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- + H (a) CuCN (b) CaCO3 (c) Ag₂CO3 (d) PbBr₂ (e) Y(OH)3 Periodic Table B W Chapter... Supporting Materials Additional Materiala [Ca²+] = 5.2 x 104 M, [CO32- ] = 6.5x 10-6 M * G Please use the values in the resources listed below instead of the textbook values. The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated. [Cu] = 1.9x10-10 M, [CN] = 1.9x10-¹0 M [Ag+] = 1.8x10-5 M, [CO32] = 2.7x10-² M [Pb²+] = 1.2x 10-2 M, [Br] = 2.4x10-2 M [Y³+] = 3.5x 10-16 M, [OH-] = 6.6x 10-³ M Constants and Factors №. webassign.net ● F 893 Supplemental Data L C C a Ⓒ + D r4- Mo in a 0.2711 g sample was precipitated giving 1.1682 g of (ΝH)2PO,. 12 MoO Find percentage Mo , P (at wt = 30.97) .N=14,Mo= 95.9,H=1 , O= 162. In a laboratory experiment you react 20.0 mL of 25% by mass C2H&N2 with 8.000 NiCl2.6H20 to obtain the product Ni(NH2CH2CH½NH2j3Cl2 complex. The C2H3N2 solution used in this experiment is 25.0% by mass, with a density (d) of 0.950 g/mL. (MW NICI2.6H2O= 237.69 g/mole, MW C2HgN2=60.10 g/mole, MW tris(ethylenediamine)nickel(II)chloride = 309.89 g/mole) a. Write down the balanced equation of the synthesis. b. Determine the number of moles of each reactant that you use. c. Determine which reactant is the limiting reactant, giving your reasoning. Show all your work to get full credit. (5 points) d. Calculate your percent yield if the dry product weighs 7.000 g.
- Gold can be determined in solutions containing high concentrations of diverse ions by ICP. Aliquots of 50.0 mL of the sample solution were transferred to each of four 100.0 mL volumetric flasks. A solution was prepared containing 10.0 mg/L Au in 20% H2SO4, and quantities of this solutions were added to the sample solution to give 0, 2.5, 5 and 10 mg/L added Au in each of the flask. The solutions were made up to a total volume of 100.0 mL, mixed and analyzed by ICP. The resulting data are presented in the following table: Added Au (mg/L) Emission Intensity (Counts) 0.0 12568 2.5 19324 5.0 26622 10.0 40021 a) Attach an excel graph for the determination showing the X intercept. b) Calculate the concentration of gold in the sample, report with its uncertainty. c) The known concentration of gold in the sample is 8.51 mg/L. Test the hypothesis that your result is equal to this value at the 95% confidence level. lThe activity of Zn2* in a saturated solution with Zn(OH)2 with 0.0100 M KNO3 (Ksp 1.20 X10-17 y Zn2* = 0.676, y OH- = 0.900) is: %3D 2.80X10-6 O 1.19X10-6 2.45 X10-6 O 4.69X10-6 O X10-6 1.99 TOSHIBAThe gravimetric factor (GF) for Ag in precipitated Ag2CrO4 equal:(Atomic (weights, Cr=24;Ag=108 ,0=16 0.078 O 0.335 O 0.235 O 0.71 O
- th acedic scuticns Balance the fallowng redex reacti ans rusine cxidatian ununbers. Explain process. Helle 34 b) Fe4, 24 (aq) c) Uo 24 34 2-The activity of Zn2+ in a saturated solution with Zn(OH)2 with 0.00500 M KNO3 (Ksp = 1.20 X10-17, y Zn²+ = 0.748 , y OH- = 0.926) is: %3D 4.50X10-6 5.45X10-6 1.25 X10-6 8.65X10-6 O 2.65X10-6A 0.64 g sample containing KCI ( mw = 74.6 ) is dissolved in 50mL of water and titrated to the Ag2CrO4 end point, requiring 26.2 mL of 0.15 M AGNO3 * ? .The %w/w KCI in the sample is
- 4. The %Mn in steel can also be determined spectrophotometrically by oxidizing the manganese to the intensely colored permanganate, MnO4-. Standard solutions of permanganate gave the following absorbances (in a 1 cm cell): ABSORBANCE CONC. OF MnO4 (g/mL) 0.210 1.05 x 10-5 0.315 1.61 x 10-5 0.429 2.21 x 10-5 0.599 2.98 x 10-5 0.801 4.04 x 10-5 The following samples of steel were thoroughly reacted to convert the manganese into permanganate and then diluted to 500.00 mL. WT. OF STEEL (g) ABSORBANCE 0.5886 0.611 0.3498 0.359 0.4555 0.482 Again using Excel, plot the calibration data and calculate the %Mn in the steel.A 0.0715 g sample of a material was analyzed for thiourea (CS(NH2)2, MM = 76.12). It was found to consume 12.34 mL of 0.00543 M KBrO3 based on the reaction below: 3CS(NH2)2 + 4BrO3- + 3H2O ⇄ 3CO(NH2)2 + 3SO42- + 4Br- + 6H+ Calculate the mass of thiourea found in the sample. Group of answer choices 95.1 mg 6.80 mg 3.83 mg 0.0535 mgSECTION: CEIT-04-101A 2. Balance the following Tedox reactions using the lon- electror Method. a.) cl02+cl' C12+CIO, ( In acidic medium) b.) CN!" + Mn O4 c.) Crq Oq*+ C,04* y CNU! + Mn0,( in basic Hedium + G*+ co,l in acidic medium) d.) Dr, Bro, + Br- (in oaste meclium)