Which of the following aqueous solutions will have the lowest freezing point? 0.10 m sodium carbonate, Na2CO3 a. 0.25 m sodium nitrate, NaNO; 0.20 m ethanol, CH;CH;OH d. 0.15 m calcium chloride, CaCl2 0.30 m potassium chloride, KCI b. c. e. Indicate which of the following reactions results in a positive ASays. a. 2 Na(s) +Cl, (g) = NaCl(s) b. Zn(s)+2 HCI(aq) 5 ZnCl, (aq) +H, (g) 4 Fe(s) + 3 0, (g) 5 2 Fe,O,(s) d. 2 H, (g)+O,(g) 5 2 H,O(g) Ba(NO,),(aq) + Na, SO, (aq) 5 BaSO,(s) + 2 NaNO, (aq) c. e.

Which of the following aqueous solutions will have the lowest freezing point? 0.10 m sodium carbonate, Na2CO3 a. 0.25 m sodium nitrate, NaNO; 0.20 m ethanol, CH;CH;OH d. 0.15 m calcium chloride, CaCl2 0.30 m potassium chloride, KCI b. c. e. Indicate which of the following reactions results in a positive ASays. a. 2 Na(s) +Cl, (g) = NaCl(s) b. Zn(s)+2 HCI(aq) 5 ZnCl, (aq) +H, (g) 4 Fe(s) + 3 0, (g) 5 2 Fe,O,(s) d. 2 H, (g)+O,(g) 5 2 H,O(g) Ba(NO,),(aq) + Na, SO, (aq) 5 BaSO,(s) + 2 NaNO, (aq) c. e.

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

Determine the freezing point of the solution. (Use Kf = 1.86 °C/m.)
A neutral solution of water at a particular temperature has a concentration of OH¯ of 4.7 \ times 107 M. What is Kw at this temperature?
how is the solubility of a solid in a liquid affected by temperature?
Which of the following solutions will have the highest concentration of chloride ions? (hint: write down the dissociation of the ionic compounds in water) OA. 0.10 mol/L MgCl2 O B. All of these solutions have the same concentration of chloride ions. O c. 0.10 mol/L LICI OD.0.05 mol/L CaCl2 O E. 0.10 mol/L AICI3
Which one statement in italics is NOT correct? Other given information is correct. O a. The enthalpy change for freezing 1 mol of water is -6.0 kJ. This process is exothermic. Ob. When 1 mole of NH4NO3 dissolves in water, the temperature of the water decreases. This dissolution process is endothermic. Oc. When sodium bicarbonate decomposes, heat is absorbed from the surroundings. Thus, the decomposition of sodium bicarbonate is exothermic. O d. The condensation of steam of liquid water is exothermic. 1 mol of Ca +1 mol Br2 has a higher enthalpy than 1 mole CaBr2. Thus, the combination reaction of calcium with bromine to give calcium bromide is exothermic. Oe.
g of water. The K for Select one: 0.5°C 0.05 °C 100.05 °C 100.5 °C Calculate the mass (in grams) of potassium bromide that will be formed from 26.18 mL of a 5.26 M potassium sulfate solution. The molar mass of potassium bromide is 119 g/mol. AIBr, + K,SO,→ KBr + + Al,(SO,), Select one: 1.18 g 8.19 g 0.30 g 32.77 g Which of the following is TRUE? Select one: Cons by the system to the surrounding.
Use the graph to estimate the solubility of NaNO, in water at 40 °C.* Effect of temperature on solubility 160 140 KNO, NaNO, 120 100 KBr. 80 NH,CL 60 Na,SO, 40 NaCl 20 10 20 30 40 50 60 70 80 90 Temperature (C) 77 g/100 g H,0 no solubility 96 g/100 g H,0 O 68 g/100 g H,0 Concentration (g/100 g H,0)
A bubble of air escaping from a diver's mask rises from a depth of 159 ft to the surface where the pressure is 1.00 atm. Initially, the bubble has a volume of 10.0 mL. Assuming none of the air dissolves in the water, how many times larger is the bubble just as it reaches the surface? Use this data: 1. The density of seawater is approximately 1.025 g mL1 2. The density of mercury is 13.6 g mL-1 times larger Use your answer to explain why scuba divers constantly exhale as they slowly rise from a deep dive. Since the pressure by a factor of approximately i , the volume must by a factor of approximately i Divers exhale to the amount of gas in their lungs, so it does not to a volume than the diver's lungs. eTextbook and Media Hint Assistance Used Pressure is inversely proportional to the volume. Set up P1V1 = P2V2 and solve for V2 after you determine the pressure at 159 feet below the surface.
Which of the following phenomena is best described by Henry’s Law?a. Increasing temperature favors an endothermic process.b. The solubility of NaCl(s) in water increases with increasing temperature.c. The solubility of MgCl2(s) in water is unaffected by pressure.d. The vapor pressure of an aqueous solution of glucose, C6H12O6, is lower than the vapor pressure of pure water.e. The solubility of O2(g) in water increases with increasing pressure.
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…
Calculate the solubility of CaF, in water at 25 °C. You'Il find K, data in the ALEKS Data tab. s. Round your answer to 2 significant digits. g x10
This question already has all soltions. Please show the steps how the answers m% in red was calculated, m%=mass %