1. Advanced Chemistry Types of Chemical Reactions and Solution Stoichiometry

5. Polar Water Molecules Interact with the Positive and Negative Ions of a Salt Assisting in the Dissolving Process

8. An Ethanol Molecule Contains a Polar O-H Bond Similar to Those in the Water Molecule

9. The Polar Water Molecule Interacts Strongly with the Polar-O-H bond in Ethanol

13. Electrical Conductivity of Aqueous Solutions

16. NaCl Dissolves

18. HCl is Completely Ionized

19. Acids An Acid is a substance that produces H + ions when it is dissolved in water.

20. Acids In conductivity studies, virtually every molecule ionizes. Therefore, strong electrolytes are strong acids.

23. Strong Bases

24. An Aqueous Solution of Sodium Hydroxide

28. Acetic Acid (HC 2 H 3 O 2 )

30. The Reaction of NH 3 in Water

41. Steps Involved in the Preparation of a Standard Aqueous Solution

42. Types of Chemical Reactions

45. Precipitation Reaction Example A more accurate representation is:

46. Reactant Solutions

47. Solution Post-Reaction

51. Simple Rules for the Solubility of Salts in Water

61. Determining the Mass of Product Formed

69. Acid-Base Reactions When a weak acid and a strong base react, the weak acid usually doesn’t ionize. However, the hydroxide ion is such a strong base that for the purposes of stoichiometric calculations it can be assumed to react completely with any weak acid.

104. Example +1 -1 0 +5 -2 +4 -1 +4 -2 +1 -2 Note that hydrogen, chlorine, and oxygen do not change oxidation states and are not involved in electron exchange. 0 +5 -2 +4 -1 +4 -2

105. Example 0 +5 -2 +4 -1 +4 -2 Tin lost 4 electrons and each Nitrogen gained 1 electron. Therefore each nitrogen must have a coefficient of 4. Balance the rest as usual

107. Figure 4.11a-b Measuring Pipets and Volumetric Pipets Measure Liquid Volume

108. Figure 4.12a-c A Measuring Pipet is Used to Add Acetic Solution to a Volumetric Flask

109. Figure 4.15 a&b The Reaction of K 2 CrO 4 and Ba(NO 3 ) 2

110. Figure 4.17 Molecular-Level Representations Illustrating the Reaction of KCl ( aq ) with AgNO 3 ( aq ) to Form AgCl ( s )

111. Determining the Mass of Product Formed

112. Performing Calculations for Acid-Base Reactions

113. Neutralization Reactions I

114. Neutralization Reactions II

115. Neutralization Titration

116. Figure 4.19 The Reaction of Solid Sodium and Gaseous Chlorine to Form Solid Sodium Chloride

117. Figure 4.20 A Summary of Oxidation-Reduction Process

118. The Half-Reaction Method (Acidic Solution)

119. The Half-Reaction Method (Basic Solution)

120. Figure 4.4a-c Electrical Conductivity of Aqueous Solutions

121. An Aqueous Solution of Co(NO 3 ) 2 .

122. Figure 4.10 Steps Involved in the Preparation of a Standard Aqueous Solution

123. Yellow Aqueous Potassium

124. Figure 4.14a-b Reactant Solutions

125. Figure 4.16 Addition of Silver Nitrate to Aqueous Solution of Potassium Chloride

126. Figure 4.17 Reaction of KCI(aq) with AgNO 3 (aq) to form AgCI(s).

127. Lead Sulfate

128. KOH and Fe(NO 3 ) 3 Mix to Create Solid Fe(OH) 3 .

129. Figure 4.18a-c The Titration of an Acid with a Base

130. Figure 4.19 The Reaction of Solid Sodium and Gaseous Chlorine to Form Solid Sodium Chloride

131. Oxidation of Copper Metal by Nitric Acid

132. Magnetite

133. Aluminum and Iodine Mix to Form Aluminum Iodide

134. Chocolate

135. When Potassium Dichromate Reacts with Ethanol, the Solution Contains Cr 3+ .

136. Table 4.2 Rules for Assigning Oxidation States

137. The End