use the following reaction for this question: 2AgCl + 1Zn -> 1ZnCl2 + 2Ag How many grams of zinc are needed in excess silver chloride solution to produce 1.0g of precipitated silver ?
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use the following reaction for this question:
2AgCl + 1Zn -> 1ZnCl2 + 2Ag
How many grams of zinc are needed in excess silver chloride solution to produce 1.0g of precipitated silver ?
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- 1,5419 g of magnetite (Fe3O4) ore; Fe+2 and Fe + 3 in concentrated HCL to form a mixtureit's unraveling. Adding HNO3 to all Fe +2s Fe +3 e and Fe+3 s NH, addingwith Fe(OH)3, precipitating into. Sediment in the form of Fe3O4 after necessary operationsand 0.8525 g. Calculate the percentage of Fe3O4 in the sample.what mass in grams of Na2S2O3 is needed to dissolve 4.7 g of AgBr in a solution volume of 1.0 L given that Ksp for AgBr is 3.3 x 10^-13 and Kf for [Ag(S2O3)2]^3- is 4.7 x 10^13?Which of the following statements is true about the solubility of CO2 (g) in H2O (l)?
- Give only typing answer with explanation and conclusion 0.1745 g of primary standard Na2C2O4 is used to set a freshly prepared KMnO4 solution and 30.24 mL of KMnO4 solution is spent at the turning point. Since 36.92 mL of this KMnO4 solution is consumed for the determination of iron in 0.5618 g ore sample, calculate the amount of iron in the ore in terms of % iron (III) oxide and % iron (III) chloride. (Fe: 56, K: 39, Mn: 55, O: 16, Na:23, C: 12, Cl: 35.5 g/mol)An acidic solution of copper (.35 M Cu+2) was treated with KOH until Cu(OH)2 precipitated. At what pH does this occur at?A student was given Mg, Zn, Fe, and Cu metals He put each of them in dil HCIcontained in different test tubes Identify which of them(i) will not displace 112 from dli HCI(ii) forms a pale green substance(iii) will give 112 with 5% 11N0(iv)will be displaced from its salt solution by all other metals
- Calculate the solubility (in g/L) of Aluminum sulfide (Al2S3) In 0.25 M Al+3 solution. (standard conditions.) {Ksp for Al2S3 is 1.5×10-27}.1. A newly discovered iron ore was weighted (5.408 g) and worked up to produced 0.3785 g of ignited Fe2O3 precipitate. What is the percent purity of the iron in the sample? 2. Distinguish between equivalence point and end point.What mass (in grams) of Na2S2O3 is needed to dissolve 0.44 g of AgBr in a solution volume of 1.0 L, given that Ksp for AgBr is 3.3×10−13 and Kf for [Ag(S2O3)2]3− is 4.7×1013?
- A 3.25 g sample of an iron-containing mineral was dissolved in an acid medium and calibrated to 500 mL. A 25.00 mL aliquot was titrated with 0.0025 M KMnO4 spending a volume of 9.32 mL. Subsequently, a 25.00 mL aliquot was passed through a Walden reducer to later titrate it with the same permanganate solution, using a volume of 14.15 mL for the titration. Determine the percentage of Fe(III) in the sample and report it as % Fe2O3To determine the amount of magnetite. Fe3O4, in an impure ore, a 1.5419 g sample is dissolved in concentrated HCl, resulting in a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize Fe2+ to Fe3+ and diluting with water, Fe3+ is precipitated as Fe(OH)3 using NH3. Filtering, rinsing and igniting the ppt provides 0.8525 g of pure Fe2O3. Calculate % Fe in the sample.Iron (55.845 g/mol) can be determined gravimetrically by precipitation as Fe(OH)3 (106.867 g/mol) and subsequent inflammation of the precipitate to convert it to Fe2O3 (159.69 g/mol). A 0.7873 g sample to be analyzed was weighed and transferred to a 400 mL beaker, where it was dissolved in 50 mL of H2O and 10 mL of 6M HCl. Then 2 mL of concentrated HNO3 was added to the solution. After boiling to remove excess HNO3 and nitrogen oxides, the solution was diluted to 200 mL, brought to boiling, and Fe(OH)3 was precipitated by the slow addition of 1:1 NH4OH solution until an odor of NH3 was detected (indicating the presence of excess NH3 in the medium). The solution was left in a water bath at 80 ºC for 30 min at rest. The precipitate was then filtered and washed with several portions of hot 1% m/v NH4NO3 until no Cl– was detected in the wash water. Finally, the precipitate was ignited at 500-550 °C, then left in a desiccator to cool and weighed as Fe2O3, resulting in a mass of 0.4512 g.…