Molality freezing-point constant

Molal boiling point constant, 269,270t Molal freezing point constant, 269,270t Molality (m) A concentration unit defined as the number of moles of solute per kilogram of solvent, 259,261-262 Molar mass The mass of one mole of a substance, 55,68-68q alcohol, 591 alkane, 591... 

Old United States silver coins, which are 10 0% Cu in Ag, melt completely at 875 0°C, pure silver melts at 960 0°C What is the molal freezing-point constant for Ag9... 

A brass sample composed of 20.0% Zn and 80.0% Cu melts completely at 995.0°C pure Cu melts at 1084.0°C. What is the molal freezing-point constant for copper ... 

Kip is the molal freezing-point constant of the solvent. Like Kbp, Kip is a property of the solvent, independent of the nature of the solutes. 

The freezing point of pure camphor is 178,4°C and its molal freezing-point constant, kf, is 40.0° dm. Find the freezing point of a solution containing 1.50 g of a compound that has the molar mass (M) 125 g/mol dissolved in 35.0 g of camphor. 

The freezing point of a sample of naphthalene was found to be 80.6°C. When 0.512 g of a substance were dissolved in 7.03 g naphthalene, the solution s freezing point was 75.2°C. What is the molar mass of the solute (Molal freezing-point constant for naphthalene is 6.80°C kg/mol.)... 

Pure benzene freezes at 5.45°C. A solution containing 7.24g C2CI4H2 in 115.3 g benzene was observed to freeze at 3.55°C. From these data, calculate the molal freezing-point constant for benzene. 

The freezing point of pure camphor is 178.4°C, and its molal freezing-point constant, Kf, is... 

Given the freezing-point depression or hoiling-point elevation and the molality of a solution, or data from which they may be found, calculate the molal freezing-point constant or molal hoiling-point constant. 

Each solvent has its own characteristic molal freezing-point constant. The values of fy for some common solvents are given in Figure 2.3. These values are most accurate for dilute solutions at 1 atmosphere of pressure. Some variations are introduced in the value of fy at other pressures and with more-concentrated solutions. The table also shows the values of a related quantity called which you will study next. 

PLAN Find the molal freezing-point constant, Ky, for water in Figure 2.3. To use the equation for freezing-point depression, Aty = K m, you need to determine the molality of the solution. 

PLAN Water is the solvent, so you will need the value of the molal-freezing-point constant for water, from Figure 2.3. The At for this solution is the difference between the f.p. of water and the f.p. of the solution. Use the equation for freezing-point depression to calculate molality. 

The proportionality constants in these equations, and fcf, are called the moM boiling point constant and the molal freezing point constant, respectively. Their magnitudes depend on the nature of the solvent (Table 10.2, page 313). Note that when the solvent is water,... 

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