Experiment VIII

Need question 4,5 and 6

FIND THE Average Molarity of the Analyte (M or mol/L)

you can only work on it for 90 mins Instructions Multiple Attempts Not allowed. This test can only be taken once. Force Completion This test can be saved and resumed later. Your answers are saved automatically. * Question Completion Status: A Moving to another question will save this response. Question 28 10 Calculate the molarity of the resulting solution prepared by diluting 25.0 mL of 18.0% ammonium chloride, NH 4CI, (density = 1.05 g/mL) to a final volume of 80.0 mL. O a. 0.0536M O b.0.00105 M OC. 1.10 M O d.0.059 M O e.0.292 M » A Moving to another question will save this response. acer

Part 2 Data Mass of Urea (g): Buret Initial Volume (mL): water Part 2 Calculation: 4.05819 24.90 A. Find the Keq for dissolving urea (saturated solution) Mass of urea used 4.05819 Moles urea = Final Temperature of saturated solution ("C): Buret Final Volume (ml): fikcal - In 1.Write the chemical equation for urea dissolving: CityN₂0 (s) + H₂0 (1) → (H₂N₂O) (aq) Volume in Liters = 2.Calculate the molarity of the urea, [Urea]eam for the saturated solution of urea in water. You must first find the moles of urea (molar mass 60.05 g/mol). Then you must use the volume given in the data (above) to find the molarity of the urea in the saturated solution. Show calculations here. 3. Calculate AG soln Volume of water used: 3.88 ML Molarity of saturated solution (NOTE: this molarity = Keq ) = To do this, use: AG soln = - RT In Keq AH-TAS soln 4. Calculate AS soln Use: AG First, re-arrange the equation given above to solve for AS soln 6 27.0 W AS soln AGOsoln Then plug in the values you got for AG°…

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LAB VI. MOLAR MASS BY FREEZING POINT DEPRESSION • Colligative properties of a solution are properties that depend on the number of solute particles dissolved. • Colligative properties of a solution include: o Vapor pressure lowering, o Boiling point elevation, o Freezing point depression, and o Osmotic pressure. • The molar mass of a solute may be determined by measuring a colligative property of a solution. • In this experiment the freezing point of a solvent would have been determined from a cooling curve. Practice problems: • Calculate the freezing point of a solution of 800 g of ethylene glycole (MW = 62.02 g/mole) in 3,000 g of water given that the K(H2O) = 1.86 °C/m. • How many moles of ethanol are dissolved in t-butanol if the change in the freezing point is 10 °C, and t-butanol's Kr is 8.37 °C/m? How many grams of ethanol are dissolved in this solution? Calculate the freezing point of a solution of 200 g of glucose (MW = 180.096 g/mole) in 2,500 g of acetic acid, given that…

Need help finding the values listed in the table

Find Molarity for HCl for Trials one through three

Using the Solubility Data for Report below answer the question: Compound                      Cold water Solubility               Hot Water Solubility Benzoic Acid            0.42 g per 100mL of water    5.79 g per 100mL of water Impurity                    0.61 g per 100mL of water     4.62 g per 100mL of water An impure sample contains 1.14 g of impurities and 5.14 g of benzoic acid. The sample is dissloved in 100mL of water and heated. The solution is then cooled. How many grams of impurity will crystalize when the solution has cooled?