Formula: ml base x N x meq. wt. x 100 %w/w = Sample weight A 4.59 ml sample of HCI, specific gravity 1.3, required 50.5 mL of 0.9544N NaOH in a titration. Calculate the %w/WHCI. MW = 36.45
Q: Aspirin powder = 0.8110g MW of Aspirin = 180g.mol-1 Volume of 0.5N HCl consumed in back titration…
A: Volume of 0.5N HCl consumed in back titration = 23.50 mL
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A: Given: The volume of NaOCl = 10 mL The volume of Na2S2O3 = 29.82 mL Molarity of Na2S2O3 = 0.0195 M
Q: 1. A 4.59 mL sample of HCl, specific gravity 1.3, required 50.5 mL of 0.9544N NaOH in a titration.…
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Q: J l (NaCIy 0.2 N.u J 250 Na = 23. Cl = 35.5)s Q1 :- prepare a standard solution of a Sodium Chloride…
A: Detail calculation is shown below
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Q: In one trial determination of the concentration of NaOCl in the diluted bleach sample, 10.00 mL of…
A: The reaction taking place is,
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Q: transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the…
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Q: Three more samples of KHP (GFW= 204.23g/mole) weighing 0.8001g, 0.7001, and 0.7666g were titrated…
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Q: Mass solute needed to prepare 0.500L of 0.2 M NaCO3 from a solid NaCO3 with a purity of 92.0wt%
A: The total mass needed to prepare 0.500 L of 0.2 M NaCO3 is calculated as shown in equation (1) where…
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Q: Potassium acid phthalate, KHC8H4O4 ( MM=204.2 ), reacts with sodium hydroxide on a 1:1 molar basis.…
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- A 25.00mL wastewater sample was analyzed for its Mg2+ content using a standard gravimetric method. the sample was diluted to 3.00L and an 11.00mL aliquot was treated to precipitate magnesium as MgNH4PO4.6H2O using (NH4)2HPO4 as the precipitating agent. the precipitate was then filtered, washed, dried, and ignited resulting in a 0.1325mg Mg2P2O7 residue. How much Mg (in ppm) is present in the original sampleAn impure sample of calcium carbonate with a mass of 7.95 g was reacted with 50.00 cm3 of 1.00 mol dm hydrochloric acid (an excess). The resulling solution was transferred to a volumetric flask and titrated with 11.10cm3 of 0.300 mol dm-3 sodium hydroxide solution. Determine the percentage purity by mass of the calcium carbonate sample.CaCO3 + HCl -> CaCl2 + H2O + CO2 HCl + NaOH -> NaCl +H2O a. Determine how many moles of hydrochloric acid were used.b. Determine how many moles of excess HCI was titratedc. Determine how much in moles calcium carbonate present in the sample.d. Calculate the mass of calcium carbonate presente. Determine the percentwge calcium carbonate is in the sample.Aspirin powder = 0.8110g MW of Aspirin = 180g.mol-1 Volume of 0.5N HCl consumed in back titration = 23.50mL Volume of 0.5N HCl consumed in blank titration = 44.50mL Percent purity (USP/NF) = Aspirin tablets contain NLT 90.0% and NMT 110.0% of the labeled amount of aspirin (C9H8O4) What is the calculated weight (in grams) of pure aspirin?..
- Gravimetric analysis of Fe3O4 (MW = 232 g/mole) may be undertaken with the following reactions: Fe3O4 → Fe2O3 → Fe (OH)3. Weight of sample containing 8.00% Fe3O4 that must be taken to obtain a precipitate of Fe(OH)3 (MW = 107 g/mole) that weighs 150 mg is . a. 0.108 g b. 0.325 g c. 1.355 g d. 4.065 g Amount of Fe2O3 (MW = 160 g/mole) from which 150 mg of Fe(OH)3 (MW = 107 g/mole) may be obtained is . a. 0.112 g b. 0.224 g c. 0.448 g d. none of the other choicesIn one trial determination of the concentration of NaOCl in the diluted bleach sample, 10.00 mL of the diluted bleach solution required 23.32 mL of 0.0195 M Na2S2O3 titrant to reach the endpoint. What is the molar concentration of NaOCl in the diluted bleach solution?The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?
- Potassium acid phthalate, KHC8H4O4 ( MM=204.2 ), reacts with sodium hydroxide on a 1:1 molar basis. A sample of the acid weighing 0.4823 g was titrated with NaOH, requiring 24.35 mL to reach the endpoint. Calculate the molar concentration of the sodium hydroxide solution.Mass solute needed to prepare 0.500L of 0.2 M NaCO3 from a solid NaCO3 with a purity of 92.0wt%Prepare 50ml of approximately 1000ppm Mn stock solution from MnCl2*4H2)
- a) What mass of Fe(NH4)2(SO4)2•2H2O(s) is required to prepare a 500 mL solution containing 100 ppm (m:v) in Fe? b) Using this stock solution, what aliquot must be used to prepare calibration solutions, 100 mL volume, of the following concentrations: 0.100 ppm, 0.500 ppm, 2.00 ppm, 4.00 ppm, and 7.00 ppm.The standard addition method is used to analyze a sample of a river water for mercury. Solution A is made by pipetting 5.00 mL of undiluted sample in to a 10 mL volumetric flask and filling to the mark with DI water. Solution B is made by pipetting 5.00 mL of undiluted sample and 3.00 mL of 15.0 ppb of Hg standard into same 10.0 mL volumetric flask and filling to the mark with DI. Solution A and B are analyzed using atomic absorption spectroscopy and give a percent transmittance values of 56 % and 33 % respectively (not blank corrected). A blank has a transmittance of 96%. What is the corrected absorbance of both solution A and B? A. Solution A: 0.123 Solution B: 0.463 B. Solution A: 0.463 Solution B: 0.234 C. Solution A: 0.123 Solution B: 0.234 D. Solution A: 0.234 Solution B: 0.463An analyst weighed 0.25045 g of the Buffalo River Sediment reference material.(RM # 8704) to determine Pb levels. The material was digested in an acid medium toBring it to a solution which was made up to the 30.2450 mL mark with distilled water. If thePb concentration in the control certificate of analysis is (150 ± 17) mg / kg, and theanalyst recovered 95%, what was the concentration of Pb in the solution?
