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Concept explainers
(a)
Interpretation:
The reason as to why it is important to specify an identity of the anion in the given case even though it is a spectator ion.
Concept introduction:
Ionic strength of a solution is calculated by adding the concentration of each ion present in the solution after multiplying it by their corresponding charges. The ionic strength of the solution is represented as,
Where,
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(b)
Interpretation:
The expected voltage for the given
Concept introduction:
Activity coefficient depends upon the charge and size of the ion, and on the properties of the solvent. Debye-Huckel limiting law, describes the relation between the ionic strength and activity coefficient of a dilute solution.
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Chapter 8 Solutions
Physical Chemistry
- Write an equation to show that hydrochloric acid , HCl , behaves as an acid in water. Write an equation to show that hypochlorous acid , HClO , behaves as an acid in water. Write a net ionic equation to show that phosphoric acid, H3PO4, behaves as an acid in water. Consider only its first ionization.arrow_forwardAs shown in the following Figure, an aqueous solution of Nal is poured into an aqueous solution of Pb(NO3)2 which results in the formation of a yellow precipitate. Assuming stoichiometric amounts of Nal and Pb(NO3)2 are reacted, give the chemical formula of the yellow precipitate and the chemical formula of all molecules and/or ions that are present in the solution (You may use the solubility matrix to answer this question). (b)arrow_forwardWhen an aqueous solution of nickel(II) bromide, NiBr2, is added to an aqueous solution of potassium sulfide, K2S, a precipitate of nickel(II) sulfide, NiS, forms. Write a balanced net ionic equation for this reaction.arrow_forward
- Hard water contains magnesium and calcium ions 1Mg2+, Ca2+2, which can precipitate out in hot water pipes and water heaters as carbonates. Write the net ionic equation for this reaction.arrow_forwarda) What mass of strontium nitrate (Sr(NO3)2) would be required to prepare 2.000 L of a 0.0180 M aqueous solution of this salt? (b) Calculate the mass percent of Sr(NO3)2 in this solution, assuming the density of the solution is 1.000 kg/L. c.) A 15.0 g sample of anhydrous sodium sulfate, Na2SO4, is dissolved in 4.83 L of water. The molar mass of sodium sulfate is 142.1 g/mol. Use the equation given to calculate the molality (m) of the solution, in mol/kg.For this situation, assume the density of water is 1.00 g/mL.arrow_forwardSuppose that 40.0 mL of 0.100 M NaOH(aq) is added to 10.0 mL of 0.200 M Cu(NO3)2(aq). (a) Write the chemical equation for the precipitation reaction, the complete ionic equation, and the net ionic equation. (b) What is the concentration of Nations (in moles per liter) in the final solution?arrow_forward
- For each of the following reactions, suggest two soluble ionic compounds that, when mixed together in water, result in the net ionic equation given: (a) 2 Ag+ (aq) + CO3²¯ (aq) → Ag₂CO3(s) (b) Mg²+ (aq) + 2 OH¯(aq) → Mg(OH)₂(s), the suspension present in milk of magnesia 3+ (c) 3 Ca³+ (aq) + 2 PO2 (aq) → Ca3(PO4)2(s), gypsum, a component of concretearrow_forwardWrite the formula for the dissolution of ammonium fluoride in water. How many TOTAL ions (ammonium cations + fluoride anions) would be produced as aqueous species in the water solvent if four molecules of ammonium fluoride dissolved?arrow_forward13.) Calculate the mass of solid MgSO̟•7H,O that must be added to precipitate out all of the PO,3- ions in the form of MgNH¸PO¸ •6H,O from 10.0 mL of a 2.0 M solution of PO,³ (aq)?arrow_forward
- (a) When acetone dissolves in water, what major species are present? Write structures, cations or anions separated by comma. (b) When potassium bromide dissolves in water, what major species are present? Write structures, cations or anions separated by comma. (c) When lithium hydroxide dissolves in water, what major species are present? Write structures, cations or anions separated by comma. (d) When sulphuric acid dissolves in water, what major species are present? Write structures, cations or anions separated by comma.arrow_forwardMuch of the sulfur used in the United States comes from the hydrogen sulfide contaminant that makes "sour" natural gas smell bad. Hydrogen sulfide is separated from the other components of natural gas mostly by taking advantage of its acid-base reaction with aqueous ethanolamine: HO(CH,),NH,(aq)+H,S(g) → HO(CH,),NH,(aq)+HS (aq) Suppose an engineer decides to study the rate of this reaction. She prepares four reaction vessels with 167.6 mL of ethanolamine solution and 20.9 g of hydrogen sulfide gas each. The volume and temperature of each vessel is shown in the table below. Arrange the reaction vessels in decreasing order of initial rate of reaction. In other words, select a "1" next to the vessel in which the engineer can reasonably expect the initial rate of reaction to be highest, a "2" next to the vessel in which the initial rate of reaction would be next highest, and so on. vessel volume temperature A B C D 5.0 L 5.0 L 5.0 L 5.0 L 49, °C 48. °C 51. °C 50. °C X initial rate of…arrow_forwardMuch of the sulfur used in the United States comes from the hydrogen sulfide contaminant that makes "sour" natural gas smell bad. Hydrogen sulfide is separated from the other components of natural gas mostly by taking advantage of its acid-base reaction with aqueous ethanolamine: HO(CH,), NH, (aq)+H,S(g) → HO(CH,),NH, (aq)+HS (aq) Suppose an engineer decides to study the rate of this reaction. She prepares four reaction vessels with 128.7 mL of ethanolamine solution and 10.1 g of hydrogen sulfide gas each. The volume and temperature of each vessel is shown in the table below. alo Arrange the reaction vessels in decreasing order of initial rate of reaction. In other words, select a "1" next to the vessel in which the engineer can reasonably expect the initial rate of reaction to be highest, a "2" next to the vessel in which the initial rate of reaction would be next highest, and so on. 18 Ar initial rate of vessel volume temperature reaction A 5.0 L 37. °С ? В 5.0 L 36. °C ? C 5.0 L 39.…arrow_forward
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
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