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Transcript
Aqueous Solutions and Types of Reactants ● Parts of a solution: ○ Solution - homogeneous mixture ○ Solute - what gets dissolved ○ Solvent - what does the dissolving ○ Soluble - can be dissolved ○ Dissociation - breaking apart into ions ■ Ex. N aCl → N a + + Cl − ● Aqueous Solutions ○ Dissolves in water ■ Water is a good solvent because the molecules are polar ■ The oxygen atoms have a partial negative charge ■ The hydrogen atoms have a partial positive charge ○ Hydration ■ Process of breaking bonds ■ H+ ions attracts negative ions ■ O- attracts positive ions Solubility and Electrolytes ○ Solubility = how of much of a substance will dissolve in a given amount of water ■ Usually g/100 ml ■ Varies greatly, but if they do dissolve, the ions are separated and can move around ■ Water can also dissolve non-ionic compounds if they have polar bonds ● ○ ● The ions in a solution that are dissolved can move about ■ Electricity is also a moving charge ■ Solutions of ionic compounds can conduct electricity ○ Strong electrolyte/solution = compound completely dissociates and conducts electricity well ○ Weak electrolyte/solution = partially dissociates into ions and conducts electricity slightly ○ Non-electrolyte = ions don’t dissociate and can’t conduct electricity Measuring Concentration and Solutions ○ Concentration = how much of a compound is dissolved Molarity (M) = Moles of solute / Liters of solution ■ 1 M = 1 mol solute/ liter solution ○ Dilution = adding more solvent to a known solution ■ The moles of solute stay the same ■ M1V1 = M2V2 ○ Stock solution = a solution of known concentration that is used to make more dilute solutions Precipitation ○ Precipitation = when aqueous solutions of ionic compounds are poured together and a solid forms (solid = precipitate) ○ We can predict the products ■ The anion and cation switch partners ■ Can only be absolutely certain by experimenting ○ Three different precipitation equations: ■ Molecular equation = written as the whole formula ■ Complete ionic equation = all solutes are dissociated if possible ■ Net ionic = balanced equation without spectator ions ● Spectator ions = ions that don’t react ○ ● ○ Solubility rules ■ All nitrates and acetates are soluble ■ Alkali metal ions (first and second columns) and ammonium ions are soluble ■ Chlorides, bromides, and iodides are soluble ● Except with lead, silver, and mercury ions ■ Sulfates are soluble ● Except with lead, silver, mercury, calcium, barium, and strontium ions ■ All other anions are insoluble (hydroxides, fluorides, sulfides, carbonates, chromates, and phosphates)
