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Compare and contrast an anticipatory standard to a reactionary standard by listing and describing some advantages and disadvantages.
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- 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…7-11. Limestone consists mainly of the mineral calcite, CaCO3. The carbonate content of 0.541 3 g of powdered limestone was measured by suspending the powder in water, adding 10.00 mL of 1.396 M HCI, and heating to dissolve the solid and expel CO2: CACO3 (s) +2H* → Ca²* +CO,T +H2O Calcium carbonate FM 100.086 The excess acid required 39.96 mL of 0.100 4 M NaOH for complete titration to a phenolphthalein end point. Find the weight percent of calcite in the limestone.Distinguish between a. Equivalence point and end point b. Primary standard and secondary standard
- Give some examples of secondary standard solutions, and give the reasonCalculate: 1)mean Experimental solubility of calcium hydroxide 2)Standard deviation 3)RSD(pph)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%
- 4. An experiment similar to the one described in this module was performed to determine the solubility and solubility product constant of lead(1l) chloride (gmm = 278.10). The equilibrium involved is PbCl2(s) = Pb2+ (aq) +2 CI¯(aq) The dissolved chloride in the filtered solution was quantitatively precipitated as AgCl by the addition of excess AgNO3 solution. The solid AgCI was filtered from solution, dried, and weighed. The following data were obtained for three samples of the filtered, saturated solution. determination 1 2 temperature of solution, °C volume of PbCl2 solution analyzed, mL mass of dry A£CI, g 20.2 20.4 20.1 25.00 22.00 20.10 0.2543 0.2276 0.2051 Calculate the following: number of moles of: AgCl(s) CI- (aq) Pb2*(aq) [CI"] in PbCl2 solution, M [Pb2+] in PbCl, solution, M Ksp average Ksp solubility of PbCl2, in g per 100 mL chemistry handbook value for solubility at 20°, g per 100 mLA student performed a titration to determine the exact concentration of NaOH(aq). The titration was performed against a standard 0.1000 M HCl(aq) solution. Phenolphthalein indicator was used. The following end-point volumes were recorded by the student in units mL: Trial Number Volume 1 25.06 2 25.15 3 25.02 4 25.17 5 25.07 Calculate the 95% confidence limit. Assume that there is no outlier. Provide your answer to the correct number of decimal places, without units, and without the ± sign. Use the T-table shown below.For the CO2 impact experiment station: 1) Obtain two plastic cups, red cabbage indicator, a straw, and plastic wrap. 2) Fill each cup approximately one-quarter to one-third full of tap water and add ~10 mL of the red cabbage indicator. 3) Place the two cups side by side on a sheet of white paper. 4) Place the straw into one of the beakers and cover that beaker with the plastic wrap. 5) Carefully blow bubbles into the test cup for 3 min. and observe both cups. 6) Compare the color to the control cup and record any differences. This the Question: Did the beaker with the solution into which CO2 was bubbled change pH/color? By how much? Is this what, you would predict, based on your knowledge of the chemistry of CO2?
- 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)A chemist received different mixtures for analysis with the statement that they contained NaOH, NaHCO3, Na2CO3, or compatible mixtures of these substances, together with inert material. From the data given, identify the respective materials, and calculate the percentage of each component. 1.000g samples and 0.2500N HCl were used in all cases. (A) For Sample W: With PP, 24.32ml was used. A duplicate sample required 48.64ml with MO. (B). For Sample X: The addition of PP caused no color change. With MO, 38.47ml of the acid was required. (C). For Sample Y: To cause a color change in the cold with PP, 15.29ml of the acid was necessary, and an additional 33.19ml was required for complete neutralization. (D) For Sample Z: The sample was titrated with acid until the pink of PP disappeared; this process required 39.96ml. On adding an excess of the acid, boiling, and titrating back with alkali, it was found that the alkali was exactly equivalent to the excess acid added.The pH of the river adjacent to the site is governed by the carbonic acid/bicarbonate buffer system as well as dissolved ions from the surrounding environment. Carbon dioxide from the atmosphere dissolves in river water to form carbonic acid by the following equilibrium: CO2{ag) + H20 S H2CO3(ag) pkа1 - 2.77 Carbonic acid dissociates in water to form the bicarbonate and carbonate ions by the following equilibrium reactions. Н2СОЗ(ag) + H205 нЗО + (ag) + нсоЗ- (ag)— pKa2 = 3.70 НСОЗ - (ag) + H20— НЗО + (ag) + соЗ 2- (аg) pКа3 %3D10.33 (a) The following equilibrium accounts for the fact that carbon dioxide is in equilibrium in carbonic acid when dissolved in water. CO2(ag) + 2H20 S H30 + (ag) + HCO3 - (ag) K = ? Calculate the value of the equilibrium constant, K for this reaction. Show all working (b) The carbonic acid/bicarbonate buffer system is depicted by pKa2. However, only 0.2% of the absorbed CO2 is converted to H2CO3 with a corresponding Ka = 4.46 x 10-Z: Write an expression for…