5. Pb(IO 3) BaCO 3 8. (NH 4) 2SO 3
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1 Chemistry 11 Solution Chemistry II Name: Date: Block: 1. Ions in Solutions 2. Solubility Table 3. Separating Ions Ions in Solutions Ionization Equation - Represents the salt breaking apart into ions. Practice: 1. KOH o NaCl (aq) à Na + (aq) + Cl - (aq) - If the salt were CaCl 2. o CaCl 2 (aq) à Ca 2+ (aq) + 2 Cl - (aq) 5. Pb(IO 3) 2 2. SrCl 2 6. Mg(OH) 2 3. NH 4NO 3 7. BaCO 3 4. Ag 2CrO 4 8. (NH 4) 2SO 3 Calculating Concentration - Mole ratios represent the relative amounts of ions in solution. NaCl (aq) à Na + (aq) + Cl - (aq) 1.0 M CaCl 2 (aq) à Ca 2+ (aq) + 2 Cl - (aq) 1.0 M
2 Practice: M KOH M Pb(IO 3) M SrCl M Mg(OH) M NH 4NO M BaCO M Ag 2CrO M (NH 4) 2SO 3 Ionization + Dilution ü A 15.0 ml sample of 3.0 M HCl was added to 10.0 ml of 2.0 M CaCl 2. Calculate the concentration of each ion in the solution. Assume no reaction occurs.
3 Practice 1. What are the concentrations of both ions in a 3.00 M solution of phosphoric acid? Practice 2. What is the sodium ion concentration when ml of water is added to ml of a 3.21 M solution of sodium phosphate? Practice 3. Determine the concentration of each ion when 45.0 ml of 7.2 M magnesium sulphate is mixed with 35.0 ml of M magnesium hydroxide. Practice 4. What is the molar concentration of each ion in solution resulting from mixing 55.0 ml of 0.15 M potassium hydroxide with 75.0 ml of 0.25 M potassium sulphate? Ions in Solutions Worksheet
4 Solubility Table When some ions are combined, they create a solid à they are NOT soluble. SOLUBLE à Dissolves in water; aqueous LOW SOLUBLE à Does not dissolve in water; solid Practice: 1. Classify the following salts as being soluble or having low solubility in water: a. Copper (II) chloride b. Aluminum hydroxide c. Sodium phosphate d. Calcium sulphate e. Iron (II) sulphide f. Strontium hydroxide g. Zinc bromide h. Cesium sulphite i. Potassium chromate 2. Write the formula for the following: a. A salt containing carbonate that is soluble b. A salt containing sulphate with low solubility c. A cation that forms a salt with low solubility with both chloride and sulphate ions d. An anion that forms soluble salts with all cations
5 3. A student is given a sample of either magnesium nitrate or strontium nitrate. When a few drops of a solution of sodium hydroxide is added to the sample, no precipitate forms. Does the sample contain magnesium nitrate or strontium nitrate? Explain your reasoning. Types of chemical equations: Formula Equation: shows the chemical formulas of the compounds and their states. 2 KI (aq) + Pb(NO 3) 2 (aq) à 2 KNO 3 (aq) + PbI 2 (s) Complete Ionic Equation: shows the soluble salts represented in their dissociated form. Net Ionic Equation: shows only the ions that take part in the reaction. Ions that are the same on both sides of the equation are called spectator ions. Practice: 1. Write the formula for the precipitate that forms when the following solutions are mixed: a. BaS and MgSO 4 b. NH 4OH and FeBr 2 c. H 3PO 4 and ZnCl 2 d. K 2CO 3 and CrSO 4 e. MnI 2 and Sr(OH) 2
6 2. Write a formula equation, complete ionic equation and net ionic equation for the following reactions: a. Strontium hydroxide and silver nitrate b. Magnesium sulphide and zinc chloride c. Sodium carbonate and barium sulphide d. (NH 4) 2S (aq) + FeSO 4 (aq) à e. H 2SO 3 (aq) + CaCl 2 (aq) à f. Copper (II) sulphate + H 2SO 3
7 Separating Ions Example: A solution may contain the ions Ca 2+, Sr 2+ and Zn 2+. How would you precipitate the ions out of solution individually? Describe your answer using a flow chart. All are cations - therefore an addition of an anion will precipitate out these cations. Low solubility means will precipitate out. 1. Which anion will precipitate just one of the ions out first? a. Which ions are left? 2. Which anion will precipitate just one of the two ions left? 3. Which anion will precipitate out the last ion left?
8 Practice: 1. For each of the following solutions, describe a process to individually remove each ion. Be sure to list the compounds that you add in order, and the method of removing the precipitate. You may wish to use a flow chart. a. Ag + Ba 2+ and Be 2+ b. Br -, SO 4 2- and S 2- c. OH -, PO 4 3- and S 2- d. Cr 3+, Ca 2+ and Mg 2+ Worksheet
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CHEM134- Fall 2018 Dr. Al-Qaisi Chapter 4b: Chemical Quantities and Aqueous Rxns So far we ve used grams (mass), In lab: What about using volume in lab? Solution Concentration and Solution Stoichiometry