Chapter 4 Lecture- Solution Stoich
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This document provides information on various chemistry concepts related to solutions and reactions in aqueous solutions. It defines key terms like electrolytes, nonelectrolytes, dissociation, and precipitation reactions. It also discusses acid-base reactions and neutralization reactions. Oxidation-reduction reactions and displacement reactions are introduced. Molarity is defined as a way to quantify concentration in solutions.
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This document summarizes key concepts in solution chemistry and stoichiometry, including:
1) Solutions, electrolytes, dissociation, and precipitation reactions are discussed. Strong and weak electrolytes are defined.
2) Acid-base reactions such as neutralization and gas-forming reactions are covered. Oxidation-reduction reactions and displacement reactions are also summarized.
3) Concepts including molarity, dilution, and titration reactions are introduced for quantitative chemical calculations.
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This document discusses various topics relating to solutions and solution chemistry, including:
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1) The definition of solutions, solvents, and solutes. A solution is a homogeneous mixture of substances where the solute is the smaller component dissolved in the solvent.
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This document discusses different types of chemical reactions including decomposition, synthesis, combustion, double replacement, and single replacement reactions. It provides examples of each type of reaction and explains the key features that define them. Double replacement reactions are highlighted, where a metal replaces a metal in a compound and a nonmetal replaces a nonmetal, forming a precipitate if one of the products is insoluble. Guidelines are provided for writing molecular, total ionic, and net ionic equations for double replacement reactions.
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1) A solution is a homogeneous mixture of two or more substances, where the solute is present in smaller amounts than the solvent.
2) An electrolyte is a substance that, when dissolved in water, allows the solution to conduct electricity through the formation of ions, while a nonelectrolyte does not form ions and the solution cannot conduct electricity.
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Polyatomic ions stay intact in aqueous solutions because they are held together by strong covalent bonds between their constituent atoms. When ionic compounds dissolve in water, the ions separate but polyatomic ions remain intact units because the covalent bonds within them are not broken by the dissociation process.
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The circulatory system transports blood throughout the body via the heart and blood vessels. The heart has four chambers and uses valves to pump oxygenated blood from the lungs and deoxygenated blood to the lungs. Blood flows through arteries, capillaries, and veins. The respiratory system exchanges gases through the nose, pharynx, trachea, bronchi, and alveoli in the lungs. Breathing is controlled by the medulla oblongata and diaphragm. Smoking damages lungs and increases risk of diseases like cancer, emphysema, and bronchitis.
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Chapter 4 Lecture- Solution Stoich
- 10. Answers: C 6 H 12 O 6 (nonelectrolyte) < HC 2 H 3 O 2 (weak electrolyte, existing mainly in the form of molecules with few ions) < NaC 2 H 3 O 2 (strong electrolyte that provides two ions, and (strong electrolyte that provides three ions, Ca 2+ and 2 NO 3 – PRACTICE EXERCISE Consider solutions in which 0.1 mol of each of the following compounds is dissolved in 1 L of water: Ca(NO 3 ) 2 (calcium nitrate), C 6 H 12 O 6 (glucose), NaC 2 H 3 O 2 (sodium acetate), and HC 2 H 3 O 2 (acetic acid). Rank the solutions in order of increasing electrical conductivity, based on the fact that the greater the number of ions in solution, the greater the conductivity.
- 12. PRACTICE EXERCISE Classify the following compounds as soluble or insoluble in water: (a) cobalt(II) hydroxide, (b) barium nitrate, (c) ammonium phosphate. Answers: (a) insoluble, (b) soluble, (c) soluble
- 24. PRACTICE EXERCISE Write the net ionic equation for the precipitation reaction that occurs when aqueous solutions of silver nitrate and potassium phosphate are mixed.
- 33. PRACTICE EXERCISE (a) Write a balanced molecular equation for the reaction of carbonic acid (H 2 CO 3 ) and potassium hydroxide (KOH). (b) Write the net ionic equation for this reaction. (H 2 SO 3 is a weak acid and therefore a weak electrolyte, whereas KOH, a strong base, and K 2 CO 3 , an ionic compound, are strong electrolytes.)
- 48. Activity Series
- 52. Dilution
- 53. Answer: 0.278 M SAMPLE EXERCISE 4.11 PRACTICE EXERCISE Calculate the molarity of a solution made by dissolving 5.00 g of glucose (C 6 H 12 O 6 ) in sufficient water to form exactly 100 mL of solution.
- 54. PRACTICE EXERCISE What is the molar concentration of K + ions in a 0.015 M solution of potassium carbonate? Answer: 0.030 M K +
- 55. PRACTICE EXERCISE (a) How many grams of Na 2 SO 4 are there in 15 mL of 0.50 M Na 2 SO 4 ? (b) How many milliliters of 0.50 M Na 2 SO 4 solution are needed to provide 0.038 mol of this salt? Answers: (a) 1.1 g, (b) 76 mL
- 56. PRACTICE EXERCISE (a) What volume of 2.50 M lead(II)nitrate solution contains 0.0500 mol of Pb 2+ ? (b) How many milliliters of 5.0 M K 2 Cr 2 O 7 solution must be diluted to prepare 250 mL of 0.10 M solution? (c) If 10.0 mL of a 10.0 M stock solution of NaOH is diluted to 250 mL, what is the concentration of the resulting stock solution? Answers: (a) 0.0200 L = 20.0 mL, (b) 5.0 mL, (c) 0.40 M
- 57. Using Molarities in Stoichiometric Calculations
- 58. PRACTICE EXERCISE (a) How many grams of NaOH are needed to neutralize 20.0 mL of 0.150 M H 2 SO 4 solution? (b) How many liters of 0.500 M HCl( aq ) are needed to react completely with 0.100 mol of Pb(NO 3 ) 2 ( aq ), forming a precipitate of PbCl 2 ( s )? Answers: (a) 0.240 g, (b) 0.400 L
- 60. Titration
- 61. PRACTICE EXERCISE What is the molarity of an NaOH solution if 48.0 mL is needed to neutralize 35.0 mL of 0.144 M H 2 SO 4 ? Answers: 0.210 M