Regents Chemistry Test Objectives: Acids/Bases & Salts

  • Be able to explain the difference between an electrolyte & a non-electrolyte
  • Know that acids, bases and salts are electrolytes
  • Be able to identify compounds as electrolytes or non-electrolytes from their formulas
  • Be able to identify acids from their formulas
  • Formulas start with H or end with COOH
  • Be able to identify bases from their formulas
  • Formulas are MOH (where M = metal)
  • Be able to identify salts from their formulas
  • Formulas consist of metal bonded to a nonmetal
  • Be able to list the properties of acids & bases
  • Know several ways to test a substance to determine if its an acid
  • Indicators, pH meter, reaction with metal (other than Cu, Ag, Au)
  • Know the names of common acids & bases (table K & L0
  • Be able to define Arrhenius acid & Arrhenius base
  • Acids produce H+1ions in aqueous solutions
  • Bases contain OH and produce OH-1ions in solution
  • Know that the terms proton(H+1), hydrogen ion (H+1) and hydronium ion (H2O+3) are used interchangeably (with reference to acids) and that the hydroxide ion (OH-1) refers to bases
  • Be able to write balanced ionization (dissociation) equations for strong acids & strong bases and know that these strong acids & bases have essentially 100% ionization
  • Be able to identify monoprotic, diprotic & triprotic acids from their formulas
  • Be able to identify monohydroxy, dihydroxy & trihydroxy bases from their formulas
  • Know what the term amphoteric means
  • Be able to define Bronsted-Lowry acidBronsted-Lowry base
  • Know that Bronsted-Lowry is known as the “alternate acid-base theory”
  • Bronsted-Lowry acids are proton donors
  • Bronsted-Lowry bases are proton acceptors
  • Know that ammonia is a Bronsted-Lowry base but not a Arrhenius base & be able to explain why
  • Know that the products of all reactions between acids & metals is hydrogen gas and a salt
  • Given a metal & an acid be able to write a balanced chemical equation describing the reaction
  • Know that only metals above hydrogen on table J will react with acids
  • Know the formula for pH & the pH scale
  • Be able to calculate pH from H+1 concentrations & be able to calculate H+1 concentration from pH values
  • Understand that square brackets mean “concentration of” the species in the brackets
  • [H]+1 means concentration of H+1 and is used as a measure of acidity
  • [OH]-1 means concentration of OH-1 and is used to assess how basic a solution is
  • Know that pH + pOH = 14 (pH = -log[H]+1 or –log[H2O]+3 ; pOH = -log [OH]-1)
  • Know the definition of pOH and use it to calculate OH- concentration
  • Know the common indicators (table M) and what colors they change in acid/base solutions
  • Know how to use indicators to determine the pH of an unknown solution
  • Litmus is red in acid; blue in base
  • Phenolphthalein is pink in base and colorless in acid
  • Be able to define neutralization and to identify neutralization reactions
  • Given an acid and a base, be able to write and balance the neutralization equation
  • Know that the net ionic equation for all neutralization reactions is:

H+1 + OH-1→ H2O

  • Recognize thattitrationis the process used to:
  • quantitatively determine the Molarity of an unknown acid or base
  • compare known volumes of 2 solutions (one acid and one base) when the concentration of only one solution is known
  • Know that titrationinvolves both neutralization & the ability to recognize the end point of the reaction
  • Be able to:
  • Describe the titration set-up, including the buret measurements
  • Understand that the endpoint occurs when the indicator changes color
  • Understand that the equivalence point occurs when the moles H+1 = moles OH-1
  • Understand that if pick an appropriate indicator, the endpoint and equivalence point occur at virtually the same time
  • Using the formula MaVa = MbVbbe able to solve titration problems
  • Used when the # of H’s in the acid = the # of OH’s in the base
  • the acid is monoprotic & the base is monohydroxy or acid is diprotic & the base is dihydroxy
  • know how to solve when the # of H’s in the acid DO NOT = the # of OH’s in the base
  • the acid is diprotic & the base is monohydroxy or when the acid is monoprotic & the base is dihydroxy
  • Know the term amphoteric
  • Be able to write equations to show that water is amphoteric
  • Be able to use the formula McVc = MdVdto prepare dilutions of a solution