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1.
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Soultions containing more H+ are?
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Acidic
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2.
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Soulitions contaning more OH- are?
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Basic
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3.
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Acids are defined as..
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A substance that increases concentration of H+
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4.
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Bases are defined as...
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A substance that increases concentration of OH-
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5.
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When bases and acids are added in correct amounts they can?
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Neutralize each other completely by producing water.
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6.
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When water ionizes to a very small extent (109) this is called?
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Autoionization of water
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7.
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The ion-product constant for water is known as?
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Kw
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8.
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If H+ is higher the substance is?
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Acidic
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9.
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If the OH- is higher the substance is?
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Basic
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10.
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H2O is also know as?
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H3O+
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11.
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pH= - log [H+] and as pH decreases H+ _____________.
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Increases
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12.
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pOH= -log [OH-] and pH + pOH =?
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14
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13.
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A substance that can transfer a proton to another substance; a proton donor (must have a hydrogen atom that it can lose as an H+ ion) this is called?
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Bronsted-Lowry acid
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14.
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A substance that can accept a proton; a proton acceptor (must have a nonbonding pair) this is called?
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Bronsted-Lowry base
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15.
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A substance that can act both as a proton donnor and a proton acepter is water, this is known as?
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Amphoteric
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16.
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An acid and base that differ only in the presence or absence of a proton is?
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Conjugate Acid-Base Pairs
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17.
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A conjugate base forms from the removal of a proton from a _________.
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Acid
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18.
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A conjugate acid forms from the removal of a proton from a ___________.
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Base
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19.
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A non OH and H ions from strong bases and acids that do not influnce pH is?
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Spectator Ions Example Cl- and Na+
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20.
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The stonger an acid, the ____________ its conjugate ________________.
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Weaker, Base
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21.
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The stonger an base, the ____________ its conjugate ________________.
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Weaker, Acid
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22.
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In every acid-base reaction, the position of the equiibrium favors transfer of the proton from ____________
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The stronger acid to the stronger base
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23.
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HCl, HBr, HI, HNO3, HClO3, HClO4,H2SO4 These are all?
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Stong Acids!
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24.
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Strong acids _______ 100%
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Ionize
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25.
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Alkali metals and the heavier alkaline earth metals (not Be) are all?
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Strong Bases
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26.
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Strong bases _______ 100%
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Ionize
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27.
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Weak ascids only ______ ionize in an aquesous solution
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Partially
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28.
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the Ka =?
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The amount weak acids ionize
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29.
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The larger the Ka the _________ the acid
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Stronger
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30.
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An acid having more than one ionizable hydrogen atom is?
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Polyprotic Acid
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31.
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the Ka is always ______ than the Ka2 because its _______ to remove the first proton from a polyprotic acid than the second
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Larger, easier
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32.
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Weak bases are substances that react to form hydroxide ion, but not a _________ reaction
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Complete
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33.
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weak base + H2O <-> ___________ + OH-
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Conjugate acid
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34.
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What is the most common weak base?
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NH3 or Ammonia
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35.
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the Kb =?
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Give indication of how far the weak base reaction proceeds to form hydroxide ion
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36.
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Weak bases in which two categories?
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Amines and anions of weak acids
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37.
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What are amines?
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A substance which is similar to ammonia and this is because they contain an unshared pair
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38.
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Ka x Kb = ?
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Kw or 1 x1 014
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39.
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As the strength or an acid increases, the strenght of its conjugate base must ___________
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Decrease
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40.
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The reaction of an ion from a salt with water to produce H+ or OH- is known as?
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Hydrolysis
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41.
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Nearly all salts are _____________
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Strong electrolytes.... meaning they ionize to 100%
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42.
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Salts derived from a strong base and strong acid have pH= ?
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pH= 7 : Neither anion nor the cation undergo hydrolysis and they have no effect on the pH of the solution.
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43.
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Salts derived from a strong base and weak acid have pH = ?
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pH= above 7 : This is because the conjugate base of the weak acid acts as a weak base generationg OH-. The cation of the strong acid is a spectator ion
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44.
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Salts derived from a weak base and a strong acid have pH = ?
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pH= below 7 : this is because the conjugate acid of the weak base is a weak acid and ionized to a small extent producing hydronum ion. The other is a spectator ion.
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45.
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Salts derived from a weak base and weak acid have a pH = ?
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pH depends on the values of Ka and Kb in the solution. Which ever is bigger the solution will either have a weakly acidic or basic or neutral.
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46.
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Lewis acid is defined as?
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Electron-pair acceptor
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47.
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Lewis base is defined as?
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electron-pair donor
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