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Rates, equilibrium and pH

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Rates, equilibrium and pH

Fichas del conjunto (37)

  1. 1Rate of ReactionThe change in concentration of a reactant or product per unit time
  2. 2How do you write a rate equation?rate = k[A][B]
    (the order in respect to the reactant is shown as the power)
  3. 3Half-lifeThe time taken for the concentration of the reactant to reduce by half
    (first order = constant half-life)
  4. 4What does the rate-concentration graph look like for a zero order reactant?What does the rate-concentration graph look like for a zero order reactant?
  5. 5What does the rate-concentration graph look like for a first order reactant?What does the rate-concentration graph look like for a first order reactant?
  6. 6What does the rate-concentration graph look like for a second order reactant?What does the rate-concentration graph look like for a second order reactant?
  7. 7Rate-determining stepThe slowest step in the reaction mechanism of a multi-step reaction
  8. 8What is the general expression for KcWhat is the general expression for Kc
  9. 9Dynamic equilibriumWhen the rate of the forward reaction is equal to the rate of the backward reaction, in a closed system.
  10. 10Standard conditions298K
    100kPa (1atm)
    1moldm^-3
  11. 11Homogenous equilibriumAn equilibrium in which all the species making up the reactants and products are in the SAME state
  12. 12Kc only changes withTemperature
  13. 13If Kc is more than one the equilibrium shifts to the ...Right and favours the products
  14. 14If Kc is less than 1 the equilibrium shifts to the...Left and favours the reactants
  15. 15How is Kc value affected by temperature?Increase in Kc - rise in temp if the forward reaction is endothermic (equilibrium shift to the right)
    Decrease in Kc - rise in temp if the forward reaction if exothermic (equilibrium shift to the left)
  16. 16An acidA proton donor
  17. 17A baseA proton acceptor
  18. 18AlkaliA base that dissolved in water to form OH- ions
  19. 19NeutralisationA chemical reaction in which an acid and a base react together to produce a salt and water
  20. 20Acid + Carbonate =salt + carbon dioxide + water
    ( remember - the ionic equation varies with states of the carbonate)
  21. 21Acid-base pairA pair of two species that transform into each other by gain or loss of a proton
  22. 22What is the general expression for the acid dissociation constant (Ka)?What is the general expression for the acid dissociation constant (Ka)?
  23. 23How do you work out the pH of a STRONG acid?[H+] = [HA]
    (due to complete dissociation)
    pH = -log [H+]
  24. 24How do you calculate the pH of a WEAK acid?How do you calculate the pH of a WEAK acid?
  25. 25What is the expression for the ionic product of water, Kw?What is the expression for the ionic product of water, Kw?
  26. 26What are the two methods for calculating the pH of a strong base?pOH and Kw
    (remember [OH-] = base concentration due to complete dissociation)
  27. 27What is a buffer solution?A mixture of a weak acid (HA) and its conjugate base (A-) that minimises pH changes on addition of small amounts of acid or base.
  28. 28General buffer equation.General buffer equation.
  29. 29How do you work out the [H+] of a buffer solution? (which can then be used to calculate the pH)How do you work out the [H+] of a buffer solution? (which can then be used to calculate the pH)
  30. 30Define equivalence pointThe point in a titration at which the volume of one solution has reacted exactly with the volume of a second solution
    (there are no reactants in excess)
  31. 31The end point is...The point in a titration is the point at which the indicator changes colour.
    (the point at which there are equal concentrations of the weak acid and conjugate base forms of the indicator)
  32. 32What indicator would be used for a strong acid - weak base titration? And state the colour changeMethyl orange
    Red (acid) --> Orange --> Yellow (base)
  33. 33What indicator would be used for a weak acid - strong base titration? And state the colour change.Phenolphthalein
    pink (base) --> colourless (acid)
    Very sudden change
  34. 34Titration curve: Where is the equivalence point?Titration curve: Where is the equivalence point?
  35. 35Define enthalpy change of neutralisationThe energy change that accompanies the neutralisation of an aqueous acid by an aqueous base/alkali to form one mole of water under standard conditions.
  36. 36Determining enthalpy change of neutralisation. How do you work out the energy change? (m = mass of solutions)Determining enthalpy change of neutralisation. How do you work out the energy change? (m = mass of solutions)
  37. 37Calculate enthalpy change of neutralisation. Remember: n = moles of limiting reactantCalculate enthalpy change of neutralisation. Remember: n = moles of limiting reactant

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Descripción
OCR Chemistry A spec
Creado por
Usuario eliminado · nov 2016
Actualizado
1 dic 2016
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31
Historial
  • Creado por sophie.holland96 · 17 feb 2014
  • Copiado por Tariq hudda · 30 nov 2016
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