27. Find the freezing point of a solution of 990 g of CH3OH in 2.5 kg of water. Use the water f.R.-depression constant: Kp(H2O) = = 1.86 °C/{mol(solute)/kg(solvent)} A) +123 °C B) +77 °C C) +23 °C D) -0.74 °C E) -23 °C

27. Find the freezing point of a solution of 990 g of CH3OH in 2.5 kg of water. Use the water f.R.-depression constant: Kp(H2O) = = 1.86 °C/{mol(solute)/kg(solvent)} A) +123 °C B) +77 °C C) +23 °C D) -0.74 °C E) -23 °C

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

How many grams of the nonelectrolyte glycerol, C3H8O3 , would have to be added to water in order to produce an 1.00-L solution with a freezing point of –2.63°C? Assume that Kf for water is 1.86°C/M. _______g
Submit Answer If 22.2 grams of an aqueous solution of calcium acetate, Ca(CH3COO)2, contains 4.73 grams of calcium acetate, what is the percentage by mass of calcium acetate in the solution? % Ca(CH3COO)2 282 F4 % 5 T G F5 B Retry Entire Group Cengage Learning Cengage Technical Support Y H [Review Topics) [References] Use the References to access important values if needed for this question. S & 6 i 7 MacBook Air F6 N 9 more group attempts remaining U F7 J 8 M I DII K ( 9 DD F9 O L ) O A F10 P : ; command option 4 F11 { [ ? 1 Previous + 1 Save and Exit 4) Next> F12 } ] S Relaunch to update delete + return shift Ⓒ
Activity 1. Solve Me! Calculate the problems below. Write your solution and box your finalanswer. Follow the flow of solving like the examples given above. You may use the K b and K fof water in the examples. 1. Calculate the freezing and boiling points of a solution prepared by dissolving 15.5 gof Al (NO 3 ) 3 in 200.0 g of water. (Molar mass of Al (NO 3 ) 3 is 212.996 g/mol). 2. A solution is prepared by dissolving 120 grams of NaCl in 450 grams of water. Findthe freezing and boiling points of this solution. (Molar mass of NaCl is 58.44 g/mol) Activity 2. Know Me! Look for a book or search the web for additional information regardingthe colligative properties of solution. Refer to the guide questions below. 1. State the effect that dissolving a solute has on each of the following physicalproperties of a solvent.a. Boiling pointb. Freezing point
None
Ksp = 1.3 x 10-32 for Ca3(PO4)2 at 25 °C, what is the molar concentration of Ca²+ at 25 °C? M (example: type in 3.4E-5 for 3.4x10-5). Please pay attention to the number of sig. figs. in your answer. The molar concentration of PO4³- is
Hand written not allowed please dear.
Direction: Answer the follow ing in your answer sheet. 1. In each pair of aqueous systems, which will have the lower vapor pressure? A. pure water or 1.0 M NaCi В. 1.0 M NaCl or 1.0 M CеHi2Os С. 1.0 м СаCI2 or 1.0 M (NH4)3РОd 2. In cach pair of aqueous systems, which will have the higher boiling point? A. pure water or a 1.0 M NaCı B. 1.0 M NaCl or 1.0 M C6H1206 C. 1.0 M CaCI2 or 1.0 M (NH4)3PO4
g/mol PHY&CHEM HW Submit Answer Fall 2023 Tutoring S.. The freezing point of ethanol, CH₂CH₂OH, is -117.300 °C at 1 atmosphere. K(ethanol) = 1.99 °C/m In a laboratory experiment, students synthesized a new compound and found that when 13.05 grams of the compound were dissolved in 208.0 grams of ethanol, the solution began to freeze at -117.982 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound? eview Topics] [References] Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining Previous Next
What is the freezing point (°C) of a solution prepared by dissolving 13.5 g of (NH4)2SO4 (formula weight = 132 g/mol) in 100 g of water? The molal freezing point depression constant for water is 1.86°C/m. Assume complete dissociation in solution. Express your answer in decimal notation and to 2 decimal places, without units.
A solution contains 3.90 g of a nonvolatile pure hydrocarbon in 95 g acetone. The boiling points of pure acetone and the solution are 55.95oC and 56.50oC, respectively. The molal boiling point constant of acetone is 1.71oC ∙ kg/mol. What is the molar mass of the hydrocarbon? Molar mass______g/mol
Name: Date: Section: Report Sheet: Determination of Molecular Weight Through Freezing Point Depression Analysis 30 Part A: Volume of Cyclohexane mL Mass of cyclohexane (d =0.7786 g/mL) 6.0 °C Freezing Point of cyclohexane 128 Part B: Molecular Weight of Naphthalene g/mol 0.23 Mass of Sample 1 Moles of Sample 1 Mass of Sample 2 0.18 Moles of Sample 2 Moles m (mol/kg solvent) T,('C) AT, Naphthalene 5.1 TRIAL 1 5.3 TRAIL 2 k, Cyclohexane CC/m) Part C: Unknown Number 0.21 0.19 Mass of Sample 1 Mass of Sample 2 Grams Unknown T,('C) AT 0.21 4.8 TRIAL 1 0.19 5.0 TRAIL 2 Moles UnknownTRIAL 1 (moles) TRIAL 2 (moles) TRIAL 1 (g/mol)TRIAL 2 (g/mol) Molecular Weight Unknown (g/mol) AVERAGE MOLECULAR WEIGHT OF UNKNOWN
will W S > 3. What is the final molar concentration if 285.0 mL of water is added to 450.0 mL of a 0.925 mol/L aluminum sulfate (Al2(SO4)3] ? JUN 10 TO 0 #3 Q E D 4 C I R F % 5 V T MacBook Pro & ^ 6 G Y 7 U H BN * 00 8 4 1 ( 9 JK M 0 V L