study guide ch 8-9

Solution chemistry chapter 8 1) A saturated solution: A) contains as much solvent as it can hold B) contains no double bonds C) contains equal amount of solute and solvent D) contains dissolved solute in equilibrium with solvent E) maximum amount of solute that given solvent can dissolve 2) Of the following, which can serve as the solvent in a solution? A) A liquid B) A solid C) A gas D) All of the above E) only A and C 3) A homogenous mixture consists of 12% ethanol, 28% methanol and 60% water. Which of these is the solute for the mixture? A) Ethanol B) Methanol C) Water D) Ethanol and methanol E) none of the above 4) A homogenous mixture consists of 34% ethanol and 66% isopropanol. Which of these is the solute of the mixture? A) Isopropanol B) Ethanol C) Both ethanol and isopropanol D) Neither ethanol nor isopropanol 5) In a solution, the solute is: A) the substance in the greatest amount B) the substance that is being dissolved C) the substance that is in smaller amount D) always a gas E) B and C 6) Which of the following statements best describes the phrase "like dissolves like"? A) The only true solutions are formed when water dissolves a polar solute. B) A solvent and a solute with similar intermolecular forces will easily make a solution. C) The only true solutions are formed when water dissolves a nonpolar solute. D) A solvent will dissolve a solute that has a similar mass. E) Both A and B 7) Which of the following can be classified as a colloid? A) Grape juice B) Kool Aid C) Blood D) Milk 8) You have been given an unknown liquid that is insoluble in water but soluble in benzene (an aromatic hydrocarbon). Which type of molecule is the unknown? A) Polar B) Nonpolar C) Neither polar nor nonpolar D) Both polar and nonpolar 9) Which one of the following compounds will be most soluble in water? A) CH3CH2CH2CH2OH B) CH3CH2OH C) CH3CH2CH2OH D) CH3OH 10) Which one of the following compounds will be most soluble in hexane? A) CH3CH2 OH B) CH3CH2CH2OH C) D) E) C and D 11) A water solution of potassium chloride is a good conductor of electricity. Due to this property, table salt is classified as a(n): A) weak electrolyte B) strong electrolyte C) non-electrolyte D) semi-electrolyte 12) A water solution of glucose does not conduct electricity. Glucose is classified as a(n): A) weak electrolyte B) strong electrolyte C) non-electrolyte D) semi-electrolyte 13) A water solution of acetic acid, vinegar, barely lights a light bulb. This property means that vinegar is a(n): A) weak electrolyte B) strong electrolyte C) non-electrolyte D) semi-electrolyte 14) Pressure has a large effect only on the solubility of ________ in liquids. A) liquid B) solid C) solid-liquid D) all of the above E0 none of the above 15) Which of the following can be an example of a weak electrolyte? A) MgCl2 B) HC2H3O2 C) HNO3 D) KOH 16) Which of the following is an example of a nonelectrolyte? A) MgCl2 B) HC2H3O29 (acetic acid) C) C12H22O11 (sugar) D) NaOH 17) In order to prevent the process of either crenation or hemolysis with red blood cells an intervenous solution concentration should be ________ to the concentration of blood. A) hypotonic B) hypertonic C) isotonic D) all of these 18). The process of crenation occurs when the concentration outside a cell is ________ and is said to be ________. A) lower in concentration; hypotonic B) lower in concentration; hypertonic C) higher in concentration; hypotonic D) higher in concentration; hypertonic E) none of the above 19) Air can be classified to be a solution of several gases. Which gas is considered to be the solute? A. O2 B. N2 C. CO2 D. H2O E. All of the above except B 20). Oxygen is dissolved into water to make a solution. If the temperature of the solution is decreased and the partial pressure of oxygen increased, the solubility of the oxygen will _____. A. decrease B. increase C. be unchanged D. cannot predict 21). Normal saline solution is 0.90% (w/v) NaCl. A solution that is 1.10 % NaCl is _____. Which of the following statements is true? A. isotonic B. hypertonic C. hypotonic D. osmotic 22).Which of these contains the largest size particles? A. solution B. colloid C. suspension D. solvent 23). The solubility of carbon dioxide in carbonated beverages can be maximized during bottling by using: high pressures and high temperatures. low pressures and low temperatures. low pressures and high temperatures. D. high pressures and low temperatures. 24). Which of the following is inaccurate statement? A. Most gases are more soluble at higher temperature B. Many solids are more soluble at higher temperature C Many gasses are more soluble at lower temperature D. Lower the pressure, higher the solubility of gases. E. both a and d 25). Arrange the terms solution, suspension, and colloid in order of increasing size of the dispersed particles. A. solution < suspension < colloid B. solution < colloid < suspension C. suspension < solution < colloid D. colloid < solution < suspension 26). which of the following is applicable to solutions? A. solute can be solid or liquid or gas B. solvent can be solid or liquid or gas C. solution can be solid or liquid or gas D. all of the above is applicable to solutions E. none of the above is applicable to solutions 27). Which of the following statement is incorrect? A. pure water is an electrolyte B. ionic compounds are electrolytes C. tap water may show electrical conductivity due to impurities D. strong electrolytes split into ions almost instantly 28) Which of the following statement is most incorrect? A. osmosis involves movement of water through semipermeable membrane B. dialysis involves movement of only water through semipermeable membrane C. dialysis involves movement of water and smaller molecules through semipermeable membrane D. osmosis involves movement of water and small molecules and ions E. B and d are correct 29). Dissolving a solid in a liquid water can be referred to as a A. solvation B. hydration C. dissolution D. all of the above E. none of the above 30) Identify the type of transport that will occur for the sodium ions that requires energy for transport a. passive diffusion b. active transport c. facilitated diffusion d. all of the above e. none of the above 31) Identify the type of transport that will occur for the CO2 molecules that requires no energy and no help from other molecule for transport a. passive diffusion b. active transport c. facilitated diffusion d. all of the above e. none of the above 32) Identify the type of transport that will occur for the molecules that requires no energy for transport but need help from another molecule a. passive diffusion b. active transport c. facilitated diffusion d. all of the above e. none of the above 33) Predict which of the following may be a strong electrolyte in water? Sugar, KCl, organic acid pyruvic acid A sugar B organic acid (pyruvic) C KCl D all of them E none of them 34) Predict which of the following may be a nonelectrolyte in water? CaCl2, KCl, organic acid acetic acid A sugar B organic acid acetic acid C KCl D all of them E none of them 35) Which of the following is a strong electrolyte?   A. pure water   B. octane   C. butane   D. sugar solution E.  none of the above 36) Which of the following is a weak electrolyte?   A. citric acid   B. octane   C. butane   D. sugar solution E none of the above 37)   The term concentration indicates a. amount of solute only b. amount of solvent only c. amount of solution only d. none of these is correct 38. If "A" contains 2% NaCl and is separated by a osmotic semipermeable membrane from "B" which contains 10% NaCl, which event will occur? A) NaCl will flow from "A" to "B". B) NaCl will flow from "B" to "A". C) Water will flow from "A" to "B". D) Water will flow from "B" to "A". E) none of the above 39) .If "A" contains 2% NaCl and starch solutions and is separated by a dialysis membrane from "B"which contains 0.5 % NaCl, which event will occur? A) Na ions and Cl ions will flow from "A" to "B". B) Na ions and Cl ions will flow from "B" to "A". C) Water will flow from "A" to "B". D) Water will flow from "B" to "A". E) A and D 40. Hydrophobic molecules are ____ water. a. attracted by b. absorbed by c. repelled by d. mixed with e. polarized by 41.A liquid that can dissolve other substances is called a a. compound. b. mixture. c. solvent. d. solute. e. solution. 42. Which of the following is/are accurate statement? A. Most gases are more soluble at higher temperature B. Many solids are more soluble at higher temperature C Many gasses are more soluble at lower temperature D. Lower the pressure, higher the solubility of gases. E. both b and c 43. Hydrophilic molecules are ____ water. a. attracted by b. absorbed by c. repelled by d. mixed with e. polarized by Part B 1) Calculate the mass percent of a solution prepared by dissolving 34.4 g of NaCl in 298 g of water. A) 10.3 % B) 11.5 % C) 0.103 % D) 0.115 % E). none of the above 2) What is the percent mass/volume (% m/v) of a solution that is made from putting 50.0 g of NaCl in 550 mL of water? Assume the volume of water does not change after dissolving solute. A) 0.0909 %w/v B) 9.09 %w/v C) 8.33 %w/v D) 10.9 %w/v E). none of the above 3) What is the %v/v concentration of a sample of wine that contains 26 mL of ethyl alcohol in 200 mL of wine? A) 0.075 %v/v B) 6.9 %v/v C) 7.5 %v/v D) 13 %v/v E). none of the above 4) What is the glucose concentration in ppm of a solution made by mixing 23.2 mg glucose with 4.000 L? A) 8.5 ppm B) 11.6 ppm C) 1.16 ppm D) 0.862 ppm E). 5.8 ppm 5) Calculate the volume (in L) of a solution that contains 3.12 moles of NaCl if the concentration of this solution is 6.67 M NaCl? A) 2.14 L B) 20.8 L C) 46.8 L D) 0.468 L E). none of the above 6) Calculate the volume (in mL) of a 2.75 M solution that must be used to make 1.25 L of a 0.150 M solution. A) 0.0682 mL B) 68.2 mL C) 0.0330 mL D) 33.0 mL E). none of the above 7) What volume of 8.25 M NaOH solution must be diluted to prepare 2.40 L of 0.500 M NaOH solution? A) 39.6 L B) 0.356 L C) 438 mL D) 145 mL E). none of the above 8). 12.5 g of ethanol (CH3OH) is dissolved into 50.0 g of water. What is the concentration (w/w) % solution? A. 20.0% B. 25.0% C. 75.0% D. 80.0% E. none of the above 9). How many grams of AgNO3 are required to make 200.0 mL of a 0.05 M solution? ( Molecular weight of solver nitrate =170 g/mol) A. 1.7 g B. 17.0 g C. 34.0 g D. 0.100 g E. none of the above 10). 0.7450 g of KCl is dissolved into a solution with a total volume of 125.0 mL. What is the molarity of the solution? ( Molecular weight of KCl = 74.5 g/mol) A. 0.200 M B. 3.75 M C. 0.804 M D. 0.08 M E. none of the above 11). What volume of 2.00 % NaCl must be diluted to make 10.00 mL of 0.90% NaCl, also known as normal saline solution? A. 4.5 mL B. 0.18 mL C. 9.0 mL D. 22.2 mL E). none of the above 12). A water sample taken from the ocean is 0.0036 g salt is present in two liter of this ocean water. What is the concentration in ppm? A. 0.036 B. 0.36 C. 1.8 D. 360 E). none of the above 13). A patient has been trying to achieve total blood cholesterol of 175 mg or less per 100 mL. A recent test result of a 5.0 mL blood sample found that 10.00 mg cholesterol were present. Has the patient reached the goal? A. No, patient has more cholesterol than his goal. B. Yes, ,patient has less cholesterol than 175 mg/100 mL. C. patient has just 175 mg of cholesterol as per his goal. D. Undetermined; we need to draw 100 mL blood to find the answer. 14). An egg yolk with the volume of 2.00 mL contains 2.5 µg vitamin D (cholecalcifoerol). What is the concentration of vitamin D in µg/100 mL? A. 12.5 µg/100 mL B. 125.0 µg/100mL C. 1.25 µg/100 mL D. 0.125 µg/100mL E. None of the above 15). A 4 g sugar cube ( C12H22O11) is dissolved in a 350 ml teacup filled with hot water. What is the molarity of this sugar solution? ( C=12, H=1, O =16) a. 0.033 M b. 0.033 M c. 0.33 M d. none of the above 16). How many grams of a compound is present in 500 mL of a 5.0 % mass /volume solution. A. 5.0 g B. 10 g C. 15 g. D. 20 g. E. none of the above 17). What is the concentration in ppm of a solution that contains 15 mg of a toxic metal in 1250 mL of a solution? A. 1.2 ppm B. 24 ppm. C. 6.0 ppm D. 12 ppm E. none of the above 18). What is the concentration in ppb of a solution that contains 1.5 mg of a toxic metal in 12 L mL of a solution? A. 12,000 ppb B. 125 ppb C. 18000 ppb D. 24000 ppb E. none of the above 19). What is the molarity of a NaOH solution if 2.0 g of NaOH is present in 400 mL of its solution. Molecular weight of NaOH = 40 g/mol A. 0.25 M B. 1.0 M C. 0.125 M D. 1.5 M E. none of the above 20).  How many grams of fructose are present in 500 mL of a 2.50 % solution? A.  25 g B. 12.5 g C. 250 g D. 1.25 g E. none of the above 21) How many liters of 4 M solution can be made using 100 grams of lithium bromide? (molar mass = 86.8 g) 0.29 L 2.9 L 0.029 L None of these 22) How many liters of 0.88 M solution can be made with 25.5 grams of lithium fluoride? (molar mass = 25.94g) 0.79 L 7.9 L 0.0079 l None of these. Chapter 9 Acids, Bases and Buffers in the Body 1) A Bronsted-Lowry acid is defined as a substance which: A) increases [H+] when placed in water B) decreases [H+] when placed in water C) acts as a proton acceptor in any system D) acts as a proton donor in any system 2) A Bronsted-Lowry base is defined as a substance which: A) acts as proton acceptor in any system B) acts as proton donor in any system C) decreases [H+] when placed in water D) increases [H+] when placed in water 3) In the following equation which is the proton donor and which is the proton acceptor? CO3-2 (aq) + H2O (l) ? HCO3- (aq) + OH- (aq) A) Donor: CO3-2; acceptor: H2O B) Donor: H2O; acceptor: CO3-2 C) Donor: HCO3-; acceptor: OH- D) Donor: OH-; acceptor: HCO3- 4) Which of the following cannot act as a Bronsted-Lowry acid? A) SO4-2 B) H2O C) CO3-2 D) HS- E) A and C 5) In the following equation identify the conjugate acid and base respectively: NH3 + HCN ? NH4+ + CN- A) NH3 and HCN B) HCN and NH3 C) NH4+ and CN- D) NH3 and NH4+ 6) Which of the following is not a strong acid? A) HCl (aq) B) HNO3 C) HC2H3O2 D) HClO4 E) all of these are strong acids 7) Which of the following is not a strong base? A) NaOH B) Al(OH)3 C) KOH D) NH4OH E) B and D 8) Given the following reaction, the equilibrium expression will be: 4 CuO (s) + CH4 (g) ? CO2 (g) + 4 Cu (s) + 2 H2O (g) A) [CuO]/[Cu] B) [CuO]4/[Cu]4 C) [Cu]4/[CuO]4 D) [CO2][H2O]2/[CH4] 9) The following reaction is exothermic. Which of the following will drive the reaction to the right (towards products)? CH4 (g) + 2 O2 (g) ? CO2 (g) + 2 H2O (g) + heat A) A decrease in temperature B) An increase in temperature C) The removal of CH4 D) The addition of CO2 10) When a system is at equilibrium: A) the reaction rate of the forward reaction is equal to the rate of the reverse. B) the reaction rate of the reverse reaction is small compared to forward. C) the reaction rate of the forward reaction is small compared to the reverse. D) the amount of product and reactant is exactly equal. 11) Given the following reaction, write the equilibrium expression: C (s) + 2 H2 (g) ? CH4 (g) A) [CH4]/[C] [H2]2 B) [C][H2] C) [CH4]/[H2]2 D) [H2]2[C]/[CH4] 12) Which one of the following is the strongest weak acid? A) HCN (Ka = 4.9 × 10-10) B) HClO (Ka = 3.0 × 10-8) C) HNO2 (Ka = 4.5 × 10-4) D) HF (Ka = 6.8 × 10-4) E) HPO4 2- ( Ka = 1.0 x 10 -12) 13) Which one of the following is the weakest acid? A) HCN (Ka = 4.9 × 10-10) B) HClO (Ka = 3.0 × 10-8) C) HNO2 (Ka = 4.5 × 10-4) D) HF (Ka = 6.8 × 10-4) E) HPO4 2- ( Ka = 1.0 x 10 -12 ) 14) Which of the following acid is the strongest weak acid? A) Formic acid pK = 3.74 B) Carbonic acid pK = 6.35 C) Phosphoric acid pK = 2.12 D) Nitrous acid pK = 3.3 15) What is the conjugate base of OH-? A) H2O B) O- C) O2 D) O-2 16) What is the conjugate acid of HS-? A) S-2 B) H2S C) HS- D) S- 17) What is the conjugate base of NH4+ A) NH4+ B) NH2- C) NH2+ D) NH3 18) Which of the following does not represent a conjugate acid-base pair? A) HCO3-/CO3-2 B) H3PO4/HPO4-2 C) OH-/O-2 D) NH4+/NH3 19) Calculate the pH of 0.000756 M HNO3. A) 11.879 B) 7.091 C) 2.121 D) 3.12 E) none of the above 20) In a basic solution, pH is ________ and [H3O+] is ________. A) = 7, 1 x 10-7 M B) > 7, < 1 x 10-7 M C) < 7, > 1 x 10-7 M D) < 7, < 1 x 10-7 M 21) What is the pH of a solution that has a [H3O+] = 1.2 × 10-3? A) 1.20 B) 2.92 C) 11.08 D) 12.80 22) What is the [H3O+] concentration of a solution that has a pH = 2.34? A) 2.3 × 10-3 M B) 4.6 × 10-3 M C) 2.2 × 10-12 M D) 1.2 × 101 M E) none of these 23) What is the [H3O+] concentration of a solution that has a pH = 11.61? A) 1.2 × 101 M B) 6.17 × 10-12 M C) 2.5 × 10-12 M D) 4.1 × 1011 M E) none of these 24) The isoelectric point of an amino acid is defined as: A) the pH at which the amino acid exits in the zwitterion form B) the pH at which it exists in the basic form C) the pH at which it exists in the acidic form D) the pH equals the pKa 25) Which of the following substances, when added to a solution of nitrous acid (HNO2), could be used to prepare a buffer solution? A) NaCl B) NaNO2 C) HC2H3O2 D) KNO2 E0 both b and d 26) Which of the following buffers is the one that is mainly contained in our blood? A) HC2H3O2/C2H3O2- B) NH4+/NH3 C) H2CO3/HCO3- D) HPO4-2/PO4-3 27) When a person hypo ventilates the condition is known as: A) respiratory acidosis B) respiratory alkalosis C) metabolic acidosis D) metabolic alkalosis 28) When a diabetic does not have enough glucose in their blood it develops a condition called: A) respiratory acidosis B) respiratory alkalosis C) metabolic acidosis D) metabolic alkalosis 29). In the reaction: The conjugate acid of water is _____. A. HNO2 B. H2O C. H3O+ D. NO2- 30). In the reaction: NO2- is the _____. A. conjugate base of H2O B. conjugate base of HNO2 C. conjugate acid of HNO2 D. conjugate base of H3O+ 31). The equation: has the following equilibrium constant expression. A. C. B. D. 32). The equation: has the following equilibrium constant expression. A. C. B. D. 33). In the Haber process for the production of ammonia, Which will shift the equilibrium to right? A. increasing the concentration of N2 B. increasing the concentration of H2 C. addition of a catalyst D. All of the above 34). In the reaction below: Glycogen (aq) [stored glucose] + H2O > blood glucose (aq) + heat If the blood glucose is used up (removed) the equilibrium will A shift to left B shift to right C not shift anywhere D hard to predict 35). In the reaction below: Glycogen (aq) [stored glucose] + H2O > blood glucose (aq) + heat If the glycogen is removed the equilibrium will A shift to left B shift to right C not shift anywhere D hard to predict 36) In the reaction below: Glycogen (aq) [stored glucose] + H2O > blood glucose (aq) + heat If the heat is added to the reaction( body at high fever) the equilibrium will A shift to left B shift to right C not shift anywhere D hard to predict 37). Basic solutions _____. A. have a H+ concentration greater than the OH- concentration and a pH greater than 7.0 B. have a H+ concentration greater than the OH- concentration and a pH less than 7.0 C. have a H+ concentration less than the OH- concentration and a pH greater than 7.0 D. have a H+ concentration less than the OH- concentration and a pH less than 7.0 38). The carbonic acid/bicarbonate buffer is important in maintaining the proper pH of human blood. Diarrhea can lead to the loss of HCO3-. According to LeChatelier's principle, removal of HCO3- will shift the above equilibrium to the ____ and result in a(n) _____ in blood pH. A. left/decrease B. right/decrease C. left/increase D. right/increase 39). Calculate the pH of solution produced by dissolving 0.001 moles of HNO3 in a half liter of water. Assume complete dissociation. A. pH = 3.0 B. pH = 2.7 C. pH = 1 x 10–3 D. pH = 1 x 103 40). What is the molar concentration of hydronium ions in a sample of a soft drink that has a pH of 5? A. 1/4 M B. 5 M C. 1 x 104 M D. 1 x 10-5M E none of these 41). When a person hypo ventilates the condition is known as: A) respiratory acidosis B) respiratory alkalosis C) metabolic acidosis D) metabolic alkalosis 42) What is the pH of a HI solution that has a molarity 1.2 × 10-3? A) 1.20 B) 2.92 C) 11.08 D) 12.80 43) The [H3O+] and the pH of a 0.021 M HCl solution? A) 4.8 x 10-13 M and 12.32 B) 4.8 x 10-13 M and -12.32 C) 0.021 M and -1.68 D) 0.012 M and 1.92 44). What is the pH of 0.021 M KOH solution? A. 12.32 B. 1.68 C. 2.1 D. 10.3 E. none of the above 45) What is the pH of 0..001 M NaOH solution? A 3 B 1 C 0.001 D 10 E 11 46). Which of the following pHs has the highest concentration of hydrogen ions? a. 1 b. 3 c. 5 d. 7 e. 9 47). For which of the following pHs, is the hydroxide ion concentration greater than the hydrogen ion concentration? a. 1 b. 3 c. 5 d. 7 e. 9 48. What category of compounds helps our body fluids to stay within a consistent pH range? a. solvents b. buffers c. solutes d. acids e. bases 49. Which of the following compounds helps to maintain our blood pH between 7.35 and 7.45? a. Water H2O b. carbonic acid H2CO3 c. hydrocloric acid HCl d. hydrogen peroxide H2O2 e. sodium hydroxide NaOH 50. For which of the following pHs, is the hydroxide ion concentration is equal to the hydrogen ion concentration? a. 1 b. 3 c. 5 d. 7 e. 9