What is the net ionic reaction for the following aq solutions mixed together? Sr(OH)2 (aq) + Al2(SO4)3 (aq). CATIONS High Solubility (aq) Low Solubility (s) Cl, Br, I Halides Most Ag+, Pb²+, Tl, Hg₂+, Hg, Cu Sr** (aq) + SO4² (aq) no reaction 3Sr++ (aq) + 35042 (aq) 52. none of these are correct +++ 2AI***+ (aq) + 60H' (aq) 2A/+++ (aq) + 3SO² (aq) Solubility Table Group 1, NH₁", Group 2 Most SrSO4(s) ANIONS OH Group 1, NHƯ, Sri Ba2+, Tl. Most 2Al(OH)3 (s) 3SrSO4 (s) SO4²- Most All Group 1 compounds, including acids, and all ammonium compounds are assumed to have high solubility in water. Ag, Pb², Ca²+, Ba²+, Sr2+, Ra² CO₂², PO4³¹, SO₂² Al₂(SO4)3 (s) 3Sr++ (aq) + 60H (aq) + 2A1+3 (aq) + 3SO4² (aq) (s) Group 1, NH4* C₂H30₂ NO3 Most All Most Ag+ None 2Al(OH)3 (s) + 3SrSO4

What is the net ionic reaction for the following aq solutions mixed together? Sr(OH)2 (aq) + Al2(SO4)3 (aq). CATIONS High Solubility (aq) Low Solubility (s) Cl, Br, I Halides Most Ag+, Pb²+, Tl, Hg₂+, Hg, Cu Sr (aq) + SO4² (aq) no reaction 3Sr++ (aq) + 35042 (aq) 52. none of these are correct +++ 2AI+ (aq) + 60H' (aq) 2A/+++ (aq) + 3SO² (aq) Solubility Table Group 1, NH₁", Group 2 Most SrSO4(s) ANIONS OH Group 1, NHƯ, Sri Ba2+, Tl. Most 2Al(OH)3 (s) 3SrSO4 (s) SO4²- Most All Group 1 compounds, including acids, and all ammonium compounds are assumed to have high solubility in water. Ag, Pb², Ca²+, Ba²+, Sr2+, Ra² CO₂², PO4³¹, SO₂² Al₂(SO4)3 (s) 3Sr++ (aq) + 60H (aq) + 2A1+3 (aq) + 3SO4² (aq) (s) Group 1, NH4 C₂H30₂ NO3 Most All Most Ag+ None 2Al(OH)3 (s) + 3SrSO4

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.25PAE

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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?
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?
Use the appropriate tables to calculate H for (a) the reaction between MgC03(s) and a strong acid to give Mg2+(aq), CO2(g), and water. (b) the precipitation of iron(III) hydroxide from the reaction between iron(III) and hydroxide ions.
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)
Which of the following ions could be used to separate Cl(aq) from SO4² (aq) by precipitating one of them? Solubility Table CATIONS Ag+ Pb2+ High Solubility (aq) Low Solubility (s) OCa²+ Be2+ NH4* Cl, Br, I Halides Most Ag+, Pb²+, Tl+, Hg₂²+, Hg, Cu 52- Group 1, NHÃ, Group 2 Most ANIONS OH- Group 1, NH4*, Sr²*, Ba²+, Tl Most SO4²- Most Ag+, Pb²+, Ca²+, Ba²+, Sr²., Ra². All Group 1 compounds, including acids, and all ammonium compounds are assumed to have high solubility in water. CO3²-, C₂H30₂ NO3 PO4³-, SO3². Group 1, Most All NH4* Most Ag+ None
2. Each of the following salts can be prepared from an acid and a base. Write the balanced molecular equation and the net ionic equation for the preparation of each. Indicate states of the reactants and products [(aq), (s), (1)]. Review solubility rules if necessary to determine the solubility of the reactants. (c) Al(NO3)3 (aq) (a) BaCl₂ (aq) (b) CsCH3CO₂ (aq)
Consider the following reactions: (i) HX(aq) + MOH(aq) --> H2O(l) + MX(aq) (ii) 2M(s) + F2(g) --> 2MF(s) (iii) MNO3(aq) + XCl(aq) --> XCl(s) + MNO3(aq) These reactions are examples of: (i) acid-base, (ii) precipitation, and (iii) precipitation, respectively (i) acid-base, (ii) redox, and (iii) precipitation, respectively none of the other options accurately describe the reactions all redox reactions all precipitation reactions
Vrite the dissociation reactions for KI(aq) in water and for (NH4)2S2O8 (aq) in wate
MnO4 (aq) + H2O2 (aq) → Mn2+ (aq) + O2 (g) (a) Sketch a flask containing an analyte solution before any potassium permanganate KMnO4 is added, list out all species present. (b) Once a stoichiometric amount of permanganate ion is added to the analyte solution (the equivalence point of the titration!), sketch the beaker with all the species remaining after the reaction goes to completion. (c) Sketch the flask one more time, past the equivalence point. How do you know when you have passed the equivalence point?
Ag+ (aq) + NH3(aq) Ag(NH3)*(aq) Ag(NH3)* (aq) + NH3(aq) → Ag(NH3)2* (aq) Equal volumes of 0.1 MAgNO3(aq) and 2.0 MNH3(aq) are mixed and the reactions represented above occur. Which Ag species will have the highest concentration in the equilibrium system shown below, and why? Ag+ (aq) + 2 NH3(aq) ⇒ Ag(NH3)2* (aq) Keqs =? (A) (B) C (D) Ag+ (aq), because Keq3 = 4 Ag+ (aq), because Keq1 < Keq2 Ag(NH3)2(aq), because Keq3 = 1.7 x 107 Keq, = 2.1 × 10³ = 8.2 x 10³ Keq2 Ag(NH3)2(aq), because Keq1 < Keq2
A solution contains 0.0150 M Pb2+(aq) and 0.0150 M Sr²+(aq). If you add SO2 -(aq), what will be the concentration of Pb2+(aq) when SrSO4(s) begins to precipitate?
Some sulfuric acid is spilled on a lab bench. You can neutralizethe acid by sprinkling sodium bicarbonate on it and thenmopping up the resulting solution. The sodium bicarbonatereacts with sulfuric acid according to:2 NaHCO3(s) + H2SO4(aq)----->Na2SO4(aq) + 2 H2O(l)+ 2 CO2(g)Sodium bicarbonate is added until the fizzing due to the formationof CO2(g) stops. If 27 mL of 6.0 M H2SO4 was spilled,what is the minimum mass of NaHCO3 that must be addedto the spill to neutralize the acid?

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