A 250 mL sample of saturated
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General Chemistry: Principles and Modern Applications, Loose Leaf Version (11th Edition)
- The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)arrow_forwardCalculate the solubility in grams per 100 mL of BaF2 in a 0.10 M BaCl2 solution.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
- An electrode is prepared from liquid mercury in contact with a saturated solution of mercury(I) chloride, Hg2Cl, containing 1.00 M Cl . The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.268 V. What is the solubility product of mercury(I) chloride?arrow_forwardThe cell potential of the following cell at 25C is 0.480 V. ZnZn2+(1M)H+(testsolution)H2(1atm)Pt What is the pH of the test solution?arrow_forwardWhat is the standard cell potential you would obtain from a cell at 25C using an electrode in which I(aq) is in contact with I2(s) and an electrode in which a chromium strip dips into a solution of Cr3(aq)?arrow_forward
- Consider a cell in which the reaction is 2Ag(s)+Cu2+(aq)2Ag+(aq)+Cu(s) (a) Calculate E° for this cell. (b) Chloride ions are added to the Ag|Ag+ half-cell to precipitate AgCl. The measured voltage is +0.060 V. Taking [Cu2+]=1.0M, calculate [Ag+]. (c) Taking [Cl-] in (b) to be 0.10 M, calculate Kspof AgCl.arrow_forwardAn 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_forwardCalculate the standard cell potential of the cell corresponding to the oxidation of oxalic acid, H2C2O4, by permanganate ion. MnO4. 5H2C2O4(aq)+2MnO4(aq)+6H+(aq)10CO2(g)+2Mn2+(aq)+8H2O(l) See Appendix C for free energies of formation: Gf for H2C2O4(aq) is 698 kJ.arrow_forward
- 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_forwardConsider 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_forward
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