Give the chemical equations that are characterised by the stepwise stability constants at 25°C in an aqueous solution for the formation of copper complexes with ethylenediamine.
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A: the product of CH3CH2COONa + H2O is
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- You have been sent to India to investigate the occurence of goiter disease attributed to iodine deficency. As part of of your investigation, you must make field measurements of traces of Iodide(I-) in groundwater. The procedure is to oxidize I- to I2 and convert the I2 into an intensely colored complex with the dye brilliant green in the organic solvent toluene. a) A 3.15x10^-6 M solution of the colored complex exhibited an absorbance of 0.267 at 635nm in a 1.00cm cuvet. A blank solution made from distilled water in place of groundwater had an absorbance of 0.019. Find the molar absroptivity of the colored complex. b)The absorbance of an unknown solution prepared from ground water was 0.175. Find the concentration of the unknown.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.A biochemical reaction takes place in a 1.00 ml solution of 0.0250 Mphosphate buffer initially at pH = 7.20 (as shown for pKas of phosphatespecies).(a) Are the concentrations of any of the four possible phosphate speciesnegligible? If so, identify them and explain your answer.(b) During the reaction, 3.80 μmol of HCl are produced. Calculate the finalpH of the reaction solution. Assume that the HCl is completely neutralizedby the buffer.
- For each of the following ionic compounds, state whether the solubility will increase, decrease, or remain unchanged as a solution at pH 7 is made acidic.(a) SrCO3 (b) Hg2Br2 (c) MnSGiven this series of equilibrium reactions. See Image(a) Which way should the reaction to “tend” at high pH? Why?(b) Which way should the reaction to “tend” at low pH? Why? (c) What Fe(III) species would be least soluble?Write the equilibrium constant expressions for the Iron(III)-thiocyanate system.
- Give the pH of 0.005 M C6H5O- (aq) at 298 K of the Ka for C6H5OH at the given T is 1.0 x 10-10Describe the conditions to be maintained during the titration of a permanganate solution with oxalate. Detail the chemical principles involved.What are the main equilibria involved in the CO2–Carbonate system and what kind of equilibrium constant is associated with each (K?)?
- Write a balanced net ionic equation to show why the solubility of ZnCO3 (s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.Consider only the FIRST STEP in the reaction with strong acid. Be sure to specify states such as (aq) or (s)Outline the dissociation reactions for carbonic acid and list the electrical charges of protonated and deprotonated forms. Attach a plot for the portions of molecules possessing each of the outlined charges as function of pH.Write a balanced net ionic equation to show why the solubility of CaCO3 (s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Here is the problem: