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Unit 2 Chemistry - Coggle Diagram

- - - - Eg. 17% (m/v) = 170g per 1 litre
  - - - Unsaturated: contains less solute than the solvent can dissolve. It can dissolve more solute
      - Supersaturated: contains more solute than a saturated solution. If this solution is disturbed, solute will come out of the solution as solid
      - Saturated: no more solute can be dissolved in the solvent at a given temperature
    - - Any point below the curve represents an unsaturated solution
      - A point on the curve represents a saturated solution
      - Any point above the curve represents a supersaturated solution
      - Each point represents the maximum amount of solute that can be dissolved in (100g of) solvent at a particular temperature
    - - Use graph to figure out g/100g at x degrees
      - Apply (x) the g/100g ratio to the given amount
  - - - solve for c2
- - - - Two species (substances) that differ by one proton (hydrogen atom)
      - Eg. HCl forms Cl when it donates a proton - HCl is an acid. Cl can also gain a proton - Cl is a base
      - ^Eg. H2O can accept a proton, making it a base. It forms H3O which is able to donate a proton, making it an acid
  - - - 0.001M = 10^-3 Molar concentration of OH ions
      - using [OH]x[H3O] = 10^-14 M^2,
      - we know that Molar concentration of H3O = 10^-11. This is a lower concentration than that of the OH, meaning it has less H3O. Because it has less H3O it is less acidic, more basic.
  - - - Figure out amount of mol in given substance using n=c/V
      - Use mol ratios to figure out mol of unknown
      - Write balanced equations
      - use V=n/c to find volume of unkown solution
      - A 0.100 M H2SO4 solution is neutralised with 10.0 mL of a solution of 0.300 M KOH. What volume of sulfuric acid was neutralised?
- - - - Stationary Phase:
      - Mobile Phase
        
        The solvent placed in the bottom of the container. The components desorb from the mobile phase
  - - - The specific requirements for the chemical being tested
      - Selection of equipment and sample size
      - Health risks associated with the sampling
      - Recording results and taking representative samples
      - The chemical that is to be analysed
      - labelling and storage requirements
      - The reason for testing
- - - - Ammonium NH4+
      - Potassium K+
      - Ethanoate CH3COO-
      - Nitrate NO3-
      - Sodium Na+
    - - Carbonates
      - Phosphates
      - Hydroxides
      - Sulfides
  - - - solvent-solvent bonds break
      - solute-solute bonds break
      - solute-solvent bonds form
      - Question: do intra or intermolecular bonds break or both?
    - - Solvent: the liquid that dissolves
      - Solute: the substance that is dissolved
      - Solution: solute dissolved in solvent
      - Dissolution: the process by which a solute is dissolved in a solvent
  - - - Full chemical equation
        
        AgNO3(aq) + NaCl(aq) => AgCl3(s) + NO3(aq)
      - Ionic equation
        
        Ag+(aq) + Cl-(aq) =>AgCl
        
        involves only the precipitate
        
        Doesn't involve spectator ions because they are still separate ions in the solution
- - - - mole ratio x n(known) = n(unknown)
      - Find the mole ratio from a balanced equation. n(unknown)/n(known)
    - - Collect precipitate by filtration. Wash (with water) to ensure no soluble components are present
      - Carefully dry precipitate and weigh to ensure the mass is not higher than it should be
      - Add precipitation solution in excess to cause complete precipitation of ion being analysed
      - Prepare sample solution
    - - Determine which compound is in excess or limiting
      - Calculate the number of moles of product can be produced using mol of limiting reactant
      - Calculate the number of moles of each reactant