A silver-30%gold alloy sample (cylindrical with 1 cm diameter and 0.3 cm height) is subjected to a selective silver dissolution in 0.1 M HNO3 at current density of 2.5 mA/cm2 . How long will it take until the total amount of silver is dissolved? Assume in average a density of 12 g/cm3 for the alloy sample.

A silver-30%gold alloy sample (cylindrical with 1 cm diameter and 0.3 cm height) is subjected to a selective silver dissolution in 0.1 M HNO3 at current density of 2.5 mA/cm2 . How long will it take until the total amount of silver is dissolved? Assume in average a density of 12 g/cm3 for the alloy sample.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 94AP

See similar textbooks

Similar questions

What is precipitation from homogeneous solution; what are the benefits of this method.
The Ksp of Cu3 (PO4), is 1.00 × 10-37. Estimate the solubility of this salt in units of g. L-1. You must show any reaction equation(s) that you may think are necessary. If a sample of solid Cu3 (PO4)2 is stirred into exactly one litre of a 0.550M solution of K3PO4 , how will the solubility of the salt compare with the answer that you have obtained in question 2.1? Explain you answer in a short sentence.
In an experiment to determine the concentration of H2SO4 in a brand of toilet cleanser, 10.0 cm3 of the cleanser was first diluted to 250.0 cm3 with distilled water. 25.0 cm3 of the diluted cleanser were titrated with 0.320 mol dm–3 NaOH solution, using methyl orange as indicator.If 29.2 cm3 of NaOH solution is used, what is the concentration of H2SO4 in the undiluted toilet cleanser?a. 2.30 mol dm–3b. 4.60 mol dm–3 c. 9.20 mol dm–3 d. 11.50 mol dm–3
The mineral pyrite, FeS2(s), can incorporate large amounts of arsenic. The dissolution of arsenic-rich pyrite can therefore release arsenic into groundwater (i.e., pyrite dissolution can be written as FeS2(s) = Fe2+ + S22-). What equation would you use to calculate whether pyrite in an aquifer will dissolve or precipitate?
Hydroxyapatite, Ca,(PO,),(OH),, has a solubility constant of Ksp = 2.34 × 10-59, and dissociates according to Ca10 (PO,),(OH),(s) = 10 Ca²+(aq) + 6 PO (aq) + 2 OH¯(aq) Solid hydroxyapatite is dissolved in water to form a saturated solution. What is the concentration of Ca2+ in this solution if [OH-]is fixed at 5.30 x 10-4 M? [Ca²*] = M
4. An experiment similar to the one described in this module was performed to determine the solubility and solubility product constant of lead(1l) chloride (gmm = 278.10). The equilibrium involved is PbCl2(s) = Pb2+ (aq) +2 CI¯(aq) The dissolved chloride in the filtered solution was quantitatively precipitated as AgCl by the addition of excess AgNO3 solution. The solid AgCI was filtered from solution, dried, and weighed. The following data were obtained for three samples of the filtered, saturated solution. determination 1 2 temperature of solution, °C volume of PbCl2 solution analyzed, mL mass of dry A£CI, g 20.2 20.4 20.1 25.00 22.00 20.10 0.2543 0.2276 0.2051 Calculate the following: number of moles of: AgCl(s) CI- (aq) Pb2*(aq) [CI"] in PbCl2 solution, M [Pb2+] in PbCl, solution, M Ksp average Ksp solubility of PbCl2, in g per 100 mL chemistry handbook value for solubility at 20°, g per 100 mL
Question 5 of 6 Construct the expression for Ksp for solid ZNCO, in aqueous solution. ZnCO,(s) = Zn²"(aq) + CO,²(aq) Based on your knowledge of how the solid will dissociate in aqueous solution, use the tiles to form the expression. Ksp [Zn'] [CO,F 5 RESET [ZNCO] 2[ZnCO] [ZnCOj [Zn] 2[Zn'] [ZnP [Zn] 2[Zn*] [Zn*p [CO,] 2[CO,] [Co,r [CO] 2[CO,P]
The concentration of ammonia in a cleaning product was determined by back titration.Firstly, 10.00 cm3 of the cleaning product was pipetted into a large conical flask,containing 250.00cm3 of 0.50 mol/l HCl to give Solution A.Following a period of reaction and shaking, 50.00cm3 of Solution A was removed anddiluted to 250 cm3 with water in a volumetric flask to give Solution B.20 cm3 samples of Solution B were titrated against 0.05 mol/l Na2CO3 solution, givingan average titre of 12.45 cm3. i) Write equations for the reactions that have taken place.ii) Determine the concentration of NH3 in the original cleaning product in mol/l,g/l, ppm, and % w/v.
(b) Suppose the laboratory Technician carried out the same titration experiment in which he/she recorded an average volume of 20 cm³ of the dilute hydrochloric acid (HC) by titrating with 0.05 mol dm³ and 25 cm³ of potassium hydroxide (KOH). Calculate the concentration of hydrochloric acid from the Technician's experiment.
The chloride in the sample is to be determined gravimetrically by precipitating and weighing AgCl. What weight in grams of sample should be taken so that the percentage of Cl is obtained by simply multiplying the weight of the AgCl precipitate by 10?
1. A 0.3516 g sample of commercial phosphate detergent was ignited at a heat to destroy the organic matter. The residue was taken up in hot HCI which converted P to H3PO4. The phosphate was precipitated as MGNH4PO4.6H2O by addition of Mg+ followed by aqueous NH3. After being filtered and washed, the precipitate was converted to Mg2P2O7 by ignition at 1000 OC. This residue weighed 0.2161 g. Calculate the percent P (30.974) in the sample? Ans 17.11%
In a lab, you diluted a sample of bleach to 1/10 concentration in a 250 vol. flask. Then quantitatively transferred into into a beaker and titrated it with a standard sodium thiosulfate solution with a molarity of 0.1215M. You repeated this 3 times. The data below is the amount of sodium thiosulfate that was titrated in the 3 runs. Calculate the molarity in each run of the diluted bleach and the concentration of undiluted bleach sample.