What is the freezing point of a solution that is made by dissolving 91.9 grams of potassium bromide, KBr, in 1000 grams of water? Assume that KBrdissociates completely into ions when it dissolves. freezing point = °C

Aluminum hydroxide has a Ksp value of 2.0x10-32.  This indicates that aluminum hydroxide is miscible in water. that almost no aluminum hydroxide will dissolve in water. the amount of aluminum hydroxide that will dissolve in water cannot be determined from this value. that a significant amount of aluminum hydroxide will dissolve in water.

Which of the following phrases best describes the term solubility?             the ability of a solvent to dissolve in a solute       the ability of a solute to dissolve in a solvent       the maximum amount of solute that will dissolve in solvent at a given temperature       the maximum amount of solvent that will dissolve in a solute at a given temperature       the amount of solvent that dissolves in a solute for each 10oC rise in temperature

A certain liquid X has a normal freezing point of -6.90 °C and a freezing point depression constant K=3.91 °C·kgmol . Calculate the freezing point of a solution made of 146.g of iron(III) chloride (FECI,) dissolved in 900. g of X. Round your answer to 3 significant digits.

What is the freezing point of a solution that is made by dissolving 36.8 grams of potassium hydroxide, KOH, in 1000 grams of water? Assume that KOH dissociates completely into ions when it dissolves. freezing point= "C

A salt has a molar solubility of 4.18 M at 21.0°C. What is the the maximum amount of salt (in moles) that can dissolve in 1.495 L of solution before the solution becomes supersaturated at 21.0°C? Assume the salt has a molar mass of 55.44 g/mol. Report your answer to 2 decimal places.

Match the term with the related statement, A mixture with particles that settle out if undisturbed. The visible erratic motion of colloid particles, under a microscope. A measure of how much solute is dissolved in a specific amount of solvent or solution. The overall energy change that occurs when a solution forms A heterogeneous mixture of intermediate size particles. The process of surrounding solute particles with solvent particles. A homogeneous mixture with particles less than 1 nm in diameter whose solute cannot be filtered out or settled out of solution. The scattering of light by dispersed colloid particles. : colloid : Tyndall effect : suspension : solvation : heat of solution : concentration : solution : Brownian motion Review DELL %24 4 7 * 00 口 #3

Determine the molal concentration of NaCl solution in water that has a freezing point of -2.1 degree celsius. Kf= 1.86 degree celsius /m for water.

34.1 % (NH4 )2SO4   (molar mass = 132.1 g mol−1) has a density of 1.15 g mL−1. What is the molarity of this solution?  (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3)     Determine the boiling point of a solution that contains 78.5 g of compound W (molar mass = 132.5 g mol–1) dissolved in 1088.6 g benzene (C6H6; molar mass = 84.156 g mol–1; Kb = 2.53 °C m–1; boiling point of pure benzene = 80.1 °C). (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3)

A solid consists of a mixture of NaNO3 and Mg(NO3)2. When 6.50 g of the solid is dissolved in 50.0 g of water, the freezing point of the solution is lowered by 5.28°C. What is the composition by mass of the solid? g NaNO3 g Mg(NO3)2