Iodine (I2) in water will combine with iodide ions (I-1) to make tri-iodide ion (I3-1) .This tri-iodide ion fits inside the coiled starch molecule making a complex and causes a blue-black colour. Write out a general word equation showing this.
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Iodine (I2) in water will combine with iodide ions (I-1) to make tri-iodide ion (I3-1) .This tri-iodide ion fits inside the coiled starch molecule making a complex and causes a blue-black colour. Write out a general word equation showing this.
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- Consider the insoluble compound nickel (II) hydroxide, Ni(OH)2. The nickel ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of Ni(OH)2 (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Ni(CN)4²-, Kf = 1.0×10³¹ . Be sure to specify states such as (aq) or (s). K = + Submit Answer + Retry Entire Group No more group attempts remainIn the second part of this experiment, a student makes a solution with initial concentrations of iron(III) and thiocyanate ions of 0.000900 M and 0.000600 M respectively. Using the Beer's Law plot produced in the first part of the lab, the student determines the equilibrium concentration of the thiocyanatoiron(III) complex (Fe(SCN)2+) to be 3.00 ×10−5 M. What are the equilibrium concentrations of the two starting ions, and what is the value of the equilibrium constant? [fe^3+]=___*10___M [SCN]=_____*10___ M Kc=_____Potassium Ferrioxalate is mixed with in 50 mL of 1 M H2SO4 In a beaker , it is then placed one-half of this solution in another beaker in the sun and the other half in a cabinet in the dark. the color of both solutions after 0, 5, 15, and 30 minutes are : In the sun it stayed clear the whole 30 min and the sample in the darkness of the cabinet turned light green, Briefly explain your observations in terms of the photochemical properties of ferrioxalate.
- In the second part of this experiment, a student makes a solution with initial concentrations of iron(III) and thiocyanate ions of 0.000900 M and 0.000600 M respectively. Using the Beer's Law plot produced in the first part of the lab, the student determines the equilibrium concentration of the thiocyanatoiron(III) complex (Fe(SCN)2+) to be 1.00×10−5 M.What are the equilibrium concentrations of the two starting ions, and what is the value of the equilibrium constant? [Fe3+]= [SCN−]= Kc =In the second part of this experiment, a student makes a solution with initial concentrations of iron(III) and thiocyanate ions of 0.000900 M and 0.000600 M respectively. Using the Beer's Law plot produced in the first part of the lab, the student determines the equilibrium concentration of the thiocyanatoiron(III) complex (Fe(SCN)2+) to be 2.00 × 10−5 M. What are the equilibrium concentrations of the two starting ions, and what is the value of the equilibrium constant? [Fe3+] = [SCN−] = Kc =Be sure to answer all parts. Report your answer to the correct number of significant figures. In the second part of this experiment, a student makes a solution with initial concentrations of iron(III) and thiocyanate ions of 0.000900 M and 0.000600 M respectively. Using the Beer's Law plot produced in the first part of the lab, the student determines the equilibrium concentration of the thiocyanatoiron(III) complex (Fe(SCN)²*) to be 3.00 x 10M. What are the equilibrium concentrations of the two starting ions, and what is the value of the equilibrium constant? [Fe**]=[ x 10 M [SCN ]=| х 10 M K.
- Calculate concentration of species in a solution containing a complex ion. In the presence of excess OH", the A1³+ (aq) ion forms a hydroxide complex ion, Al(OH)4. Calculate the concentration of free Al³+ ion when 1.97x10-2 mol AI(NO3)3(s) is added to 1.00 L of solution in which [OH- ] is held constant (buffered at pH 12.50). For Al(OH)4, Kf = 1.1x1033. [A1³+] = MConsider the insoluble compound silver chloride, AgCl. The silver ion also forms a complex with cyanide ions. Write a net ionic equation to show why the solubility of AgCl(s) increases in the presence of cyanide and calculate the equilibrium constant for this reaction. Solubility product constant data is found in the Chemistry References. For Ag(CN)₂, Kf = 1.3×1021. Be sure to specify states such as (aq) or (s). K = + +Consider the insoluble compound silver bromide, AgBr. The silver ion also forms a complex with cyanide ions. Write a net ionic equation to show why the solubility of AgBr(s) increases in the presence of cyanide and calculate the equilibrium constant for this reaction. Solubility product constant data is found in the Chemistry References. For Ag(CN)₂, Kf = 1.3×1021. Be sure to specify states such as (aq) or (s). K= + +
- When a strong base is added to a solution of CuSO4, which is pale blue, a precipitate forms and the solution above the precipitate is colorless. What is the net chemical equation that describes this reaction? Include the phases of all species in the chemical equation. When ammonia is then added, the precipitate dissolves and the solution turns a deep navy blue. What is the net chemical equation that describes this event? Include the phases of all species in the chemical equation. Cu(OH)₂(s) + 4NH₂(aq) → [Cu(NH₂)]²+ (aq) + 2OH¯(aq) Tip: Plus signs (+) can be typed from the keyboard. Reaction arrows can be found in the Tools menu of the answer module. Include phases in the balanced chemical equation. Click on the (aq) button in the tools to select the phase to add. Phases should not be subscripted.A method for testing the presence of unreacted salicylic acid in your aspirin synthesis is to add a 1% FeCl3(aq) solution to observe a color change (or not). If a magenta color forms, what has occurred? Select one: The ester group formed a bidentate ligand with the free Fe3+ in solution. The phenol group was deprotonated and reacted with free Fe³+ in solution. O The carboxylic acid group was reduced to a secondary alcohol. O A ketone formed producing a smell similar to nail polish removerPLEASE I NEED TO UNDERSTAND HOW TO SOLVE THIS. A 1.000-gram sample of NaOH (39.997 g/mol) which has been exposed to the air for some time (NaOH will adsorb water and CO2 from the ambient air) is dissolved in water and then diluted to 500.00 mL, 100.0 mL of this solution required 38.60 mL of 0.01062 M HCl to be titrated to a methyl orange endpoint (~pH 3). A second 100.00 mL portion is treated with excess BaCl2 and then diluted to 250 mL and filtered. 200 mL of the filtrate required 29.62 mL of HCl to titrate to phenolphthalein (~pH 8-9) endpoint. Calculate in the original sample:a.) the percentage of NaOHb.) the percentage of Na2CO3 (105.9898 g/mol)Make sure you use at least four significant figures for this calculation. Note that the adsorbed CO2 is converted to Na2CO3. The Ksp for BaCO3 (s) is 2.58 x 10-9 (extremely insoluble).