Given: Mass of lauric acid (g): 8.000g Mass of benzoic acid (g): 1.027g Freezing temperature of pure lactic acid(°C): 43.3°C Freezing point of the benzoic acid-lauric acid mixture(°C): 39.8°C   Question: Calculate molality (m,) in mol/kg, using the formula ΔTf = m × Kf. The Kf value for lauric acid is 3.9°C x kg/mol.

Q: The normal freezing point of cyclohexane is 6.50 °C. A solution is prepared by dissolving 258.0 mg…

A: Here the solvent is cyclohexane whose Kf value is 20.0 oC/m, and the solute is the unknown…

Q: The freezing point of a pure solvent was 7.39 ºC .  A solution of 5.00 g of an unknown…

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Q: The normal boiling point of a certain liquid X is 133.8 °C, but when 65. g of urea ((NH,),CO) are…

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Q: pure solvent has a freezing point of 23.6°C with a mass of 58.69g. Solute is added to solvent where…

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Q: 1) What is the molality of the solution with a boiling point elevation of 2.56 degrees Celsius? The…

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Q: 6.) Calculate the molality of the solution (m) Use the equation: Tf (solution) – Tf (solvent) = –i…

A: Molality = number of moles of solute ÷ mass of solvent in kg

Q: What is the freezing and boiling point of an electrolyte solution containing 5.0 grams sodium…

A: You have given the following data - mass of solute, w = 5..0 g Volume of Solute, V = 800 mL = 0.800…

Q: 5.152g of Na2CO3(s) is added to 75.0mL of water at 21.20°C. When the dissolution is complete, the…

A: Molarity of the solution can be calculated by using Following formula - Molarity = mass×1000/molar…

Q: 8. What is the freezing point of a solution of 12.0 g of CCl4 dissolved in 750.0 g of benzene? The…

A: Find the freezing point of a solution of carbon tetrachloride dissolved in benzene.

Q: on of the solute, how many grams of KNO3 must be added to 275 mL of water to produce a solution that…

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Q: 13.65 g of an unknown compound decreased the freezing point of 346 g of benzene (Kf= 5.12 ∘C  /m) by…

A: Given:: Mass of unknown = 13.65 g Molar mass = x = ? Kf= 5.12 ℃ m-1 Depression in freezing point ,…

Q: Highways are salted to reduce ice on roads. What is the freezing point when 2 samples of 125 g NaCl…

A: When a non-volatile solute is added to a solvent, the freezing point of a solvent decreases and this…

Q: - 1 The molal freezing point depression constant K₁=2.02 °C-kg-mol for a certain substance X. When…

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Q: When 28.2 g of urea (CH4N₂O) are dissolved in 1150. g of a certain mystery liquid X, the freezing…

A: Given,mass of urea ( CH4N2O ) = 28.2 gmass of solvent 'X' = 1150. gchange in freezing point of urea…

Q: (a) Differentiate between molarity and molality in a solution. What is the effect of temperature…

A: a) The molarity is the concentration term that can be expressed as the mathematical ratio between…

Q: A certain liquid X has a normal freezing point of 3.70 °C and a freezing point depression constant…

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Q: Colligative Properties The boiling point of chloroform (CHCl3) is 61.7C.  When a nonvolatile solute…

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Q: When 397.g of benzamide C7H7NO are dissolved in 1400.g of a certain mystery liquid X, the freezing…

A: First of all we calculate the Kf of mystery liquid X using benzamide. For this purpose we use…

Q: The freezing point of water H2O is 0.00°C at 1 atmosphere. A nonvolatile, nonelectrolyte that…

A: The depression in the freezing point is a colligative property and it is directly proportional to…

Q: A certain liquid X has a normal freezing point of -4.00 °C and a freezing point depression constant…

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Q: What is the freezing point of a 1,4-dioxane solution if that same solution boils at 103.0 °C? The…

A: From the formula of elevation in boiling point, and depression in freezing point, we can solve the…

Q: 1. A student determines the molar mass of methanol, CH3OH by the same method used in this…

A: Answer: This question is based on the colligative property of the solution. Colligative property of…

Q: Suppose that a solution made from an unknown solute dissolved in solvent X. Its molality is 0.0125…

A: Given: The molality of the solution is 0.0125 m. Its boiling point of unkown solute is 0.047°C more…

Q: When 498. mg of a certain molecular compound X are dissolved in 25.0 g of dibenzyl ether…

A: A numerical problem based on properties of liquids. A set of data for depression of freezing point…

Q: When 258. g of alanine (C,H,NO,) are dissolved in 850. g of a certain mystery liquid X, the freezing…

A: Recall the following relation for depression of freezing point of a solution…

Q: Please provide detailed solution and give the explanation of the concept..

A: The freezing point of a solution is lower than that of the pure solvent. This is known as freezing…

Q: When 6.31 g of a certain nonvolatile solute is dissolved in 505 g of water, the freezing point of…

A: Given data is as follows: The mass of nonvolatile solute = 6.31 g The mass of water = 505 g = 0.505…

Q: Suppose that a solution made from an unknown solute dissolved in solvent X. Its molality is 0.0125…

A: Answer

Q: 15.2 g of camphor dissolved in naphthalene lower the freezing temperature of naphthalene from 80.0…

A: Given: Mass of camphor=15.2 g Molar mass of camphor=152 g/mol Lowered freezing point of…

Q: 17.55 g of an unknown compound decreased the freezing point of 138 g of benzene (Kf= 5.12 ∘C  /m) by…

A: Detail mathematical calculation is shown below

Q: student determines the molar mass of methanol, CH3OH by the same method used in this experiment.…

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Q: The normal freezing point of a certain liquid x is -6.20 °C, but when 36. g of iron(III) chloride…

A: We will calculate the molal freezing point depression constant Kf. Given: The normal freezing point…

Q: Camphor, C10H16O, melts at 179.8˚C, it has particularly large freezing point depression constant, Kf…

A: Given:  Camphor,C10H16O melts at 179.8˚C freezing point depression constant, Kf = 40.˚C/molal…

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

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Q: Assuming that NaCl will dissolve perfectly and form an ideal solution, what mass of NaCl is needed…

A: The freezing point depression is calculated by using the following formula. ∆Tf = m×Kf Where, Kf =…

Q: 1-A sample of pure t-butyl alcohol weighing 6.22 g was found to have a freezing point of 24.7 °C.…

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Q: At 300 K consider a colloidal solution, M = 150 kg/mol, in a gravity field. If the concentration of…

A: Temperature = 300K Mol mass = M = 150kg/mol Colloid concentration at top = Mtop = 0.0008M Colloid…

Q: Given that the value of kf for water is 1.86°C/m, what is the freezing point of an aqueous solution…

A: given mass of NaCl = 427 g molar mass of NaCl = 58.5g mass of water = 1kg Kf of water = 1.86°C/m New…

Q: When 5.71g of naphthalene is added to 152g of benzene the solution freezes at 3.98 degrees Celsius.…

A: Recall the data from the question, mass of naphthalene=5.71 g mass of solvent=152 g  Solvent in…

Q: a) Calculate the freezing point of a solution containing 13.2 gg FeCl3FeCl3 in 156 gg water. b)…

A: Three numerical problems based on colligative properties, which are to be accomplished.

Q: 3. You are asked to calculate the Kf for t-butyl alcohol (MW = 74.122 g/mol). You gather the…

A: Given data:Determine the key information needed to calculate the The freezing point is defined as…

Q: Benzene is a common industrial solvent (molar mass: 78.11 g/mol). Its normal freezing point is 5.50…

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Q: Given that the value of Kf for water is 1.86°C/m, what is the freezing point of an aqueous solution…

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Q: The freezing point of a liquid will change when a solute is added. Explain how the addition of salt…

A: Freezing point depression of a solution means addition of a solute to a solvent lowers the freezing…

Q: A 6.06-gram sample of a compound is dissolved in 250. grams of benzene. The freezing point of this…

A: Given: The mass of the unknown compound dissolved in benzene = 6.06 g The mass of benzene = 250 g…

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.