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 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.

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

5. Calculate the solubility (g/L) of Ag;PO4 (Mw= 419 g/mol). Ksp = 1.8 x 10-18

Magnesium chloride is often used to melt ice on sidewalks. Considering that the solubility of magnesium chloride (95.21 g/mol) in water is 54.3 g per 100.0 g of water, what is the lowest temperature that you would expect to be able to melt ice with magnesium chloride? Assume ideal behavior. (Kf(water)= 1.86°C/m) A. -29.2°C B. -31.8°C C. -25.0°C D. -10.6°C E. -41.0°C

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

Consider a 1.000-L stock solution of 9.69 M Na3PO4. A 2.000-mL aliquot is taken from this stock solution and diluted to a final volume of 1.000 L. A 5.000-mL aliquot is then taken from this new solution and further diluted to make a new solution with a final volume of 750.0 mL.   Calculate Na+ in the final solution.