For dissolving an ionic compound in a solvent like the water molecules, it must be sufficient to stabilize the ions which result from breaking of the ionic bond. Since water is a polar molecule and it has a permanent dipole. The O atom of the water molecule has a partial negative charge and H atoms have usually a partial positive charge. When an ionic substance is placed in water, the water molecules attract the cation and anions ions from the crystal. As a result of this, the ionic particles are then free to move around within the solution. The cations have several water molecules around them and all the O atoms of the solvent will close to the positive ion of the ionic compound. While the anions have several water molecules around them and all the H atoms of the solvent will close to the negative ion of the ionic compound. Furthermore, the "shell" of water molecules around the ionic compound will reduce the attractions between the ions.
explain why ionic substances show a wide range of solubilities in water
2. Why do ionic substances with higher lattice energies tend to be less soluble in water than substances with lower lattice energies? 3. Which would you expect to have the larger hydration energy, SO or CIOA? Explain. 4. Ethyl alcohol, CH CH2OH, is miscible with water at 20°C, but pentyl alcohol, CH3CH2CH2CH2CH2OH, is soluble in water only to the extent of 2.7 g/100 ml. Explain.
Explain why some substances dissolve in water and others do not. A complete answer will include an explanation of electrostatic attractions and their relationship to energy.
The following ionic compounds are dissolved in water. For each of the substances below, identify the ions formed once dissolved in water. Make sure the reactions are all balanced. a) HI (aq) = b) K2SO3 (aq) = c) Ba(NO3)2 (aq) = d) NH4OH (aq) = H2SO4 (aq) =
Electrolytes Electrolytes are substances that produce ions in water. Most ionic compounds break apart into ions in water and are therefore electrolytes. Covalently bonded compounds do not usually dissociate (break apart) in water and are nonelectrolytes. Write a balanced equation for the dissociation of the following ionic compounds. EXAMPLE: CaCl - Ca?"(aq) + 2 Cl(aq) 1. BaSO4 2. NaCl 3. KOH 4. MgCl2 Note that some of the ionic compounds above produce more than one mole of anion or cation...
The water solubilities of oxalic acid and sodium oxalate at room temp are 10g/100ml and 3.7g/100ml respectively. Could you prepare oxalic acid by adding HCl to a solution of sodium oxalate, cooling it to room temp, and filtering the resulting mixture? Explain why or why not.
1. Ionic solids easily dissolve in water. Using sodium chloride as an example, explain the mechanism by which the dissolution is made possible. 5. Describe the typical characteristic of hygroscopic food substances. 2. Describe the roles dipole and hydrogen bonding play in the dissolution of polar molecules in water. 3. Crackers have an aof 0.3. What happens when they are exposed to air with 80% relative humidity? 4. What is a Moisture Sorption Isotherm (MSI)? 1. Ionic solids easily dissolve...
Solubitity Depends on Bond Type and Molecular Struetwre L Solubilitity and Bond Type Ionic, Non-polar Covalent, and rolar Covalent Compounds SolvemWater Substance Hexane Hexane Water Acetone Barium sulfate 3 Heptane Isopropandl Naphthalene Potassium Iodide Sodium bicarbonate Sucrose Xylene o Vegetable oil Analysis: Look at your data for heptane, naphthalene, and vegetable oil. Are they more soluble in water or in hexane? What is it about the structures of these compounds that explains this result? 1. Look at your data for...
Choose all the answers that are true about water.? 1. Water dissolves substances that are polar (polar covalent bonds). 2. Water dissolves substances that are non-polar (non-polar covalent bonds) 3. water is an excellent solvent. 4. Water dissolves substances with ionic bonds, such as NaCl.
Why might a “cafeteria plan” be popular for a workforce that has a wide range of ages?
Interpretation of Reactions by Ionic Type Equations. Aqueous solutions of the following substances or their mixtures with water if they are only slightly soluble, are mixed. Write first the conventional equation, second the total ionic equation, and lastly the net ionic equation. If you predict no appreciable reaction, indicate this, and state why. a. Magnesium chloride and sodium carbonate b.Aqueous ammonia and hydrofluoric acid c.Aqueous ammonia and hydrofluoric acid d.Ammonium chloride and sodium hydroxide e.Barium chloride and calcium nitrate f.Potassium...