1. All of the fundamental principles below are important in understanding the formation of solutions except which one? (A) Molecules with similar molecular masses are required to form solutions. (B) Starting at equilibrium, moving particles apart while in the solid or liquid phases requires added energy proportional to the attractive forces. (C) Bringing particles together releases energy in proportion to their attractive forces. (D) The total energies in steps 1 to 3 indicates if a solution will form.

1. All of the fundamental principles below are important in understanding the formation of solutions except which one? (A) Molecules with similar molecular masses are required to form solutions. (B) Starting at equilibrium, moving particles apart while in the solid or liquid phases requires added energy proportional to the attractive forces. (C) Bringing particles together releases energy in proportion to their attractive forces. (D) The total energies in steps 1 to 3 indicates if a solution will form.

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

3. If 122.3 grams of strontium chloride is mixed with 925.0 g of water, what will the freezing and boiling point of the resulting solution be?
A recent snowstorm had the potential to create icy road conditions, which led to the closure of several roads in the area. One way ice on the road could be reduced is to apply a layer of NaCl. The expected rainfall for the area was approximately 6.0 inches, which would have created about 1.75 liters of standing water per square foot. How much NaCl, in grams, per square foot would have to be used to prevent ice formation if the temperature was only supposed to reach -2.5 C°? The kf of water is 1.86 1/C*mc and the density is 1 g/mL.
Will the calculated Molarity of NaOH be too high or too low or unaffected if the following happen: When you answer the question, consider how the situation affects the calculation of molarity of NaOH and moles NaOH, which is calculated from the mass of KHP. For each answer, you must supply a clear explanation for your answer. Often times, students will restate the facts rather than explaining why they chose the answer they chose. a) You add the weighed KHP to a flask containing a 60mL of water rather than 50 mL of water. Explain. Your answer must contain a well-thought-out and clearly written explanation. b) The buret is still wet with water on the inside when you add your NaOH solution. Explain c) The KHP is wet when you weigh it. Explain. d) You titrate past the equivalence point by 0.50mL Answer a-d
at a certain temperature,1.85 grams of barium hydroxide will dissolve to form 100.0 ml of a saturated barium hydroxide solution. the molar mass barium hydroxide is 171.34 grams/mole. what is the concentration of the solution in unit molarity? what is the constitution of the hydroxide ion in the same solution?
14) Which of the following terms best describes a carbonated beverage?(a) compound (b) heterogeneous mixture(c) homogeneous mixture (d) substance(e) none of the above show step solutions 15) Alum is used in styptic pencils to stop minor bleeding. If the formula is Al2(SO4)3 what is the total number of atoms in one formula unit of alum?(a) 10 (b) 12 (c) 14 (d) 17 (e) 2116) Using atomic notation, indicate the isotope having 25 p+, 30 n0,and 25 e-a. 2580Mn b. 2555Mn c. 5525Mn d. 2555Zn e. 3055Zn Show step by step solutions 17) Element X has two natural isotopes: X-6 (6.015 amu) and X-7 (7.016 amu).Calculate the atomic mass of element X given the abundance of X-7 is 92.5%.(a) 6.09 amu (b) 6.50 amu(c) 6.52 amu (d) 6.94 amu(e) 12.5 amu Show step by step solutions 18) Which of the following photons of visible light is most energetic?(a) blue (b) red(c) violet (d) yellow(e) all visible light photons have the same energy Show step by step solutions 19) Which element has the following…
A sample of 0.892 g of potassium chloride (KCl) is dissolved in 54.6 g of water. What is the percent by mass of KCl in the solution?
In a laboratory, a 15.0 mL sample of KCl solution is poured into an evaporating dish with a mass of 24.10 g. The combined mass of the evaporating dish and KCl solution is 41.50 g. After heating, the evaporating dish and dry KCl have a combined mass of 28.28 g. a) what is the mass percent (m/m) of the KCl soultion? b) what is the molarity (M) of the KCl soultion? c) if water is added to 10.0 g of the inital KCl solution to give a final volume of 60.0 mL, what is the molarity of the diluted KCl soultion?
A student adds 6.00 g of a solid to 30.0 mL of water. The solid has a molar mass of 72.0 g/mol. What is the molar concentration of the solution? (If necessary to the calculation, assume that 1.00 mL of water has a mass of 1.00g and that the solution volume is 30.0 mL.
A chemistry student adds a quantity of an unknown solid compound X to 550. mL of distilled water at 30.° C. After 10 minutes of stirring, all of the X has dissolved. The student then drains off the solution and evaporates the water under vacuum. A precipitate is left behind. The student washes, dries and weighs the precipitate. It weighs 19.3 g. O yes Ox10 Using only the information above, can you calculate the solubility of X in water at 30.° C? O no If you said yes, calculate it. Be sure your answer has a unit symbol and the right number of significant digits.
2) If iron(II) sulfate is heated too strongly, the following reaction will occur FeSO4(s) FeO(s) + SO3(g) Wo Migl If you are heating a sample of FeSO4 6H₂O and this reaction occurs along with dehydration, what will happen to the experimental percent water? Explain your answer.
Colligative properties are those that depend on the number of solute particles. Because electrolytes dissociate into ions, the concentration of particles in the solution is greater than the formula-unit concentration of the solution. For example, if 1 mol of NazSO4 totally dissociates, 3 mol of ions are produced (2 mol of Nat ions and 1 mol of SO, ions). Thus, a colligative property such as osmotic pressure will be three times greater for a 1 M NazSO, solution than for a 1 M nonelectrolyte solution. Part A Assuming complete dissociation of the solute, how many grams of KNO3 must be added to 275 mL of water to produce a solution that freezes at - 14.5 °C? The freezing point for pure water is 0.0 °C and Kf is equal to 1.86 °C/m. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) However, complete dissociation of electrolytes does not always occur. The extent the van't Hoff factor, i: dissociation is expressed by HA moles of…
Draw some simple pictures to illustrate at the atomic level the dissolution of solid sodium chloride (salt) in water that you observed. Be sure to indicate solute-solute, solute - water, and water - water interactions, as appropriate on your diagrams.