1. Write a balanced chemical reaction for the precipitation of Fe (after the addition of ammonium nitrate). 2. Why is AgNO3 used to test the presence of Cl? Write the chemical reaction.
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1. Write a balanced
2. Why is AgNO3 used to test the presence of Cl? Write the chemical reaction.
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- Balance these equations by providing the missingcoefficients:(a) __ Fe1s2 + __O21g2¡__Fe2O31s2(b) __ Al1s2 + __ HCl1aq2¡__ AlCl31aq2 + __ H21g2(c) __ CaCO31s2 + __ HCl1aq2¡__ CaCl21aq2 +__ CO21g2 + __ H2O1l2Calculate for the theoretical yield of Rochelle salt (MW = 282.83) (a) that will be obtained from 6.6 grams of monohydrated Sodium carbonate (124.01). What is the reacting ratio? Refer to the choices below. (b) that will be obtained from 15g of Potassium bitartrate (MW = 188.10). Refer to the choices below. Rochelle salt: 2KHC4H4O6 + Na2CO3.H2O + 6H2O ---->2 C4H4O6KNa.4H2O +CO2 A 22.55 g B 25.47 g C 30.11 g D 32.64 gA weight of 0.50 g was taken impure container containing sodium carbonate and bicarbonate. Dissolved in water and then crushed with hydrochloric acid (0.1 N), the burette reading game was at the endpoint of phenolphthalein of 10.5 ml and at the end point of the orange methylation point 30.1 ml. The percentage of sodium carbonate was in ................. knowing that the weights are: Na: 23, C: 12, O: 16
- In the synthesis of benzoic acid, 3.5 mL of toluene were used and mixed with potassium permanganate solution. In making the potassium permanganate solution, 7 grams of the powder were dissolved in 150 mL of water. The resulting crystals were purified and the yield 1.53 grams. Identify the limiting reagent and compute for the number of moles that it consumed. What is the theoretical yield? What is the percentage yield? MW toluene = 94.14, density=0.87 g/mL , MW KMnO4 = 158, density = 2.7 g/mL , MW Benzoic acid = 122, density = 1.27 g/mLPls give with reason, the type and name of the reaction.Solid residue weighing 7.158 g from an aluminum refining process was dissolved in acid to give Al3+ in solution. The solution was treated with 8-hydroxyquinoline to precipitate (8-hydroxyquinoline)3Al (FM 462.462 g/mol), which was ignited to give Al2O3 (FM 101.961 g/mol) weighing 1.178 g. Find the weight percent of Al (FM 26.982 g/mol) in the original mixture.
- Potassium dichromate has several industrial applications. To determine the purity of the salt that will be used in different industrial processes, a sample mass equal to 2.660 g was dissolved and quantitatively transferred to a 500.00 mL flask. An aliquot of 25.00 mL of this solution was treated with excess KI and the released iodine was titrated with 0.1000 mol L-1 sodium thiosulfate, spending 27.00 mL. Calculate the purity of the analyzed salt. Data:K = 39.10 O = 16.00 Cr = 52.00 I = 126.9 S = 32.077 determination of sodium, potassium and calcium in water samples by ICP-OES. 1. kindly assist me with discussion in the experiment 2. results of the experiment 3 experimental/ methodologyCalcium oxalate monohydrate [Ca(O2CCO2)·H2O, also written as CaC2O4·H2O] is a sparingly soluble salt that is the other major component of kidney stones [along with Ca3(PO4)2]. Its solubility in water at 25°C is 7.36 × 10−4 g/100 mL. Calculate its Ksp. MW CaC2O4·H2O = 146.1 g/mol
- Congratulations, you have just been hired at a local laboratory. Your first task is to prepare 10.0 mL of a 1.50 x 10-6 M solution of a small protein (FW: 3600 g/mole). Available to you are an electronic balance that is accurate to the nearest 0.001 g, a 1.00-mL pipette, and 10-mL volumetric flasks. Describe how to prepare the desired solution. (Note that the amount of protein is so small that you will need to make a more concentrated stock solution and dilute it.)Uranium as U(VI) (as the uranyl ion; UO22+) is soluble and moves easily with groundwater, but U(VI) (as uraninite; UO2) is relatively insoluble. Several microorganisms are able to mediate this process. As such, in many uranium-contaminated aquifers, the reduction of soluble uranyl to insoluble uraninite by microorganisms has been proposed as a way to remove the dissolved uranium from water and keep it “locked up” in the subsurface. If the U(VI) is primarily complexed with carbonate (as UO2(CO3)34-), how does that influence the energy yield (or “reducibility”) of the U(VI), assuming “standard” conditions (i.e. not taking concentrations of any products or reactants into account? What about at pH 7? Under what kind of conditions would you expect to find UO2(CO3)34- vs UO22+ (and why)?Yttrium (III) carbonate (MM = 357.84 g/mol) has a Ksp of 1.0 x10-31. If 15.5 g Y2(CO3)3 is stirred into 2.16 L H2O, how many micrograms of yttrium (III) carbonate will dissolve?Report your answer to the nearest whole number.