Solution 1 Solution 2 Solution 3 Volume stock solution (mL) 4.00 4.00 4.00 Volume DI water (mL) 1.00 2.00 3.00 Concentration iron(III) thiocyanate ion [FESCN2*] (M)
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- Cerium(IV) is a strong oxidizing agent commonly used in redox titrations. Which of the following statemnt is/are NOT true for cerium(IV)? I.A Ce** standard solution is prepared using primary-standard-grade ammonium hexanitratocerate(IV), (NH4)2Ce(NO3); dissolved in hot hydrochloric acid solution. II. Ce** is yellow and Ce3* is colorless. The color change is abrupt enough that Ce** can serve as its own indicator. III. Ce**/Ce* exists in different formal potential in different acids due to the interaction of the anions part of the acid with Ce** IV. Analysis of many organic analyte such as alcohol, aldehydes can be determined using Ce**by an indirect method involving a technique of back titration of unreacted excess Ce*with standard iron Il titrant O a. 1,11,IV O b. 1, II, III O. I,II O d. II, II, IV O e. I, II, III, IVWhich of the following salts does NOT cause permanent hardness? A FeCl, B CaCl, © Ca(HCO,), (НСО ,), D MgSO 4What 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/explanation
- A 0.4852g sample of an iron ore was dissolved in acid to the 3+ state, then precipitated as Fe2O3 x H2O. The pp was filtered, washed and calcined to Fe2O3, which gave a weight of 0.2481g. Calculate the Fe % in the sample.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. lWhat is the percentage of Nickel in an ore if, when analyzed by the cyanide method, 20.00mL of KCN solution (containing 1.00mmol of AgNO3 per milliliter) are used? Wt of sample used = 0.2500g
- 0.1745 g of primary standard Na2C2O4 is used to set a freshly prepared KMnO4 solution and 30.24 mL of KMnO4 solution is spent at the turning point. Since 36.92 mL of this KMnO4 solution is consumed for the determination of iron in 0.5618 g ore sample, calculate the amount of iron in the ore in terms of % iron (III) oxide and % iron (III) chloride. (Fe: 56, K: 39, Mn: 55, O: 16, Na:23, C: 12, Cl: 35.5 g/mol) (Please type answer)Which of these expressions correctly expresses the solubilityproductconstant for Ag3PO4 in water?(a) [Ag][PO4] (b) [Ag+][PO43 - ] (c) [Ag+]3[PO43 - ](d) [Ag+[[PO43 - ]3 (e) [Ag+]3[PO43 - ]3what volume of decinormal k2cr2o7 solution would be needed to convert 1.19 g of tin to stannic chloride in acidic medium?
- 2 MnO4- (aq) + 5 C2O42- (aq) + 16 H+ (aq) « 2Mn2+ (aq) + 10 CO2 (g) + 8 H2O(l) 0.4040 g of the unknown compound (K2Zy(C2O4)z . nH2O) was dissolved in 100.0 mL water to make a solution. It was then heated to 80oC and titrated with a KMnO4 solution as shown below: The molarity of KMnO4 = 0.0.02321 M Volume used = 29.25 mL A.) What is the % Oxalate by mass for the unknown solid titrated?A 0.2795-g sample of an organic mixture containing only C6H6Cl6 (290.83 g/mol) and C14H9Cl5 (354.49 g/mol) was burned in a stream of oxygen in a in a quartz tubeb. The products (CO2, H2O and HCl) were passed through a solution of NaHCO3. After acidification, the chloride in the solution yielded 0.7161 g of AgCl (143.32 g/mol). Calculate the percentage of each halogen compound in the sample. A mixture containing only FeCl3 (162.21) and AlCl3 (133.34) weighs 5.95 g. The chlorides areconverted to the hydrous oxides and ignited to Fe2O3 (159.69) and Al2O3 (101.96) The oxidesmixture weighs 2.62 g. Calculate the percent Fe (55.85) and Al (26.98) in the original mixture.A Chemist collected a 0.4891-g sample of an ore for Fe determination by a redox titration with K2Cr2O7.The ore was carefully crushed prior to weighing and dissolved in HCl and using a Jones reductor the ironin the sample was brought into the +2 oxidation state. After titration with diphenylamine sulfonic acid,itrequired 36.92 mL of 0.02153 M K2Cr2O7 to reach the end point. Calculate the iron content of the ore as%w/w Fe2O3