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What quantity in moles is BaI2 present in ?
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- The thiourea in a 1.455-g sample of organic material was extracted into a dilute H2SO4 solution and titrated with 37.31 mL of 0.009372 M Hg2+ via the reaction. Calculate the percent (NH2)2CS (76.12 g/mol) in the sample. 4 (NH2)2CS + Hg2+ → [(NH2)2CS]4Hg2+25 mL of a bleach (NaOCl) sample is diluted to 500 mL. An excessive amount of KI is added to the 20 mL solution taken from here and the I2 released is titrated with 35.5 mL of 0.0409 M NaS2O3. Accordingly, calculate the weight percent by volume of NaOCl in the sample. (Ma(NaOC:74,4 g/mol)Calculate the weight of pure sodium carbonate that is necessary to prepare 2.806 L of 0.223 N Na2CO3 (105.99 g/mol) from the primary-standard solid. Assume the solution is to be used for titrations in which the reaction is: CO32- + 2H+ ----> H2O + CO2 Express you answers in 3 decimal places
- If 100.0 mL of 0.167 M Na2SO4 is added to 100.0 mL of 0.897 M Pb(NO3)2, How many grams of PbSO4 can be produced? ??2??4(??) + ??(??3)2(??) → 2????3(??) + ????4(?)a) convert 0.750 moles of CuCl2 to mass in grams. b) 25cm3 of sodium hydroxide solution of unknown concentration was filtrated with dilute sulphuric acide of concentration of 0.050 moldm-3 . 20cm3 was required to neturalie the sodiu hydroxide. calculate the concentration of the sodium hydroxide solution in moldm-3 nb. write the balanced equation use mole ratio to covert moles of sulphuric acid to moles of sodium hydroxide place moles in volume given cm3 then convert cm3 to dm350.0mL of 0.180 M sodium hydroxide solution is added to 50mL of .200 M lactic acid solution. The reaction goes to completion. It can be written CH3CHOH2H + OH ---> CH3CHOHCO2 + H2O What is the limiting reactant? How many moles of it were used?
- Sodium carbonate is a reagent that may be used to standardizeacids in the same way. In such standardization it was found that a 0.432-g sample ofsodium carbonate required 22.3 mL of a sulfuric acid solution to reach the end point forthe reaction.Na2CO3(aq) + H2SO4(aq) -----> H2O(l) + CO2(g) + Na2SO4(aq)What is the molarity of the H2SO4?1.00 grams of table salt was dissolved in 100 mL water and excess AgNO3 reagent was added and yielded 2.3789 grams of precipitate. Calculate the percentage of NaCl in the table salt. Answer must be in 2 significant figures.the thiourea in a 1.455-g sample of organic material was extracted into a dilute H2SO4 solution and titrated with 37.31 mL of 0.009372 M Hg21 via the reaction. Find the percentage of (NH2) 2CS (76.12 g/mol)in the sample?
- What is the minimum concentration of Ca2+ (M or mol/L) required to form a precipitate with a 0.025 M Na3PO4 solution? (Ksp for Ca3(PO4)2 is 1.0 × 10-26) Enter your answer as scientific notation with the correct number of sig figs, without any units. Use the format #e#TOPIC: GRAVIMETRY SHOW THE SOLUTION The mercury in a 0.7152-g sample was precipitated with an excess of paraperiodic acid, H5IO6, according to the following reactions:5 Hg+2 + 2 H5IO6 ---> Hg5(IO6)2(s) + 10 H+The precipitate was filtered, washed free of precipitating agent, dried and found to weigh 0.3408-g. Calculate the percentage of Hg2Cl2 in the sample. Molar Masses: Hg5(IO6)2 = 1448.75 Hg2Cl2 = 472.09 Answer: 38.82% Hg2Cl2 An iron ore was analyzed by dissolving a 1.1324-g sample in concentrated HCl. The resulting solution was diluted with water, and the iron (III) was precipitated as the hydrous oxide Fe2O3·xH20 by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.5394 g of pure Fe2O3. Calculate (a) % Fe, and (b) % Fe3O4 in the sampleMolar Masses: Fe2O3 = 159.69 Fe = 55.847 Fe3O4 = 231.54 Answer: 33.32% Fe and 46.04% Fe3O4The thiourea in a 1.455-g sample of organic material was extracted into a dilute H2SO4 solution and titrated with 37.31 mL of 0.009372 M Hg2+ via the reaction below. Find the percentage of (NH2)2CS (76.12 g/mol) in the sample. 4(NH2)2CS + Hg2+= (NH2)2CS 4Hg2+