3 O and OH H 2 O H 2 O H 3 O OH Kw is the equilibrium constant K wH3 O x OH 100

3 o and oh h 2 o h 2 o h 3 o oh kw is the equilibrium

This preview shows page 3 - 4 out of 4 pages.

3 O + and OH - . H 2 O + H 2 O ↔ H 3 O + + OH - K w is the equilibrium constant, K w =[H 3 O + ] x [OH - ]=1.00 x 10 -14 In pure water or a neutral solution: [H 3 O + ]=[OH - ]= 1.0 x 10 -7 M In acidic solutions [H 3 O + ] >[ OH - ] and [H 3 O + ] > 1.0 x 10 -7 M and [OH - ] < 1.0 x 10 -7 M In basic solutions [H 3 O + ] < [ OH - ] and [H 3 O + ] <1.0 x 10 -7 M and [OH - ] >1.0 x 10 -7 M 11.6 The pH Scale pH= -log[H 3 O + ] pH < 7 pH = 7 pH > 7 11.7 Reactions of Acids and Bases 1. Acids react with many metals to produce H 2 and the salt of the metal, which causes corrosions of active metals. Zn (s) + HCl (aq) à ZnCl 2(aq) + H 2(g) 2. Acids react with salts of carbonates and bicarbonates to produce CO 2 + H 2 O+ another salt. CaCO 3 + 2HCl à CaCl 2 + CO 2 + H 2 O NaHCO 3 + HCl à NaCl + CO 2 + H 2 O 3. Acids and bases neutralize each other forming salts and water HCl + NaOH à NaCl + H 2 O 2HCl + Mg(OH) 2 à MgCl 2 +2H 2 O 3H 2 SO 4 + 2Al(OH) 3 à Al 2 (SO 4 ) 3 + 6H 2 O The net ionic equation of strong acid/base neutralization is H + + OH - à H 2 O Salts are ionic compounds that have cations of the base and anions of the acid.
Acid-Base properties of salt solutions Salt components Example Explanation Salts of strong acids and strong bases produce neutral solutions, pH = 7. NaCl Neither Na + nor Cl - reacts with water. Salts of weak acids and strong bases form basic solutions, pH > 7. Na HCO 3 KF Li 3 PO 4 Na + doesn’t react with water; HCO 3 - reacts with water to produce its conjugate acid H 2 CO 3 and OH - . Thus, the solution is basic.

You've reached the end of your free preview.

Want to read all 4 pages?

• Fall '10
• LingChen
• pH, Acids, NH3

What students are saying

• As a current student on this bumpy collegiate pathway, I stumbled upon Course Hero, where I can find study resources for nearly all my courses, get online help from tutors 24/7, and even share my old projects, papers, and lecture notes with other students.

Kiran Temple University Fox School of Business ‘17, Course Hero Intern

• I cannot even describe how much Course Hero helped me this summer. It’s truly become something I can always rely on and help me. In the end, I was not only able to survive summer classes, but I was able to thrive thanks to Course Hero.

Dana University of Pennsylvania ‘17, Course Hero Intern

• The ability to access any university’s resources through Course Hero proved invaluable in my case. I was behind on Tulane coursework and actually used UCLA’s materials to help me move forward and get everything together on time.

Jill Tulane University ‘16, Course Hero Intern