Ice cubes from a freezer have a temperature of about -12°C (10°F), which is cold enough, but contact with the warmer ice cream mixture causes them to melt to liquid at 0°C, which is too warm. To obtain a liquid that is cold enough, salt (NaCl) is dissolved in water, and ice is added to the saltwater. The salt lowers the freezing point of the water enough so that it can freeze the liquid inside the ice cream maker. The instructions for an ice cream maker say to add one part salt to eight parts water (by mass). What is the freezing point of this solution (in degrees Celsius and degrees Fahrenheit)? Assume that the NaCl dissociates fully into ions, and that the solution is ideal.

At 25 Celsius and 775 torr carbon dioxide has a solubitilty of 0.0347 M in water. What is the solubility at 25 Celsius and 1290 torr S=    M

The normal freezing point of a certain liquid X is 4.70°C, but when 83.g of benzamide (C7H7NO) is dissolved in 850.g of X the solution freezes at 0.6°C instead. Use this information to calculate the molal freezing point depression constant Kf of X. Be sure your answer is rounded to the correct number of significant digits.

An online study examined the lowering of freezing point when 0.222 g of an unknown molecular solute was dissolved in 11.45 g of cyclohexane. The freezing point of pure cyclohexane was 6.6oC and the freezing point of the solution of the unknown was 3.3oC. The freezing point lowering constant, Kf, for cyclohexane is 20.0oC*(kg/mol). What is the molar mass of the unknown in g/mol? Enter your answer without units.

16. Every year, oral rehydration therapy (ORT) –the feeding of an electrolyte solution -saves the lives of countless children worldwide who become severely dehydrated as a result of diarrhea. One requirement of the solution used is that it be isotonic with human blood. An ORT solution contains 3.5 g NaCl, 1.5 g KCI, 2.9 g Na3CgH507 (sodium citrate), and 20.0 g C6H1206 (glucose) per liter. What is the freezing point of this solution? You may assume that the density of the solution is 1.00 g/mL and that the freezing point depression constant (Kf) for water is 1.86 °C/m. -0.59 oC -1.86 oC 0.00 oC +0.51 оС -7.44 oC

At 70 °C, the solubility of an unknown solute is 65.7 g/100.0 g of water. What mass of the solute can dissolve in 125.5 g of water at the same temperature?

Do both, just one, or neither of the following solutions conductelectricity? If just one, which one?

The freezing point of ethanol, CH3CH₂OH, is -117.300 °C at 1 atmosphere. Kf(ethanol) = 1.99 °C/m In a laboratory experiment, students synthesized a new compound and found that when 11.23 grams of the compound were dissolved in 266.2 grams of ethanol, the solution began to freeze at -117.394 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound? g/mol

O SIMPLE REACTIONS Predicting the products of dissolution The names and chemical formulae of some chemical compounds are written in the first two columns of the table below. Each compound is soluble in water. Imagine that a few tenths of a mole of each compound is dissolved in a liter of water. Then, write down in the third column of the table the chemical formula of the major chemical species that will be present in this solution. For example, you know water itself will be present, so you can begin each list with the chemical formula for water (H,O). Note: "major" chemical species are those present in concentrations greater than 10 9- mol/L. major species present when dissolved in water compound formula O.. acetonitrile CH,CN CH,CN, H,O ? ammonium bromide NH,Br NH, Br , H,0 iron(III) iodide Fel3 Explanation Check

A 0.547 g sample of an unknown solute dissolved in 14.0 g of tert-butanol produces a solution with a freezing point of 22.70 °C. What is the molar mass of the solute? For tert-butanol T = 25.50 °C, kf = 9.10 °C · kg · mol-. molar mass = g/mol