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(a) An aqueous solution contains 12.6 ppm of dissolved Ca(NO3)2 (which gives Ca2+ + 2NO3- ). Find the concentration of NO3- in parts per million.
(b) How many ppm of Ca(NO3)2 are in 0.144 mM Ca(NO3)2?
(c) How many ppm of nitrate (NO3-) are in 0.144 mM Ca(NO3)2?
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- 4. If the following values are used... Measure the mass of 0.400 g of cobalt(II) nitrate hexahydrate (Co(NO;)2 -6H2O), and dissolve it in 15.0 mL of distilled or deionized water using a clean beaker. Using a graduated cylinder, measure out 10.0 mL of a prepared 0.10-M sodium phosphate (NazPO4) solution. ... determine which compound, (Na3PO4 or Co(N03)2 ·6H2O) will be the limiting reagent. Then determine the theoretical yield.Nickel sulfate, NiSO 4 , reacts with sodium phosphate, Na 3 PO 4 , to give a pale yellow-greenprecipitate of nickel phosphate, Ni 3 (PO 4 ) 2 , and a solution of sodium sulfate, Na 2 SO 4.. How manymilliliters of 0.375 M N i SO 4 will react with 45.7 mL of 0.265 M Na 3 PO 4 ? . Show balanced chemicalreaction of the problem.1. A silver nitrate solution contains 14.77 g of primary standard AgNO3 in 1.00 L. What volume of this solution will be needed to react with a) 0.2631 g of NaCl? b) 0.1799 g of Na CrO4? c) 64.13 mg of NazAsO4?
- The hardness of water (hardness count) is usually expressed in parts per million (by mass) of CaCO3. What is the molar concentration of Ca2+ ions in a water sample with a hardness count of 175mg CaCO3/L?0.6465 grams of bleach, Ca(OCl)2, is dissolved in acid and treated with excess KI. Calculate the weight percent of Ca(OCl)2 in the bleaching powder when the released iodine is titrated with 36.92 mL of 0.06608 M Na2S2O3 (MaCa(OCl)2: 143 g/mol). A. 6.74B. 13.48C. 20.22D. 26.96A 3.026 grams of Cu (II) salt is dissolved in water and then diluted to 250 mL in a volumetric flask. Iodine is liberated when one gram of KI solution is added to 50.0 mL of aliquot sample. A 23.33 mL of 0.04668 M Na,S,O, solution is required to titrate the iodine liberated. Calculate the weight percent of the Cu in the salt. (A) 11.43%, just before end point (B) 12.43%, just before end point (C) 11.43%, after equivalence point (D) 12.43%, after equivalence point
- 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 molar analytical concentration 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.(e) the number of millimoles of K+ in 50.0 mL of this solution.(f) ppm Fe(CN)63- .(g) pK for the solution.(h) pFe(CN)6 for the solution.(a.) Titration of a 12.0 mL solution of HCl requires 22.4 mL of 0.12 M NaOH. What is the molarity of the HCl solution? (b.) Titration of a 10.0 mL solution of NH3 requires 15.0 mL of 0.0250 M H2SO4. What is the molarity of the NH3 solution?Fe3+ in 50 mL solution, which is known to contain Fe3+, was precipitated as Fe(OH)3 and after necessary procedures, it was brought to constant weight as Fe2O3. Since the weight is found to be 0.3994 g, find the Fe3+ concentration in the solution in terms of molarity. (Fe: 55.85, O: 16.00 g / mol)
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