وامت أول1) 25 mL Ag No3 react with 5mM Nacli 35 mlof(AgNo3 ) silver Selution is required to titrateSample o Zn Clz. How many millimole oZnClz are present inthe Sample:CSO) that

Answered: Image /qna-images/answer/a7d90663-3ec5-4a0a-aba6-b92f981b6880.jpg

Answered: وامت اول 1) 25 mL Ag Nos reacd with 5mM…

وامت اول 1) 25 mL Ag Nos reacd with 5mM Nacls 35 ml of (AgNo3 ) silver Selution is required to titrate Sample os Zn Clz. How many millimoleo ZnClz are present inthe Sample: (SO) that

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter30: Determination Of Iron By Reaction With Permanganate-a Redox Titration

Section: Chapter Questions

Problem 3ASA

See similar textbooks

Similar questions

68. Aluminum ion may be precipitated from aqueous solution by addition of hydroxide ion, forming Al(OH)3. A large excess of hydroxide ion must not be added, however, because the precipitate of Al(OH)3 will redissolve as a soluble compound containing aluminum ions and hydroxide ions begins to form. How many grains of solid NaOH should be added to 10.0 mL of 0.250 M A1Cl3 to just precipitate all the aluminum?
A solution contains 1.0102 mol of Kl and 0.10 mol of KCl per liter. AgNO3 is gradually added to this solution. Which forms first, solid AgI or solid AgCl?
A solution contains 1.0105 mol of KBr and 0.10 mol of KCl per liter. AgNO3 is gradually added to this solution. Which forms first, solid AgBr or solid AgCl?
Both AgCl and Agl dissolve in NH3.. (a) What mass of AgI dissolves in 1.0 L of 1.0 M NH3?. (b) VNhat mass of AgCl dissolves in 1.0 L of 1.0 M NH3?
The equilibrium constant for the reaction Hg2+(aq)+2Cl(aq)HgCl2(aq) is 1.61013, Is HgCl2 a strong electrolyte or a weak electrolyte? Mm are the concentrations of Hg2+ and Cl- in a 0.015-M solution of HgCl2?
An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker at various times during the titration. These are presented out of order. Note: Counter-ions and water molecules have been omitted from the illustrations for clarity. (a) (b) (c) (d) (e) a. Is the acid a weak or strong acid? How can you tell? b. Arrange the beakers in order of what the contents would look like as the titration progresses. c. For which beaker would pH = pKa? Explain your answer. d. Which beaker represents the equivalence point of the titration? Explain your answer. e. For which beaker would the Ka value for the acid not be necessary to determine the pH? Explain your answer.
Gold metal will not dissolve in either concentrated nitric acid or concentrated hydrochloric acid It will dissolve, however, in aqua regia, a mixture of the two concentrated acids. The products of the reaction are the AuCl4 ion and gaseous NO. Write a balanced equation for the dissolution of gold in aqua regia.
Suggest a method for separating a precipitate consisting of a mixture of solid CuS and solid Cu(OH)2.
In a titration of cyanide ion, 28.72 mL of 0.0100 M AgNO3 is added before precipitation begins. [The reaction of Ag+ with CN- goes to completion, producing the Ag(CN)2- complex. Precipitation of solid AgCN takes place when excess Ag+ is added to the solution, above the amount needed to complete the formation of Ag(CN)2-. How many grams of NaCN were in the original sample?
Perform these calculations for nickel(II) carbonate. (a) With what volume of water must a precipitate containing NiCO3 be washed to dissolve 0.100 g of this compound? Assume that the wash water becomes saturated with NiCO3(Ksp=1.36107). (b) If the NiCO3 were a contaminant in a sample of COCO3(Ksp=1.01012), what mass of COCO3 would have been lost? Keep in mind that both NiCO3 and COCO3 dissolve in the same solution.
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
Twenty-five milliliters of a solution (d=1.107g/mL)containing 15.25% by mass of sulfuric acid is added to 50.0 mL of 2.45 M barium chloride. (a) What is the expected precipitate? (b) How many grams of precipitate are obtained? (c) What is the chloride concentration after precipitation is complete?