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- From 0.8 av. lb of 20% w/w KOH solution, 72.6 O 121 142 86.2 Next g of 12 percent w/w KOH may be produced.Caustic potash that has been exposed to air is found on analysis to contain 90.00% KOH, 2.38% K2CO3 and 7.62% H2O. What weight of residue will be obtained if 1.00 g of this sample is added to 46.00 mL of 1.00 N HCl and the resulting solution, after neutralization with 1.070N KOH is evaporated to dryness?1. A student synthesized 3.214g of Ni(NH3)„Cl2 from 4.023g of N¡C12•6H2O. He dissolved 0.81g of Ni(NH3)nCl2 in 40 mL of 1.0M HCI to make a sample for analysis. Molar mass: Ni 58.7; Cl2 71; NH3 1T; H2O 18. (1) A 0.20M Ni²* standard solution had an absorbance of 1.666, while his sample had an absorbance of 0.705. Calculate the Ni2+ concentration in his sample and the mass percent of Ni in the product. Note: A = ɛbc. (2) The student used 38.75 mL of 0.498M NaOH to neutralize excess HCl in 40mL of the sample. Calculate the mass percent of NH3 in the product.
- FSC 8 1921. Brightspace A Aktiv Chemistry C D Z < Q + # At F2 @ 2 What volume in mL of 0.3000 M NaCl solution is required to produce 0.2700 moles of NaCl? W S app.101edu.co Walmart - Hiring Ce... X F3 X # 3 11. Unit 12: Late Adulthood - Develo X E JC 4 D F4 с 144 $ JU F5 R LL F ► 11 % 5 V F6 t 44 T G A 6 F7 Simulation play - Labster B Y H F8 & 7 8 U N Question 7 of 9 DELL F9 X D * 8 J F10 ( M Walmart - Hiring Center 9 F11 JI K 2 O ) O F12 L P 4 : 7 +/- PrtScr W 8 Insert { ( **A516.7 mg sample containing a mixture of K2SO, and (NH4)2S0, was dissolved in water and treated with BaCl2,precipitating the S042- as BaSO4. The resulting precipitate was isolated by filtration, rinsed free of impurities, and dried to a constant weight, yielding 863.5 mg of BaSO4. What is the %w/w K2SO4 in the sample?Approximately 6 mL of conc. perchloric acid ( 72% ) was transferred to a bottle and diluted with about 1 liter of water. A sample containing 251.5 mg of primary standard Na2B4O7.10H2O (Fwt= 382g/mol) required 27.41 mL of the HClO4 solution to reach the methyl red end point. What is the molar concentration of the HClO4 solution? Na2B4O7.10H2O + HClO4 ------------> NaClO4 H2B4O7.10H2O
- . 1.066-g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous Al2O3 xH2O. The precipitate was filtered and ignited at 1000°C to give anhydrous Al2O3, which weighed 0.1000 g. Express the result of this analysis in terms of: a. % NH4 Al(SO4)2 =| b. % Al2O3 = % % c. % Al = %An impure sample of calcium carbonate with a mass of 7.95 g was reacted with 50.00 cm3 of 1.00 mol dm hydrochloric acid (an excess). The resulling solution was transferred to a volumetric flask and titrated with 11.10cm3 of 0.300 mol dm-3 sodium hydroxide solution. Determine the percentage purity by mass of the calcium carbonate sample.CaCO3 + HCl -> CaCl2 + H2O + CO2 HCl + NaOH -> NaCl +H2O a. Determine how many moles of hydrochloric acid were used.b. Determine how many moles of excess HCI was titratedc. Determine how much in moles calcium carbonate present in the sample.d. Calculate the mass of calcium carbonate presente. Determine the percentwge calcium carbonate is in the sample.How to prepare 250cm3 of a solution of carbonate with concentration 0.100 mol dm-3
- The aluminum in a 1.200-g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous Al2O3.xH2O. The precipitate was filtered and ignited at to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysis in terms of %NH4Al(So4)2 %Al2O3 %AlThe aluminum in a 1.200 g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous Al(OH)3.xH2O. The precipitate was filtered and ignited at 10000C to give anhydrous Al2O3 which weighed 0.1798 g. Express the result of this analysis in terms of % Al2O3.b My Questi x Co. How to Ca X N NSU Login X PeriodicTa X M Action Re x 0 mySigTau XG 4.25 ml to X ( NBA FinalX G scientific X + enow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator%3Dassignment-take [References] A 1:1 mixture by moles of nitrous oxide and oxygen is often used as a sedative in dentistry. If the total pressure of this mixture in a cylinder is 3.75 atm, what is the partial pressure of each gas? Partial pressure of nitrous oxide = atm Partial pressure of oxygen = atm Submit Answer Try Another Version 3 item attempts remaining Previous Next Email Instructor Save and Exit Cengage Learning | Cengage Technical Support