11. Explain briefly the preparation of 250 mL 10% (w/v) of Ca (NO3)2 in the laboratory. 12 Drimany standard sodium carbonate solutions containing 0 25 of Na.CO, roquirod 30 60
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- The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mL1 ) The density of a 5.26MNaHCO 3 (84.0 g/mol) is 1.19g / m * l . Its molality is 2) Calculate the pAg^ + at the equivalence point in the titration of 25.0ml of 0.0823 M Kl with 0.051M AgNO 3 . Ksp Agl=8.3*10^ -16 3) Commercial concentrated aqueous nitric acid is 70.4% HNO3(63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is 4) Consider the titration of 25ml of 0.0823M KI with 0.051M AGNO3, Kspagi =8.3x10-16 Calculate pAg* after adding 39.0 ml I03 Ag* + 103 ====AglO3 5) Commercial concentrated aqueous nitric acid is 70.4 1\%HNO 3 (63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is: 6) What mass in g of Na 2 CO 3 [106 g/mol] is required to prepare 250 ml of 0.3M aqueous solution in Na^ + [23.g/mol] ? 7) Calculate pAg^ + after adding 42.30ml AgNO 3 In the titration of of 0.0823M Kl with 0.051M AgNO 3 . KspAgl = 8.3 * 10 ^ - 16 8) The milliliters of concentrated HClO 4 (100.5 g/mol),6 60% by mass,…Balanced eqation: 2 H3PO4 + 3 Ca(OH)2 → 6 HOH + Ca3(PO4)2 What is the molar concentration of 325.25 mL H3PO4 is needed to reach the equivalence point with 475.60 mL of 0.465 M Ca(OH)2?
- What is the solubility of Sr(IO₃)₂ in a solution that contains 0.0300 M Sr²⁺ ions? (Ksp of Sr(IO₃)₂ is 1.14×10⁻⁷) What is the solubility of Sr(IO₃)₂ in a solution that contains 0.0550 M IO₃⁻ ions? (Ksp of Sr(IO₃)₂ is 1.14×10⁻⁷)In the titration of 25.00 mL of a water sample, it took 19.040 mL of 4.965x 10−3 M EDTA solution to reach the endpoint. The total hardness is always listed in parts-per-million (ppm) of CaCO3 (or mg CaCO3 / Kg H2O). Since the density of water is 1.0 g/mL, one ppm would be the same as the number of mg of CaCO3 per liter of water. Determine the number of moles of CaCO3 present in the titrated sample of water, assuming that all the Ca2+ combines with CO32−. (enter your answer with 3 significant figures)Consider the reaction of a 20.0 mL of 0.220 M C₅H₅NHCl (Ka = 5.9 x 10⁻⁶) with 12.0 mL of 0.211 M CsOH. How many moles of C₅H₅NH⁺ would be present at the start of the titration? How many moles of OH- would be present if 12.0 mL of OH- were added What species would be left in the beaker after the reaction goes to completion
- A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 16.3 mL of HNO₃ was required. write the balanced chemical equation for the reaction. How many moles of HNO3 are used in the titration? How many moles of Ca(OH)2 had to be present in the initial reaction? What was the concentration of the initial Ca(OH)2 solution?Determine the Concentration of Ethanoic Acid in Vinegar Equipment / Apparatus: 250-mL conical flasks Clamp Burette Graduated cylinder Pipette Reagents / Materials: Vinegar Phenolphthalein indicator 0.2 M NaOH (standardized) Calculation: Molarity (M) of ethanoic acid The average measured volume of the NaOH from titration: Average volume of NaOH used = (21.5ml + 21.5ml + 21.6ml) / 3 =21.5ml No of mole of NaOH = Concentration of NaOH (0.2M) × Average volume of NaOH used When an acid is completely neutralized: No of moles of CH3COOH = No of moles of NaOH Using the moles of CH3COOH, the molarity of ethanoic acid in the 5.0-mL sample of vinegar is calculated: Molarity (M) CH3COOH = moles CH3COOH / volume of vinegar (0.005 dm3). Calculation: Mass / Volume Percent (m/v) of ethanoic acid To calculate the percent (m/v) of CH3COOH in vinegar, we convert the moles of ethanoic acid to grams using the molar mass of ethanoic acid, 60.1 g/mole. Mass of CH3COOH =…Which of the statements given below is correct? A. Iodometry is a method in which I2 solution is used as a titrant and substances that can reduce iodine to iodine can be determined. B. Starch indicator is added to the medium at the beginning of the titration. A. All metal salts other than alkali salts dissolved in water cause hardness. D. 1 German hardness is the hardness of water containing cation equivalent to 1 mg CaCO3 in 100 mL.
- 1. An acid solution is prepared by dissolving 19.264 grams of pure KHC2O4.H2C2O4.2H2O in water and diluting to exactly 900 ml. Fifty milliliters (50.00 mL) of this solution are neutralized by 35.00 ml. of KOH solution. What is the normality of each solution? 2. What mass of Ca(OH)2 is present in a sample if it is titrated to its equivalence point with 44.02 mL of 0.0885 M HNO3? The balanced chemical equation is as follows: 2HNO3 + Ca(OH)2 → Ca(NO3)2 + 2H2O ; Balanced.Bay Water Titration The concentration of Cl- in ocean water is about 500-600 mM. The baywater is diluted by a factor of 12.5 using a 20.00 mL volumetric pipet and a 250 mL volumetric flask. Using a 15.00 mL volumetric pipet, 15.00 mL is transferred into three clean Erlenmeyer flasks. 10 mL of 1% dextrin solution, 20 mL of de-ionized water, and 3-4 drops of indicator are added and titrated each with the AgNO3 solution. From the procedure, find: Dilution factor Volume of diluted bay water Then calculate: The [Cl-] of diluted bay water The [Cl-] of bay water Consider this information: [AgNO3] = 0.04043177 trial # Veq 1 13.91 2 13.73 3 13.9 4 13.86 5 13.87 6 13.84 average 13.85167 [Cl-]Bay = ([AgNO3](Veq(ave))/Vdil bay water pipeted) (Vflask/Vbay water)A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 28.4 mL of HNO₃ was required. Given that 0.00966 mol of HNO₃ are used in the titration, how many moles of Ca(OH)₂ had to be present in the initial reaction?