500 g calcium polysulphide and 1.5 kg hydrochloric acid 343.4g precipitated sulfur 250 mg per Precipitated sulfur 1U0 jars per box Ointment jar IC. SYNTHE SIS AND PACKAGING Balanced Chemical Reaction % composition by mass of each compound Mass to Mass Stoichiometry Calculation Limiting Reagent Excess Reagent Amount (g) in excess % Yield Number of dosage form and packaging that can be produced from stoichiometric calculation

500 g calcium polysulphide and 1.5 kg hydrochloric acid 343.4g precipitated sulfur 250 mg per Precipitated sulfur 1U0 jars per box Ointment jar IC. SYNTHE SIS AND PACKAGING Balanced Chemical Reaction % composition by mass of each compound Mass to Mass Stoichiometry Calculation Limiting Reagent Excess Reagent Amount (g) in excess % Yield Number of dosage form and packaging that can be produced from stoichiometric calculation

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.23QAP

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On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
Sodium bicarbonate (baking soda), NaHCO3, can be purified by dissolving it in hot water (60 C), filtering to remove insoluble impurities, cooling to 0 C to precipitate solid NaHCO3, and then filtering to remove the solid, leaving soluble impurities in solution. Any NaHCO3 that remains in solution is not recovered. The solubility of NaHCO3 in hot water of 60 C is 164 g/L. Its solubility in cold water of 0 C is 69 g/L. What is the percent yield of NaHCO3 when ills purified by this method?
A sample of magnetite (impure Fe3O4) weighing 0.4500 g is fused with oxidizing flux and the ferric compound formed is eventually precipitated as ferric hydroxide and ignited to ferric oxide (Fe2O3MM 159.70 g/mol) which weighs 0.4890 g. Calculate % Fe. At. mass Fe 55.85 O 16.00
ce Carrington -STOICHIOMET X wer.html?state=%7B"ids"%3A%5B"1J1faQoGnmRQnPpCs1180ZWUfe Z8de9E"%5D%2C'action"%3A'open"%2 Carrington - STOICHIOMETRY WORKSHEET#1.doc 3. How many formula units of CuCI can be produced by 75.0 g of Cu O? Cu20 + HCI → CuCl + H2O 4. If 35.0 g of oxygen gas is produced by the following reaction, how many liters of hydrogen gas are produced? H2O → H2 + O2
(6) total lonio al 1unio eanATion (C) ne t lonio componnd 24. NH4OH Co(NO,)2 (a) balancedeauation (b) total lonlceauation ccl net lonic eauation
An essentially 100% yield is necessary for a chemicalreaction used to analyze a compound, but it is almostnever expected for a reaction that is used to synthesizea compound. Explain this difference
Active Ingredient Actual Yield Formulatio Dosage Form Packaging Raw Materials n 1.5 kgs cream of tartar and 2.5 kg sodium carbonate monohydrate 1.20 kgs Seignette salt 160 mg per 5 mL 100 ml per Seignette salt Syrup bottle SYNTHESIS AND PACKAGING Balanced Chemical Reaction % composition by mass of each compound Mass to Mass Stoichiometry Calculation Limiting Reagent Excess Reagent Amount (g) in excess % Yield Number of dosage form and packaging that can be produced from stoichiometric calculation
+. ca(NO3), ,+ ?H3PO4 Caz(poht_+HNO3 -> Whan the eguation is balanced, the coefficient in frot of H3P04 is ?
Active Raw Materials Actual Yield Formulation Packaging Dosage Form Ingredient Aspirin 2 kgs. Salicylic acid and 2.5 kgs. acetic anhydride 1180 g aspirin 80 mg per tablet Tablet 20 tablets per blister pack IC. SYNTHESIS AND PACKAGING Balanced Chemical Reaction % composition by mass of each compound Mass to Mass Stoichiometry Calculation Limiting Reagent Excess Reagent Amount (g) in excess % Yield Number of dosage form and packaging that can be produced from stoichiometric calculation
| Log In Q Englis 6 Self-Se G Gramn Tn Cours G traduc Build a C How M Co x G Eleme Balanc Parapl ge.com/course.html?courseld%=17244391&0penVellumHMAC=c6d3335eldc533558bc46d6c41bbfdf9#10001 E Reading list + Stoichiometry Review | Constants | Periodic Table raLA How many O2 molecules are needed to react with 6.73 g of S? Elemental S reacts with O2 to form SO3 according to the reaction Express your answer numerically in units of molecules. 25 + 302-2S0, > View Available Hint(s) as depicted here (Figure 1) 0.210 molecules Submit Previous Answers Figure X Incorrect; Try Again; 5 attempts remaining The value entered is the number of moles of S in 6.73 g. You need to find the number of molecules of O, needed to react with 6.73 g of S. 1 of 1 You may want to review Hint 4How to convert moles to moleciules Part B Oxygen Sulfur What is the theoretical yield of SO, produced by 6.73 g of S? Express your answer numerically in grams. Pearson O vA 3:48
15. A 94.6 grams of silver 126.4 of in the cess? - 230Lused) %3D7.79excess Al requi unbalanced equation: AgNO:(aq) + KBr(aq)→ AgBr(s) + KNO:(aq) a. Which reactant is limiting? Which reactant is in excess? b. What is the theoretical amount of AgBr(s) produced given the limiting reactant. If a student reported 15.5grams of the AgBr(s) being produced, what is the percent yield? c.
what mass of On is required for the Complete combustion of 59,79of pentane, CgH2. to cO. and HgO PP.0 of