CaC2O4 (Ksp = 4.0 x 10‒9) is suspended in water. Which will increase the [C2O42‒] in solution? choose one: Addition of NaOH(aq) Addition of EDTA4‒(aq) Addition of Ca2+(aq)
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CaC2O4 (Ksp = 4.0 x 10‒9) is suspended in water. Which will increase the [C2O42‒] in solution?
choose one:
Addition of NaOH(aq)
Addition of EDTA4‒(aq)
Addition of Ca2+(aq)
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- The grid has six lettered boxes, each of which contains an item that may be used to answer the questions that follow. Items may be used more than once and there may be more than one correct item in response to a question. Place the letter(s) of the correct selection(s) on the appropriate line. Could dissolve Zn(OH)2 _____________ Could be used to prepare a buffer from __________ Halfway to the equivalence point in the titration of a weak, monoprotic acid with strong base ________ SO2-related atmospheric phenomenon __________ Species formed by a Lewis acid-base reaction ________ General condition required for precipitation to occur ________ [conj. base] = [conj. acid] in a buffer ___________Suppose the Kc value for Cobalt (II) hexahydrate is 6.80 and suppose upon heating the solution turned pink. If a group of student started mixed 10.5 mL of a 1.25 M [Co(H2O)6]2+(aq) solution with 12.5 mL of a 1.55 M solution of NaCl(aq) with 15.25 mL of a 1.39 M [CoCl4]-2(aq) solution then what color is the solution at equilibrium? [Co(H2O)6]2+(aq) + 4 Cl-(aq) [CoCl4]-2(aq) + 6 H2O(L) Multiple choices pink purple green black orange brown blue colorless yellow gray red greenIdentify the driving force for the chemical reaction: Pb(NO3)2(ag) + 2NAOH (ag) + Pb(OH)2(s) + 2NANO3(aq) Formation of a precipitate. Formation of a water neutralization of an acid and base reduction and oxidation. O There is no driving force.
- Suppose the Kc value for Cobalt (II) hexahydrate is 6.80 and suppose upon heating the solution turned pink. If a group of student started mixed 10.5 mL of a 1.25 M [Co(H2O)6]2+(aq) solution with 12.5 mL of a 1.55 M solution of NaCl(aq) with 15.25 mL of a 1.39 M [CoCl4]-2(aq) solution then what is the value of the ion product (Qc)? Hint: first determine the number of moles of each ion and then divide by the total volume of the solution to get new Molarity when mixing solutions. [Co(H2O)6]2+(aq) + 4 Cl-(aq) ↔ [CoCl4]-2(aq) + 6 H2O(L) Multiple choices: 24.53 0.0487 28.78 0.0443 0.0311 20.54 0.0408 36.43 22.56 32.18 0.0274 0.0347What is the concentration (in millimolar) of F- ions when 33 mg of MgF2 completely dissociates in 2.5 L of water? 2.1 x 104 mM 2.1 x 102 mM 0.53 mM 0.42 mM 1.1 mM O 1.1 x 102 mM 4.2 x 104 mM 0.21 mM 4.2 x 102 mMHow many moles of Ca2+ and OH-ions are produced for every one mole of Ca(OH)2 that dissolves in solution? Ca(OH)2(s)↔Ca2+(aq) + 2OH–(aq)
- Fluoride treatment strengthens tooth enamel by converting hydroxyapatite, Ca5(PO4)OH, into fluorapatite, Ca5(PO4)3F. Fluoraparite is stronger and more resistant to acid than hydroxyapatite. If the solubility of fluorapatite is 6.1 x 10^-8 mol/L, what is its Ksp? Ca5(PO4)3F(s) -> 5Ca^2+ + 3PO4^3- + F-Calculate the value of Keq. How well do these values compare to each other? Fe3 = 0.002 M , SCN = 0.002 M Keq= [FeSCN^2]/ [Fe^3][SCN^-]Calculate the pH of a blood plasma sample with a total CO₂ concentration of 25.6 mM and bicarbonate concentration of 24.5 mM. The relevant pKa of carbonic acid is 6.1. Enter the answer with three significant figures. pH = Hyperventilating can result in a decrease in CO₂(g) concentration in the blood. How would this affect the pH of the extracellular fluid? The pH does not change appreciably. The pH increases. The pH decreases.
- Good explanation Asap Thanks Hemoglobin, Hb, has four Fe atoms per α molecule that, on average, bind about three O2 molecules. Hb(aq)+3O 2 (g) = Hb(O 2 ) 3 (aq)Discuss mountain or space sickness (high altitude) in terms of this balance.Explain the difference in pH between diH2O and tap waterCalcium carbonate, CaCO3, has Ksp = 8.7 x 10–9. If a swimming pool water contain 225 mg/L of Ca2+, what is the maximum concentration of carbonate ion (CO32-) in the pool water that will not cause the precipitation of CaCO3?