Calculate the freezing point of an aqueous 0.10 m FeCl3 solution using a van’t Hoff factor of 3.2.

Q: The freezing points of 0.0956 mammonium chloride and 0.0388 mammonium sulfate in water were found to…

A: In dilute solution the Van't Hoff factor for a salts are the number of ions produced by one formula…

Q: The freezing point of a 0.20 m solution of magnesium sulfate (MgSO4) is −1.8°C. What is the value of…

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Q: Calculate the molality and van't Hoff factor (i) for the following aqueous solution: 0.750 mass %…

A: Colligative properties are the properties which depend on the number of atoms or molecules or ions…

Q: what is the molality of a solution if a nonvolatile solute increased the boiling point of pure…

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Q: A student dissolves 35g of CaCl2in 150.g of water and finds the freezing point of the solution to be…

A: Molar mass of CaCl2   = 111g/mol

Q: A 0.50 m MgSO4 solution has a Van 't Hoff factor of 1.30, find the freezing point for this solution?…

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Q: If a 0.650 molal aqueous solution freezes at −2.50 ∘C, what is the van't Hoff factor, i, of the…

A: Since we know that  ∆Tf = i kf m  Where ,            ∆Tf = depression in freezing point…

Q: van't Hoff factor

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Q: The osmotic pressure of a 0.010 M aqueous solution of CaCl2 is found to be 0.674 atm at 25 °C.…

A: When a substance is dissolved in a solvent, the ratio between the actual concentration of the…

Q: A 0.95 m aqueous solution of an ionic compound with the formula MX has a freezing point of -3.0 °C.…

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Q: What is the minimum mass of ethylene glycol (C2H6O2) that must be dissolved in 14.5 kg of water to…

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Q: freezing points

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Q: 14. The freezing point of a 0.0925 m solution of ammonium chloride was found to be -0.325°C. What is…

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Q: If a 0.640 m aqueous solution freezes at -3.40 °C, what is the van't Hoff factor, i, of the solute?…

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Q: A 1.2 m aqueous solution of an ionic compound with the formula M2X3 has a boiling point of 102.8oC.…

A: The value for van't Hoff factor gets altered as per the compound's nature. It gets symbolized as…

Q: The osmotic pressure of 0.010 M solution of CaCl2 and urea at 25 degrees celsius are 0.605 atm and…

A: Given : Osmotic pressure of CaCl2 solution = 0.605 atm Osmotic pressure of urea solution = 0.245 atm…

Q: The boiling point of an aqueous 1.83 m (NH4)2SO4 (molar mass = 132.15 g/mol) solution is 102.5°C.…

A: Given; Boiling point of aqueous  (NH4)2SO4  solution (Tb) = 102.5°C Boiling point of pure water…

Q: What is the  vant Hoff  factor if  0.15 m CrCl3 freezes at -0.91oC?

A: Van't Hoff Factor can be calculated as  The number of ions observed in the solution/ total moles of…

Q: Predict the freezing point of a solution prepared by dissolving 8.9 g MgCl2 in 98 g H20. Kf for…

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Q: When 74.7 g of urea (CH₂N₂O). are dissolved in 900. g of a certain mystery liquid X, the freezing…

A: Given: Mass of urea is 74.7 g. Mass of liquid X is 900 g or 0.9 kg. Mass of KBr is 74.7 g. To find:…

Q: A 1.0 m solution of K2SO4 in water has a freezing point of -4.3 °C. What is the value of the van't…

A: since you have posted a multiple questions in single session, we are entitiled to answer only first…

Q: Calculate the molality of a solution containing 10.8 g of ethylene glycol (C2H6O2) in 360 g of…

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Q: A 7.00 x 10-² M aqueous solution of aluminium chloride (AlCl3) is prepared for use in an experiment.…

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Q: What is the Van't Hoff factor (i) of Titanium (IV) nitrate when dissolved in water? Assume ideal…

A: Van't Hoff factor (i) is equal to the number of ions that a molecule of a given substance will form…

Q: A 4.2 m aqueous solution of an ionic compound with the formula MX2 has a boiling point of 103.5 ∘C.…

A: Given:Molality = 4.2 m = 4.2 mol/kg.Boiling point of solution = 103.5 ℃.Boiling point of water = 100…

Q: When 66.8 grams of a solute (molar mass = 56.8 g mol–1) was dissolved in 375.4 grams of water, the…

A: Given data: To (boiling point of water) is 100.0°C Tb (boiling point of solution) is 105.1°C Kb of…

Q: A 2.86 g magnesium chloride, MgCl2 (MW = 95.211 g/mol) in a 1L solution at 25°C has an osmotic…

A: Weight of magnesium chloride= 2.86g MW of MgCl2=95.211g/mol  Volume=1L Osmotic pressure=2.15 atm…

Q: The osmotic pressure of a 0.010 M potassium iodide (KI) solution at 25°C is 0.465 atm. Calculate the…

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Q: For each of the following substances, determine the ideal van't Hoff factor when dissolved in water…

A: Vant Hoff factor is the ratio between the actual concentration of the particles produced when the…

Q: The osmotic pressure of 1.66 x 102 M solutions of CaCl, and urea at 25°C are 1.01 and 0.407 atm,…

A: Molarity of the solution ( CaCl2 and urea ) = 1.66 × 10-2 M Temperature of the solution T = 25 °C =…

Q: A 0.137 m solution of sodium ferrocyanide (NaFe(CN)6.10H2O) in water has a freezing point depression…

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Q: A 2 molal aqueous solution boiled at 102.0°C at sea level. At what temperature was it expected to…

A: the aqueous solution is expected to boil at 100 degree Celsius. vant hoff factor can be calculated…

Q: If a 0.900 m aqueous solution freezes at -2.00 Celsius, what is the van't Hoff factor, i, of the…

A: Given: Molality of solution = 0.900 m Freezing point of solution = -2.00oC Freezing point of pure…

Q: Determine the Van’t Hoff factor for the following solutions: a. 0.25 M KCl b. 0.0017 M CaCl2…

A: Van’t Hoff factor is the number of moles of ions produced by the dissolution of 1 mole of salt.

Q: A2.4 m aqueous solution of an ionic compound has a boiling point of 102.7°C. Calculate the van't…

A: Given, molality = 2.4 m Boiling Point of compound = 102.7 oC Boiling Point of water = 100 oC ∆Tf  =…

Q: 29.4 g of potassium sulfate (K2SO4, 174.258 g/mol) are dissolved in 248 g of water. The van't Hoff…

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Q: . A 0.137 m solution of sodium ferrocyanide (NaFe(CN)6.10H20) in water has a freezing point…

A: Given-> Molality = 0.137 m Freezing point depression = 0.755 °C Kf = 1.86 °C/m

Q: A water solution containing an unknown quantity of a non electrolyte solute has a freezing point of…

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Q: A mixture of table salt and ice is used to chill the contents of hand-operated ice-cream makers.…

A: Given, van’t Hoff factor, i = 1.44Then,

Q: Choose the aqueous solution that has the highest boiling point. Assume ideal van't Hoff factors. O…

A: Boiling point elevation: The formula used here is, ∆Tb = i × Kb × m Tb(solution) - Tb°(water) = i ×…

Q: Assuming ideal solution behavior, what is the freezing temperature of a solution of 115.0 g of…

A: Given : mass of sucrose i.e solute = 115 g and molar mass or formula weight = 342.3 g/mol And mass…

Q: What is the Van't Hoff factor of Carbon Monoxide when dissolved in water? Assume ideal behavior

A: van't Hoff factor is actually the measurement of solute effects on collegtive properties such as ,…

Q: From your predicted value of the van't Hoff factor, calculate the boiling point of a 1.62  m aqueous…

A: When a solute is dissolved in water, the boiling point of water is incresed known as elevation in…

Q: Define the following terms :(i) Mole fraction(ii) Isotonic solutions(iii) van’t Hoff factor(iv)…

A: “Since you have asked multiple questions, we will solve the first three question for you. If you…

Q: When 153. g of glycine (C,H,NO2) are dissolved in 1400. g of a certain mystery liquid X, the…

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Q: A 1.2 m aqueous solution of an ionic compound with the formula MX2 has a boiling point of 101.4 °C.…

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Q: Which of these substances is expected to have the smallest ideal van't Hoff factor in very dilute…

A: Van't Hoff factor of any compound is defined as the number of ions produced by the dissociation of 1…

Q: Assuming ideal solution behavior, what is the boiling point of a solution of 150.0 g of nonvolatile…

A: The boiling point of water is 100 degree centigrade and the freezing point of the water is 0 degree…

Q: If a 0.630 m aqueous solution freezes at -3.10 °C, what is the van't Hoff factor, i, of the solute?…

A: Use the relation  ∆Tf=ikfm

Q: b) List the following solutions in order of decreasing freezing point: 0.04 molal glycerol (C3H8O3);…

A: b) Given: Molality of C3H8O3 = 0.04 m Molality of KBr = 0.025 m And molality of C6H5OH = 0.030 m

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.