Unit B Chapter 4 Electrolytes Precipitation (aka Double Replacement or Metathesis) Reactions Acids & Bases Neutralization Reactions Oxidation Reduction Concentration of Solutions Solution Stoichiometry

Reactions in Aqueous Solutions Unit B Chapter 4.1- 4.3, 4.5 slide view

Which of the compounds listed below are insoluble (select all that apply): NiCO3 Ba(NO3)2 C6H12O6 Na3PO3 ZnS K2CrO4 Al2(SO4)3 SnF2 Do the problem without your solubility table.

Which of the compounds listed below are insoluble: NiCO3 Ba(NO3)2 C6H12O6 Na3PO3 ZnS K2CrO4 Al2(SO4)3 SnF2 Remember that nitrates and alkali salts are always soluble. Sugar is also of course soluble. Sulfates are usually soluble Carbonates and sulfides are usually NOT soluble Do the problem without your solubility table.

In the following reaction, which ions are spectator ions: AgNO3 + NaCl → NaNO3 + AgCl ? Ag+ and NO3− Na+ and Cl− Cl− and NO3− Na+ and NO3− Ag+ and Cl− Can you do the problem without your solubility table?

In the following reaction, which ions are spectator ions: AgNO3 + NaCl → NaNO3 + AgCl ? Ag+ and NO3− Na+ and Cl− Cl− and NO3− Na+ and NO3− Since silver chloride is the precipitate, the nitrate and alkali salts are the spectator ions. Ag+ and Cl− Can you do the problem without your solubility table?

Identify the precipitate when sodium hydroxide is combined with aluminum nitrate. NaNO3 AlOH3 NaOH AlOH Al(OH)3 Do the problem without your solubility table.

Alkali nitrates will always be soluble. Identify the precipitate when sodium hydroxide is combined with aluminum nitrate. NaNO3 AlOH3 NaOH AlOH Al(OH)3 Alkali nitrates will always be soluble. By process of elimination, the precipitate must be the aluminum hydroxide. Do the problem without your solubility table.

133 g of aluminum chloride in 1 L of water would be considered (select all that apply) soluble ionized dissociated aqueous concentrated dilute weak electrolyte strong electrolyte acidic

133 g of AlCl3 in 1 L of water would be considered AlCl3 → Al3+ + 3Cl− soluble ionized dissociated aqueous concentrated dilute weak electrolyte strong electrolyte acidic generally <0.1 M is considered dilute (for reasons you don’t know yet…) slide show

Electrolytes Compounds that dissolve and dissociate into ions Strong or weak = amount ionized Concentrated or dilute = amount dissolved Electrolytes are Soluble ionic compounds Acids or bases Molecular compounds tend to be non-electrolytes

Dissolving & Dissociating When ionic compounds dissolve they dissociate Observe the orientation of the water molecules as the solvate around the dissociated ions When molecular compounds dissolve, they do not dissociate Slide View

Which solution represented below is a nonelectrolyte? 1 2 3

Which solution represented below is a nonelectrolyte? 1 2 3 1 there are no ions in the solution Which representation would coduct electricity the best?

Write the reaction that best represents the dissolving of magnesium chloride in water MgCl → Mg(aq) + Cl(aq) MgCl → Mg+ + Cl− MgCl2 → Mg2+ + (Cl−)2 MgCl2 → Mg2+ + Cl−2 MgCl2 → Mg + Cl2 MgCl2 → Mg2+ + 2Cl−

Write the reaction that best represents the dissolving of magnesium chloride in water MgCl → Mg(aq) + Cl(aq) MgCl → Mg+ + Cl− MgCl2 → Mg2+ + (Cl−)2 MgCl2 → Mg2+ + Cl−2 MgCl2 → Mg + Cl2 MgCl2 → Mg2+ + 2Cl− Be sure you know the correct charges, and show the charge on the dissociated ions. Remember that multiple amounts of the same ion separate from each other, 2Cl− not Cl2−

Write the reaction that best represents the dissolving of perchloric acid in water HClO4 → H+ + ClO4− HClO4 → H+ + 4ClO− HClO4 → H+ + Cl− + 4O2−

Write the reaction that best represents the dissolving of perchloric acid in water HClO4 → H+ + ClO4− HClO4 → H+ + 4ClO− HClO4 → H+ + Cl− + 4O2−

Write the reaction that best represents the dissolving of chlorous acid in water HClO2 → H+ + ClO2− HClO2 → H+ + 2ClO− HClO2 → H+ + Cl− + 2O2− HClO2  H+ + ClO2− HClO2  H+ + 2ClO−

Write the reaction that best represents the dissolving of chlorous acid in water HClO2 → H+ + ClO2− HClO2 → H+ + 2ClO− HClO2 → H+ + Cl− + 2O2− Polyatomic ions do NOT break up in aqueous solutions, so the chlorite ion does not break apart in solution. HClO2  H+ + ClO2− This is a weak acid so you should use the double arrows to indicate only some of the acid ionizes. HClO2  H+ + 2ClO−

Rank the following in order of increasing conductivity in water: (equal moles of each substance put in the water) C6H12O6, KBr, HF, Zn(OH)2 Least conductive → more conductive C6H12O6 < KBr < HF < Zn(OH)2 Zn(OH)2 < C6H12O6 < HF < KBr C6H12O6 < Zn(OH)2 < HF < KBr C6H12O6 < HF < Zn(OH)2 < KBr C6H12O6 < Zn(OH)2 < KBr < HF KBr < Zn(OH)2 < HF < C6H12O6

Rank the following in order of increasing conductivity in water: (equal moles of each substance put in the water) C6H12O6, KBr, HF, Zn(OH)2 Remember that conductivity is related to the amount of ions in solution C6H12O6 < KBr < HF < Zn(OH)2 Zn(OH)2 < C6H12O6 < HF < KBr C6H12O6 < Zn(OH)2 < HF < KBr Molecular sugar is least conductive, next is zinc hydroxide, because although it is a base (and actually a strong base), it is very insoluble, hydrofluoric acid is weak, and KBr is a soluble salt. Time to memorize the 7 strong acids: HCl, HBr, HI, HNO3, H2SO4, HClO3, HClO4 C6H12O6 < Zn(OH)2 < KBr < HF KBr < Zn(OH)2 < HF < C6H12O6

C3H7OH < HClO < KCl < AlCl3 Rank the following in order of increasing conductivity in water: (equal moles of each substance put in the water) C3H7OH, KCl, HClO, AlCl3 C3H7OH < HClO < KCl < AlCl3 AlCl3 < C3H7OH < KCl <HClO HClO < C3H7OH < KCl < AlCl3 C3H7OH < HClO < KCl = AlCl3 C3H7OH < KCl < AlCl3 < HClO

Rank the following in order of increasing conductivity in water: (equal moles of each substance put in the water) C3H7OH, KCl, HClO, AlCl3 C3H7OH < HClO < KCl < AlCl3 C3H7OH is an alcohol, it is molecular and therefore least conductive. HClO, perchlorous acid is a weak acid. KCl, AlCl3 are salts and you might think are equally conductive, but because AlCl3 dissociates into 4 ions (Al+3 and 3 Cl−) it produces more ions per equal concentration and thus is a more conductive solution. AlCl3 < C3H7OH < KCl <HClO HClO < C3H7OH < KCl < AlCl3 C3H7OH < HClO < KCl = AlCl3 C3H7OH < KCl < AlCl3 < HClO

Calculate the concentration of chloride ion when 5 Calculate the concentration of chloride ion when 5.8 g of sodium chloride and 4.8 g of magnesium chloride is dissolved to produce 400 ml of solution. No Calculator 0.05 M 0.50 M 0.10 M 2.0 M 0.15 M 0.40 M 0.20 M 0.75 M

Calculate the concentration of chloride ion when 5 Calculate the concentration of chloride ion when 5.8 g of sodium chloride and 4.8 g of magnesium chloride is dissolved to produce 400 ml of solution. 0.05 M 0.10 M 0.15 M 0.20 M 0.50 M 2.0 M No Calculator

When 30. ml of 0. 50 M K2SO4 are added to 70. mL of 0 When 30. ml of 0.50 M K2SO4 are added to 70. mL of 0.50 M of KMnO4, the resulting concentration of potassium is No Calculator 1.0 0.85 0.65 0.50 0.33 27

When 30. ml of 0. 50 M K2SO4 are added to 70. mL of 0 When 30. ml of 0.50 M K2SO4 are added to 70. mL of 0.50 M of KMnO4, the resulting concentration of potassium is 1.0 0.85 0.65 0.50 0.33 No Calculator