What mass of solid Lanthanum (III) oxalate nonahydrate { Laz ( C2O4 )3 · 9 H2O } can be obtained from 650 mL of 0.0170 M aqueous solution of LaCl3 by adding a stoichiometric amount of sodium oxalate ?
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- What mass of solid Lanthanum (III) oxalate nonahydrate { La2 ( C2O4 )3 ∙ 9 H2O } can be obtained from 650 mL of 0.0170 M aqueous solution of LaCl3 by adding a stoichiometric amount of sodium oxalate ? with solution/explanationThe mass of K3PO4 needed to prepare 250.0mL of an aqueous solution in which PO4-3 concentration is 0.0550M. The answer is ……………………… How many grams of silver sample is equal to 0.0417 mole of silver The answer is ……………………… When 38.0 mL of 0.1250 M H2SO4 is added to 100 mL of a solution of PbI2, a precipitate of PbSO4 forms. The PbSO4 is then filtered from the solution, dried, and weighed. If the recovered PbSO4 is found to have a mass of 0.0471g, what was the concentration of iodide ions in the original solution The answer is ……………………………… Express 96.342 m using 2 significant figures The answer is ………………………………. The oxidation number of sulfur in (Na2S2O5) is? The answer is ………………………………If 28.70 mL of 0.0200 M KMnO4 is required to titreate a 0.250 g sample of K3[Fe(C2O4)3]x3H20, what is the percent C2O42- in the complex?
- What will be the solubility of Fe(OH)3 (Ksp = 1.6 × 10–39) in:a. 0.0250 M FeCl3 solution?b. a solution buffered at pH 8.00? (First, calculate the OH– concentration at this pH)A solution was prepared by dissolving 1210 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 785 mL. Calculate b) the weight/volume percentage of K3Fe(CN)6, the number of millimoles of K+ in 35.0 mL of this solution, and the ppm of Fe(CN)63-For the aqueous [Ni(NH3 )6]2+ complex Kf=5.50 x 108 at 25C . Suppose equal volumes of 0.0024 M Ni(NO3 )2solution 0.94M NH3solution are mixed. Calculate the equilibrium molarity of aqueous Ni2+ ion. Round your answer to 2 significant digits.
- 4. a. Describe the preparation of 1.67 L of 5.00% (w/v) K2Cr2O7 from the solid salt. b. What is the ppm K2CR2O7 in the above solution?Explain the fowlling. (a) Metaalic K is dessloved in liquid NH3 to form dilute soloution. ...(i) b).. more K is added to form conc.soloution.....(ii) c).. soloution (i) & (ii) are evaporated completely. d).. soloution (i) is treated with Fe2O3.(a) In early studies it was observed that when the complex [Co(NH3)4Br2]Br was placed in water, the electrical conductivityof a 0.05 M solution changed from an initial value of191 ohm-1 to a final value of 374 ohm-1 over a period of anhour or so. Suggest an explanation for the observed results.(b) Write a balanced chemical equation to describe the reaction.(c) A 500-mL solution is made up by dissolving 3.87 g ofthe complex. As soon as the solution is formed, and beforeany change in conductivity has occurred, a 25.00-mLportion of the solution is titrated with 0.0100 M AgNO3solution. What volume of AgNO3 solution do you expectto be required to precipitate the free Br-(aq)? (d) Based onthe response you gave to part (b), what volume of AgNO3 solution would be required to titrate a fresh 25.00-mL sampleof [Co(NH3)4Br2]Br after all conductivity changes haveoccurred?
- In the presence of aqueous cyanide, cadmium(II) ions will form the complex Cd(CN)42-. Determine the molar concentration of free uncomplexed cadmium(II) ion in the solution when 47.3g of Cd(NO3)2 is dissolved in exactly one litter of 2.0M sodium cyanide. Kf of Cd(CN)42- at 25 degrees C is 7.2x1016(a) Explain why Mg(OH)2 precipitates when CO32- ion isadded to a solution containing Mg2+. (b) Will Mg(OH)2precipitate when 4.0 g of Na2CO3 is added to 1.00 L of asolution containing 125 ppm of Mg2+?For the aqueous [Cu(NH3)4 ] 2+ complex kf =5.6 x1011 at25°C .Suppose equal volumes of 0.0062M Cu(NO3)2 solution and 0.88M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Cu2+ ion.Round your answer to 2 significant digits.