**Problem: Boiling Point Elevation Calculation****Instructions:**In addition to filling in the blanks below, show all of your work for this problem on paper for later upload.**Question:**Because you need water boiling at 100.0 °C for your recipe, how many grams of salt (NaCl(s)) would you need to add to 3.50 kg of water to raise the boiling point of water in Denver from the boiling point found in Problem 21 to 100.0 °C? Assume that the salt completely dissolves and fully dissociates in the water. If you did not get an answer for Problem 22, use 97.0 °C as the boiling point of water in Denver.**Step-by-Step Solution:**1. **Identify the boiling point elevation equation:** \[ \Delta T_b = i \cdot K_b \cdot m \] where: - \(\Delta T_b\) = Boiling point elevation - \(i\) = Van 't Hoff factor (number of particles the solute dissociates into) - \(K_b\) = ebullioscopic constant (for water, \(K_b = 0.512\) °C kg/mol) - \(m\) = Molality of the solution2. **Calculate the boiling point elevation \( \Delta T_b \):** \[ \Delta T_b = 100.0 \, °C - 97.0 \, °C = 3.0 \, °C \]3. **Determine the Van 't Hoff factor (i) for NaCl:** NaCl dissociates into 2 ions (Na⁺ and Cl⁻), so \( i = 2 \).4. **Calculate the molality (m):** \[ m = \frac{\Delta T_b}{i \cdot K_b} = \frac{3.0}{2 \cdot 0.512} = \frac{3.0}{1.024} \approx 2.93 \, \text{mol/kg} \]5. **Calculate the number of moles of NaCl needed:** \[ \text{moles of NaCl} = m \times \text{mass of water in kg} = 2

Given data, Mass of water = 3.5 Kg Initial temperature = 97.0oC Final temperature = 100.0oC Kb of…

In addition to filling in the blanks below, show all of your work for this problem on paper for later upload. Because you need water boiling at 100.0 °C for your recipe, how many grams of salt (NaCl(s)) would you need to add to 3.50 kg of water to raise the boiling point of water in Denver from the boiling point found in Problem 21 to 100.0 °C? Assume that the salt completely dissolves and fully dissociates in the water. If you did not get an answer for Problem 22, use 97.0 °C as the boiling point of water in Denver. Enter your value in the first box and an appropriate unit of measure in the second box.

In addition to filling in the blanks below, show all of your work for this problem on paper for later upload. Because you need water boiling at 100.0 °C for your recipe, how many grams of salt (NaCl(s)) would you need to add to 3.50 kg of water to raise the boiling point of water in Denver from the boiling point found in Problem 21 to 100.0 °C? Assume that the salt completely dissolves and fully dissociates in the water. If you did not get an answer for Problem 22, use 97.0 °C as the boiling point of water in Denver. Enter your value in the first box and an appropriate unit of measure in the second box.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A certain liquid X has a normal freezing point of 0.90°C and a freezing point depression constant Kf=6.96·°C·kgmol−1.A solution is prepared by dissolving some barium hydroxide (Ba(OH)2) in 900.g of X. This solution freezes at−3.7°C. Calculate the mass of Ba(OH)2 that was dissolved. Round your answer to 2 significant digits.
A student needs to prepare 250 mL of a 0.850 M aqueous solution of sucrose, C,„H„O,¡(aq), which is used frequently in biological experiments. 200 mL 250 mL 150 200 100 150 50 100 260mL. A How should the correct amount of solute be obtained? Which type of glassware should be used to make this solution (assuming that the accuracy of the concentration Measure out x mol of solid sucrose on a molemet. is important)? OC O Measure out x g of solid sucrose on a balance. O A O Measure out x cm of sucrose with a ruler. Publish
Calculate the amount of salt in a commercial cold-pack containing ammonium nitrate (ΔHsol = + 25.7 kJ/mol) if the final temperature of the cold-pack is 3ºC. Assume that the initial temperature of water is 25ºC, mass of solution is 25 g and the specific heat of the solution is 4.184 J/g.K.
g The solubility of Ni(OH)2 in water at 25 °C is measured to be 4.9 × 10-4 Use this information to calculate Ksp for Ni(OH)2. Round your answer to 2 significant digits. 8 0 x10 L 3
You place 0.03531g of CaCl₂ into a 500.0 mL volumetric flask and dissolve the solid with water to the mark on the flask. You then dilute 2.75 mL of this solution to 50.0 mL in a volumetric flask. What is the concentration of Ca in ppm in the resulting solution? [You can assume a density of 1.000 g/mL for the solution]
5.21 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.18 J/g･°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.
The binary compound M2X has a solubility of 9.4 × 10−7 mol/L and a molar mass, ℳ = 126.04 g/mol. Calculate the Ksp for this compound. Report your answer to TWO significant figures. Enter your answer in scientific notation using the appropriate boxes. Remember, a number like 1.6, in scientific notation is 1.6 × 100. Note: Your answer is assumed to be reduced to the highest power possible.
128 CHAPTER 5 3. A chart of vapor pressure information at different temperatures for various liquids is given below. Vapor Pressure (torr) Temperature Water Ethyl Alcohol Carbon Tetrachloride O'H 4. 24 (C) HOʻHƆ 12 34 0. 25 116 09 224 95 316 75 294 675 731 760 1723 1486 The questions below refer to the following experiment: three flasks, each containing one of the three liquids listed in the table are hooked to a vacuum pump. The pressure in each flask is reduced to 50 torr and the temperature of each flask is maintained at 25°C. blano (b) (a) Under these conditions, which liquid(s) would you observe boiling? Explain. (b) Explain why, if both liquids are maintained at 25°C, the vapor pressure of CCI, is higher than the vapor pressure of C,H,OH. Refer to both molecules in your discussion. CH H'C CH enstud-S-otoahib-CS-uot OBO 2ADI ud,8gada al sanm alom omss odi ovard asonatadue dhol () palom alimis bas Dwal s ad mot ab at a tmioq gaiilam Dwal inlqx ToonanoROT atidio ym li mol diW )…
3.56 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70 °C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g･ °C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.
You are a chemist and FBI crime scene investigator and find a sealed bag containing a suspicious white substance. The substance turns out to be a powder containing fentanyl (C22H28N2O, 336.470 g/mol) and lactose (C12H22O11) 342.298 g/mol). To find out exactly how much fentanyl was in the bag, you use a 100.0 mL volumetric flask to dissolve 1.000 g of the white powder in water. The osmotic pressure for the solution at laboratory temperature, 21.7 °C, is 538.2 mmHg. What percent of the white powder is fentanyl?
A student prepares a 0.20M aqueous solution of acetic acid (CH3CO₂H). Calculate the fraction of acetic acid that is in the dissociated form in his solution. Express your answer as a percentage. You will probably find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits. % 0 ☐x10 x
4.06 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.18 J/g･°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.