b) Water "softeners" work via the principle of ion-exchange. The tank of a water softener is filled with a soluble salt such as sodium chloride. As "hard" water passes through the tank, the undesirable ions in hard water (e.g., calcium, magnesium, and iron III) are exchanged for the more desirable "soft" (meaning more soluble) ions like sodium. Explain how swapping the "soft"-water sodium ions for "hard"-water ions would influence the behavior (the cleaning effectiveness) of soaps and detergents.

b) Water "softeners" work via the principle of ion-exchange. The tank of a water softener is filled with a soluble salt such as sodium chloride. As "hard" water passes through the tank, the undesirable ions in hard water (e.g., calcium, magnesium, and iron III) are exchanged for the more desirable "soft" (meaning more soluble) ions like sodium. Explain how swapping the "soft"-water sodium ions for "hard"-water ions would influence the behavior (the cleaning effectiveness) of soaps and detergents.

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter16: Solutions

Section: Chapter Questions

Problem 37E

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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?
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 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?
On the basis of the general solubility rules given in Table 7.1, predict which of the following substances are not likely to be soluble in water. Indicate which specific rule(s) led to your conclusion. :math>PbSe. BaCO3 :math>Mg(OH)2f. AlPO4 :math>Na2SO4g. PbCl2 :math>(NH4)2Sh. CaSO4
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?
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?
A sample of solid calcium hydroxide, Ca(OH)2, is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00102M HCl requires 36.6 mL of the acid to reach the end point. Ca(OH)2(aq)+2HCl(aq)CaCl2(aq)+2H2O(l) What is the molarity?
On the basis of the general solubility rules given in Table 7.1, predict which of the following substances are likely to be appreciably soluble in water. Indicate which specific rule(s) led to your conclusion. :math>Ba(NO3)2e. KCl :math>K2SO4f. Hg2Cl2 :math>PbSO4g. (NH4)2CO3 :math>Cu(OH)2h. Cr2S3
Relative solubilities of salts in liquid ammonia can differsignificantly from those in water. Thus, silver bromide issoluble in ammonia, but barium bromide is not (thereverse of the situation in water). Write a balanced equation for the reaction of anammonia solution of barium nitrate with an ammoniasolution of silver bromide. Silver nitrate is soluble inliquid ammonia. What volume of a 0.50 M solution of silver bromidewill react completely with 0.215 L of a 0.076 M solutionof barium nitrate in ammonia? What mass of barium bromide will precipitate fromthe reaction in part (b)?
A student tries to determine experimentally the molar mass of aspirin (HAsp). She takes 1.00 g of aspirin, dissolves it in water, and neutralizes it with 17.6 mL of 0.315 M KOH. The equation for the reaction is HAsp(aq)+OH(aq)Asp(aq)+H2OWhat is the molar mass of aspirin?
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?
A 0.5504-g sample of KHP (potassium hydrogen phthalate, KHC8H4O4; molar mass = 204.22 g/mol) is completely dissolved in enough deionized water to make 50.00 mL of solution. The resulting solution is titrated with a NaOH solution of unknown concentration. If 21.50 mL of the base solution is needed to reach the end-point, what is the molar concentration of NaOH solution? The reaction occurs as follows: NaOH(aq) + KHC8H4O4(aq) --> NaKC8H4O4(aq) + H2O(l) (A) 0.2457 M (B) 0.1254 M (C) 0.05390 M (D) 0.03823 M

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