Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. solution A iron(II) chloride barium nitrate iron(III) bromide solution B cadmium acetate potassium chloride potassium hydroxide Does a precipitate form when A and B are mixed? yes O no O yes O yes O no O no empirical formula of precipitate 0 0 0 X 00

Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. solution A iron(II) chloride barium nitrate iron(III) bromide solution B cadmium acetate potassium chloride potassium hydroxide Does a precipitate form when A and B are mixed? yes O no O yes O yes O no O no empirical formula of precipitate 0 0 0 X 00

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 76QAP

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Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the formula KHC8H4O4. This is often written in the short-hand notation as KHP. If 25.0mL of a potassium hydroxide solution are needed to neutralize 2.26g of KHP, what is the molarity of the potassium hydroxide solution? Potassium hydrogen phthalate sometimes called potassium biphthalate, as shown on this bottle is an acid that is convenient to store and use because it is a solid.
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
The equation for a reaction by which a solution of sodium carbonate may be standardized is 2HC7H5O2+Na2CO32NaC7H5O2+H2O+CO2. A student determines that 5.038g of HC7H5O2 uses 51.89mL of sodium carbonate solution in the titration. Find the molarity of the sodium carbonate.
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)
A solution contains 0.00740 M calcium ion. A concentrated sodium fluoride solution is added dropwise to precipitate calcium fluoride (assume no volume change). a At what concentration of F does precipitate start to form? b When [F] = 9.5 104 M, what is the calcium-ion concentration? What percentage of the calcium ion has precipitated?
Solubility and Solubility Product You put 0.10-mol samples of KNO3, (NH4)2S, K2S, MnS, AgCl, and BaSO4 into separate flasks and add 1.0 L of water to each one. Then you stir the solutions for 5 minutes at room temperature. Assume that you have 1.0 L of solution in each case. a Are there any beakers where you would observe solid still present? How do you know? b Can you calculate the potassium ion concentration, K+, for the solutions of KNO3 and K2S? If so, do the calculations, and then compare these K+ concentrations. c For the solutions of (NH4)2S, K2S, and MnS, how do the concentrations of sulfide ion, S2, compare? (You dont need to calculate an answer at this point; just provide a rough comparison.) Be sure to justify your answer. d Are there any cases where you need more information to calculate the sulfide-ion concentration for the solutions of (NH4)2S, K2S, and MnS from part c? If so, what additional information do you need? e Consider all of the solutions listed at the beginning of this problem. For which ones do you need more information than is given in the question to determine the concentrations of the ions present? Where can you find this information? f How is the solubility of an ionic compound related to the concentrations of the ions of the dissolved compound in solution?
In the chapter discussion of precipitate formation, we ran the precipitation reaction to completion and then let some of the precipitate redissolve to get back to equilibrium. To see why, redo Example 15-6, where Initial Cocentration (mol/L) Equilibrium Concentration (mol)/L [Mg2+]0 = 3.75 103 [F]0 = 6.25 102 reactstoformMgF2ymol/Mg2+ [Mg2+] = 3.75 103 y [F] = 6.25 102 2y
Recommend a specific cation for the quantitative precipitation of carbonate ion andjustify your recommendations.
app.101edu.co Question 16 of 25 A 185.0 mL sample of 1.200 M Pb(NO3), is mixed with 139.50 mL of 1.500 M NaCl, and the PbCl, precipitate is filtered from the solution. Then 200.0 mL of 3.000 M NaBr is added to the remaining solution, and the PbBr2 precipitate is also collected and dried. What is the mass (in grams) of the PbBr2 precipitate, assuming the yield in each precipitation step is 100%? 1 3 6. 8. 6. +/- 2. LO
A series of sulfate samples is to be analyzed by precipitationas BaSO4. If it is known that the sulfate contentin these samples ranges between 20% and 55%, whatminimum sample mass should be taken to ensure thata precipitate mass no smaller than 0.200 g is produced?What is the maximum precipitate mass to be expectedif this quantity of sample is taken?
The corect solubility product expression for A(SO,), is: A) K = (x) (2x) D) K, = (2x) (x) B)K, = (4x)(2x)? E) K, = (x) (2x) C) K, = (x)² (2x) F) K, = 2x %3D %3D O A O E O F B O D
A chemist wishes to precipitate yttrium cations out of a 1.00 L solution. if the concentration of (in solution is 0.428 M and the K of yttrium iodate is 1.12 x 10, what mass of potassium lodate (00 must be added so that precipitation may begin? The molar mass of potassium lodate is 21A.00 g/mol. (27) (A) (B) (C) (D) 91.6g 64.0 ug (6.4 x 10* g) 411 mg 56.0 ng 137 mg (5.6 x 10* g) (E)

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