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- What will be the new boilng point of 491ml benzene (Kb = 2.53 oC•Kg/mol; Bp = 80.1oC) when mixed with 11g of naphthalene (MW = 128.17 g/mol) to make a non- eletrolyte solution? Density of benzene = 0.876 g/ml) Round you answer in 2 decimal places, unit is not required.Give example and explanation of each words: Standard Solution Supernatant liquid Abscissa Atomic mass Concentration Density Equilibrium Constant Formula massANSWER THEM ALL FOR AN UPVOTE. ASAP PLEASE. The theoretical weight of 10 tablets is 9.35g. Each tablet contains 425mg of the active ingredient. Using this data, determine the amount of additive needed to prepare 160, 000 tablets. How many grams of drug are required to make 500ml of 25.0% solution?
- 14. 25.00 cm³ of 0.300 mol/dm³ sodium hydroxide solution is exactly neutralized by 0.100 mol/dm³ sulfuric acid. Calculate the volume of sulfuric acid needed in ml. Using dimensional analysisBoiling Point Elevation/Freezing Point DepressionT = m KWhere: T = T(solution) - T(pure solvent) * m = (# moles solute / Kg solvent) Kb = boiling point elevation constant. Kf = freezing point depression constant. Kb and Kf depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow. Solvent Formula Kb (°C / m) Kf (°C / m) Water H2O 0.512 -1.86 Ethanol CH3CH2OH 1.22 -1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 -5.12 Diethyl ether CH3CH2OCH2CH3 2.02 note that ΔT as defined above will be a negative number for freezing point depression. Therefore, Kf must also be given as a negative number.The solubility of benzoic acid in water is 0.21g per 100mL of water at 10 degrees celsius, 0.27g per 100mL at 18 degrees celsius, and 6.80g per 100mL at 95 degrees celsius. A. At least how much water would be needed to dissolve a 2.00g sample of benzoic acid at 95 degrees celsius? B. If you carried out a recrystallization by dissolving your 2.00g sample in water at 95 degrees celsius, then cooling it to 18 degrees celsius, what would be the maximum yield of benzoic acid? How would the yield be affected if the recrystallization mixture was cooled to 10 degrees celsius instead?
- The partial molar volumes of acetone and chloroform, in a solution in which the molar fraction of chloroform is 0.4693, are 74.166 cm3mol-1 and 80.235 cm3 mol-1, respectively. What is the volume of 1,000 kg of this solution? Data: M.M. (acetone) = 58.08 gmol-1; M.M. (chloroform) = 119.07 gmol-1.Use the following steps to determinr the percent error of the freezing point depressions you determined experimentally from the expected freezing point depression for each solute. Show sample calculations for sodium chloride solution. a. Use the actual molar mass of each solute to determine the expected motality of 0.234g of each solute in 4.00x10-3kg of water. Sample Calculation: b. Determine the expected freezing point depression for a solution with this motality. Sample Calculation: c. Determine the percent error of the freezing point depression you determine experimentally from the expected freezing point depression for each solute. Sample Calculation:Which of the following is/are proper lab techniques in solution preparation? Choose one or more best answer: a. Quickly adding 90mL of distilled water onto 10mL of concentrated acid to make 100mL of diluted acid solution b. Adding NaOH pellets in the volumetric flask and immediately diluting to mark c. Quantitatively transferring dissolved solids from a beaker by pouring washings into the final container d. Using cold distilled water to dilute a solution to mark so it does not get hot e. Using a volumetric pipette when applicable to get the most accurate aliquot volume f. After diluting to around 90mL before the mark, transfer the solution into a beaker to cool down more efficiently. g. Storing everything in plastic containers as plastic is more inert than glass for most chemicals Note: Just answer, no explanation needed. Thanks
- Part II. Determination of molecular weight for ethyl alcohol Freezing point, °C DTf Mass of solute, g mass of solvent, kg Calculated molecular weight, g/mol -2.30 0C ΔTf = T0f – Tf 0.0 °C -(-2.30 °C) = 2.30 0C 6.202 g 0.1kg Click or tap here to enter text.What is the kinetic property observed in suspension? What is the optical property observed in solutions?Bristol Community College Fall River, Massachusetts Experiment 6: Molar Mass of a Molecular Solid from Freezing Point-Depression Measurement Name: __________________________________ Date: _______________ Approved: ___________ DATA SHEET Mass of lauric acid (in Part II) Mass of benzoic acid (in Part II) Freezing temperature of pure lauric acid (from Part I) data from Video 2 of Part I Freezing temperature of solution (from Part II) data from Video referenced in Part II Freezing point depression, Tf ( = Tf, lauric acid – Tf, solution) Molality (m) of solution ( Eq. 1) Moles of benzoic acid ( Eq. 2) Experimental molar mass of benzoic acid (Eq. 3) Calculate the molar mass of benzoic acid, C6H5COOH. Percent error Summary Questions A student determines…