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Mass solute needed to prepare 0.500L of 0.2 M NaCO3 from a solid NaCO3 with a purity of 92.0wt%
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- A solution is made by dissolving 0.455 g of PbBr2 in 100 g of H2O at 50C. Based on the data in Table 8-1, should this solution be characterized as a. saturated or unsaturated b. dilute or concentratedA 12.63 g sample of calcium ore was dissolved in HCl and gravimetrically analyzed, through the precipitation of calcium into CaC2O4 · H2O. The precipitate was filtered, washed, dried, and ignited at 500 oC until the weight was constant, giving a final mass of 2.35 grams pure CaCO3 (100.087 g/mol). Calculate the % Calcium (40.078 g/mol) in the sample.How much amount of solids (in grams) do you need to prepare the following solutions? 1. 500.0 mL 0.1000 M stock EDTA solutiona. Weigh an appropriate amount of Na2H2EDTA2H2O (FW=372.24) to the nearest 0.1 mg 2. 100.0 mL 0.0500 M stock Ca2+ solutiona. Weigh appropriate amount of pure CaCO3 (FW=100.09) to the nearest 0.1 mg into a 250 mL beaker.
- Precipitimetry The chloride in a 4.321-g food sample was precipitated through the addition of 50.00 mL of a standard AgNO3 solution (10.00 mL AgNO3 = 11.22 mL KSCN). The precipitate was coated with nitrobenzene and the mixture was diluted to 250.0 mL. A 50.00 mL aliquot was taken from the diluted solution and required 4.56 mL back titration with a %3D standard KSCN solution (22.33 mL KSCN = 0.9758 g AgNO3). %3D Formula Masses: AgNO3 = 169.87; CI = 35.45 Calculate the following: 1. Molar concentration of KSCN solution M %3D 2. Molar concentration of AgNO3 solution M %3D 3. % (w/w) chloride in the original sample =148. Addition of 50.00 mL of 2.238 m H2SO4 (solution density = 1.1243 g/mL) to 50.00 mL of 2.238 M BaCl2 gives a white precipitate. (a) What is the mass of the precipitate in grams? (b) If you filter the mixture and add more H2SO4 solution to the filtrate, would you obtain more precipitate? Explain.e 6.30 L of 0.262 M NaOH from the concentrated commercial reagent [50% NaOH (w/w), sp gr 1.525]. Take mL of the concentrated reagent and dilute to 6.3 L with water. f 3.90 L of a solution that is 16.0 ppm in K*, starting with solid KĄ Fe (CN),. Dissolve mg K4 Fe (CN)6 in enough water to give a final volume 9, of 3.9 L.
- The aluminum in a 1.200-g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous Al2O3.xH2O. The precipitate was filtered and ignited at to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysis in terms of %NH4Al(So4)2 %Al2O3 %AlEmpirical formula is 6C. % of Sulphur= [S] x 100 S0.0- yd ebivic 32 x 100% = 50%m %3D [1 (32) +2(16)] (CH,)n=2x42 [Hint: M,= 2x V.D] (12+2)n=84; n=6; hence compound is C,H,2 Mg + 2HCI → MgCl, + H, 7A. 8. From the equation: alumoeluaalch = slumot leohioma 1mol Mg produces 1mol H, Or 24g Mg produces 22.4dm' H, ei sid 9B. Compare Q57 n negyoro lo on lsic CHAPTER 3 eo to easm yd. THE ATOMIC STRUCTURE. ELECTRONIC CONFIGURATION. PERIODICITY OF ELEMENTS. - The periodic classification of the elements is an arrangement of the elements in order of their A. atomic weights B. isotopic weights C. molecular weight D. atomic numbers E. atom masses (1978:Q5) SD . The nucleus of an atom contains A. protons only B. neutron only C. protons and electrons D. neutrons and electrons E. protons and neutrons not iso(1978:Q28) - The size(diameters) of five atoms are in order RFrom 0.8 av. lb of 20% w/w KOH solution, 72.6 O 121 142 86.2 Next g of 12 percent w/w KOH may be produced.3 Bal, (aq)+ 2 Nag POq Caq) 7 BalPO42 + l6 Nal laq • Consider the reaction of 30.0mL of 0.270M Balz with 20.0 mL of 0.3ISM Naz PO4. Lwhat quantity in meles of Balz are preset in the solution? are produced /What quantitg in moles of precipitate E ali Bal were consumed based on the balanced chomical equation? 6) What auantity in males of Na3 Pla aro present in soluction? d) What quantity in moles of precipitate are paduced if all the Naz PO, were cansumed based on the balanced chemi.cal equation? e) which reactant is limisting f What mass (in g) of precipitate is firemed when the limiting reactant is considered?A solution was prepared by dissolving 367 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 750.0 mL. Calculate (a) the molar analytical concentration and Normality of K3Fe(CN)6. (b) the molar concentration of K+. (c) the molar concentration of Fe(CN)63-. (d) the weight/volume percentage of K3Fe(CN)6.12. 3.000 g BaCl₂.H₂O (molar mass=244.263 g/mol) was added to a solution of 100 mL of 0.050 M Na₂CO3. BaCl₂ (aq) + Na₂CO3 (aq) → BaCO3 (s) + 2NaCl Ksp for BaCO3 = 1.1 x 10-¹5 Calculate the concentration of CO2 in the resulting solution. a) 5M b) 0.050 M c) 0.072 M d) 1.5 x 10-¹³ M e) 1.5 x 10-14 MSEE MORE QUESTIONS