Chem reactions in aqeous solutions

• how to calculate M (molar mass) = M= m/n
• how to calculate moles (n) = n= m/M
• how to calculate concentration (C) = C= n/V
• Limiting reagent= the reactant that is used up first in a reaction(less of this reactant than the other)
• Gulliver affect= a great amount of weak interactions that together are very hard to break
• 2 unusual properties of water= higher mp's and bp's due to extensive hydrogen bonding.
• hydration= when water is applied to a solute
• Strong electrolyte= completely dissociate into ions
• weak electrolytes= incompletely dissociate into ions.
• Q= concentration of products during reaction/before equilibrium is reached
• K= concentration of products at equilibrium
• Qe at equilibrium
• Kc equilibrium constant
• Equilibrium= forward and reverse reaction rates are the same
• Q<K= reaction lies to the right
• Q>K = reaction lies to the left
• K depends on/ is only affected by= temperature
• Magic poem= products raised to their stoichiometric powers divided by reactants raised to their's, pure solids and pure liquids do not appear
• In Kc reactions do not include= solids and liquids as their concentrations remain constant
• Big no. on top= reaction is further to the right
• small no. on top= reaction is further the left
• ICE table letters= Initial, Change, Equilm
• At equilibrium a system can react to= changes in amounts of products or reactants, and pressure
• Le Chatalier's= The system when undergoing a stress will respond in a way that returns it to equilibrium
• if reactant is added= equilibrium moves to the right
• if reactant is decreased= equilibrium moves to the left
• Decreasing pressure causes= side of reaction with more gas molecules to increase because gas fills up space
• Saturation= when no more solute can dissolve
• Ksp= dissolution shown by the concentration of products multiplied
• if Qsp> Ksp =ppt
• if Qsp<Ksp no ppt
• Lewis acid= electron pair acceptor
• Lewis base= electron pair donor
• Bronsted-Lowry acid = proton donor
• Bronsted-Lowry base= proton acceptor
• conjugate acids and bases differ by what?

  a single proton
• Bronsted acids must have a what? proton attached to an electronegative element via a polar bond.
• what makes a bronste-lowry base?

  at least one pair of lone electrons in order to accept a bond with a H+
• water is a?

  weak electrolyte
• pH= -log [H3O+]