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- How many grams of A1C13 are produced from 55.5 mL of a 3.6 M HC1 solution? 2A1+ 6HCI→2AICI,+3H,The first goal is to make the oxalic acid standard solution. You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. Molar mass of H2C2O4•2H2O = 126.07 g/mol Mass of H2C2O4•2H2O = 1.5232g Volume of H2C2O4•2H2O solution = 250.0mL What is the Molarity H2C2O4 standard solution ?The first goal is to make the oxalic acid standard solution. You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. Molar mass of H2C2O4•2H2O = 126.07 g/mol Mass of H2C2O4•2H2O = 1.5232g what is the Number of moles of H2C2O4•2H2O?
- Calculate the final molarity of H2O2H2O2 if 5.2 mL5.2 mL of a 3.0% w/w H2O23.0% w/w H2O2 solution, which has a density of 1.0 g/mL,1.0 g/mL, is added to 5.2 mL5.2 mL of a starch-iodide solution.A 500-mg tablet of commercial vitamin C tablet was dissolved in 50 mL water, treated with excess KI solution and 3 drops of starch solution. The solution required 4.8 mL of 0.05 M KIO3 to reach the endpoint. Calculate the % by weight of vitamin C in the tablet. (Molar mass of vitamin C = 172.16 g mol-1) IO3‐ + 5 I‐ + 6 H+ → 3 I2 + 3 H2O (1) I2 + C6H8O6 → C6H8O6* + 2 H+ + 2 I‐ (2) I2 + starch → (I2 - starch) (deep blue color) (3) *oxidized product of vitamin CMagnesium Chloride is available as magnesium chloride hexahydrate in an injectable solution that supplies 1.97 mEq of magnesium per milliliter. What is the percent strength of magnesium chloride hexahydrate in this solution?
- 25.00 mL of a solution containing 3.6 M H2O2 What mass of a 30.00% (w/w) hydrogen peroxide solution is required to provide the mass calculated above. (Start with the amount from the prvious question) (a30.00% w/w solution means 30.00gsolute/100 gsolution)? ( Keep an extra digit)A 2.00 L bottle of soda when cold (0 °C), has a CO2 concentration of 0.105 M. When the bottle is opened andheated to 50 °C, most of the CO2 leaves the solution, and the CO2 concentration drops to 0.026 M. How manyGrams of CO2 bubbled out and left the solution? Use stiochemistry with divider lines in between numbers for the conversion factors and the answer is 7.0g CO210) The following questions use the balanced chemical equation below.3 Cu(NO3)2 + 2 K3PO4 º 6 KNO3 + Cu3(PO4)2(a) Calculate the volume of 0.750M Cu(NO3)2 solution required to react completely with 2.48L of a 1.19MK3PO4 solution. Use stiochemistry with divider lines in between numbers for the conversion factors (b) How many grams of Cu3(PO4)2 will be formed from the complete reaction of 18.5 mL of a 0.625MCu(NO3)2 solution?Use stiochemistry with divider lines in between numbers for the conversion factors The answer is 10a. 5.90L 10b. 1.47g 11) The following questions use the balanced chemical equation below.Zn + 2 HBr º…a) A matriculation student carried out an experiment involving a reaction between an acid and a base as shown in the following reaction: CH;COOH(aq) + NaOH(aq) → CH;COONA(aq) + H2O(1) In this experiment, 20.0 cm of 2.0 M of NaOH solution was added to 30.0 cm of 1.00 M CH3COOH solution in a plastic eup. A maximum rise of 5.8°C in temperature was recorded. [Heat capacity of the plastic cup = 37.30 J°C-!. Assume density of solution = density of water] (i) Name the enthalpy for this reaction. (ii) Calculate the standard enthalpy for this reaction.
- 1. Copper metal and aqueous iron (III) chloride were made to react to reduce iron to Fe²+ while oxidizing copper to Cu²+. What mass (in g) of copper metal is needed to react with 50 mL of 20.5 wt.% iron (III) chloride (solution density is 2.9 g/mL)?6. A water has the following composition: lon meq/L Cat+ 2.1 Mg** 1.3 Nat 0.8 -1 HCO3-¹ 1.9 SO42 1.8 CI 0.5 What are the values of TH, CH, NCH and alkalinity (Alk) in units of meq/L ? _meq/L _meq/L _meq/L ΤΗ CH NCH ALK _meq/L 10A 0.2088 g sample of primary-standard-grade sodium carbonate, Na₂CO₃ (105.99 g/mol) was dissolved in water and diluted to 100.00 mL in a volumetric flask. A 30.00-mL portion of this solution was used to standardize a hydrochloric acid (HCl) solution based on the following reaction: CO₃²⁻ + 2H⁺ → H₂O + CO₂. If 36.09 mL of the HCl solution was used to reach the end point, what is the molarity of the HCl?