A solution of ZnCl was prepared and added to a well on a 24-well plastic plate. A piece of metal was added to the solution. The ZnCl solution reacted with the piece of metal that was added to the solution. What could the metal be? O AI O Zn Sn O Cu O Not enough information

A solution of ZnCl was prepared and added to a well on a 24-well plastic plate. A piece of metal was added to the solution. The ZnCl solution reacted with the piece of metal that was added to the solution. What could the metal be? O AI O Zn Sn O Cu O Not enough information

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 3ALQ

See similar textbooks

Similar questions

The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing small water-soluble ions and molecules. The iron in the aqueous solution is reduced to iron(II) ion and then titrated against potassium permanganate. In the titration, iron(ll) is oxidized to iron(III) and permanganate is reduced to manganese(II) ion. A 5.00-g sample of hemoglobin requires 32.3 mL of a 0.002100 M solution of potassium permanganate. The reaction with permanganate ion is MnO4(aq)+8H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+(aq)+4H2O What is the mass percent of iron in hemoglobin?
Balance the following equations. (a) Zn(s) + VO2+(aq) Zn2+(aq) + V3+(aq)(acid solution) (b) Zn(s) + VO3(aq) V2+(aq) + Zn2+(aq)(acid solution) (c) Zn(s) + ClO(aq) Zn(OH)2(s) + Cl(aq)(basic solution) (d) ClO(aq) + [Cr(OH)4](aq) Cl(aq) + Cr2O42(aq)(basic solution)
Nickel(II) formate [Ni(HCO2)2] is widely used as a catalyst precursor and to make metallic nickel. It can be prepared in the general chemistry laboratory by treating nickel(II) acetate with formic acid (HCO2H). Ni(CH3CO2)2(aq) + 2 HCO2H(aq) Ni(HCO2)2(aq) + 2 CH3CO2H(aq) Green crystalline Ni(HCO2)2 is precipitated after adding ethanol to the solution. (a) What is the theoretical yield of nickel(II) formate from 0.500 g of nickel(II) acetate and excess formic acid? (b) Is nickel(II) formate paramagnetic or diamagnetic? If it is paramagnetic, how many unpaired electrons would you expect? (c) If nickel(II) formate is heated to 300 C in the absence of air for 30 minutes, the salt decomposes to form pure nickel powder. What mass of nickel powder should be produced by heating 253 mg of nickel(II) formate? Are nickel atoms paramagnetic?
Is prepared by dissolving a definite weight of a substance in a definite volume. a. primary standard b. secondary standard c. standard addition d. standard sample e. standard solution
In a oxidation reduction titration, during the analysis of an unknown oxalate, how would the calculated percent oxalate of the unknown be affected? 1. The unknown solid sodium oxalate was dissolved in 75 mL of water rather than the 100 mL of water. 2. A few drop of KMnO4 titrant missed the reaction flask containing the unknown sodium oxalate 3. When weighing out the solid unknown sodium oxalate, the actual mass is 0.758 grams. However, the mass is mistakenly recorded in the lab notebook as 0.785 grams.
To remove the tarnish (Ag2S) on a silver spoon the following steps are carried out. the spoon is placed in a large pan filled with water so the spoon was totally immersed. A few tablespoonfuls of baking soda (sodium bicarbonate), which readily dissolves. Is added. Some aluminum foil is placed at the bottom of the pan in contact with the spoon and then heated the solution to about 80° After a few minutes, the spoon is removed and rinsed with cold water. The tarnish is gone and the spoon regains its original shiny appearance. Describe with equations the electrochemical basis for the procedure. Adding NaCl instead of NaHCO3 would also work because both compounds arestrong electrolytes. What is the added advantage of using NaHCO3? (Hint: Consider the pH of the solution.) What is the purpose of heating the solution? Some commercial tarnish removers containing a fluid (or paste) that is a dilute HCl solution. Rubbing the spoon with the fluid will also remove the tarnish. Name two…
A 11.00 gram sample of Vodka was analysed for its alcohol content. The sample was placed in a300 mL volumetric flask and made to the mark with distilled water. A 20.0 mL aliquot of the dilutedVodka was taken from the volumetric flask and placed in a conical flask containing some distilled water from a previous washing.The 20.0 mL aliquots were titrated against a 0.1302 M Cr2O72-solution and an average titre of13.25 mL was obtained.The reaction between the alcohol and the dichromate solution is given below2Cr2O72–(aq) + 3CH3CH2OH(aq) + 16H+(aq)  4Cr3+(aq) + 3CH3COOH(aq) + 11H2O(l)a) Calculate the amount in mol of Cr2O72– in the average titre. b) Calculate the percentage, by mass, of ethanol in the vodka.
H8. A student performed titration of an unknown reducing substance (molar mass 200. g/mol) in a sample using potassium permanganate solution as titrant. The concentration of potassium permanganate solution is 0.1900 M. The volume of sample solution is 25.00 mL. The density of this sample solution is 1.091 g/mL. The concentration of sample solution (m/m%) is 4.67%. The titration consumed 6.02 mL of potassium permanganate solution to reach the endpoint (light pink). Determine the mole ratio between permanganate and the unknown substance in the sample (molKMnO4 / molunknown)
One method for removal of metal ions from a solution is to convert the metal to its elemental form so it can be filtered out as a solid. Which metal can be used to remove aluminum ions from solution? Group of answer choices cobalt copper lead zinc none of these
A titration was conducted to determine the concentration of a potassium permanganate (KMnO4) solution. Three trials were used. KMnO4 (which has a purple color) was placed into a buret. The KMnO4 solution was slowly titrated into an Erlenmeyer flask containing 20.00 mL of an acidified solution of 1.000 M Fe(NO3)2 (which is colorless). The unbalanced chemical reaction that takes place when permanganate mixes with iron (II) under acidic conditions is shown below. MnO4- + Fe2+ ⟶⟶ Mn2+ + Fe3+ At the end point of this titration, permanganate will have mixed with iron (II) in the correct stoichiometric amount (according to the balanced equation) to produce manganese (II) and iron (III) which are both colorless. Trial #1 required 23.86 mL of potassium permanganate to reach the end point. Calculate the [KMnO4] in moles/liter. Trial #2 required 23.48 mL of potassium permanganate to reach the end point. Calculate the [KMnO4] in moles/liter. Trial #3 required 23.92 mL of…
Which zinc solution is saturated? 1x10-5 M ZnCO3 (Ksp=1.0x10-10) 4.0x10-6M Zn(OH)2 (Ksp=3.0x10-16) 1.5x10-4M ZnC2O4 (Ksp=2.7x10-8) 4.0x10-13 M ZnS (Ksp=2x10-25)
Ores are analyzed by dissolving some of the ore and then performing an analysis of a metal (expressed in grams); usually the concentration of the metal is expressed as % of the amount of the ore (in grams) dissolved. An ore containing Sn was dissolved and then titrated with MnO4-. When 14.1960 g was dissolved and titrated with 0.1535 M MnO4- the titration required 35.32 mL to reach the endpoint. What was the % Sn in the ore?5Sn2+(aq) + 2MnO4-(aq) + 16H+(aq) ↔ 5Sn4+(aq) + 2Mn2+(aq) + 8H2O(l) 18.14%