Acids, Bases, Solubility, and Chemical Reactions Chemistry Notes PDF
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These notes cover concepts like acids, bases, solubility, and chemical reactions, with formulas and calculations. They include pH scales, indicators, types of reactions (e.g., formation, decomposition), and examples. Ideal for secondary school chemistry students.
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# Acids, Bases, Solubility, and Chemical Reactions ## Chemical Formula with Multivalent Elements 1. Write name first element 2. Place metallic ion of first element in Roman numerals 3. Write name second element suffix "ide" 4. No prefixes - **Example:** Fe(ClO<sub>3</sub>)<sub>2</sub> is **Iron (...
# Acids, Bases, Solubility, and Chemical Reactions ## Chemical Formula with Multivalent Elements 1. Write name first element 2. Place metallic ion of first element in Roman numerals 3. Write name second element suffix "ide" 4. No prefixes - **Example:** Fe(ClO<sub>3</sub>)<sub>2</sub> is **Iron (II) Hydrochlorite** ## pH Scale | | 0 | 1 | 2 | 3 | 4 | 5 | 6 | 7 | 8 | 9 | 10 | 11 | 12 | 13 | 14 | 15 | |-------------|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---| | | | | | | | | | | | | | | | | | | | **Acids** | | | | | | | | | | | | | | | | | | **Neutral** | | | | | | | | **H<sub>2</sub>O** | | | | | | | | | | **Bases** | | | | | | | | | | | | | | | | | ## Properties **Acids:** Contain hydrogen (H+) - Substances that release hydrogen ions **Bases:** Substances that dissolve in water - Release hydroxide (OH-) ions. ## Indicators & pH **Litmus paper:** Turns blue for bases, red for acid, no change when neutral. **Phenolphthalein:** Colorless in acid, pink in base, colorless in neutral. ## Taste / Feel **Acids:** Sour, corrosive **Bases:** Bitter, slippery **Neutral:** Tasteless ## Solubility **Solute:** Substance that dissolves. **Solvent:** Substance does dissolving. **Aqueous (aq):** When dissolved. **Precipitate:** When not dissolved. ## Mole Calculations - 1 mol of a chemical is 6.02 x 10<sup>23</sup> particles/atoms or molecules of substance. - 6.02 x 10<sup>23</sup> is Avogadro's number. ### Atomic Mass/Mole - One mole iron has 6.02 x 10<sup>23</sup> atoms & is 55.85g. - One mole magnesium has 6.02 x 10<sup>23</sup> atoms & is 14.31g. ### Calculating Molar Mass - Add molar mass of elements, multiply by subscript numbers. ### Example: How many moles in 22g of Argon? m = 22g M = 39.95g/mol ```text 22g x 1mol/39.95g = 0.55 mols ``` #### Calculating Molecular Mass Example: How many moles in 68g of copper (II) hydroxide, Cu(OH)<sub>2</sub>? m = 68g M = 63.55 + 16.00(2) + 1.01(2) = 97.57g/mol ```text 68g x 1mol/97.57g = 0.70 mols ``` ### How Many Grams in 1.11 Moles of Manganese (IV) Sulfate, Mn(SO<sub>4</sub>)<sub>2</sub>? m = 1.11 mol M = 54.94 + 32.07(2) + 16(8) = 247.08g/mol ```text 1.11 mol x 247.08g/mol = 274.9g ``` ### How Many Molecules in 2.25 Moles? ```text 2.25 mol x 6.02 x 10<sup>23</sup> molecules/mol = 1.35 x 10<sup>24</sup> molecules ``` ### How Many Moles in a Substance of 3.4x10<sup>26</sup> Molecules? ```text 3.4 x 10<sup>26</sup> molecules * 1mol/6.02x10<sup>23</sup> molecules = 5.6 x 10<sup>2</sup> mol ``` ### How Many Molecules in 35 Grams of Na<sub>2</sub>CO<sub>3</sub>? m = 35g M = 22.99(2) + 12.01 + 16(3) = 105.99g/mol ```text 35g x 1mol/ 105.99g/mol x 6.02 x 10<sup>23</sup> molecules/mol = 2.0 x 10<sup>23</sup> molecules ``` ### How Many Molecules in 39.58g of Ammonia? m = 39.58g M = 14.01 + 1.01(3) = 17.03g/mol ```text 39.58g x 1 mol/17.03g/mol = 2.32 mol ``` ```text 2.32 mol x 6.02 x 10<sup>23</sup> molecules/mol = 1.4 x 10<sup>24</sup> molecules ``` ## Reactions - Chemical reactions occur when one or more substances change from different substances. - **Chemical Change:** Must occur. - **Reactants:** Substances undergo change (left side equation) - **Products:** Substances formed (right side equation) - **Evidence of Chemical Reaction:** Temperature change, odor change, color change, or formation of gas/solid. ### Endothermic Reactions - Low reactants, high products - Overall positive energy change (gain energy). - Absorbs energy from surrounding, decrease surrounding temperature. ### Exothermic Reactions - High reactants, low products - Overall negative energy change (lose energy) - Releases energy into surroundings, increases surrounding temperature. ## Types of Reactions **Formation:** Two or more elements combine (x + y -> xy, H2 + O2 -> H<sub>2</sub>O) **Decomposition:** One compound breaks down into two or more (xy -> x + y, H<sub>2</sub>O -> H<sub>2</sub> + O<sub>2</sub> ) **Single Replacement:** One element takes place of another (A + BX -> AX + B, Na + H<sub>2</sub>O -> NaOH + H<sub>2</sub>) **Double Replacement:** Two compounds exchange places (AX + BY -> AY + BX, Bal<sub>2</sub> + Na<sub>2</sub>SO<sub>4</sub> -> BaSO<sub>4</sub> + 2NaI) **Combustion:** Hydrocarbons burned with oxygen (hydrocarbon + O<sub>2</sub> -> CO<sub>2</sub> + H<sub>2</sub>O + heat & light) **Neutralization:** Acid and base produce water and a neutral salt (acid + base -> water + neutral salt, HBr + Ca(OH)<sub>2</sub> -> H<sub>2</sub>O + CaBr)
