To 10,00 ml of 0,0500 mol/l solution of potassium bromide – 9,00 ml of solution of 0,05500 mol/l silver nitrate were added. Calculate pBr of this solution. pKs(AgBr) = 12,28 Express numerical result with an accuracy of: X,XX 3.
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- A standard solution is prepared by completely dissolving 0.4 grams of CaCl2 and 0.2 grams of MgCO3 salts in 1-Liter DI water in a glass bottle closed to the atmosphere. The equilibrium pH of the standard solution is adjusted to 7.3 using acid-base solutions. Assuming the amounts of acid and based used in the initial pH adjustment is negligible, calculate : Temporary and permanent hardness of the solution as mg/L CaCO3. Total alkalinity and acidity as mg/L CaCO3. Useful information for problem :An experiment to observe the effect of ionic strength on the solubility of Ca(OH)2 was conducted. Ca(OH)2 was added to 250 mL 0.01 M KCl, stirred until equilibrium. This was then filtered, and 50 mL of the filtrate was measured out. The 50 mL filtrate was then titrated with standardized 0.13 M HCl solution until phenolphtalein endpoint (11 mL). How do I solve for the solubility s of Ca(OH)2? Please provide an explanation of the process (do I multiply ionic strength μ to the solubility [where s = [Ca(OH)2) = [Ca2+] = 1/2[OH-]?)An experiment to observe the effect of ionic strength on the solubility of Ca(OH)2 was conducted. Ca(OH)2 was added to 250 mL 0.01 M KCl, stirred until equilibrium. This was then filtered, and 50 mL of the filtrate was measured out. The 50 mL filtrate was then titrated with standardized 0.13 M HCl solution until phenolphtalein endpoint (11 mL). How do I solve for the solubility s of Ca(OH)2? Please provide an explanation of the process (do I multiply ionic strength μ to the solubility [where s = [Ca(OH)2) = [Ca2+] = 1/2[OH-]?) I would like to know how the diverse ion effect would affect the solubility of Ca(OH)2. How does the ionic strength μ of KCl affect this?
- A reprecipitation was employed to remove occluded nitrate from BaSO4 precipitate prior to isotopic analysis of oxygen for geologic studies.9 Approximately 30 mg of BaSO4 crystals were mixed with 15 mL of 0.05 M DTPA in 1 M NaOH. After dissolving the solid with vigorous shaking at 708C, it was reprecipitated by adding 10 M HCl dropwise to obtain pH 3–4 and allowing the mixture to stand for 1 h. The solid was isolated by centrifugation, removal of the mother liquor, and resuspension in deionized water. Centrifugation and washing was repeated a secondtime to reduce the molar ratio NO-3 /SO-4 2 from 0.25 in the original precipitate to 0.001 in the purified material. What will be the predominant species of sulfate and DTPA at pH 14 and pH 3? Explain why BaSO4 dissolves in DTPA in 1 M NaOH and then reprecipitates when the pH is lowered to 3–4.A sample is analyzed for chloride by the Volhard method. From the following data, calculate the percentage of chloride present:Weight of sample = 6.0000 g dissolved and diluted to 200 mLAliquot used = 25.00 mL AgNO3 added = 40.00ml of 0.1234MKSCN for back titration = 13.20ml of 0.0930MDissolved 0.273 grams of pure sodium oxalate (NaCO) in distilled water and added sulfuric acid and titration the solution at 70 ° C by using 42.68 ml of KMNO. solution and has exceeded end point limits by using 1.46 ml of standard oxalic acid (HCO) with 0.1024 N Calculate the normlity of KMNO Note that the molecular weight of sodium oxalate (NaCO) = 134 and its equivalent weight = 67
- A commercial vinegar was analyzed by titration to determine the percent acetic acid. Briefly, 10.00 mL of vinegar sample was diluted to 100. mL solution in a volumetric flask. A 25.00 mL aliquot from the diluted vinegar required 25.55 mL of 0.1005 M sodium hydroxide to reach the phenolphthalein endpoint From this experiment which is the standard solution used in titration? CH3COOH NaOH NaCH3COO C20H14O4The pKb of ammonia is 4.74. Ksp of Mg(OH)2 is 5.6 x 10-12 If one 100 mL 0.1 M MgCl2 to 100 mL 0.1M NH3, would a precipitate of Mg(OH)2 form? Show using calculations why this would or would not happen.Calculate the mass of sodium acetate required to mix with 100mL of 0.1M acetic acid (HC2H3O2) toprepare a pH 4.2 buffer solution.
- The distribution constant for iodine between an organic solvent and H2O is 85. Find the concentration of iodine remaining in the aqueous layer after extraction of 50mL of 1.00x10-3 M iodine with two portion of 25mL organic solvent?Calculate the molar solubility of thallium chloride in 0.15 M NaCl at 25°C. Ksp for TlCl is 1.7 × 10-4.A 0.2182g sample of NaCl was assayed by the Volhard Method using 50mL of 0.0985N AgNO3 and 11.75mL of 0.1340N NH4SCN. Calculate the %NaCl in the sample