**Question:**Which of the following aqueous solutions will have the lowest freezing point?**Options:**a) \(0.10 \, m\) sodium carbonate, \( \text{Na}_2\text{CO}_3\)b) \(0.15 \, m\) calcium chloride, \( \text{CaCl}_2\)c) \(0.20 \, m\) ethanol, \( \text{CH}_3\text{CH}_2\text{OH}\)d) \(0.30 \, m\) potassium chloride, \( \text{KCl}\)e) \(0.25 \, m\) sodium nitrate, \( \text{NaNO}_3\)**Discussion:**In terms of freezing point depression, the solution with the highest number of total ions will have the lowest freezing point. Consider the dissociation of each compound in water:- Sodium carbonate (\( \text{Na}_2\text{CO}_3 \)) dissociates to 3 ions: \(2 \, \text{Na}^+ + \text{CO}_3^{2-}\).- Calcium chloride (\( \text{CaCl}_2 \)) dissociates to 3 ions: \( \text{Ca}^{2+} + 2 \, \text{Cl}^- \).- Ethanol (\( \text{CH}_3\text{CH}_2\text{OH} \)) does not dissociate.- Potassium chloride (\( \text{KCl} \)) dissociates to 2 ions: \( \text{K}^+ + \text{Cl}^- \).- Sodium nitrate (\( \text{NaNO}_3 \)) dissociates to 2 ions: \( \text{Na}^+ + \text{NO}_3^- \).Calculate the ion concentrations for each:- a) \(0.10 \times 3 = 0.30 \, m\) ions- b) \(0.15 \times 3 = 0.45 \, m\) ions- c) Non-electrolyte, so \(0.20 \, m\) molecules- d) \(0.30 \times 2 = 0.60 \, m\) ions- e) \(0.25 \times 2 =

The solutions given are a) 0.10 m sodium carbonate, Na2CO3 (i = 3) b) 0.15 m calcium chloride,…

Which of the following aqueous solutions will have the lowest freezing point? Oa) 0.10 m sodium carbonate, Na₂CO3 Ob) 0.15 m calcium chloride, CaCl₂ O c) 0.20 methanol, CH3CH₂OH d) 0.30 m potassium chloride, KCI 0.25 m sodium nitrate, NaNO3

Which of the following aqueous solutions will have the lowest freezing point? Oa) 0.10 m sodium carbonate, Na₂CO3 Ob) 0.15 m calcium chloride, CaCl₂ O c) 0.20 methanol, CH3CH₂OH d) 0.30 m potassium chloride, KCI 0.25 m sodium nitrate, NaNO3

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

An aqueous solution of ethanol (molar mass = 46.07 g/mol) has a molality of 12.15 m and a density of 1.100 g/mL. What is the molarity of ethanol in the solution?
Say you added a 6.0 M of NaOH solution to an aqueous solution of NaCl (NaCl in H2O). Would the addition of the NaOH solution change the identity of the NaCl solute in the water?
Which of the following 0.300 M solutions would contain the highest concentration of potassium ions? potassium bromide potassium hydrogen carbonate potassium iodide potassium hypochlorite potassium phosphate
The diagram below shows the different parts of a solution. Match each letter to the term it represents in the diagram. solution A B Solubility a b C 0 C 3] X
What is the mass percent of an aqueous sodium hydroxide solution in which the molarity of NaOH is 9.98 M? The density of the solution is 1.33 g/mL.
Which of the following phrases best describes the term solubility? the ability of a solvent to dissolve in a solute the ability of a solute to dissolve in a solvent the maximum amount of solute that will dissolve in solvent at a given temperature the maximum amount of solvent that will dissolve in a solute at a given temperature the amount of solvent that dissolves in a solute for each 10oC rise in temperature
If a 24 g sample of a nonelectrolyte is dissolved in 156 g of water, the resulting solution will freeze at –1.13°C. What is the molar mass of the nonelectrolyte?
Name and Concentration Ionic or Covalent Bond (Solute) Electrolyte or Non-electrolyte Isotonic, Hypertonic, or Hypotonic Deionized water (solvent) 0.5 M glucose 1 M glucose 3 M glucose 0.25 M KCl 0.5 M KCl 1.5 M KCl
< 11 of 19 I Review Constants | Periodic Table Part B A student placed 16.0 g of glucose (C6H12O6) in a volumetric flask, added enough water to dissolve the glucose by swirling, then carefully added additional water until the 100. mL mark on the neck of the flask was reached. The flask was then shaken until the solution was uniform. A 45.0 mL sample of this glucose solution was diluted to 0.500 L. How many grams of glucose are in 100. mL of the final solution? Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) ? Value Units
Predict the gas that is expected to have the highest molar concentration in aqueous solution at a fixed temperature and pressure? CO2 O Ne O H2 O N2
Which of the following solutions will boil last under identical heating? (Do not forget that some things may dissociate, forming more ions) 0.020 M glucose O 0.020 M NaCl O 0.015 M CaCl₂ O 0.010 M HCI O 0,010 M Na₂S
Suppose a 0.036M aqueous solution of phosphoric acid (H3PO4) is prepared. Calculate the equilibirum molarity of HPO4^2- Round your answer to 2 significant figures.