Understanding Organic Reactions, Voltaic Cells, and Salt Hydrolysis
Classified in Chemistry
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Organic Reactions
Halogenation Substitution of Alkanes
CH4 + Cl2 → CH3Cl + HCl
Obtaining Alcohol from Halogenated Alkanes
CH3-CH2-CH2-CH2Cl + KOH → CH3-CH2-CH2OH + KCl
Addition Reactions to Double and Triple Bonds
Hydrogenation
Hydrogen is added to alkenes and alkynes to give alkanes in the presence of a metal catalyst.
CH3-CH=CH-CH3 + H2 → CH3-CH2-CH2-CH3
Halogenation
Alkenes and alkynes react with halogens to give halogenated compounds.
CH3-CH=CH2 + Br2 → CH3-CHBr-CH2Br
Adding Hydracids
Acid hydrogen is added to the carbon with more hydrogens (Markovnikov's rule).
CH2=CH2 + HI → CH3CH2I
Water Addition
Water is added to alkenes in the presence of acid and also follows Markovnikov's rule.
Voltaic Battery
A voltaic battery is a device that allows an electric current from a spontaneous redox reaction.
Daniel Cell
A Daniel cell is a voltaic cell (copper-zinc) with several essential components:
- A zinc electrode (anode): A zinc sheet is inserted into an aqueous solution of a soluble zinc salt (ZnSO4). Oxidation occurs at the anode, decreasing its mass.
Zn(s) → Zn2+(aq) + 2e-
- A copper electrode (cathode): A copper foil is immersed in a solution of a soluble copper(II) salt (CuSO4). Reduction occurs at the cathode, increasing its mass.
Cu2+(aq) + 2e- → Cu(s)
- An outer conductor: A metallic conductor allows the constant flow of electrons from the anode to the cathode.
- A voltmeter: Measures the electromotive force (emf) of the battery.
- A salt bridge: Closes the circuit and maintains electroneutrality in both solutions.
Salt Hydrolysis
Salt hydrolysis is the acid-base reaction between the ions of a salt and water.
- Salts from a strong acid and strong base: Hydrolysis does not occur, and the solution is neutral (pH = 7).
- Salts from a strong base and weak acid: Hydrolysis occurs, and the solution is alkaline (pH > 7).
- Salts from a weak base and strong acid: Hydrolysis occurs, and the solution is acidic (pH < 7).
- Salts from a weak acid and weak base: Hydrolysis occurs, and the solution's pH depends on the relative strengths of the acid and base.