D Question 26 1 pts The freezing point of a 0.0925 m solution of ammonium chloride...
1 point What is the freezing point of an aqueous solution prepared by dissolving 113 g potassium carbonate (K,CO3, 138 g/mol) in 2.50 kg water. Use the ideal van 't Hoff factor. [K (water) - 1.86 °C/m) -1.83 °C +1.83 °C -0.609 °C -1.23 °C Previous Submit
Calculate the molality of an aqueous solution of KBr whose freezing point is -4.95 degrees celsius. The Kf of water is 1.86 degrees C/m. Calculate the ideal Van't Hoff factor for KBr? Show work
13. A 0.230 m solution of an unknown electrolyte depresses the freezing point of water by 0.821°C. What is the Van't Hoff factor for this electrolyte? The freezing point depression constant for water is 1.86 °C/m. a. 0.521 b. 1.92 c. 2.00 d. 2.30 e. 4.41
(5 pts) At 20°C, a 0.376 M aqueous solution of ammonium chloride has a density of 1.0045 g/mL. What is the mass % of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol. 5) (5 pts) At 20°C, an aqueous solution that is 24.0% by mass in ammonium chloride has a density of 1.0674 g/mL. What is the molarity of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol. i got 3.82...
1) An aqueous solution containing 15.9 g of an unknown molecular (nonelectrolyte) compound in 103.0 g of water was found to have a freezing point of -1.5 ∘C. Calculate the molar mass of the unknown compound. b) Determine the required concentration (in percent by mass) for an aqueous ethylene glycol (C2H6O2) solution to have a boiling point of 109.3 ∘C. c) What mass of salt (NaCl) should you add to 1.90 L of water in an ice cream maker to...
Colligative properties, such as boiling point elevation, depend on the number of dissolved particles in solution. For nonelectrolytes, no dissociation occurs, and so you can use the number of moles of solute to calculate both molality and molarity. In contrast, electrolytes dissociate, and therefore the molality and molarity must be calculated based on the number of moles of dissociated particles or ions. There are two ions per formula unit of NaCl. Therefore, we would expect the freezing-point depression ΔTf of...
0 Question 36 6 pts What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C2H602) and 85.0 g H202 (For water, K - 1.86°C/m) 0 -17.6°C O-176°C O -1.50°C O 17.6°C O 1.50°C Question 37 10 pts
Question 3 1 pts Consider a 0.1 M solution of the weak acid CH3COOH with a pH of 2.88. You add NaCH3COO (sodium acetate) until the salt concentration is 0.1 M. What is the new pH? You do not need to calculate this and the numbers below are all fake. This is about the pattern. You can answer this based on your knowledge of the common ion effect and the pH scale. 1.97 2.88 3.17 6.34 7.00
1. What is the boiling point of a 3.0 m Ca(NO3)2 solution in water? Where: the change in boiling point (ΔTb) = mKb m is the molality of the solution Kb (the boiling point constant) for water is 0.512 2. The freezing point of ethanol (C2H5OH) is -114.6 °C. What is the freezing point (°C) of a solution prepared by dissolving 50.0 g of glycerin a nonelectrolyte) in 200.0 g of ethanol? Where: ΔTf = mKf The molal freezing point depression...
Q(27) The pH of a 0.050 M aqueous solution of ammonium chloride falls within what range? A) 0-2 B) 2-7 C)7-9 D) 9-12 E) 12-14 Q(28) Based on the information in the table below: which acid in aqueous solution is the weakest? Name Formula Ka Acetic Acid CH3COOH 1.8X10-5 Benzoic Acid C6H5COOH 6.3 X10-5 Formic Acid HCOOH 1.7 X 104 Hydrofluoric Acid HF 7.1 X 104 A) CH3COOH B) C6H5COOH C) HCOOH D) HF Q(29) K = 2.39 for the...