Practice problem-chapter 5

Chapter 5 Practice Problems: I. Dilutions: 1. If I add 25 mL of water to 125 mL of a 0.15 M NaOH solution, what will be the molarity of the diluted solution? 2. If I add water to 100 mL of a 0.15 M NaOH solution until the final volume is 150 mL, what will the molarity of the diluted solution? 3. How much 0.05 M HCl solution can be made by diluting 250 mL of 10 M HCl? 4. I have 345 mL of a 1.5 M NaCl solution. If I boil the water until the volume of the solution is 250 mL, what will the molarity of the solution? 5. How much water would I need to add to 500 mL of a 2.4 M KCl solution to make a 1.0 M solution? II. Molarity 1. How many grams of potassium carbonate are needed to make 200 mL of a 2.5 M solution? 2. How many liters of 4 M solution can be made using 100 grams of lithium bromide? 3. What is the concentration of an aqueous solution with a volume of 450 mL that contains 200 grams of iron (II) chloride? 1 4.) How many grams of ammonium sulfate are needed to make a 0.25 M solution at a concentration of 6 M? 5.) What is the concentration of a solution with a volume of 2.5 liters containing 660 grams of calcium phosphate? 6.) How many grams of copper (II) fluoride are needed to make 6.7 liters of a 1.2 M solution? 7.) How many liters of a 0.88 M solution can be made with 22.5 grams of lithium fluoride? III. Label each of the following as strong, weak, or non-electrolyes. 1. HCl 2. NH3 3. NaCl 4. KNO3 5. C12H22O11 6. NaOH 7. CH3COOH 2 8. H2O 9. KBr IV. Identify the following as strong or weak acids. 1. HBr (aq) 2. HNO2 (aq) 3. HNO3 (aq) 4. H2SO4 (aq) 5. HSO4- V. Complete and balance the following equations carried out in aqueous solution. Also, writing the complete ionic and net ionic equations. 1. Molecular Eq. : ____ Na3PO4 (aq) + ____ KOH (aq) → Complete Ionic: Net Ionic: 3 2. Molecular Eq. : ____ Al (s) + ____ HNO3 (aq) → Complete Ionic: Net Ionic: 3. Molecular Eq. : ____ BaBr2 (aq) + ____ H2SO4 (aq) → Complete Ionic: Net Ionic: 4. Molecular Eq. : ____ Zn(NO3)2 (aq) + ____ H2S (aq) → Complete Ionic: Net Ionic: 5. Molecular Eq. : ____ Na3PO4 (aq) + ____ CaCl2 (aq) → Complete Ionic: 4 Net Ionic: 6. Molecular Eq. : ____ H2SO4 (aq) + ____ Bi(OH)3 (s) → Complete Ionic: Net Ionic: 7. Molecular Eq. : ____ Pb(NO3)2 (aq) + ____ H2S (aq) → Complete Ionic: Net Ionic: 8. Molecular Eq. : ____ HgSO4 (aq) + ____ Mg(ClO3)2 (aq) → Complete Ionic: Net Ionic: 9. Molecular Eq. : ____ SrCl2 (aq) + ____ AgNO3 (aq) → 5 Complete Ionic: Net Ionic: 10. Molecular Eq. : ____ Cu(NO3)2 + ____ (NH4)2S (aq) → Complete Ionic: Net Ionic: VI. Acid-Base Reactions: 1. Write the balanced formula equation for the acid-base reactions that occur when the following are mixed. a. potassium hydroxide (aq) and nitric acid b. barium hydroxide (aq) and hydrochloric acid c. perchloric acid (aq) and solid iron (III) hydroxide d. solid silver hydroxide and hydrobromic acid e. aqueous strontium hydroxide and hydroiodic acid 2. What volume of each of the following acids will react completely with 50.00 mL of 0.200 M NaOH? a. 0.100 M HCl 6 b. 0.150 M HNO3 c. 0.200 M HC2H3O2 (1 acidic hydrogen) 3. What volume of 0.0200 M calcium hydroxide is required to neutralize 35.00 mL of 0.0500 M nitric acid? 4. A 30.0 mL sample of an unknown strong base is neutralized after the addition of 12.0 mL of a 0.150 M HNO3 solution. If the unknown base concentration is 0.0300 M, give some possible identities for the unknown base. VII. Oxidation-Reduction Reactions 1. Assign oxidation states for all atoms in each of the following compounds. a. KMnO4 b. NiO2 c. Na4Fe(OH)6 d. (NH4)2HPO4 e. P4O6 7 f. Fe3O4 g. XeOF4 h. SF4 i. CO j. C6H12O6 2. Specify which of the following are oxidation-reduction reactions, and identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced. a. Cu (s) + 2 Ag+ (aq) → 2 Ag (s) + Cu2+ (aq) b. HCl (g) + NH3 (g) → NH4Cl(s) c. SiCl4 (l) + 2 H2O (l) → 4 HCl (aq) + SiO2 (s) d. SiCl4 (l) + 2 Mg (s) → 2 MgCl2 (s) + Si (s) e. Al(OH)4- (aq) → AlO2- (aq) + 2 H2O (l) f. CH4 (g) + H2O (g) → CO (g) + 3 H2 (g) g. 2 AgNO3 (aq) + Cu (s) → Cu(NO3)2 (aq) + 2 Ag (s) h. Zn (s) + 2 HCl (aq) → ZnCl2 (aq) + H2 (g) i. 2 H+ (aq) + 2 CrO42- (aq) → Cr2O72- (aq) + H2O (l) 8 9

Practice problem-chapter 5

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