an acetic acid solution is 4.00M and has a density of 1.04g/mL. what is the mass/mass percent concentration of HC2H3O2(60.06 g/mol)? a ) 0.347% b) 0.375% c) 37.5% d) 23.1% e) 36.0 %

Solutions of hydrogen in palladium may be formed by exposing Pd metal to H2 gas. The concentration of hydrogen in the palladium depends on the pressure of H2 gas applied, but in a more complex fashion than can be described by Henry's law. Under certain conditions, 0.94 g of hydrogen gas is dissolved in 215 g of palladium metal (solution density = 10.8 g cm3). (a) Determine the molarity of this solution. (b) Determine the molality of this solution. (c) Determine the percent by mass of hydrogen atoms in this solution.

The Henry's law constant for the solubility of argon gas in water is 1.0103M/atm at 30C. (a) Express the constant in M/mm Hg. (b) If the partial pressure of argon gas at 30C is 693 mm Hg, what is the concentration (in M) of the dissolved argon gas at 30C? (c) How many grams of argon gas can be dissolved in 29 L of water at 693 mm Hg and 30C? (Ignore the partial pressure of water.)

Solutions Introduced directly into the bloodstream have to be isotonic with blood; that is, they must have the same osmotic pressure as blood. An aqueous NaCl solution has to be 0.90% by mass to be isotonic with blood. What is the molarity of the sodium ions in solution? Take the density of the solution to be 1.00 g/mL.

The freezing point of 0.10 M KHSO3 is -0.38C. Which of the following equations best represents what happens when KHSO3 dissolves in water? (a) KHSO3(s)KHSO3(aq) (b) KHSO3(s) K+(aq)+HSO3(aq) (c) KHSO3(s) K+(aq)+SO32(aq)+ H+(aq)

How do colloids differ from solutions with regard to dispersed particle size and homogeneity?

The Henry's law constant for the solubility of helium gas in water is 3.8104M/atm at 25C. (a) Express the constant for the solubility of helium gas in M/mm Hg. (b) If the partial pressure of He at 25C is 293 mm Hg, what is the concentration of dissolved He in mol/L at 25C? (c) What volume of helium gas can be dissolved in 10.00 L of water at 293 mm Hg and 25C? (Ignore the partial pressure of water.)

A patient has a “cholesterol count” of 214. Like manyblood-chemistry measurements,this result is measured inunits of milligrams per deciliter (mgdL1). Determine the molar concentration of cholesterol inthis patient’s blood, taking the molar mass of cholesterolto be 386.64gmol1. Estimate the molality of cholesterol in the patient’sblood. If 214 is a typical cholesterol reading among men inthe United States, determine the volume of such bloodrequired to furnish 8.10 g of cholesterol.

Sodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride (CaCl2) is sometimes used for this purpose too. Let us compare the effectiveness of equal masses of these two compounds in lowering the freezing point of water, by calculating the freezing point depression of solutions containing 200. g of each salt in 1.00 kg of water. (An advantage of CaCl2 is that it acts more quickly because it is hygroscopic, that is. it absorbs moisture from the air to give a solution and begin the process. A disadvantage is that this compound is more costly.)

An aqueous solution of M2O is prepared by dissolving 10.91 g of the electrolyte in 435 mL of H2O(d=1.00g/mL). The solution freezes at -4.68C. What is M+? (Assume complete dissociation of M2O to M+ and O2-.)