6. Mixing 25.00 ml of 0.1000 M NaOH with 20.00 mL of 0.8000 M HCI causes the temperature of the mixture (initially 25.00°C) to increase to 29.92°C. What is the enthalpy of neutralization for this reaction?
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- What would (triangle) Hrxn be for this new situation with 40 ml of both 1.0 M NaOH and 1.0 M HCl, Ccal=166.8, Tempertre final was 28.9 C, the initial temperature was 22.1 C.From the following data find the percentages of Na2CO3 and NaHCO3 in a mixture of these chemicals and inert constituents: a) A 0.5000 g sample required 45.50 mL 0.1050 N HCl to reach the methyl orange end point. b) 25.00 mL of 0.1000 N KOH is added to 0.2500 g of the sample; BaCl2 is added to precipitate the BaCO3 and 12.00 mL 0.1050 N HCl is required to reach the phenolphthalein end point.please draw (in chemical structures) the balanced reaction of mixture of 0.3 grams of thiamine hydrochloride in 0.45 mL of water and 3.0 ml of 95 percent ethanol and then add 2 M NaOH
- 1. A 0.3516 g sample of commercial phosphate detergent was ignited at a heat to destroy the organic matter. The residue was taken up in hot HCI which converted P to H3PO4. The phosphate was precipitated as MGNH4PO4.6H2O by addition of Mg+ followed by aqueous NH3. After being filtered and washed, the precipitate was converted to Mg2P2O7 by ignition at 1000 OC. This residue weighed 0.2161 g. Calculate the percent P (30.974) in the sample? Ans 17.11%Part A. Heat of Neutralization Table 1. Heat of neutralization data Sample 1 Sample 2 [1] Volume of HCI (mL) 50.2 50.2 [2] Temperature of HCI (°C) 24.8 24.3 [3] Volume of NaOH (mL) 49.8 49.9 [4] Temperature of mixture after reaction (°C) 31.8 31.0 Part B. Enthalpy of Solution of Salts Table 2. Enthalpy of solution of salts data FON*HN MgSO4 [1] Mass of salt (g) 2.000 2.001 [2] Volume of DI water (mL) 50.1 50.1 [3] Temperature of DI water (*C) 25.0 24.5 [4] Temperature of mixture after dissolution (*C) 22.0 31.2 Part C. Specific Heat of a Metal Enter the number corresponding to the identity of the metal. 1. Zinc 2. Aluminum 3. Steel 4. Tin [1] Mass of metal (g) 19.985 [2] Volume of DI water (mL) 49.8 [3] Tinitial metal ("C) 97.0 [4] Tinitial water (°C) 24.7 [5] Tinal of mixture after addition of metal (°C) 25.9Five drops of dichlorofluorescein have been added to a solution containing 0.800 g sample which required 25.30 mL of 0.100 M AgNO3. (c) Calculate the weight percent NaCl in the original sample.
- A 600.0 mg sample consist only of CaC2O4 and MgC2O4 was heated at 500°C converting the two salts to CaCO3 and MgCO3. The resulting precipitate weighed 465.0 mg. If the sample had been heated at 900°C, the products would be CaO and MgO, what would the mixture of oxides weigh? (FW: CaC2O4=128.1; MgC2O4=112.3; CaCO3=100.1; MgCO3=84.31; CaO=56.08; MgO=40.31)What is the Kc expression for the following reaction? 2 NO2(g) + H2O(1) --> HNO2(aq) + HNOglaq) [[HNO2(aq)] [HNOglaq)] [NO2(g)]^2 OHNO,(aq)] [HNO3(aq)] [NO2(g)]^2 (H20(10) (HNO2(aq)) [HNOglaq)] 2 [NO2(g]]^2 [H2O(1) [HNO2(aq)) + [HNO3laq)] 2 INO2(g)] + [H20()]1. Calculate the solubility of calcium carbonate water temperature of 5 °C; at that temperature, Ksp = 8.1 x 10-9 for CaCO3, Ka = 2.8 x 10-11 for HCO3-, and Kw = 2.0 x 10-15
- 9. An aqueous solution of sulfuric acid is prepared by mixing a secondary standard of sulfuric acid with deionized water. The aforementioned acid is to be used as a titrant hence its concentration must be accurately determined. To do this, Engr. Polinar, standardized the titrant by titrating two liters of ammonia at 0.90 atm and 30 deg C. From the experiment, 134 mL of the titrant was necessary to neutralize the ammonia. Determine the concentration of the acid in terms of normality? 10. Engr. Forcadela is optimizing a plastic formulation by manipulating the phosgene concentration injected as a gas during the reaction. To obtain credible results, he considered the propensity of phosgene to dissociate into carbon monoxide and chlorine gas at 395 deg C. Performing an experiment at the aforementioned temperature, an equilibrium is reached amongst the species where the total pressure is at 3 atm. If the equilibrium constant expression in terms of concentration for the reaction at 395 deg C…Based on your knowledge of acid strength, which correctly pairs each acis with its Gibbs Free Energy of ionization in aqueous solution? I. HI (AG° = 8 kJ); HF (AG° =-71 kJ); HCI (AG° - -53 kJ) II. HI (AG° = -53 kJ); HF (AG° =-71 kJ); HCI (AG° = 8 kJ) II. HI (AG° = -71 kJ); HF (AG° = 8 kJ); HCI (AG° = -53 kJ) IV. HI (AG° = -53 kJ); HF (AG° = 8 kJ ); HCI (AG° = -71kJ)(a) In performing a titration, why is it better to use a solution of a concentration such that 30-45 mL is required, instead of a more concentrated solution that might only require about 5 mL to reach the end point? (b) To make a standardized NaOH solution, why is it better to prepare a NaOH solution of approxi- mate concentration and then standardize with KHP, rather than to weigh accurately some NAOH pellets, dissolve them, and dilute the solution in a volumetric flask? (c ) In analyzing a 0.003 weak acid by titration with 0.00300 M NaOH, why would you be able to obtain greater accuracy by using a pH meter instead of using a color-change indicator such as phenolphthalein?