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A: A dimensional quantity from the following has to be selected.
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Q: why is the mass of water in the molality solution 240. Is that not the mass of the solution and not…
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Q: List two applications of freezing point depression.
A: Colligative properties: The colligative properties are those properties of solutions that depend on…
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Q: In the determination of molecular weight through freezing point depression analysis. The volume of…
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A: Given that, when red blood cells enter a hypertonic solution? The cells contract as water diffuses…
Q: 1.Define the following concentration terms and give their unit A. Percentage by mass B. Mole…
A: A. Percentage by mass ( mass % ) It is the percentage ratio of mass of solute to mass of…
Q: Molarity Molality Normality Mole fraction Percent composition Percent Yield
A: Number of moles = mass(g)/ molar mass Number of gmEq = weight of substance /equivalent weight of…
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Q: Which of the following is expected to form an ideal solution?
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Q: number of moles of the solution mole fraction of the solute What is its -mole fraction of the…
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Q: Calculate the freezing point, in degrees Celsius, of a solution c
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Q: A solution contains 3.86g of magnesium chloride and 250g of water. Compute for the freezing point…
A: Applying formula ∆T = i×kf×m
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Q: Why does a gas mixed with another gas not form a colloidal system?
A: A heterogeneous mixture of two distinct states of matter is termed as a colloid system. There isa…
Q: Why are boiling point elevation and freezing point depression considered colligative properties?
A: Colligative property: Properties which depends upon the number of solute particle present in the…
Q: A solution contains 3.86g of magnesium chloride and 250g of water. Compute for the freezing point…
A: Freezing point of solvent is greater than freezing point of solutions
Q: The number of moles of the three components A, B and C in solution are, respectively, equal to 14,…
A: Answer :- Mole fraction of A = 0.14 Mole fraction of B = 0.25 Mole fraction of C = 0.61…
Q: Suppose you dissolve a solute in water that results in a freezing point temperature of -0.19 degrees…
A: When solute molecules are introduced to a solvent, the depression in freezing point is observed…
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A: The difference between strong and weak electrolyte are given in step two.
Q: Calculate the osmotic pressure of a solution
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A: While rounding off, we need to round off to least number of significant digits required.
Q: How can we calculate the freezing point of a solution prepared from a solvent and nonvolatile…
A: Given : Non-volatile solute in a solution To find : Calculation of a freezing point of solution.…
Q: What is the boiling point elevation of a 1 molal aqueous solution?
A: Elevation in boiling point is observed when a non-volatile solute is added to a pure solvent to form…
Q: The molality concentration defines as the No. of moles of solute per 1 kg. of solvent true False
A: We have given a statement and we have to find that the statement is true or false. Statement : The…
Q: Compute the freezing point of 0.5 moles of bromine (Br2) dissolved in 507 grams of chloroform.
A: Moles of bromine = 0.5 mol Mass of chloroform = 507 g= 0.507kg Molality = 0.5mol/0.507kg = 0.986 m…
Q: the van't Hoff factor i for iron chloride,
A: Given :- depression of freezing point = 0.2976 °C molality = 0.050 m kf = 1.86 °C/m To calculate…
Q: What is the osmotic pressure, in atm,
A: Formula :- π = iCRT where π is osmotic pressure i is Van't hoff factor C is the molar…
Q: Why is the freezing point of a pure solvent constant, while that a solution decrease with steady…
A: The depression is a colligative property in the freezing point of a solution i.e. it depends upon…
Q: how do you find the osmotic pressure with given the temperature
A: Osmosis is a process in which solvent Molecules move from lower concentrated solution to higher…
Q: The freezing point of a 1 liter aqueous solution containing 10g of an unknown solute is -0.1 °C.…
A: We know that ∆Tf = kf ×m×i
Q: nd Datasheet a dilute solute that is nonvola na concentrated solute that is
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- a concentrated H2SO4 has the following composition specific gravity 1.84 and purity of H2SO4 is 97 percent by weight. express in mole/LShow calculations for the experimental percentage of water for Trial 1Percentage of Water in Hydrate AverageIn benzene, dimerization occurs with benzene due to hydrogen bonding. In 110 g of benzene, 1.70g of acetic acid is dissolved that increases the boiling point by 0.40 oC. What is the expected degree of association of acetic acid? (Use Kb=2.57 Kg mol-1 )?
- Example: Calculation the weight of barium iodate Ba(IO3)2 if it dissolved in 500mL of distilled water (D.W) at 25 °C if M.wt of ppt = 487 g/mole and %3D Ksp= 1.57x10.Polyethylene glycol 400 (PEG400) is a nonvolatile liquid polymer, which when mixed with water canbe used as a base for parenteral formulations. The designation “400” means that the molecular weightof PEG molecules is approximately 400 g/mol. Preparation with water (ΔHv = 40.7 kJ/mol) requires that the two be mixed at 56 oC, at which the equilibrium vapor pressure of pure water is 16.5 kPa. a. If 105 g of PEG400 are added to 500 g of water at 56 oC, what will the boiling temperature of the solution be?Some water dissolves in liquid methane at -161°C to givea solution in which the mole fraction of water is 6.0 × 10-5. Determine the mass of water dissolved in 1.00 L ofthis solution if the density of the solution is 0.78 g cm-3.
- Osmotic pressures are often reported in units of atmospheres or mm Hg. The latter impliesthat the height of a column of liquid can be used as a measure of pressure. This is, in fact, thebasis of the torricellian barometer from which the units of “torr” come. The pressure, P, isrelated to the height of the column by:P = ρghwhere ρ is the density of the liquid, g is the acceleration due to gravity and h is the height. Whatwill be the height (in mm) of a column of aqueous solution with a density of 0.9987 g/mL, if theosmotic pressure of the solution at 25 °C is 1.4 mm Hg? The density of mercury at thistemperature is 13.8 g/mLIf 124.4 mL of water is shaken with oxygen gas at 0.81atm, it will dissolve 0.0036 g O2. Estimate the Henry's law constant for the oxygen gas in water in units of g mL ^-1atm^-1.You are handed a 15.85% by mass aqueous KCl (m.m. = 74.5513 g mol–1) solution (at 25 °C). Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the following: Vapor pressure of the solution in atm
- d.Under what temperature and pressure (high / low) conditions do real gases behave ideally? Explain your answer. e. If you had two solutions, and you added equal molar amounts of NaCl to one and CaCl2 to the other, which of these two solutions had the greatest freezing point depression? What if instead of NaCl we used KCl, would that change the result? Explain your answer. f. Explain the hydrophobic effect. (0.5 Bonus: which thermodynamic property is at the origin of this effect) SHORT ANSWER PLEASE279.28 mL of 1.22 M organic salt was mixed with 168.14 mL of Ethanol (d= 0.789 g/mL, MW 46.07g/mole). Pure ethanol has a vapor pressure of 0.059 atm what will be the vapor pressure of the solution?You are handed a 15.85% by mass aqueous KCl (m.m. = 74.5513 g mol–1) solution (at 25 °C). Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the following: Boiling point of solution (in °C to one decimal place) Freezing point of solution (in °C to two decimal places) Vapor pressure of the solution (in atm to three decimal places) Osmotic pressure (in atm to three decimal places)