of 0.0200 M K2Cr207. Titration of the unreacted Cr207 requires 21.48 mL of 0.1014 M Fe2*. Calculate the %w/v ethanol in the brandy. Which is the titrant in this problem? C2H402 Fe2+ C2H60 O Cr207 2-
25.00 mL of a solution containing KIO4 is treated with excess potassium iodide. IO4- + 8H+ + 7I- → 4I2 + 4H2O The resulting solution is titrated with 0.15 M sodium thiosulfate pentahydrate. The average titre was 21.76 mL. I2 + 2S2O32- → 2I- + S4O62- What mass of KIO4 (in g) was dissolved in water to make the original solution?
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?
Fe3+ in 50 mL solution, which is known to contain Fe3+, was precipitated as Fe(OH)3 and after necessary procedures, it was brought to constant weight as Fe2O3. Since the weight is found to be 0.3994 g, find the Fe3+ concentration in the solution in terms of molarity. (Fe: 55.85, O: 16.00 g / mol)
A 0.5145-g sample of a water-soluble fertilizer was dissolved and analyzed for nitrogen using the Kjeldahl method. After digestion, the distilled ammonia was collected in 100 mL of 0.1334 M boric acid. This solution required 29.38 mL of 0.202 M HCl for titration to the methyl red end point. Calculate the % N (AW =14 g/mol) in the fertilizer. Type the numerical answer only.

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