Chemistry Study Sheet Unit 4 PDF

Study Sheet for Chemistry: Unit 4 Section 1: Solutions Solvent: The component in the greatest amount (e.g., water in most aqueous solutions). Solute: The component in the smallest amount, dissolved in the solvent. To determine solubility: ○ Compare the ratio of solute...

Study Sheet for Chemistry: Unit 4 Section 1: Solutions Solvent: The component in the greatest amount (e.g., water in most aqueous solutions). Solute: The component in the smallest amount, dissolved in the solvent. To determine solubility: ○ Compare the ratio of solute to solvent in different solutions at the same temperature. Concentration (% m/v): 𝑀𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 (𝑔) = 𝐶𝑜𝑛𝑐𝑒𝑛𝑡𝑟𝑎𝑡𝑖𝑜𝑛×𝑉𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 (𝑚𝐿)÷100 Section 2: Concentrations Percent Concentrations: ○ Mass/Volume (% m/v): 𝑀𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 (𝑔) 𝐶𝑜𝑛𝑐𝑒𝑛𝑡𝑟𝑎𝑡𝑖𝑜𝑛 = 𝑉𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 (𝑚𝐿) ​×100 ○ Mass/Mass (% m/m): 𝑀𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 (𝑔) 𝐶𝑜𝑛𝑐𝑒𝑛𝑡𝑟𝑎𝑡𝑖𝑜𝑛 = 𝑇𝑜𝑡𝑎𝑙 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 (𝑔) ​×100 ○ Volume/Volume (% v/v): 𝑉𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 (𝑚𝐿) 𝐶𝑜𝑛𝑐𝑒𝑛𝑡𝑟𝑎𝑡𝑖𝑜𝑛 = 𝑇𝑜𝑡𝑎𝑙 𝑣𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 (𝑚𝐿) ​×100 ○ Use dilution formulas to adjust concentration levels: C1V1 = C2V2 Section 3: Molarity and Dilutions Molarity (M): 𝑀𝑜𝑙𝑒𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 𝑀= 𝐿𝑖𝑡𝑒𝑟𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 ​ For dilution problems: ○ Combine stock and water volumes to find final concentration using the dilution formula: M1V1 = M2V2 Ionic Solutions: ○ Calculate ion concentration by multiplying molarity by the number of ions dissociated per formula unit. Section 4: Precipitation Reactions Net Ionic Equations: ○ Simplify to show only reacting ions forming a precipitate. ○ Example: Ca2+(aq) + 2Cl- (aq) → CaCl2 (s) ○ Use stoichiometry to calculate precipitate mass: 𝑀𝑎𝑠𝑠 = 𝑀𝑜𝑙𝑒𝑠 𝑜𝑓 𝑙𝑖𝑚𝑖𝑡𝑖𝑛𝑔 𝑟𝑒𝑎𝑔𝑒𝑛𝑡 × 𝑀𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑝𝑟𝑒𝑐𝑖𝑝𝑖𝑡𝑎𝑡𝑒 ○ Solubility Rules: ○ Nitrates (NO3−), alkali metals, and ammonium salts are soluble. ○ Sulfates (SO42−) and halides (Cl −, Br −, I −) are soluble, except with Pb, Ba, or Hg. Section 5: Acids and Bases Arrhenius Acid/Base: ○ Acid: Increases [H +] ions in solution. ○ Base: Increases [OH +] ions in solution. pH Indicators: ○ Phenol red: Yellow in acidic, red in basic. ○ Phenolphthalein: Colorless in acidic, pink in basic. Titration: ○ Use M1V1 = M2V2 to find unknown concentrations. ○ Example: HCl + NaOH → NaCl + H2O