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- Formaldehyde (CH2O, MM = 30.03) has a multitude of uses includingtissue preservation. Formalin is a commercially available solution offormaldehyde and has a concentration of 19.6 m formaldehyde anda density of 1.09 g/cm3. What is the molarity of formaldehyde inthe solution?To prepare 50 mL solutions of 0.01 M KMnO4 in water (calculation to prepare chemicals in spectrophotometer)Sample: Saline 0.900% (m/v), in sodium chloride (NaCl). Data: M.A. (g/mol): Na = 22.9898; K = 39.0983; Cr=51.9961; Ag = 107.8682; Cl = 35.453; N=14.0067; O = 15.9994. Material available in the laboratory's warehouse: Reagents: distilled water; standardized solution of silver nitrate (AgNO₃), at a concentration of 0.09980 mols/L; Potassium chromate solution (K₂CrO₄) 1%; ammoniacal ferric alum solution [Fe(NH₄)(SO₄)₂] and; nitrobenzene (or cooking oil, alternatively); 0.1000 mols/L potassium thiocyanate (KSCN) standard solution. Glassware: beakers of all sizes available on the market; 50, 100, 150, 200 and 250 ml Erlenmeyers; 10.00 and 25.00 mL volumetric pipettes; 15.00 mL burette; 30.00, 50.00 and 100.00 mL volumetric flasks Calculate the molarity of saline, in terms of the NaCl concentration (concentration in mols/L). (a) 0.900 mols/L (b) 5.84 mols/L (c) 0.154 mols/L (d) 0.0154 mols/L
- 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?43. In the preparation of Rochelle salt (MW = 282.83 g/mol), 7.2 grams of monohydrated Sodium carbonate (MW = 124.01 g/mol) dissolved in 80 mL water was made to react with 20g of Potassium bitartrate (MW = 188.10 g/mol). What is the amount of Rochelle salt obtained from Monohydrated Sodium carbonate? Rochelle's Salt:2 KHC4H4O6 + Na2CO3.H2O + 6 H2O -> 2 KNaC4H4O6.4H2O + CO2 ↑ a 38.77 g b 28.74 g c 36.48 g d 32.84 gPotassium permanganate in acidic solution is used to titrate a solution of copper(I) ions, with which it reacts according to MnO4-(aq) + 5Cu+(aq)+8H3O+(aq)Mn2+(aq) + 5Cu2+(aq)+12H2O(l) A potassium permanganate solution is prepared by dissolving 23.14 g of KMnO4 in water and diluting to a total volume of 1.000 L. A total of 15.61 mL of this solution is required to reach the endpoint in a titration of a 200.0-mL sample containing Cu+(aq). Determine the concentration of Cu+ in the original solution.
- Are the following statements true or false? A) Magnesium chloride and sodium hydroxide is Mg2+(aq) + 2OH-(aq) Mg(OH)2(s) :T or F? B) Lead(II) nitrate and sodium chloride, no reaction occurs: T or F?Calculate the percent purity of copper in an ore in terms of Cu2O from the given data: Weight of copper ore - 1.20-g Volume of Na2S2O3 used - 40.00-mL (1.00-mL Na2S2O3 ≈ 0.004175-g KBrO3) Molar Masses: KBrO3 = 167.0 Cu2O = 143.1 Note: Reaction between KBrO3 and Na2S2O3 happens based on the pattern of reaction in problem no.2. Bromate is used in place of iodate.A formula for compounding state qs ad 250 ml. This expression means
- The aluminium in a 1.2 g sample of impure NH4Al (SO4)2 was precipitated as hydrous Al2O3. The precipitate was filtered and ignited at 100° c to give anhydrous Al2O3 which weighed 0.1798 g. Calculate the % Al in the sample. (number of moles Al = 2; Al2O3 = 1)Calculate the mass of Na2S203.5H20 needed to prepare 250 cm3 of a 0.011 M solution in a volumetric flask. (RMM = 248)5. A 0.5664 g ore sample is dissolved in nitric acid and then filtered. The aluminum is present in solution as Al3+. The solution is made basic with ammonium hydroxide, NH4OH, and the aluminum hydroxide, Al(OH)3 (FW 78.004), precipitates. This gel is filtered in a porous glass crucible, rinsed with dilute ammonium hydroxide, ignited, cooled in a desiccator, and weighed. The resulting alumina, Al2O3 (FW 101.94), weighed 0.1605 g. Why is the solution filtered after acid dissolution? To remove insoluble matrix material (like sand, etc.) 6. In #5, why rinse with ammonium hydroxide solution? To avoid peptization or loss of precipitate. Ammonium hydroxide is a volatile electrolyte. 7. In #5, what chemical transformation takes place during ignition? (Show the balanced chemical equation) 2Al(OH)3 -> Al2O3 + 3H2O 8. In #5, why use a desiccator during cooling? To avoid weight gain by adsorption of atmospheric water. 9. In #5, calculate the weight percent Al (AW 26.9815) in the sample.