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Q: Is the interaction between an ammonia ligand and a metal cation a Lewis acid-base interaction?
A: The interaction between ammonia ligand and a metal cation is a Lewis acid-base interaction.
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Q: Draw a reasonable structure for a complex between Fe3+ and nitrilotriacetic acid, N(CH2CO2H)3.
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Q: 1. In what form must iron exist in order to be measured by the phenanthroline method? 2. List some…
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Q: Is the interaction between an ammonia ligand and a metal cation a Lewis acid–baseinteraction? If so,…
A: The interaction between ammonia ligand and a metal cation is a Lewis acid-base interaction.
Give an example of a double salt that can be formed via ligand exchange and give the reactions involved
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- Group III (Al3+, Cr3+, Fe3+, Zn2+) cations produce very soluble sulphides so they can be precipitated by relatively high amounts of sulfide ion; this can be achieved by adding a basic solution of H2S.(A) if both sentences are true, (B) if both sentences are false, (C) if the first sentence is true but the second is false, and (D) if the first sentence is false but the second is true. 1. In oxygen fixation, the alkaline-iodide-azide solution was used to acidify the solution. The brown hydrated precipitate that formed in the process of oxygen fixation was magnesium hydroxide. 2.Visual inspection is enough to determine if water is of appropriate quality. The standards for drinking water quality are typically set by governments or by international standards. 3.Deeper levels of water often do not reach 100% air saturation equilibrium because they are not shallow enough to be affected by the waves and photosynthesis at the surface. The dissolved oxygen content is an important index when considering its suitability for town supply. 4. The normality (N) of a solution is determined by multiplying the molarity of the solution by its volume. In the standardization of the sodium thiosulfate…Draw an example of a compound that would serve as a cation exchanger and is weakly acidic.
- Explain why different products are obtained in the electrolysis of molten ZnCl2 and in the electrolysis of an aqueous solution of ZnCl.What method is used to precipitate arsenic (III) ions? Treatment with thioacetamide, acetic acid followed by hydrogen peroxide, magnesium nitrate and silver nitrate with acetic acid. Treatment with thioacetamide, acetic acid, hydrochloric acid followed by magnesium nitrate and silver nitrate with acetic acid. Treatment with thioacetamide followed by hydrogen peroxide, magnesium nitrate and silver nitrate with acetic acid. Treatment with thioacetamide, acetic acid, hydrochloric acid followed by hydrogen peroxide, magnesium nitrate and silver nitrate with acetic acid. C Treatment with acetic acid, hydrochloric acid and hydrogen peroxide.1) The amount of warfarin, used for anticoagulant medications, in a sample was calculated as follows. A 13.96 g sample was first treated with an alkaline I2 solution to convert C19H1604 to CHI3. This treatment gives one mole of CHI3 for every mole of C19H1604 that was initially present in the sample. The iodine in CHI3 is then precipitated as AgI(s) by treatment with excess AgNO3(aq): CHI3(aq) + 3AgNO3(aq) + H20(1) → 3A£I(s) + 3HNO3(aq) + CO(g) If 0.1386 g solid AgI were obtained, then what is the percentage by mass of warfarin in the sample analyzed?
- How would I find the formation constant using the given information?Give a proposal for the purification of Cobalt(II)sulphate CoSO4.7H2OIs there a way to predict how much electrical force is required to exactly balance the tendency of an ion to diffuse down its concentration gradient? How are these two factors mathematically related?
- a Nitrogen(I) oxide and hydrogen gases react to form ammonia gas and steam. b Hydrogen peroxide reacts with an acidic aqueous solution of sodium hypochlorite to form oxygen and chlorine gases. C Tin metal reduces the vanadyl ion (VO²+) to vanadium(III) ions in acidic solution. Tin(II) ions are also formed.Would you expect an aqueous solution of manganese (VII) oxide to have a ph greater or less than 7.0? Justify your answerDiscuss the solubility product constant values of silver halides in accordance with HSAB theory.