Reaction in Aqueous Solution Chapter 4

Precipitation reactions Form a solid---precipitate! Remember: Solubility Rules Found on page 91 figure 4.2 Or on the web Or you saved them from last year Yep ya gotta know em

Are the following soluble or insoluble? BaCl2 soluble Mg(OH)2 insoluble Cr2(CO3)3 K3PO4 All Chloride are soluble except Ag+Hg2+Pb2+ All hydroxides are insoluble except Ca2+ Sr2+ Ba 2+ All carbonates are insoluble except group I and NH4+ All group I elements are soluble!

Net ionic equations Ba(NO3)2 + Na2CO3

BaCl2 + NaOH All aqueous—no precipitate—no rxn!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!

When sodium hydroxide and copper (II) sulfate react a with precipitate is formed. What volume of 0.216 M NaOH solution is required to produce 4.328 g of precipitate? Net ionic equation?

= 0.411 L NaOH

Acid-base reactions Acids Bases Produce H+ in water Strong acids Completely dissociate in water HCl HBr HI H2SO4 HClO4 HClO3 HNO3 Bases Produce OH- in water Strong bases Completely dissociate in water Group I metals Heavier group II metals

Strong acid-strong base -neutralization

Weak acid-strong base

Strong acid-weak base

Acid –base titrations Used to determine an unknown concentration of either the acid or the base The concentration of the other solution is known and so is the volume of both solutions Equivalence point The point at which the reaction is complete Moles of acid = moles of base

What volume of 0. 10 M NaOH is required to completely neutralize 250 What volume of 0.10 M NaOH is required to completely neutralize 250.00 mL of 0.30 M HCl? = 0.75 L NaOH

If 25. 0mL of 0. 500 M NaOH is required to react with 15 If 25.0mL of 0.500 M NaOH is required to react with 15.0 mL HCl what is the molarity of HCl ?

Oxidation-reduction reactions Redox Oxidation-loss of electrons Oxidation number increases Reduction-gain of electrons Oxidation number decreases Oxidizing agent The element that undergoes reduction Reducing agent The element that undergoes oxidation

Balancing Balance the atoms Break the equation into two half reaction Oxidation Reduction Balance O’s with H20 Balance H’s with H+ Balance the charge with electrons If confused do not use the book’s method!

Balance using half reactions Oxidizing agent Use pen as pointer to assign oxidation numbers Reducing agent

In a basic solution Balance all redox in acidic solution unless stated

Balance in a basic solution Oxidizing agent Use pointer pen to assign ox numbers Reducing agent

10 OH- + + 10 OH- = 10 H2O =8 H2O

What volume of 0.684 M KMnO4 solution is required to completely react with 27.50 mL of 0.250 M Fe(NO3)2