When an ionic compound such as sodium chloride (NaCl) is placed in water, the component  atoms of the NaCl crystal dissociate into individual sodium ions (Na+) and chloride ions (Cl-). In contrast, the atoms of covalently bonded molecules (e.g., glucose, sucrose, glycerol) do not generally dissociate when placed in aqueous solution. Which of the following solutions would be  expected to contain the greatest number of solute particles (molecules or ions)? EXPLAIN WHY THE ANSWER

at a certain temperature,1.85 grams of barium hydroxide will dissolve to form 100.0 ml of a saturated barium hydroxide solution. the molar mass barium hydroxide is 171.34 grams/mole. what is the concentration of the solution in unit molarity? what is the constitution of the hydroxide ion in the same solution?

5.00 g of solid Al(NO3)3 was added to enough water to make a solution with a total volume of 100.0 mL.  Al(NO3)3 is very soluble in water and this much solid will fully dissolve in a 100.0 mL solution.  If 65 mL of water was added to the original 100.0 mL Al(NO3)3 solution described to the left in order to dilute the solution.  Calculate the new diluted solution concentration, in Molarity? Assume the volumes of the 2 solutions are additive.

What mass of sodium chloride is required to prepare 100.0 mL of a 0.215 M NaCl solution? Your answer should have 3 sig figs

The solubility of an ionic solid is 122.7g/100g of water at room temperature. What is the maximum amount of ionic solid that will dissolve in 94.79g of water at this temperature?

A bottle of anhydrous copper(II) sulfate was accidentally left uncapped for an afternoon, allowing it to pick up water from the environment. To determine the degree to which the compound was hydrated, a sample was analyzed. The initial weight of the partially hydrated copper(II) sulfate was 9.782. After drying to constant weight, the weight was 7.232. How may waters of hydration are present?

Colligative properties are those that depend on the number of solute particles. Because electrolytes dissociate into ions, the concentration of particles in the solution is greater than the formula-unit concentration of the solution. For example, if 1 mol of NazSO4 totally dissociates, 3 mol of ions are produced (2 mol of Nat ions and 1 mol of SO, ions). Thus, a colligative property such as osmotic pressure will be three times greater for a 1 M NazSO, solution than for a 1 M nonelectrolyte solution. Part A Assuming complete dissociation of the solute, how many grams of KNO3 must be added to 275 mL of water to produce a solution that freezes at - 14.5 °C? The freezing point for pure water is 0.0 °C and Kf is equal to 1.86 °C/m. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) However, complete dissociation of electrolytes does not always occur. The extent the van't Hoff factor, i: dissociation is expressed by HA moles of…

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A student needs to prepare 50.0 mL of a 1.20 M aqueous H2O2 solution. Calculate the volume of 4.6 M H2O2 stock solution that should be used to prepare the solution.

Draw some simple pictures to illustrate at the atomic level the dissolution of solid sodium chloride (salt) in water that you observed. Be sure to indicate solute-solute, solute - water, and water - water interactions, as appropriate on your diagrams.