The resultant solution had a freezing point of 177.9 °C when 0.270 g of the solute was dissolved in 50.0 g of C10H160. (Kt = 37.7 °C.kg/mol for pure C10H160 at 179.8 %3D °C.) The quantity of CO2 generated when 0.270 g of the substance was burnt in excess of O2 reacted fully with 20.0 mL of 2.00 M KOH solution according to the equation. 20H-(aq) + CO2(g) → CO3-2(aq) + H2O(1) What is the molecular formula of the compound? C6H6 C6H12

The resultant solution had a freezing point of 177.9 °C when 0.270 g of the solute was dissolved in 50.0 g of C10H160. (Kt = 37.7 °C.kg/mol for pure C10H160 at 179.8 %3D °C.) The quantity of CO2 generated when 0.270 g of the substance was burnt in excess of O2 reacted fully with 20.0 mL of 2.00 M KOH solution according to the equation. 20H-(aq) + CO2(g) → CO3-2(aq) + H2O(1) What is the molecular formula of the compound? C6H6 C6H12

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.39QE: The density of a 3.75 M aqueous sulfuric acid solution in a car battery is 1.225 g/mL. Express the...

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The density of a 3.75 M aqueous sulfuric acid solution in a car battery is 1.225 g/mL. Express the concentration of the solution in molality, mole fraction H2SO2, and mass percentage of H2SO4.
The maximum solid solubility of carbon in ferrite occurs at 0.022 wt% C and 727 ° C, the eutectoid composition is 0.76 wt% C, the maximum solid solubility of carbon in austenite occurs at 2.14 wt% C and 1147 ° C, and the cementite composition is 6.7 wt% C. For 2122 g of a 3.2134 wt% C steel at 726 ° C, what will be the mass of carbon present as part of a compound?(a) 67.9 g(b) 74.2 g(c) 58.7 g(d) 83.5 g
An excess amount of Ba(NO3)2 was added to 2 liters of water at 25 oC until the solution is saturated. Because Ba(NO3)2 is only slightly soluble in water, the excess Ba(NO3)2 was filtered out to get a solid-free mixture. The proponents of the experiment thought about using the concept of colligative properties, specifically boiling point elevation, to determine Ksp. It was observed in their experiments that the solution boils at 100.15 deg C. Kb of water = 0.51 K-kg/mol. Barium nitrate dissociates using: Solve the ff: a) Amount of Ba(NO3)2 dissolved in grams. MW of Ba(NO3)2 = 261.3 g/molb) Solubility product, Kspc) Vapor pressure of the solution in kPa
For the calculation of the solubility c of a gas in a solvent, it is often convenient to use the expression c = Kp, where K is the Henry’s law constant. Breathing air at high pressures, such as in scuba diving, results in an increased concentration of dissolved nitrogen. The Henry’s law constant for the solubility of nitrogen is 0.18 μg/(g H2O atm). What mass of nitrogen is dissolved in 100 g of water saturated with air at 4.0 atm and 20 °C? Compare your answer to that for 100 g of water saturated with air at 1.0 atm. (Air is 78.08 mol per cent N2.) If nitrogen is four times as soluble in fatty tissues as in water, what is the increase in nitrogen concentration in fatty tissue in going from 1 atm to 4 atm?
A solution is prepared by dissolving iodine, I2, in tetrachloromethane,CCI4 at 25 °c. What are the mole fractions of the solute and solvent for a solute of molality 0.100 mol kg-1? Hence calculate the change in the chemical potential of the solvent caused by the solute.
What mass of a non-electrolyte solute is required, when mixed with 225 g H2O, to change the equilibrium vapor pressure of H2O from 1.013 x 105 Pa to 8.104 x104 Pa, at approximately 110 °C? The molar mass of the non-electrolyte solute is 62.07 g mol−1. Assume ideal behaviour for the solution.
A student using a calibrated solution calorimeter measured a temperature decrease of 1.10 K when 1.00 g of KNO3 was added to 74.40 g of deionized water in the calorimeter. The specific heat capacity of the solution calorimeter was found to be 4.15 J/gK. Calculate the experimental value of the molar heat of solution of KNO3, ΔH soln. Was the dissolution of this salt exothermic or endothermic?
The osmotic pressure at the base of a houseplant kept at 27ºC is 1.6 × 104 N/m2. Calculate the molar concentration of the dissolved molecules in the plant’s veins if there are no dissolved molecules in the soil water.
The solubility of alum in 25 mL 1.4 M KOH plus 10 mL 9 M H2SO4 (our solution) is approximately 1.0 g at 1.0 °C, and 1.7 g at 6.0 °C. Estimate the amount of alum left in the solution if the temperature of the solution at the time of filtration was 5.0oC
The solubility of Ni(OH)2 in water at 25c is measured to be 4.9 x 10^-4 g/L. Use this information to calculate Ksp for Ni(OH)2.
The enthalpy of fusion of anthracene is 28.8 kJ mol−1 and its melting point is 217°C. Calculate its ideal solubility in benzene at 26°C.
A solution is prepared by dissolving 40.00 g of MgCl2 (f.w. = 95.211 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 2 L of 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 freezing point of the solution.