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What would be the observation following mixing BaCl2 and Pb(NO3)2?
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- 1. A student synthesized 3.214g of Ni(NH3),C2 from 4.023g of NiCl2•6H2O. He dissolved 0.81g of Ni(NH3)nCl2 in 40 mL of 1.0M HCl to make a sample for analysis. Molar mass: Ni 58.7; Cl2 71; NH3 17; H2O 18. (1) A 0.20M Ni²* standard solution had an absorbance of 1.666, while his sample had an absorbance of 0.705. Calculate the Ni2+ concentration in his sample and the mass percent of Ni in the product. Note: A = ɛbc.3. Use the following atomic masses (in g/mol): As = 74.92; O = 16; K = 39.1; Cr = 52; Na = 23; Cl = 35.45; Ba = 137.33; S = 32.06, Twenty tabs of Ascorbic Acid weighed 4.25g and a powdered sample of 0.3075g consumed 21.5mL of 0.1085N I2 solution. What was the amount of ascorbic acid per dose of two tablets? Each mL of 0.1N I2 is equivalent to 8.803mg of ascorbic acid.1. The reaction below will give us: a. 2b. 4c. 3d. 3 and 4e. 1
- 4. If the following values are used... Measure the mass of 0.400 g of cobalt(II) nitrate hexahydrate (Co(NO;)2 -6H2O), and dissolve it in 15.0 mL of distilled or deionized water using a clean beaker. Using a graduated cylinder, measure out 10.0 mL of a prepared 0.10-M sodium phosphate (NazPO4) solution. ... determine which compound, (Na3PO4 or Co(N03)2 ·6H2O) will be the limiting reagent. Then determine the theoretical yield.You were assigned to assay a product sample of milk of magnesia. A 0.600-g sample was reacted with 25.00 mL 0.10590 N H2SO4. The excess unreacted acid in the solution required 13.00 mL of 0.09500 N NaOH when titrated to reach the methyl red end point. In terms of Mg(OH)2 content, does the sample product conform to the USP requirement? Justify your answer through calculations.1. It is assumed for the calibration solutions that all of the SCN is converted to FESCN2*. What would happen to the calculated Keq if this assumption were incorrect? 2. A student mixes 5.00 mL of 2.00 mM iron (III) nitrate with 5.00 mL of 2.00 mM sodium thiocyanate. The student determines that the concentration of FeSCN2* is 1.05x104 M. Calculate Keg-
- The digestion of a 0.1159 gram sample of a phosphorous-containing compound in a mixture of HNO3 and H2SO4 resulted in the formation of CO2, H2O, and H3PO4. Addition of ammonium molybdate yielded a solid having the composition (NH4)3PO4·12MoO3 (FW = 1876.3). This precipitate was filtered, washed, and dissolved in 50.00 mL of 0.2000 M NaOH: (NH4)3PO4•12MoO3(s)+26OH-(aq)->HPO42-(aq)+12MoO42-(aq)+14H2O(l)+3NH3(g) After the solution was boiled to remove the NH3, the excess NaOH was back-titrated with 14.84 mL of 0.1626 M HCl to a phenolphthalein end point. Calculate the percent phosphorous (FW = 30.9737) in the sample.Mass of KxFe(C2O4)y · zH2O : 4.70 g Mass of sample : 0.175 g Mass of FeCl3 used in preparation : 1.60 g Molarity of standard NaOH used : 0.100 V1, volume of standard NaOH required for first equivalence point : 7.750 mL V2, volume of standard NaOH required for second equivalence point : 19.70 mL Calculate the volume of standard NaOH that reacted with iron :Some people have an allergic reaction to the food preservative sulfite (SO32−). Sulfite in wine was measured by the following procedure: To 50.0 mL of wine were added 5.00 mL of solution containing (0.8043 g KIO3 + 5 g KI)/100 mL. Acidification with 1.0 mL of 6.0 M H2SO4 quantitatively converted IO3− into I3−. The I3− reacted with SO32− to generate SO42−, leaving excess I3− in solution. The excess I3− required 12.86 mL of 0.04818 M Na2S2O3 to reach a starch end point. lO_3^- + 8l^- + 6H^+ rightarrow 3l_3^- + 3H_2O l_3^- + SO_3^2 - + H_2O rightarrow 3l^- + SO_4^2- + 2H^+ l_3^- + 2S_2O_3^2- rightarrow 3l^- + S_4O_6^2- Find the concentration of sulfite in the wine. Express your answer in mol/L and in mg SO32− per liter._____mol/L HINTS: Don't use scientific notation, do put zero before decimal point, carefully evaluate significant figures.
- a) An aqueous solution contains 12.6 ppm of dissolved Ca(NO3)2 (which gives Ca21 1 2NO32). Find the concentration of NO23 in parts per million.(b) How many ppm of Ca(NO3)2 are in 0.144 mM Ca(NO3)2? (c) How many ppm of nitrate (NO23 ) are in 0.144 mM Ca(NO3)2?1. A student synthesized 3.214g of Ni(NH3)„Cl2 from 4.023g of N¡C12•6H2O. He dissolved 0.81g of Ni(NH3)nCl2 in 40 mL of 1.0M HCI to make a sample for analysis. Molar mass: Ni 58.7; Cl2 71; NH3 1T; H2O 18. (1) A 0.20M Ni²* standard solution had an absorbance of 1.666, while his sample had an absorbance of 0.705. Calculate the Ni2+ concentration in his sample and the mass percent of Ni in the product. Note: A = ɛbc. (2) The student used 38.75 mL of 0.498M NaOH to neutralize excess HCl in 40mL of the sample. Calculate the mass percent of NH3 in the product.(6) HBr (7) NaOH Na,Cr,0, (8) (9) H3C DMSO H2SO, CI