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For EDTA,what is meant by aY4- and how does it vary with pH?
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- commercially available forms of EDTA are the free acid form, H4Y• it is in the form of the disodium salt, Na2H2Y.2H2O. Why?From the reaction CaCO3+CO2+H2O= Ca2+ + 2HCO3- A.) Show how it affects the chemistry of water, alkalinity and hardness of water B.) Its relationship to microbial degradation of organic matterOCN-(aq) + OCI-(aq) → CO₂2-(aq) + N2(g) + Cl(aq) (basic media)
- Why is commercially available EDTA in the form of disodium salt, Na2H2Y.2H2O? to decrease EDTA solubility in water because of difficulty in synthesizing other forms of EDTA to increase the binding capacity of EDTA with metal ions to increase EDTA solubility in waterA copper storage tank containing dilute H2SO4 at pH = 3 is blanketed with hydrogen at 1 atm. Calculate the maximum Cu" contamination of the acid in moles Cu per liter. What is the corresponding contamination if the hydrogen partial pressure is reduced to 10* atm?The following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300 M)|H2(1.00 atm),Pt Calculate the dissociation constant of HA, neglecting the junction potential.
- 1) Balance the following in acidic solution: (a) Н2О + Sn2+ Н,0 + Sn++ (b) PBO2 + Hg –→ H* + P²+ (c) Al + Cry0; – A+ + Cr+Which of the following does NOT form a 1:1 ratio with an EDTA molecule? * O Li O Mg O Bi O AICalcium in powdered milk is determined by dry ashing a 3.00g sample then titrating the calcium with 12.10mL EDTA solution. The EDTA was standardized by titrating 10.00mL of a Zn solution by dissolving 0.632g Zn metal in acid and dilution to 1.00L (10.80 mL EDTA required for titration). What is the concentration of Ca in the powdered milk in ppm?
- The reaction of divalent manganese with oxygen in aqueous solution is given as follows: Mn2+ + 1/2O2(aq) + H2O = MnO2(s) + 2H+ The equilibrium constant (K) for this reaction is 23.7. It has been found that a lake water sample that contains no oxygen at 25 C, pH = 8.5, originally contained 0.6 mg/L of Mn2+. The sample was aerated (atmospheric conditions of the dissolved oxyen concentration is 9.2 mg/L) and after 10 days of contact with atmospheric oxygen, the Mn2+ concentration was 0.4 mg/L. The molecular weight of Mn is 55, O is 16 and H is 1. The change in free energy of formation at standard conditions (kcal/mole) are as follows: Mn2+ = -54.4, O2(aq) = +3.93, H2O = -56.69, MnO2(s) = -111.1, H+ = 0. (a) Assuming that the pH remains constant during aeration, will the precipitate continue to form after the measurement on the tenth day? (b) What should the Mn2+ concentration be (in moles/L) at equilibrium, assuming that pH and presence of dissolved oxygen are the same as in part "a".…A solution was prepared by dissolving about 3.0 g of NaH2Y2·2H2O in approximately 1 L of water and standardizing it against 50.00-mL aliquots of 0.004423 M Mg2+. An average titration of 30.27 mL was required. Calculate the molar concentration of the EDTA.If concentration of [CrO4 ] in Expt. 7 is found to be 6.7 x 105 M, what is the experimental Ksp of Ag,CrO4? a) 3.0 x 1013 b) 6.0 x 1013 c) 1.2 x 1012 d) 1.8 x 108 Ksp of Ag.CrO4 = [Ag]° [CrO,?] Ag,CrO4 2 Ag+(aq) + CrO,-(aq), moles, and concentration, of Ag+ are twice those of Cro Ksp of Ag.CrO, = [Ag"] [CrO,] = [2Cro.1°[CrO,] = [CrO.,*]