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What is the most stable oxidation state of chromium in acid and base?
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- cion 12 of 13> OAttempt 4 A solution is made by mixing 500.0 mL of 0.04794 M Na, HASO, with 500.0 mL of 0.02554 M NAOH. Complete the mass balance expressions for the sodium and arsenate species in the final solution. (HASO + (H, AsO 1+ [H, AsO,+ [Aso 1 Incorrect (Na") = 3.67 xid 2 M. Incorrect(iii) 5.0, 25.0, 50.0 and 100.0 g aliquots of MgCl2 were dissolved in 4 separate 250 ml samples of distilled water. Calculate [H30*] and the pH for each of the resulting solutions and comment on the relationship between [MgCl2] and pH.8. The following questions concern the reaction HA(aq) + B(aq) 2 HB1†(aq) + A1-(aq). What can you say about: (a) the magnitude of K for this reaction (K >> 1 or K > solution that results from reacting equal mole quantities of HA with B, when [HB1*] or [HA] << [HB1*]), and (c) the pH of the (a) K (b) Relative concentration (c) pH HA is a weaker acid than HB1+. HA is a weak acid and B is a strong base. HA is a strong acid and B is a strong base. HA is a strong acid and B is a weak base.
- Like any equilibrium constant, Kᵥᵥ changes with tempera-ture. (a) Given that autoionization is endothermic, how does Kᵥᵥ change with rising T? Explain with a reaction that includes heatas reactant or product. (b) In many medical applications, the value of Kᵥᵥ at 37°C (body temperature) may be more appropri-ate than the value at 25°C, 1.0X10⁻¹⁴. The pH of pure water at 37°C is 6.80. Calculate Kᵥᵥ, pOH, and [OH] at this temperature.Course : Environmental Chemistry 1. Chromium (Cr) is a non-essential heavy metal that is toxic. Explain: (a) Cr specimens in water bodies in the pH range of 6-8;(b) Explain and give reasons, among cr specimens mentioned in question 1a, how it is available for aquatic biota! ;(c) Describe the toxicity of Cr(III) VS Cr(VI)!( Please type the answer, so i can moev it to word easily, thanks )explain anharmonicity.
- What are the respective concentrations (M) of Mg2+ and Cl- afforded by dissolving 0.325 mol MgCl2 in water and diluting to 250 mL? A) 0.0013 and 0.0013 B) 2.60 and 2.60 C) 1.30 and 2.60 D) 1.30 and.1.30 E 0.0013 and 0.0026Calculate the (Ka) value for the reaction of CH3COOH with NH3 that the pH of the solution is (6.46) and the (Kb = 1.75 x 10 5).Which of these expressions correctly expresses the solubilityproductconstant for Ag3PO4 in water?(a) [Ag][PO4] (b) [Ag+][PO43 - ] (c) [Ag+]3[PO43 - ](d) [Ag+[[PO43 - ]3 (e) [Ag+]3[PO43 - ]3
- Complete the charge balance equation for an aqueous solution of H₂CO3 that ionizes to HCO3 and CO2-. [H+] || [OH-] 2[CO3-] + Answer Bank 2[H+] [HCO3] + D 3[H+] [CO] [H₂CO3]Calculate the ionic strength of 0.00025 M La(IO3)3 (assuming complete dissociation at this low concentration and no hydrolysis reaction to make LaOH2+). (with correct sig figs)Calculate the concentrations of [H3O+], [HSO4-] and [SO42-] in 0.50 M sulfuric acid solution atequilibrium.