If all the solute is dissolved in diagram 1 (Figure 1), how would heating or cooling the solution cause each of the following changes? ct; Try Again; 3 attempts remaining in 2 of 2 blanks incorrectly. on the left to the appropriate blanks on the right to complete the sentences. Reset cooled 1. From diagram 2 to 1, the solution has been since most solid solutes are more lower soluble at temperatures. higher heated Figure < 1 of 1> Previous Answers Request Answer ct; Try Again; 4 attempts remaining in 2 of 2 blanks incorrectly. Solid

If all the solute is dissolved in diagram 1 (Figure 1), how would heating or cooling the solution cause each of the following changes? ct; Try Again; 3 attempts remaining in 2 of 2 blanks incorrectly. on the left to the appropriate blanks on the right to complete the sentences. Reset cooled 1. From diagram 2 to 1, the solution has been since most solid solutes are more lower soluble at temperatures. higher heated Figure < 1 of 1> Previous Answers Request Answer ct; Try Again; 4 attempts remaining in 2 of 2 blanks incorrectly. Solid

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...

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Part C. Solubility versus Temperature 1. (a) Which solution(s) containing 1.0 g of salt (NaCl and NH,CI are both considered "salts") per 5 ml. of water is (are) unsaturated and why? 2. (a) Temperature of each solution before heating: NaCl: NH,Cl: (b) Which solution(s) containing 2.4 g total of salt per 5 ml of water is (are) saturated at room temperature and why? 3. (a) Temperature of each solution in the hot water bath: NaCl: NH.CI: (b) Which salt is least soluble at elevated temperatures? (c) Classify the salt solutions at elevated temperatures as either saturated or unsaturated. NaCl: NH.CI: 4. (a) Did the salt solution(s) that were unsaturated at the elevated temperatures become saturated when cooled? How do you know? 6.
A Moving to another question will save this response. estion 20 2- produces a net migration of water only if the concentration of colloidal size particles is different on the two sides of the membrane. A Moving to another question will save this response. S W 3 E D 80 F3 $ 4 888 R F % 5 F5 T G MacBook Pro 6 & H F7 8
When 0.258 g of a unknown molecular compound, was dissolved in 40.0 g of benzene, the freezing point of the solution was lowered to 5.23 °C. What is the molecular weight of the unknown compound? Kf benzene = 5.12 °C/m. Tf = 5.5 °C. * solve with steps and explains and equations please??
The second picture are the answers choices
ne > My courses > 1802 > Topic 1 Final Exam What is the molality of NaCl in a solution that is 2.5 M NaCl, with a density of 1.02 g/mL? formual mass of NaCl = 58.5 g/mol of PREVIOUS ACTIVITY second exam Type here to search
The solubilities of three salts in water are shown in the graph. For each salt, determine how much will remain undissolved if 500 g is mixed into a liter of pure water at 40 °C. One significant figure is sufficient in each answer. Pb(NO3)2: KC1: K₂Cr₂O7: OD g 6.D Solubility (g/L) 1000 900 800 700 600 500 400 300 200 100 Pb(NO3)2 K₂Cr₂O, КСІ 0 10 20 30 40 50 60 70 80 90 100 Temperature (℃)
SUBJECT : GENERAL CHEMISTRY 2 TOPIC : THE SOLUTION PROCESS AND FACTOS AFFECTING SOLUBILITY
Colligative Properties Question 14: What is the boiling point of water (in °C) after it has been salted to cook pasta? (Ko = 0.51 "C/m; Kr = 1.86 °C/m, Estimate values for the Van't Hoff factors.) Assume that you add 3 tablespoons of salt (NaCl) for every 4 quarts of water. Conversions: 1.057 quarts = 1 liter 1T salt = 17 g salt 1 g water = 1 mL water (assume density of 1 g/mL)
Can you please type out the answer, don’t write it on paper!
PLACE THE GIVEN, UNKNOWN, AND FORMULA TO USE.COMPUTE USING 3 SIGNIFICANT FIGURES FOR EACH STEP AND FOR THE FINAL ANSWER.
3. Why is molality and not molarity used to express concentration in the equations for freezing point depression and boiling point elevation?