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"; Water/Solution Chemistry, Chemistry Homework Help - Chem Homework Help
Water/Solution Chemistry, chemistry homework help

QUESTION 1Which of the following properties is NOT a property of water?strong surface tensionhigh capillary action with glassability to dissolve polar moleculesspontaneous dissociation into gases3 points Save AnswerQUESTION 2Every solution is composed of a solvent and at least one:suspensionsolutesolidsaturated substance3 points Save AnswerQUESTION 3Why 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 AnswerQUESTION 4A solution in which equilibrium exists between dissolved and undissolved solute must be:dilutesaturatedunsaturatedconcentrated3 points Save AnswerQUESTION 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 AnswerQUESTION 6Using solubility rules, determine if the following compounds are soluble in water.insolubleRead Answer Items for Question 6solubleRead Answer Items for Question 6AnswerA. Ca(NO3)2B. Mg3(PO4)24 points Save AnswerQUESTION 7Predict whether the following double-replacement reaction will produce a precipitate: MgCl2 + Li2CO3 Imported Asset MgCO3 + 2 LiCl.No; all products are solubleYes; the MgCO3 will precipitateYes; the LiCl will precipitateYes; both the MgCO3 and the LiCl will precipitate3 points Save AnswerQUESTION 8Write 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 AnswerQUESTION 9A 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 AnswerQUESTION 10You 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 AnswerQUESTION 11Which 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 solutionthe vapor pressure of the solute and the concentration of the solventthe concentration of the solute and the molar mass of the solventthe vapor pressure of the solvent and the concentration of the (non-volatile) solute particles3 points Save AnswerQUESTION 12Calculate 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 °C1.4 °C-1.4 °C-4.8 °C3 points Save AnswerQUESTION 13Acids generally:enhance the properties of basesrelease hydrogen gas when mixed with metalsfeel slipperytaste bitter3 points Save AnswerQUESTION 14Which material is most likely to be a base?salt watervinegarcoffeeorange juice3 points Save AnswerQUESTION 15Write 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 AnswerQUESTION 16Rank the acid-base definitions from most specific (exclusive) to most general (inclusive):Arrhenius, Brønsted-Lowry, LewisArrhenius, Lewis, Brønsted-LowryBrønsted-Lowry, Lewis, ArrheniusLewis, Arrhenius, Brønsted-Lowry1 points Save AnswerQUESTION 17Acids:are generally proton donorsproduce H+ ions in solutionare electron pair acceptorsmay include all of these characteristics1 points Save AnswerQUESTION 18Bases:are generally proton acceptorsproduce OH− ions in solutionare electron pair donorsmay include all of these characteristics1 points Save AnswerQUESTION 19The formula HNO3 is named:nitrous acidnitric acidhydrogen nitrogen trioxidehydrogen nitrite3 points Save AnswerQUESTION 20Weak acids:are always more soluble than strong acidshave a higher degree of dissociation than do strong acidsonly ionize a fraction of their moleculesalways produce weak conjugate bases3 points Save AnswerQUESTION 21Milk is only slightly acidic. The pH of milk is closest to:24683 points Save AnswerQUESTION 22The 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 AnswerQUESTION 23A solution has a [OH−] of 1 x 10−9. What is the pOH of this solution?579123 points Save AnswerQUESTION 24When 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 hydrideOH− from the strong base to form water and a saltsalt that is producedwater molecule that is produced3 points Save AnswerQUESTION 25Write 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 AnswerQUESTION 26How many milliliters of a 0.100 M NaOH solution are required to neutralize 25.0 milliliters of 0.150 M HCl?25.0 ml37.5 ml125 ml167 ml3 points Save AnswerQUESTION 27If a small amount of excess acid is added to a buffered solution, the pH of the solution should:change sharply and then neutralizeremain very close to the original pH valuefluctuate rapidly between high and low values and then achieve a neutral balanceneutralize instantaneously3 points Save AnswerQUESTION 28Oxidation numbers can be used to identify the element that is being oxidized and the element that is being reduced in a redox equation.TRUEFALSE2 points Save AnswerQUESTION 29Although 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 AnswerQUESTION 30Although 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 AnswerQUESTION 31Identify 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 AnswerQUESTION 32Balance 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 AnswerQUESTION 33In a similar way to oxidation-reduction reactions, half-reactions can be written for electrochemical reactions.TRUEFALSE2 points Save AnswerQUESTION 34Voltaic 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.

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