Description QUESTION 1 Which of the following properties is NOT a property of water? strong surfa ...

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Description QUESTION 1 Which of the following properties is NOT a property of water? strong surface tension high capillary action with glass ability to dissolve polar molecules spontaneous dissociation into gases 3 points Save Answer QUESTION 2 Every solution is composed of a solvent and at least one: suspension solute solid saturated substance 3 points Save Answer QUESTION 3 Why does stirring increase the rate of solution formation for a solid solute in a liquid solvent? Stirring brings solute particles closer together and provides them with additional energy. Stirring mixes solute particles with solvent particles more thoroughly, providing more chances of interaction. Stirring makes the entire solution warmer so that the temperature increases noticeably. Stirring agitates the solute particles and increases the rate of precipitation. 3 points Save Answer QUESTION 4 A solution in which equilibrium exists between dissolved and undissolved solute must be: dilute saturated unsaturated concentrated 3 points Save Answer QUESTION 5 Imported Asset At which temperature would a 40-gram KCl per 100 grams of water solution, be considered supersaturated? 30° 50° 70° 80° 3 points Save Answer QUESTION 6 Using solubility rules, determine if the following compounds are soluble in water. insoluble Read Answer Items for Question 6 soluble Read Answer Items for Question 6 Answer A. Ca(NO3)2 B. Mg3(PO4)2 4 points Save Answer QUESTION 7 Predict whether the following double-replacement reaction will produce a precipitate: MgCl2 + Li2CO3 Imported Asset MgCO3 + 2 LiCl. No; all products are soluble Yes; the MgCO3 will precipitate Yes; the LiCl will precipitate Yes; both the MgCO3 and the LiCl will precipitate 3 points Save Answer QUESTION 8 Write the overall, ionic and net ionic equations for the following reaction. Nitric acid (HNO3) and barium hydroxide (Ba(OH)2) (please respond with a few sentences explaining) 4 points Save Answer QUESTION 9 A solution is prepared by mixing 0.767 kg of sulfuric acid (H2SO4) with 2.71 kg of water to make 3.00 L of solution. What is the percentage composition by mass of sulfuric acid in this solution? 22.0% 25.6% 27.1% 28.3% 3 points Save Answer QUESTION 10 You have 100 milliliters of a 0.50 M MgBr2 solution and dilute it to a total volume of 200 milliliters. What is the molarity of the resulting solution? (please respond with a few sentences explaining) 4 points Save Answer QUESTION 11 Which two factors determine the vapor pressure of a solution containing a non-volatile solute dissolved in a volatile solvent, at a given temperature? the molar mass of the solute and the volume of the solution the vapor pressure of the solute and the concentration of the solvent the concentration of the solute and the molar mass of the solvent the vapor pressure of the solvent and the concentration of the (non-volatile) solute particles 3 points Save Answer QUESTION 12 Calculate the freezing point of a 2.6-molal aqueous sucrose solution. The freezing point depression constant for water is 1.86 degrees C/molal. 4.8 °C 1.4 °C -1.4 °C -4.8 °C 3 points Save Answer QUESTION 13 Acids generally: enhance the properties of bases release hydrogen gas when mixed with metals feel slippery taste bitter 3 points Save Answer QUESTION 14 Which material is most likely to be a base? salt water vinegar coffee orange juice 3 points Save Answer QUESTION 15 Write an overall equation for the acid-base reaction that would be required to produce the following salt. MgCl2 (please respond with a few sentences explaining) 4 points Save Answer QUESTION 16 Rank the acid-base definitions from most specific (exclusive) to most general (inclusive): Arrhenius, Brønsted-Lowry, Lewis Arrhenius, Lewis, Brønsted-Lowry Brønsted-Lowry, Lewis, Arrhenius Lewis, Arrhenius, Brønsted-Lowry 1 points Save Answer QUESTION 17 Acids: are generally proton donors produce H+ ions in solution are electron pair acceptors may include all of these characteristics 1 points Save Answer QUESTION 18 Bases: are generally proton acceptors produce OH? ions in solution are electron pair donors may include all of these characteristics 1 points Save Answer QUESTION 19 The formula HNO3 is named: nitrous acid nitric acid hydrogen nitrogen trioxide hydrogen nitrite 3 points Save Answer QUESTION 20 Weak acids: are always more soluble than strong acids have a higher degree of dissociation than do strong acids only ionize a fraction of their molecules always produce weak conjugate bases 3 points Save Answer QUESTION 21 Milk is only slightly acidic. The pH of milk is closest to: 2 4 6 8 3 points Save Answer QUESTION 22 The pH of a solution measures the [H3O+] in the solution. If one solution has a pH of 4 and another solution has a pH of 3, how does the [H3O+] in the two solutions compare? They are in a 1:1 ratio. They are in a 1:10 ratio. They are in a 1:100 ratio. They are in a 1:1000 ratio. 3 points Save Answer QUESTION 23 A solution has a [OH?] of 1 x 10?9. What is the pOH of this solution? 5 7 9 12 3 points Save Answer QUESTION 24 When weak acids react with strong bases, the H+ from the weak acid is transferred to the: metal of the strong base to form a metal hydride OH? from the strong base to form water and a salt salt that is produced water molecule that is produced 3 points Save Answer QUESTION 25 Write the overall, ionic and net ionic equations for the following reaction.Hydrochloric acid (HCl) and potassium hydroxide (KOH) (please respond with a few sentences explaining) 4 points Save Answer QUESTION 26 How many milliliters of a 0.100 M NaOH solution are required to neutralize 25.0 milliliters of 0.150 M HCl? 25.0 ml 37.5 ml 125 ml 167 ml 3 points Save Answer QUESTION 27 If a small amount of excess acid is added to a buffered solution, the pH of the solution should: change sharply and then neutralize remain very close to the original pH value fluctuate rapidly between high and low values and then achieve a neutral balance neutralize instantaneously 3 points Save Answer QUESTION 28 Oxidation numbers can be used to identify the element that is being oxidized and the element that is being reduced in a redox equation. TRUE FALSE 2 points Save Answer QUESTION 29 Although aluminum is a more active metal than iron, and therefore, oxidizes more quickly than iron, aluminum degrades much more slowly than iron. This is because: There is more aluminum than iron available on the Earth. Aluminum oxide coats the exposed aluminum surfaces preventing further corrosion. The iron is more reactive with a greater number of environmental agents. The iron oxide is much more soluble in water than the aluminum oxide. 3 points Save Answer QUESTION 30 Although Group 7A ions may have different oxidation states depending on which other elements are in the compound, the most common oxidation number for Group 7A (Group 17) ions is: 1? 3+ 5+ 7+ 3 points Save Answer QUESTION 31 Identify the oxidizing agent in the following equation: Al (s) + 3 Ag+ (aq) Imported Asset Al+3 (aq) + 3 Ag (s). Al (s) Ag+ (aq) Al+3 (aq) Ag (s) 3 points Save Answer QUESTION 32 Balance the following oxidation-reduction reaction and indicate which atoms have undergone oxidation and reduction.____FeCl3 + ____H2S Imported Asset ____FeCl2 + ____S + ____HCl (please respond with a few sentences explaining) 4 points Save Answer QUESTION 33 In a similar way to oxidation-reduction reactions, half-reactions can be written for electrochemical reactions. TRUE FALSE 2 points Save Answer QUESTION 34 Voltaic cells and electrolytic cells are similar because: Both cells use a salt bridge to keep the electrons flowing within the cells. Both cells have a positive anode. Both cells have a negative cathode. Both cells require the input of energy.