Chem 112 Week of March 14-18 Notes
Chem 112 Week of March 14-18 Notes Chem 112
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This 1 page Class Notes was uploaded by Rebecca Plummer on Saturday March 19, 2016. The Class Notes belongs to Chem 112 at Pennsylvania State University taught by Dr. Raymond Shaak in Spring 2016. Since its upload, it has received 13 views. For similar materials see General Chemistry in Chemistry at Pennsylvania State University.
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Date Created: 03/19/16
Rebecca Plummer Dr. Raymond Schaak 3/18/16 Acids and Bases Bronsted-Lowry Acid: Acids donate protons (H ) + + Bronsted-Lowry Base: Bases accept protons (H ) Strong acids and bases completely dissociate in water Weak acids and bases dissociate in water too but not completely Neutral substances do not dissociate at all in water Strong acids have a low pH value (1, 2, 3…) Strong bases have a high pH value (12, 13, 14…) Neutral substances have a pH of 7 + - pH = -log [H ] pOH = -log [OH ] pH is the negative log of the concentration of the H ions - pOH is the negative log of the concentration of the OH ions When looking for the pOH when you only have H ions, calculate the pH and then subtract that number by 14. Ka: equilibrium constant for acids o K ia directly proportional to pH As pH increases, K aaso increases Large K as related to a stronger weak acid pK a -log (K ) a o used to express the strength of acids o pK ia inversely proportional to pH and K a As pK ancreases, pH decreases Smaller pK ia related to a stronger weak acid Conjugate Acids and Bases o K aad K (ebuilibrium constant for bases) are inversely proportional Kw= K ∙aK b pK w pK + pa b K w [H ][OH ] - Ions with barely any acidity or basicity are spectator ions Amphoteric: species that can be an acid or a base