Quick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent

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1 Quick Review - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent

2 Water H 2 O Is water an ionic or a covalent compound? Covalent, which means electrons are shared, but they are not shared equally, O attracts electrons better than H. This means water is a polar molecule. This polarity gives water its ability to dissolve compounds.

3 Water H 2 O When ionic compounds dissolve in water they break into their respective ions. This process is called hydration and is denoted by aq. Ex: NaCl (s) Na + (aq) + Cl - (aq) Cations are attracted to the negative ends of water molecules and anions are attracted to the positive ends.

4 Solubility Solubility of ionic compounds depends on the relative attractions of the ions for each other and the attractions of ions for water. Polar covalent compounds can also dissolve in water see C 2 H 5 OH below for an example.

5 Solubility Rules Utilize the solubility rules in order to determine the solubility of an ionic compound. You do NOT need to memorize these rules, just know how to use them. insoluble insoluble Exceptions: Salts of alkali metals and ammonium cations.

6 Electrolytes Strong Weak Nonelectrolyte

7 Strong Electrolytes When dissolved in solution if ions dissociate completely they produce strong electrolytes. Strong electrolytes include: soluble ionic compounds, strong acids and strong bases. Soluble ionic compounds: NaNO 3 (s) Na + (aq) + NO 3- (aq) Strong acids (HCl, HBr, HI, HNO 3, HClO 4 and H 2 SO 4 ): HI (aq) H + (aq) + I - (aq) Strong bases (soluble metal hydroxide salts): Sr(OH) 2 (s) Sr 2+ (aq) + 2OH - (aq)

8 Weak and Nonelectrolytes Weak electrolytes only some ions present; conduct electricity, but only slightly, compounds are not 100 % ionized. Weak electrolytes include weak acids and weak bases. Weak acids CH 3 COOH, HF, HCN, H 2 S, HNO 2, H 2 SO 3, H 3 PO 4 we will ignore weak bases for now. Nonelectrolytes no ions present in solution, does not conduct electricity. Examples: Table sugar, ethanol.

9 Concentration Amounts of chemical substances in solution are usually described in terms of concentrations. M = molarity = moles of solute liters of solution Compound dissolved in solution Solvent Conventional units are mol/l expressed as M

10 Concentration Question - Calculate the concentration of all ions present in the following solution: (a) mol of Ca(NO 3 ) 2 in ml of solution.

11 Dilution Dilution is the process of adding solvent to lower the concentration of solute in a solution. In a dilution the concentration changes but NOT the number of moles of solute. Moles of solute after dilution = Moles of solute before dilution M 2 V 2 = M 1 V 1 Solutions are typically diluted in order to work with useful quantities.

12 Dilution Example We want to prepare 500. ml of 1.00 M acetic acid (CH 3 COOH) from a 17.4 M stock solution of acetic acid. What volume of stock solution is required?

13 Precipitation Reactions Precipitation Reactions are double displacement reactions where the cations and anions of the two reacting salts switch. The result is the formation of a solid precipitate. In general in a precipitation reaction two soluble compounds are mixed and an insoluble compound precipitates. Solubility rules are used to predict the precipitates.

14 Precipitation Reactions Question What happens when a solution of barium nitrate and potassium chromate are mixed

15 Precipitation Reactions insoluble insoluble Exceptions: Salts of alkali metals and ammonium cations.

16 Precipitation Reactions Molecular equation: Complete ionic equation: Net ionic equation:

17 Precipitation Reactions Ba(NO 3 ) 2 (aq) + K 2 CrO 4 (aq) BaCrO 4 (s) + 2 KNO 3 (aq)

18 Solution Stoichiometry What mass of barium sulfate can be produced when ml of a M solution of barium chloride is mixed with ml of a M solution of iron (III) sulfate?

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