1) The fizz produced when an Alka-Seltzer tablet is dissolved in water is due to the reaction between NaHCO3 and citric acid CO:(8) + H;O(I) + Na,C,H;O,(aq) NaHCO3(aq) + H;C,H;O,(aq) a) In a certain experiment 1.00 g of NAHCO3 and 1.00 g of citric acid are allowed to react. Which is the limiting reactant? b) How many grams of sodium citrate (the last compound in the equation) form? c) How many grams of the excess reactant remain after the limiting reactant is completely consumed? d) If 0.723 g of sodium citrate was obtained in this reaction, then what is the percentage yield?,

1) The fizz produced when an Alka-Seltzer tablet is dissolved in water is due to the reaction between NaHCO3 and citric acid CO:(8) + H;O(I) + Na,C,H;O,(aq) NaHCO3(aq) + H;C,H;O,(aq) a) In a certain experiment 1.00 g of NAHCO3 and 1.00 g of citric acid are allowed to react. Which is the limiting reactant? b) How many grams of sodium citrate (the last compound in the equation) form? c) How many grams of the excess reactant remain after the limiting reactant is completely consumed? d) If 0.723 g of sodium citrate was obtained in this reaction, then what is the percentage yield?,

EBK A SMALL SCALE APPROACH TO ORGANIC L

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Chapter13: Isolation Of Eugenol From Clov

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Lakes that have been acidified by acid rain can be neutralizedby the addition of limestone (CaCO3). How muchlimestone in kilograms would be required to completelyneutralize a 5.2 * 109-L lake containing 5.0 * 10-3 g ofH2SO4 per liter?
Consider Palmitic acid C16H32O2, a common fatty acid used in the manufacture of soap. A solution of palmitic acid is prepared by mixing 112 g palmitic acid with 725 mL of benzene C6H6. The density of the resulting solution is 0.902 g/mL. Palmitic acid (molar mass = 256 g/mol and density = 0.852 g/mL); Benzene (molar mass = 78 g/mol and density = 0.879 g/mL) What is the %m/m of the solution? Final answer must be rounded off to 1 decimal place, and shall NOT have any unit.
8. The data in the table below was obtained for the reaction: A + B → P
7. Given that the kf of water in a car radiator filled with liquid in the ratio of 62 g of ethylene glycol (HOCH₂ CH₂OH) in 500 g of water is.... (A) -0.93 °C (B) -1.86 C (C) -3.73 C (D) -7.64 °C (E) -5.58 C
Consider Palmitic acid C16H32O2, a common fatty acid used in the manufacture of soap. A solution of palmitic acid is prepared by mixing 112 g palmitic acid with 725 mL of benzene C6H6. The density of the resulting solution is 0.902 g/mL. Palmitic acid (molar mass = 256 g/mol and density = 0.852 g/mL); Benzene (molar mass = 78 g/mol and density = 0.879 g/mL) A. What is the %m/m of the solution? B. What is the molarity of the solution? C. What is the mole fraction of the solvent?
A sample of an industrial waste water is analyzed and found to contain 16.5ppb Fe2+. How many grams of iron could be recovered from 1.81×103 kg of this waste water? Answer:_______ grams Fe
Consider Palmitic acid C16H32O2, a common fatty acid used in the manufacture of soap. A solution of palmitic acid is prepared by mixing 112 g palmitic acid with 725 mL of benzene C6H6. The density of the resulting solution is 0.902 g/mL. Palmitic acid (molar mass = 256 g/mol and density = 0.852 g/mL); Benzene (molar mass = 78 g/mol and density = 0.879 g/mL) 1. What is the % m/m of the solution? 2. What is the mole fraction of the solvent? 3. What is the molarity of the solution? Based from the calculated molarity of the solution in #3, you are to prepare 250 mL of the said molar concentration. If you have an available 2M stock solution of Palmitic acid, How many mL of the 2M palmitic acid stock solution will you need? and; 4. How many mL of solvent do you need to add to the amount gotten from the 2M Palmitic acid stock solution in order to prepare 250 mL total volume of your desired solution?
Calcium peroxytoctahydrate is synthesized according to the following reaction. During the synthesis based on 3.5 g calcium carbonate, 7.5 mL of 18% HCl with a density of 1.19 and 5.5 mL of 25% NH3 with a density of 0.91 were used, and further hydrogen peroxide and excess water were added to the medium. Since 2.35 g of calcium peroxytoctahydrate is obtained in this way, what is the% yield of the experiment? (HCl: 36.5 g/mol; NH3: 17 g/mol; CaCO3: 100 g/mol; CaO2.8H2O: 216 g/mol) CaCO3 + 2HCl 2NH3 + H2O2 + 7H2O → CaO2.8H2O + CO2 + 2NH4+ + 2 Cl-
Knowing that the reaction yield: FeS2 + O2 → Fe2O3 + SO2 is 75%, from 360 g of iron disulfide, calculate: a) The amount of iron (III) oxide produced. b) The volume of SO2, measured at 0 ºC and 1 atm, that will be obtained.
When a Vitamin C (ascorbic acid; MM = 176.12 g mol-1) tablet is crushed, dissolved and titrated with 0.0340 M KIO3(aq) to a purple/blue endpoint (given by a starch indicator), the volume of KIO3 used is 29.80 mL. If 60 mg of ascorbic acid is the recommended dietary allowance (i.e., 100% of the RDA), then what is the % RDA for the Vitamin C in the tablet? KIO3(aq) + 5 KI + 6 H+ → 3 I2(aq) + 3 H2O I2 (aq) + ascorbic acid → 2 I- + dehydroascorbic acid
Write the empirical formula for the hydrated KAl(SO4)2, based on moles of anhydrous KSI(SO4)2= 0.046 mol molar mass of H2O= 18g/ mol moles of H2O= 0.0444mol ratio pf moles H20 to moles of anhydrous KAI(SO4)2= 9.65/1 . Show all work including units. Hint: if the ratio of moles of H2O to moles of anhydrous KAl(SO4)2 was 4, then the empirical formula would be: KAl(SO4)2•4H2O.
18.2 Balance the following chemical equation for the stoichiometric combustion of methane with oxygen. ____ CH4(g) + ______O2(g) ⟶ ______ CO2(g)+ ______H2O(g) What are the coefficients for O2(g) and CO2 (g)?

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