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GENERAL CHEMISTRY(LL)-W/MASTERINGCHEM.
- The formation constant for the mercury(II) acetate complex is Hg2++ 2OAc- Hg(OAc)2(aq) Kf = 2.7 108 Calculate the standard potential for the half-reaction Hg(OAc)2(aq) + 2e- Hg(l) + 2OAc-arrow_forwardCalculate the standard potential for the half-reaction Al (C2O4)2- + 3e- Al(s ) + 2C2O42- if the formation constant for the complex is 1.3 1013.arrow_forwardAssuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products): (a) Agl. (b) Ag2SO4. (c) Mn(OH)2. (d) Sr(OH)28H2O (e) the mineral brucite, Mg(OH)2arrow_forward
- Use Table 17.1 to predict what reaction, if any, will occur if sulfur is added to acidic aqueous solutions of the following species at standard conditions. (a) MgBr2 (b) Sn(NO3)2(c) Cr(ClO3)2arrow_forwardThe solubility of cadmium oxalate. CdC2O4, in 0.150 M ammonia is 6.1 103 mol/L. What is the oxalate-ion concentration in the saturated solution? If the solubility product constant for cadmium oxalate is 1.5 108, what must be the cadmium-ion concentration in the solution? Now calculate the formation constant for the complex ion Cd(NH3)42+.arrow_forwardThe photographs below (a) show what occurs when a solution of iron(III) nitrate is treated with a few drops of aqueous potassium thiocyanate. The nearly colorless iron(III) ion is converted to a red [Fe(H2O)5SCN)2+ ion. (This is a classic test for the presence of iron(III) ions in solution.) [Fe(H2O)6]3+(aq) + SCN(aq) [Fe(H2O)5SCN]2+(aq) + H2O() (a) As more KSCN is added to the solution, the color becomes even more red. Explain this observation. (b) Silver ions form a white precipitate with SCN ions. What would you observe on adding a few drops of aqueous silver nitrate to a red solution of [Fe(H2O)5 SCN]+ ions? Explain your observation.arrow_forward
- An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?arrow_forwardThe standard reduction potential for the reaction [Co( H 2 O)6]3+(aq)+e[CO( H 2 O)6]2+(aq) is about 1.8 V. The reduction potential for the reaction [Co( NH 3 )6]3+(aq)+e[Co( NH 3 )6]2+(aq) is +0.1 V. Calculate the cell potentials to show whether the complex ions,. [Co( H 2 O)6]2+ and or [Co( NH 3 )6]2+, can be oxidized to the corresponding Cobalt (III) complex by oxygen.arrow_forwardCalculate the solubility of copper(II) iodate, Cu(IO3)2 (Ksp = 7.4 108), in (a) water. (b) a 0.10 M copper(II) nitrate solution.arrow_forward
- Consider the equation G = -nF. What are the four terms in this equation? Why does a minus sign appear in the equation? What does the superscript o indicate?arrow_forwardThe equilibrium constant for the following reaction is 1.0 1023: Cr3+(aq)+H2EDTA2(aq)CrEDTA(aq)+2H+(aq) EDTA is used as a complexing agent in chemical analysis. Solutions of EDTA, usually containing the disodium salt Na2H2EDTA, are used to treat heavy metal poisoning. Calculate [Cr3+] at equilibrium in a solution originally 0.0010 M in Cr3+ and 0.050 M in H2EDTA2 and buffered at pH = 6.00.arrow_forwardIn some old European churches, the stained-glass windowshave so darkened from corrosion and age that hardly anylight comes through. Microprobe analysis showed that tinycracks anddefects on the glass surface were enriched ininsoluble Mn(III) and Mn(IV) compounds. From AppendixE, suggest a reducing agent and conditions that might successfullyconvert thesecompounds to soluble Mn(II) withoutsimultaneously reducing Fe(III) (which gives the glassits colors) to Fe(II). Take MnO2 as representative of theinsoluble Mn(III) and Mn(IV) compounds.arrow_forward
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