Ppt Chapter 16 Acid Base Equilibria Powerpoint Presentation Free 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. 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.
Ppt Chapter 16 Acid Base Equilibria Powerpoint Presentation Free 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. 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. 16.10.1 factors that affect acid strength. strength of acid depends on: 1) polarity of h x bond. 2) strength of h x bond. 3) stability of conjugate base, x . molecule will transfer proton if h x bond is polarized. in ionic hydrides h acts as proton acceptor because of negative charge. • acid base neutralization reaction will be discussed in detail in chapter 17 (sections 17.1 17.3). • acid rain will be discussed in chapter 18 (section 18.2). • inverse relationship between conjugate acids and bases will be mentioned in chapter 20 (section 20.4). • acid base properties in proton transfer reactions involving oh–, h 2o, nh.
Chapter 16 Acid Base Equilibria 16.10.1 factors that affect acid strength. strength of acid depends on: 1) polarity of h x bond. 2) strength of h x bond. 3) stability of conjugate base, x . molecule will transfer proton if h x bond is polarized. in ionic hydrides h acts as proton acceptor because of negative charge. • acid base neutralization reaction will be discussed in detail in chapter 17 (sections 17.1 17.3). • acid rain will be discussed in chapter 18 (section 18.2). • inverse relationship between conjugate acids and bases will be mentioned in chapter 20 (section 20.4). • acid base properties in proton transfer reactions involving oh–, h 2o, nh. 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. Bh. (aq) 16.2 brønsted‐lowry acids & bases. ‐ the h ion in water ‐‐ h o . 3 is called the hydronium ion and is what truly happens when h is in water ‐‐ since all aqueous solution are in water we will use h3o & h interchangeably ‐ conjugate acid‐base pairs ‐‐ conjugate acid: the acid that is created after the brønsted.
Chapter 16 Acid Base Equilibria 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. Bh. (aq) 16.2 brønsted‐lowry acids & bases. ‐ the h ion in water ‐‐ h o . 3 is called the hydronium ion and is what truly happens when h is in water ‐‐ since all aqueous solution are in water we will use h3o & h interchangeably ‐ conjugate acid‐base pairs ‐‐ conjugate acid: the acid that is created after the brønsted.
Chapter 16 вђ Acid Base Equilibria Summaries Chemistry Docsity
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