Chapter 16 Acid Base Equilibria Strong bases are strong electrolytes and dissociate completely in solution. for example: naoh(aq) na (aq) oh–(aq) the poh (and thus the ph) of a strong base may be calculated using the initial molarity of the base. not all bases contain the oh– ion. ionic metal oxides, hydrides, and nitrides are basic. Chapter 16. acid base equilibria and solubility equilibria what we will learn: • homogeneous and heterogeneous solution equilibria • common ion effect • buffer solutions • acid base titrations • acid base indicators • solubility equilibria • separation of ions by fractional precipitation • common ion effect and solubility.
Chapter 16 Acid Base Equilibria Ppt Download 16.10: acid base behavior and chemical structure. inductive effects and charge delocalization significantly influence the acidity or basicity of a compound. the acid–base strength of a molecule depends strongly on its structure. the weaker the a–h or b–h bond, the more likely it is to dissociate to form an h h ion. An acid has a higher [h3o ] than pure water, so its ph is <7. a base has a lower [h3o ] than pure water, so its ph is >7. these are the ph values for several common substances fig. 16.5. the “p” in ph tells us to take the negative base 10 logarithm of the quantity (in this case, hydronium ions). Acid–base equilibrium •every acid–base reaction, equilibrium favors: –transfer of the proton from the stronger acid –to the stronger base forming: •the weaker acid •the weaker base. hcl h o h o cl(aq l aq aq) 23 ()® () ( ) 2 hois a much stronger basethan cl sothe equilibrium lies far to the right(k>>1.) acetate ion is a stronger. H3o (aq) oh (aq) ! h2o(l) h2o(l) acid 1 base 2 acid 2 base 1 write a balanced equation showing how the following substances behave as acids in. water and identify the conjugate acid base pairs. . hno3 hco3 h3po4 h2po4. amphoterism amphoteric substances can act as either an acid or a base. h2o is the most important.
Ppt Chapter 16 Acid Base Equilibria Powerpoint Presentation Free Acid–base equilibrium •every acid–base reaction, equilibrium favors: –transfer of the proton from the stronger acid –to the stronger base forming: •the weaker acid •the weaker base. hcl h o h o cl(aq l aq aq) 23 ()® () ( ) 2 hois a much stronger basethan cl sothe equilibrium lies far to the right(k>>1.) acetate ion is a stronger. H3o (aq) oh (aq) ! h2o(l) h2o(l) acid 1 base 2 acid 2 base 1 write a balanced equation showing how the following substances behave as acids in. water and identify the conjugate acid base pairs. . hno3 hco3 h3po4 h2po4. amphoterism amphoteric substances can act as either an acid or a base. h2o is the most important. Citric acid, which is present in citrus fruits, is a triprotic acid (table 16.3). (a) calculate the $\mathrm{ph}$ of a $0.040 \mathrm{m}$ solution of citric acid. (b) did you have to make any approximations or assumptions in completing your calculations?. Phenylacetic acid (c 6 h 5 ch 2 cooh) is one of the substances that accumulates in the blood of people with phenylketonuria, an inherited disorder that can cause mental retardation or even death. a 0.085 m solution of c 6 h 5 ch 2 cooh has a ph of 2.68. calculate the k a value for this acid. allison parrett.
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