How many grams of sample which contains 18.00% Na2O (61.98) should be taken for analysis in order to obtain a precipitate of Na3AsO3 (191.89) which weighs 0.3000 g?
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How many grams of sample which contains 18.00% Na2O (61.98) should be taken for analysis in order to obtain a precipitate of Na3AsO3 (191.89) which weighs 0.3000 g?
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- If a sample of silver coin weighing 0.2500 g gives a precipitate of AgCl weighing 0.2991 g, What wt of AgI could have been obtained from the same wt of sample?A sample of soluble salt weighs 1.2 g and contains chloride, bromide and iodide. With AgNO3, a precipitate is obtained which weighs 0.4500 g. On heating this precipitate with Cl2 gas, the AgBr and AgI are converted to AgCl, and the precipitate then weighs 0.3300 g. A similar sample, when treated with palladous chloride, precipitates only PdI2, and this precipitate weighs 0.0900 grams. (*)Find the approximate percentage of chlorine, bromine and iodine in the sampleThe mass of K3PO4 needed to prepare 250.0mL of an aqueous solution in which PO4-3 concentration is 0.0550M. The answer is ……………………… How many grams of silver sample is equal to 0.0417 mole of silver The answer is ……………………… When 38.0 mL of 0.1250 M H2SO4 is added to 100 mL of a solution of PbI2, a precipitate of PbSO4 forms. The PbSO4 is then filtered from the solution, dried, and weighed. If the recovered PbSO4 is found to have a mass of 0.0471g, what was the concentration of iodide ions in the original solution The answer is ……………………………… Express 96.342 m using 2 significant figures The answer is ………………………………. The oxidation number of sulfur in (Na2S2O5) is? The answer is ………………………………
- The arsenic in a 1.22-g sample of a pesticide was converted toAsO43- by suitable chemical treatment. It was then titratedusing Ag+ to form Ag3AsO4 as a precipitate. (a) What is theoxidation state of As in AsO43-? (b) Name Ag3AsO4 by analogyto the corresponding compound containing phosphorusin place of arsenic. (c) If it took 25.0 mL of 0.102 M Ag+to reach the equivalence point in this titration, what is themass percentage of arsenic in the pesticide?A 0.5g sample of CaCO3 is dissolved in an acidic solution. The calcium is precipitated as Ca2C2O4H2O and the dry precipitate is found to weigh 0,72. What is the percentage of CaO in the the sampleIf 20.0 mL of 0.250 M sodium chloride is added to 25.0 mL of 0.200 M silver (I) perchlorate, what mass (g) of precipitate will be formed?
- What happens when too much NaSCN is prepared in solution of mixtures of standard solutions of Fe(NO3)3 and NaSCN, so that [SCN^-] is higher than expected? What does this do to the measured Keq?What wt of magnetite should be taken for analysis in order that after converting to a precipitate of Fe2O3.xH2O, the percentage of Fe3O4 in the sample can be found by multiplying the wt in grams of the ignited precipitate (Fe2O3) by 100.What is the acid/base ratio? Why is it important in the titrimetric process? (Particularly in Double Indicator Titration Method in Determination of % SO3in a Soluble Sample)
- Calculate the percent yield when .631g of precipitate is collected from the reaction of 35.0ml of .100M silver nitrate and 45.oml of .0800M sodium bromide.The chloride in the sample is to be determined gravimetrically by precipitating and weighing AgCl. What weight in grams of sample should be taken so that the percentage of Cl is obtained by simply multiplying the weight of the AgCl precipitate by 10?Suppose that 0.323 g of an unknown sulfate salt is dissolved in 50 mL of water. The solution is acidified with 6 M HCl, heated, and an excess of aqueous BaCl2 is slowly added to the mixture resulting in the formation of a white precipitate. 1) Assuming that 0.433 g of precipitate is recovered calculate the percent by mass of SO42− in the unknown salt. 2) If it is assumed that the salt is an alkali sulfate determine the identity of the alkali cation.