Kémia beugró Quiz

Mass conversions: mg to g to kg (1000 mg = 1 g, 1000 g = 1 kg)
Volume conversions: cm³ to dm³ to m³ (1000 cm³ = 1 dm³, 1000 dm³ = 1 m³)
Amount of substance conversions: mmol to mol (1000 mmol = 1 mol)
Density conversions: g/cm³ to kg/m³ (1 g/cm³ = 1000 kg/m³)
Pressure conversions: MPa to kPa to Pa (1 MPa = 1000 kPa, 1 kPa = 1000 Pa)

Mass percentage/mass fraction: Calculate mass fraction or mass percentage using the formula:
Mass fraction = mass of substance / (mass of substance + mass of water) Mass percentage = (mass of substance / (mass of substance + mass of water)) * 100
Molar percentage/molar fraction Calculate molar fraction or molar percentage using the formula: Molar fraction = moles of substance / (moles of substance + moles of water) Molar percentage = (moles of substance / (moles of substance + moles of water)) * 100
Amount concentration: Amount concentration (c) = moles of substance / volume of solution (in liters)
Density: Density (ρ) = mass of substance / volume of solution (in appropriate units)
Mass concentration: Mass concentration (y) = mass of substance / volume of solution (in appropriate units)

Example calculations involve determining solute quantities in solutions given solution mass and percentage, density, and volume.

Key ionic compounds are provided for determining formulas
- Nitrite (NO₂⁻), Nitrate (NO₃⁻), Iron (II) (Fe²⁺), Iron (III) (Fe³⁺), Carbonate (CO₃²⁻), Ammonium (NH₄⁺), etc.

Chlorine containing disinfectants include Sodium hypochlorite (NaOCl), Calcium hypochlorite (Ca(OCl)₂), and Hypochlorous acid (HOCl)
Chlorine free disinfectants include Iodine, Ozone, and Hydrogen peroxide
Ions that cause water hardness include Mg²⁺ and Ca²⁺
"Heavy water" is water with a high concentration of Mg and Ca salts
Bleach components include NaOCl and H₂O
Chlorinated lime formula is Ca(OCl)₂

Reaction rate describes the change in reactant/product concentrations per unit time
Reaction rate can be influenced by temperature, pressure, and concentration
Half-life is the time for a reactant concentration to decrease by half
Catalysis speeds up reactions by opening alternative paths or lowering activation energy
Inhibition counteracts catalysis by blocking the catalyst's active site

Electrolysis is using an electric current to cause a chemical change
Galvanic cells use chemical reactions to generate electrical energy
Anode is the negative electrode (where oxidation occurs)
Cathode is the positive electrode (where reduction occurs)
Cations move from anode to cathode through the salt bridge
Anions move from cathode to anode through the salt bridge
Oxidation involves the loss of electrons
Reduction involves gaining electrons
Components of pH measurement involve glass electrode (sensitive to H⁺ concentration) and a reference electrode (constant). Metal corrosion is the oxidation of metals to their oxides/sulfides. Local cells form at varying metal surface areas exposed to an electrolyte.

Mass action law describes the equilibrium constant (K) for a reversible reaction
Le Chatelier's Principle states how a system in equilibrium responds to changes in conditions. The system adjusts to minimize the effect of the change
Arrhenius theory defines acids as substances that release H+ ions, and bases as substances that release OH- ions.
Brönsted-Lowry theory defines acids as proton donors, and bases as proton acceptors.
Ion Product of water(K_w) is the concentration of hydronium and hydroxide ions in water. pH is the negative logarithm of the hydrogen ion concentration. pOH is the negative logarithm of the hydroxide ion concentration.
Weak acids partially dissociate in solution, while strong acids completely dissociate
Substances that prevent large changes in pH are called buffers and are made of a weak acid/base and a salt. Hydrophilic salts dissolve in water and can be acidic or basic based on their chemistry.

Chemical compounds result from combining atoms in specific proportions
Isotopes are atoms of the same element with different numbers of neutrons but the same number of protons
Valence electrons are located in the outermost electron shell; they are involved in forming chemical bonds.
Hydrogen bonds occur when electronegative atoms (F, O, N) are bound to hydrogen

Boiling point increases with external pressure because more energy is required to overcome the increased opposition
Equilibrium vapor pressure is the pressure exerted by a vapor and the condensed phase at a given temperature in a closed system
Factors affecting gas solubility in liquids are temperature, pressure, and the nature of the solute and solvent
Osmosis is the movement of a solvent through a membrane to equalize solute concentrations
Osmotic pressure is the pressure needed to halt osmosis
Isotonic solutions have equal solute concentrations
Hypertonic solutions have a higher solute concentration outside the cell than inside
Hypotonic solutions have a lower solute concentration outside the cell than inside

Exothermic processes release heat to the surroundings
Endothermic processes absorb heat from the surroundings
Heat of combustion is the heat released when a substance reacts completely with oxygen