Chapter 15. Applications of Aqueous Equilibria. The Common Ion Effect. A common ion is an ion that is produced by multiple species in solution (other than H) It comes from having a salt dissolved in the same solution as an acid.By reina
Buffers. Buffered Solutions. A buffered solution is one that resists a change in its pH when either hydroxide ions or protons (H 3 O + ) are added. Very little change in pH is witnessed even when a strong acid or base is added. The components of a buffer are a conjugate acid-base pair.By nirav
Acids, Bases, and pH. Acid Compound that increases the amount of hydrogen ions (H + ) that are present Usually starts with hydrogen (H) in their chemical formula Examples: Hydrochloric acid (HCl) Citric acid (H 3 C 6 H 5 O 7 ) Lactic acid (HC 3 H 5 O 3 ). Strong AcidsBy alice
Acids and Bases. Three Definitions. Arrhenius acid – produces H + in soln base – produces OH - in soln Bronsted-Lowry acid – H + donor base – H + acceptor Lewis acid – electron pair acceptor base – electron pair donor. Conjugate acid-base pairs.By tan
Podcast 18.3. K w , pH, pOH, pK a , pK b. Ion Product Constant for Water (K w ). Occasionally, in water, a H + is transferred between H 2 O molecules. Simple K w Problems. The [OH - ] of a solution is 1.0 x 10 - 3 M. What is the [H 3 O + ]?By ashton-wong
Chemistry 142 Chapter 16: Aqueous Ionic Equilibrium. Outline Common Ion Buffers Titration Curves Acid-Base Indicators Solubility Equilibrium Precipitation Qualitative Analysis Complex Ion Equilibrium. Chapter 16 – Aqueous Ionic Equilibrium Example – Common Ion.By rogan-richardson
Chapter 17 Additional Aspects of Aqueous Equilibria. 17.1 The Common Ion Effect. CH 3 COOH ( aq ) + H 2 O ( l ). H 3 O + ( aq ) + CH 3 COO − ( aq). The Common-Ion Effect. Consider a solution of acetic acid:By tpatrick
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