Unit 9 - Acids and Bases - Regents Flashcards

1
Q

Definition of Acid (4)

A
  1. Arrhenius Definition - Increases H+ conc. in (aq)
  2. Bronsted - Lowry Definition - H+ donor to Bases
  3. Acids start with H
  4. H+ in (aq) always associates w/ H2O to form Hydronium
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2
Q

Definition of Coordinate Covalent Bond (2)

A
  1. Positive Ion
  2. Takes an unbonded PAIR of e-
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3
Q

Definition of Hydronium (3)

A
  1. H3O+
  2. Forms from Coordinate Covalent Bond
  3. H+ in (aq) associates 1/ H2O
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4
Q

Definition of Base (5)

Two Definitions, 3 Things to Remember

A
  1. Arrenhius - Increases OH- concentration in (aq)
  2. Proton Acceptor/Electron Donor
  3. NOT ALL BASES HAVE AN OH GROUP
  4. Base = Metal + OH
  5. There are NO ORGANIC Arrhenius bases
    Ex: NH3 is a weak Base, R - OH is not a Base (Alcohol = Organic)
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5
Q

Definition of Salts (4)

A
  1. Ionic Compounds
  2. Dissociate to form
  3. Positive Ions other than H+
  4. Negative Ions other than OH-
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6
Q

Definition of Electrolytes
2 Definition, 4 in Context of Acids & Bases

A
  1. Conductors of Electricity in H2O
  2. Mobile e- in Solution
  3. Strong Acids/Bases are Good Conductors
  4. bc they’re nearly 100% dissociated
  5. Weak Acids/Bases are not Good Conductors
  6. bc they do not have 100% dissociation
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7
Q

What are the properties of acids? (5)

A
  1. Electrolytes
  2. Ph < 7
  3. Sour Taste
  4. React w/ metal to produce H gas
  5. React w/ bases to form salt & H2O in neutralization rxn
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8
Q

How can acids be identified by indicators? (2)

A
  1. Causes Blue Litmus Paper to shift to Red
  2. Causes Phenolphthalein to shift to Colorlessness
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9
Q

What are the properties of bases? (5)

A
  1. Electrolytes
  2. Ph > 7
  3. AKA Alkaline
  4. Bitter/Chalky/Soapy/Slippery
  5. React w/ acids to form salt & H2O in neutralization rxn
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10
Q

Definition of pH (2)

A
  1. Parts of Hydrogen
  2. Measure of how acidic or basic a solution is
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11
Q

Definition of pH Scale (3)

A
  1. Numerical scale ranging from 0 to 14
  2. Each single decrease on scale is 10x increase H3O+/H+ (decrease OH-)
  3. Each single increase on scale is 10x decrease H3O+/H+ (increase OH-)
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12
Q

What exactly did pH measure? (3)

A
  1. H+ Concentration
  2. NOT STRENGTH OF AN ACID OR BASE
  3. STRENGTH IS DEPENDENT ON DISSOCIATION
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13
Q

What is the formula to determine the pH? (5)

A
  1. -log (Concentration of H+)
  2. 14 - (-log (Concentration of OH-)
  3. BC 14 = pH + pOH
  4. When give a % of dissociation, multiply w/ molarity
  5. For an acid w/ more than 1 H/OH, multiply w/ molarity
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14
Q

What are methods to find the pH? (3)

A
  1. Paper (Litmus) Tests (Does not Damage Sample)
  2. Indicator Dyes (Damages Sample)
  3. pH Meters
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15
Q

What are Paper Tests for pH? (3)

A
  1. Tests for pH
  2. Litmus paper and pH strips
  3. Treated w/ indicators that change color when exposed
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16
Q

What is Litmus Paper? (3)

A
  1. Red litmus turns blue in alkaline solutions
  2. Blue litmus turns red in acidic solutions
  3. Acidic/alkaline result but not a pH value
17
Q

What are pH strips? (3)

A
  1. More Advanced than Litmus Paper
  2. Features many color zones & provides pH
  3. Once dipped in sample, colors are matched to a pH color chart
18
Q

What are Indicator Dyes for pH? (6)

A
  1. Tests for pH
  2. Change color based on a certain range
  3. Dictates pH range
  4. Only accurate within a certain range indicating color change
  5. Functions by reacting w/ H⁺ & OH⁻
  6. Damages sample bc involve chemical rxns
19
Q

What are pH Meters? (3)

A
  1. Tests for pH
  2. Tests Voltage of Electrolyte
  3. Converts Voltage to pH
20
Q

Definition of Neutralization Reaction

A

Acid & Base React to form Salt & H2O

21
Q

Definition of Titration

A
  1. Conc. of Acid/Base Solution can be Determined
  2. Need to know 3 Variables (MₐM₆ = BₐB₆)
  3. Burette is used (lab equipment)
22
Q

What must be done if the subscripts of acids & bases are not 1:1 when titrating?

A
  1. Ma is affected by the number of H+
  2. Mb is affected by the number of OH-
  3. MaVa (Number of H+) = MbVb (Number of OH-)