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Identifying Acids and Bases quiz #9

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Terms in this set (40)

  • Conjugate acid of HPO4^2-
    The conjugate acid of HPO4^2- is H2PO4-.
  • Conjugate acid of H2PO4-
    The conjugate acid of H2PO4- is H3PO4.
  • Conjugate acid of S2-
    The conjugate acid of S2- is HS-.
  • Write the formula of the conjugate acid of CH3CHO-.
    The conjugate acid of CH3CHO- is CH3CHO.
  • Identify the conjugate acid for each base.
    Add a proton (H+) to each base to identify its conjugate acid.
  • Conjugate base of HCO3-
    The conjugate base of HCO3- is CO3^2-.
  • Classify each of these compounds as a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither.
    Acids donate protons; bases accept protons; others are neither.
  • Classify these compounds as acid, base, salt, or other.
    Acids release H+; bases release OH-; salts are ionic compounds from acid-base reactions.
  • In each row of the table, select the stronger base.
    The base that ionizes more completely in water is the stronger base.
  • HCO3- conjugate base
    The conjugate base of HCO3- is CO3^2-.
  • HClO3 ionic or molecular?
    HClO3 is a molecular compound.
  • Is H3PO4 a weak acid?
    H3PO4 is a weak acid.
  • Conjugate base of H2PO4-
    The conjugate base of H2PO4- is HPO4^2-.
  • Conjugate base of H2CO3
    The conjugate base of H2CO3 is HCO3-.
  • Classify each salt as acidic, basic, or neutral.
    Salts from strong acid/strong base are neutral; strong acid/weak base are acidic; weak acid/strong base are basic.
  • Classify each of the following acids as strong or weak.
    Strong acids: HCl, HBr, HI, HNO3, H2SO4, HClO4; others are weak.
  • A monoprotic weak acid HA dissociates in water according to the reaction
    HA + H2O ⇌ H3O+ + A-.
  • Identify the conjugate base for each acid.
    Remove a proton (H+) from each acid to identify its conjugate base.
  • HBr is an Arrhenius acid because
    HBr produces H+ ions in water.
  • C2H5NH3Cl acid or base?
    C2H5NH3Cl is an acidic salt.
  • Identify the conjugate acid for each base.
    Add a proton (H+) to each base to identify its conjugate acid.
  • Classify these salts as acidic, basic, or neutral.
    Salts from strong acid/strong base are neutral; strong acid/weak base are acidic; weak acid/strong base are basic.
  • H2CO3 conjugate base
    The conjugate base of H2CO3 is HCO3-.
  • HI is considered an acid because
    HI releases H+ ions in water.
  • Conjugate base of H2O
    The conjugate base of H2O is OH-.
  • Conjugate acid of HCO3-
    The conjugate acid of HCO3- is H2CO3.
  • Conjugate base of H3PO4
    The conjugate base of H3PO4 is H2PO4-.
  • Conjugate base of HSO4-
    The conjugate base of HSO4- is SO4^2-.
  • Conjugate acid of CH3NH2
    The conjugate acid of CH3NH2 is CH3NH3+.
  • All of the following are Lewis bases except
    A species that cannot donate an electron pair is not a Lewis base.
  • Of the following, which is the strongest base?
    NaOH is the strongest base among common bases.
  • H2O conjugate base
    The conjugate base of H2O is OH-.
  • NH3 strong or weak?
    NH3 is a weak base.
  • Write the formula of the conjugate acid of each of the following bases:
    Add a proton (H+) to each base to write its conjugate acid.
  • H3BO3 conjugate base
    The conjugate base of H3BO3 is H2BO3-.
  • What is the strongest common acid?
    Among common acids, HI or HClO4 is the strongest.
  • Conjugate base of HBr
    The conjugate base of HBr is Br-.
  • Cyanide and water react in a proton transfer reaction to form hydrogen cyanide and hydroxide.
    CN- + H2O ⇌ HCN + OH-.
  • For the following reaction, identify the Lewis acid.
    The Lewis acid is the species that accepts an electron pair.
  • What is the conjugate acid of HCO3-?
    The conjugate acid of HCO3- is H2CO3.