Describe the preparation of the following reagents: 1. 300 mL of a solution that is 0.0376 N MgI2 from a pure solid reagent 2. 400 mL of 40 ppt Cl- from 0.01 M PbCl2
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- How many grams of CaF2 will be soluble in 250 ml of 0.510 M KF solution? (ksp of CaF2 = 3.90 x 10-11) (atomic weights: Ca 40.0; K 39.1; O 16.0; F 19.0)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.Compare the solubility of ferrihydrite (Fe(OH)3) and goethite (FeOOH), with dissolution reactions shown below. Fe(OH)3 3 H+ --> Fe3+ + 3 H2O FeOOH + 3 H+ --> Fe3+ + 2 H2O
- A solution was prepared by dissolving 1210 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 775 mL. Calculate (a) the weight/volume percentage of K3Fe(CN)6.(B) the number of millimoles of K+ in 50.0 mL of this solution.(C) ppm Fe(CN)63- .(D) pK for the solution.(E) pFe(CN)6 for the solution.A solution was prepared by dissolving 1210 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 785 mL. Calculate b) the weight/volume percentage of K3Fe(CN)6, the number of millimoles of K+ in 35.0 mL of this solution, and the ppm of Fe(CN)63-1. Describe the preparation of (a) 500 mL of 0.0750 M AgNO3from the solid reagent .(b) 1.00 L of 0.285 M HCl, starting with a 6.00 M solution of the reagent. (c) 400 mL of a solution that is 0.0810 M in K+, starting with solid K4Fe(CN)6. (d) 600 mL of 3.00% (w/v) aqueous BaCl2from a 0.400 M BaCl2solution. (e) 2.00 L of 0.120 M HClO4from the commercial reagent [71.0% HClO4(w/w), specificgravity1.67]. (f) 9.00 L of a solution that is 60.0 ppm in Na+, starting with solid Na2SO4 EXPLAIN EACH ITEM
- 1. Describe the preparation of (a) 500 mL of 0.0750 M AgNO3from the solid reagent .(b) 1.00 L of 0.285 M HCl, starting with a 6.00 M solution of the reagent. (c) 400 mL of a solution that is 0.0810 M in K+, starting with solid K4Fe(CN)6. (d) 600 mL of 3.00% (w/v) aqueous BaCl2from a 0.400 M BaCl2solution. (e) 2.00 L of 0.120 M HClO4from the commercial reagent [71.0% HClO4(w/w), specificgravity1.67]. (f) 9.00 L of a solution that is 60.0 ppm in Na+, starting with solid Na2SO4What 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?4. a. Describe the preparation of 1.67 L of 5.00% (w/v) K2Cr2O7 from the solid salt. b. What is the ppm K2CR2O7 in the above solution?
- The 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 ………………………………Twenty grams of potassium dichromote (K2C2O7) is dissolved in 150 mL of water. What is its normality as a solution? a) 0.70N b) 1.81 N c) 1.41 N d) 0.91 N The solution in the previous problem was used in titration producing chromium(II) oxide (CrO). What is the normality of the solution in the said reactin? a) 0.70N b) 1.81 N c) 1.41 N d) 0.91 NThe Ksp of Ca3(PO4)2 is 1.3 × 10−26. Estimate the solubility of this salt in units of g. L-1