Write a balanced net ionic equation to show why the solubility of AgCN(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Use the pull-down boxes to specify states such as (aq) or (s). Knet + + + ◆
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- Write a balanced net ionic equation to show why the solubility of Cu(OH)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.Be sure to specify states such as (aq) or (s). + + K =Write a balanced net ionic equation to show why the solubility of Ni(CN)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.Use the pull-down boxes to specify states such as (aq) or (s).Will Mn(OH)2 precipitate from a 0.01 M solution of MnCl2 at pH = 9? Ksp(Mn(OH)2) = 1,0 x 10-13. Discuss from solubility diagrams and prove by calculation.calculation. Co is a metal that is present in every lithium battery to stabilize its charge and toincrease stability. Every cell phone, tablet and electric car relies on the availability ofcobalt, 97% of which is extracted from mines in places like the Congo, where essentially slave labor is used.Cobalt ions form complexes with e.g. CN- . You see solubility diagrams and fraction diagrams for CoCO3 with and without the addition of 10 mM CN- .. Explain whythe solubility of cobalt carbonate increases at high pH when cyanide ions are present.Write reaction formulas for the formation of the dominant cobalt cyanide complexes.
- Sometimes it is not possible to indicate the end point of a titration.a) How can one proceed then and what is the name of the type of titration that can be performed? Briefly describe. An example in which this method can be used is in the determination of mercury, which forms strong complexes with EDTA, but for which there is no suitable indicator that can indicate the end point. b) You are given the task of determining the Hg2 + concentration in a sample solution? After adding an excess of EDTA, the sample solution is titrated with a magnesium solution. 20.00 ml of a 0.0452 M EDTA solution was added to 30.00 ml of sample solutionThe excess EDTA was determined by adding 0.0500 M Mg 2+ solution, consuming 4.37 ml to the end point.If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3.Ksp = (c) The Ksp of Mg3(PO4)2 at 25 oC is 1.04e-24. What is the molar solubility of Mg3(PO4)2?solubility = mol/LThe solubility of Sr(OH)2 is 3.2 x 104 g/L a) Write a balanced equation for the solubility equilibrium b) Write the expression for the solubility product constant Ksp and calculate its value c) Calculate the pH of a saturated solution of Sr(OH) 2 d) 25 ml of 3 x 10-4 SOLUTION of SrS04 is added to 35 ml of 3.21 x 10-6 molar NaH solution. Does a precipitate form? Explain and show calculations to support your answer
- Use systematic treatment of equilibrium to calculate the molar solubility of AgIO3 in an aqueous solution with a pH of 2.00. Ignore activity coefficients. Ksp for AgIO3 is 3.17*10-8 and Ka for HIO3 is 0.17.Discuss the titration curve (variation of pH with respect to addition oftitrant) with suitable diagram and reactions involved when potassiumhydroxide (KOH) a strong base is added as titrant to acetic acid(CH3COOH) a weak acid analyte.A student has a sea water sample which contains Ca2+ ions . Describe briefly how he willdetermine the concentration of Ca2+ ion in the sample using a simple titration. Explain the colourchanges at the endpoint. Which medium is suitable for performing the titration, acidic or basic medium and why?
- Calculate the potential of the solution in the titration of 50.0 mL 0.100 M Fe2+ in 1.00 M HClO4 with 0.0167 M Cr2O72- at 10.00 mL titrant added.b. A student has a sea water sample which contains Ca2+ ions . Describe briefly how he willdetermine the concentration of Ca2+ ion in the sample using a simple titration. Explain the colourchanges at the endpoint. Which medium is suitable for performing the titration, acidic or basic medium and why?In the determination of chloride by the Mob method, what will be the equiliblium concentration of silver ions in mgil, on the basis of the solubility product principle, when the chloride concentation has been reduced to 0.2 ma? (b) If the concentration of chromate indicator used is 5X M, how much excess silver ion in mgil must be present before the formation of a red precipitate will begi(a) In the defermination of chloride by the Mohr method, what will be the equilibrium concentration of silver ions in meL., an the basis of the solubility. pcoduct principle, when the chloride concencration has beea reduced to 0.2m 1.2m? (b) If -3 the concentration of chromate indicator ased is 5 x 10M, bow much excess silver ion in mel, must be present before the formatice of a red precipitate will begin?