Which of the solu... A titration is: A) a way to determine the pH of a solution B) another way to describe a "hydrogen acceptor" C) another way to describe a "hydrogen donor" D) a way to describe a covalent bond, If the concentration of H_2SO_4 is 0.48 M and 19 mL were required to neutralize 27 mL of NaOH, what is the concentration of the NaOH? The dissociation equilibrium constants for the protonated form of alanine (a diprotic amino acid, H2X+) are Ka1 = 4.6 x 10-3 and Ka2 = 2.0 x 10-10. When a 15.3-mL sample of a 0.454 M aqueous hydrofluoric acid solution is titrated with a 0.390 M aqueous sodium hydroxide solution, what is the pH after 26.7 mL of sodium hydroxide has been added? A volume of 80.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H_2SO_4). Sketch the titration curve of 20.0 mL of 0.10 M HNO3 (Ka is "very large"; strong acid) using 0.10 M NaOH. A volume of 40.0 mL of a 0.340 M HNO3 solution is titrated with 0.610 M KOH. 8. How many moles of acid (H+) are required to titrate 0.75 moles of oxalate, C2O42-? Note: density of vinegar... What molarity of a 93.92 mL magnesium hydroxide solution is required to neutralize 18.58 mL of a 1.866 M solution of hydrochloric acid solution, which creates as products, magnesium chloride and wa... You are titrating 100 mL of HCl with 0.5M NaOH and the equivalence point is reached after the addition of 15 mL of NaOH. Determine the volume of 0.210 M KOH solution required to neutralize each of the following samples of sulfuric acid. Which of the following conjugate acid-base pairs will function as a buffer? What is the pH at the equivalence point? The Keq for the equilibrium below is 7.52 â 10-2 at 480.0 °C. What species is being oxidized in the overall reaction? A 0.1375 M solution of potassium hydroxide is used to titrate 35.00 mL of 0.257 M hydrobromic acid. A 20.0-mL sample of a 0.0875 M solution of acetic acid, CH3COOH, is titrated with a 0.115 M solution of KOH. When 1.30 mol of CO2 and 1.30 mol of H2 are placed in a 3.00-L container at 395 âC, the following reaction occurs: In which direction is this process exothermic? HCl(aq) + NaOH(aq) \rightarrow NaCl(aq) + H2O(l) Which of the follo... During a titration a student uses 19.25 mL of 0.0134 M NaOH solution to titrate 15.0 mL of an unknown monoprotic acid solution. 0.025 mol/L. How many milliliters of 8.00 times 10^(-2) M NaOH are required to titrate the following solution to the equivalence point? A buffer is prepared by adding 18.0 g of sodium acetate (CH3COONa) to 520 mL of a 0.140 M acetic acid (CH3COOH) solution. These substances react as follows: The equilibrium constant, K c, for the reaction H2 (g) + I2 (g) â 2HI (g) at 425°C is 54.8. Police officer B. lab technician C. geneticist D. nutritionist, The techniques of titration would be commonly practiced in which career field? Titration of a 23.0 mL solution of KOH requires 13.0 mL of 0.0250 M H2SO4 solution. You used 1.86 mL of 0.067 N NaOH to do a VA titration of a 10 mL sample of wine; what is the VA? A total of 10.0 mL of NaOH requires 11.25 mL of HCl. If the equilibrium concentration of N2O4 is 0.00251 M, calculate the equilibrium concentration of NO2. If you needed 22.5 mL of 0.15 M Na2S2O3 to reach the endpoint, how many moles of I2 were present in the solution? The normal boiling point of benzene is 80.1°C and ÎHvap is 30.7 kJ/mol. Determine the concentration of HCL. \\ a. Explain the terms enthalpy of formation and equivalence point. 100.0 mL of 0.40 M HNO3 is titrated with a 0.20 M KOH solution. Suppose you have 25.00 mL of phosphoric acid, and you do not know what it's concentration is. 25 mL of 0.10 M HCl is titrated with 0.10 M NaOH. A 5.109 g sample requires 36.97 mL of titrant ( N a O H solution) to reach the endpoint. Which compound is the acid? Titration A: A strong monoprotic base is titrated with a strong monoprotic acid. Assume the volumes are additive. Studyres contains millions of educational documents, questions and answers, notes about the course, tutoring questions, cards and course recommendations that will help you learn and learn. To ensure that the mass added is consistent with the standard kilogram. Consider two gas cylinders of the same volume and temperature, one containing 1.0 mol of propane, C3H8, and the other 2.0 mol of methane, CH4. Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory to standardize strong base solutions. Assume we have 25 mL of 2.5 M HCl and a solution of NaOH of unknown concentration. B. The reaction AâB is first order reaction in [A]. 40 mL of 0.10 M sodium hydroxide is added to 60 mL of 0.10 M hydrochloric acid. You titrate this sample at 25 C by gradually adding 0.50 mol/L NaOH solution. Find the training resources you need for all your activities. A 20 mL sample of Ca(OH)_2 was titrated with 0.05125 M HCl. It requires 35 hours for the chlorine gas to effuse from the system. What is the molarity of the KOH solution? 6.2 c. 7.5 d. 8.6 e. 7.1. In a titration of a weak base with a strong acid, which of the following statements is true? a. Consider the following chemical reaction: How many milliliters of 0.0991 M NaOH are required to titrate 25.0 mL of 0.0839 M HBr to the equivalence point? Write... Why is the standardization of NaOH necessary? Answer in moles of barium hydroxide. d. CH3COOH is a stronger acid ⦠Constant-boiling HCl can be used as a primary standard for acid-base titrations. Assume the temperature is 25 degrees Celsius. Calculate the pH for the following cases in the titration of 50.0 mL of 0.200 M HClO (aq) with 0.200 M KOH (aq). When 20.97 mL of aqueous NaOH was added to 1.369 g of cyclohexylamino ehtanesulfonic acid dissolved in 43.46 mL of water, the pH was 9.24. Calculate the pH of the base solution afte... A student was asked to determine the mass, in grams, of calcium carbonate present in a 0.125 g sample of chalk. The unbalanced equation for the reaction is below. If your titration solution is 0.411 M in NaOH and the endpoint occurs at 14.00 mL of titrant, how many mmol of NaOH are required to reach the endpoint? The following reaction occurs and equilibrium is established: At 1285 âC the equilibrium constant for the reaction Br2(g)â2Br(g) is Kc=1.04Ã10â3. If 18.9 mL of 0.800 M HCl solution is needed to neutralize 5.00 mL of a household ammonia solution, what is the molar concentration of the ammonia? 2Cl^- (aq) + Hg (NO_3)_2 (aq) to 2NO_3... 128 mL of 1.50 x 10^{-2} M NaOH is used to titrate 225 mL of a monoprotic acid with unknown concentration to reach the equivalence point. Which statement is correct about this reaction mixture? Suppose a pinhole is in the cork that stoppers the flask in which the equilibrium mixture is found, where PPCl3 = PCl2. A standard solution of 0.25 M H2SO4 is used to determine the concentration of a 220 mL LiOH solution. The concentration of hydronium (in M) in the final solution is closest to: a. If 140 mL of HCl is required, what is the concentration (in molarity) of the Ca(OH)2 solution? Using the table below, place the following equilibria in order of smallest to largest value of Kc: Calculate [H+] for [OHâ]=5.1Ã10â4 M. Calculate [H+] for [OHâ]=8.1Ã10â9 M. Calculate [H+] for a solution in which [OHâ] is 100 times greater than [H+]. Download. If it requires 24.5 mL of 0.102 M NaOH to neutralize a 25.0 mL aliquot of HCl (aq), what is the molarity of the HCl? Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCl. Earn Transferable Credit & Get your Degree. a) Police officer b) Lab technician c) Geneticist d) Nutritionist. The concentration of acetic acid in the sample was ________ M. A 25.0 mL sample of an HCl solution is titrated with a 0.139 M NaOH solution. Q. Upon titration, it was found that 60 mL of 4 M HCl completely neutralized the CaCO3 solution. Consider the following reaction: 2HCI + Ba(OH)_2 (s) to BaCl_2 + 2H_2O When 3.16 g samples of Ba(OH)_2 titrated to the equivalence point with an HCI solution, the following data were recorded f... How many grams of potassium hydrogen phthalate (KHP) will be required to titrate 15 mL of 0.122 M NaOH solution? What are some real-world uses for the titration process? (A) At the midpoint (half way to stoichiometric point) pH equals pK_b. (For HF, pK_a = 3.18 at 25 degre... What volume of 0.1700 M NaOH is required to titrate 22.00 mL of 0.1100 M HCl? HBr(aq) + NaOH(aq) arrow H2O(l) + NaBr(aq). When metallic aluminum is added to a solution containing iron(II) sulfate a reaction occurs. A solution of NaOH is standardized by titration with 0.100 N HCL. If 0.3909 g of the sample requires 49.59 mL of 0.1000 M N a O H to neutralize the H 3 C 6 H 5 O 7 completely, what is t... You have 0.6559 g of an unknown monoprotic acid, HA, which reacts with NaOH according to the balanced equation: HA + NaOH to NaA + H2O. a. The resulting solution has an osmotic pressure of 0.605 atm at 25 âC. b. Using the values given for ÎHâ and ÎSâ, calculate ÎGâ for each of the following reactions at 298 K. For a particular reaction, ÎH = -30 kJ and ÎS = -95 J/K . (b) Half-life period (t1/2) for first order reaction : 0.693 t½ = k Pseudo chemical reaction : The chemical reaction which looks like higher order reaction but in real it follows lower order reaction. Why? To determine the concentration of a solution of sulfuric acid, a 75.00-mL sample is placed in a flask and titrated with a 0.1268 M solution of rubidium hydroxide. Knowing that 32.4 mL of base were required to reach the end point with a sample... Why is Volhard's method called as 'back/residual titration' method? If 0.6986 g of HKP requires 43.92 ml of Na O H . The pK_b of pyridine is 8.77. What volume, in milliliters, of the NaOH solution is required? Determine the concentration of OH^- in the resulting solution. A certain reaction X + Y â Z is described as being first order in [X] and third order overall. For the reaction below at 25 0C ÎG= -354 kJ/mol, determine the value of ÎG at 1727 0C and state if the reaction remains spontaneous. The addition of 143 mL of H2SO4 resulted in complete neutralization. What is the equivalence point volume expected for the complete titration? The concentration of aqueous sodium hypochlorite, NaOCl(aq), in laundry bleach can be determined by titrating a sample of laundry bleach with an iodide solution, as represented by the equation belo... 20.60 mL of 0.0100 M aqueous HCl is required to titrate 30.00 mL of an aqueous solution of NaOH to the equivalence point. Express your answer with the appropriate units. A 13.3 mL solution of 0.100 mol L^{-1} CH_3COOH is titrated using 0.150 mol L^{-1} NaOH. 5 mL b. You titrate 25.00 mL of this solution with a 0.80 mol/L NaOH solution. The second trial involved the titratio... What is the most likely equivalence point pH for lithium hydroxide titrated with hydrobromic acid? Explain how you can use the laboratory technique of titration to determine the concentration of an acetic acid solution. a. A volume of 4.99 mL of the base was required to reach the endpoint. Ka for acrylic acid is 5.5 \times 10^{-5}. In the titration of 50.0 mL of HCl of unknown concentration, the phenolphthalein indicator present in the colorless solution turns pink when 26.5 mL of 0.130 M Ca(OH)2 is added. At constant temperature, the PCl5 reaches equilibrium with its decomposition products as follows to have a Ptotal of 1.40 atm. What is the concentration of a HNO3 solution if 10.0 mL of the solution is neutralized by 3.6 mL of a 0.20 M NaOH solution? What is the molarity of an HCl solution if 22.5 mL of a 0.100 M NaOH solution are needed to titrate a 25.0 mL sample of the acid? A 25.0 mL sample of 0.150 M acetic acid is titrated with a 0.150 M NaOH solution. Give the balanced net ionic equation for the reaction that takes place during titration. If 25.0 mL of 0.100 M HCl is titrated with 0.150 M Ba(OH)2, what volume of barium hydroxide is required to neutralize the acid? The equivalence point is reached when 20.6 mL of the base is added. A diprotic acid is titrated with NaOH and the first equivalence point volume occurs at 14.32 mL. A 19.5 mL solution of 0.100 mol L^{-1} CH_3COOH is titrated using 0.150 mol L^{-1} NaOH. In a titration of 20.23 mL of 0.1615 M H_2SO_4, 43.65 mL of a NaOH solution are needed. Titration the residual HCI took 10 ml of a NaOH solution. The vapor pressure of ethanol (C2H5OH) at 19 âC is 40.0 torr. (The heat of vaporization of water in this temperature range is 2.4 kJ/g. The density of the resulting solution is 1.05 g/mL. Discuss the equivalence point. Calculate the concentration of the base. b. Wh... An analytical chemist is titrating 84.6 mL of a 0.5800 M solution of ethylamine (C2H5NH2) with a 0.7400 M solution of HNO3. A sample of 7.00 mL of household cleaner containing ammonia (NH3) was titrated with a 0.5M solution of HNO3. Select all that apply. Calculate the pH at the stoichiometric point when 25 mL of 0.093 M propionic acid is titrated with 0.33 M NaOH. HSOââ» + HâO â SOâ²⻠+ HâOâº. B. A 0.1501 M solution of hydrochloric acid is used to titrate 30.02 mL of a calcium hydroxide solution to determine its concentration. A sample of a 25.0-mL hydrochloric acid solution required 28.6 mL of a 0.175 M solution of sodium hydroxide for neutralization. It has the unwieldy formula of KHC8H4O4. The Henry's law constant for helium gas in water at 30 âC is 3.7Ã10â4M/atm; the constant for N2 at 30 âC is 6.0Ã10â4M/atm. An impure sample of benzoic acid (C_6H_5COOH, 122.12 g/mol) is titrated with 0.9855 M NaOH. 19.35 mL, of HCl solution were required to reach the equivalence point. What is the concentration (molarity) of the Ca(OH)_2? london dispersion forces and dipole-dipole interactions. Examples: Fe, Au, Co, Br, C, O, N, F. Ionic charges are not yet supported and will be ignored. The reaction represented below is observed to proceed spontaneously to the right in aqueous solution. Express your answer to 2 decimal places. Oxalic acid (H2C2O4) is present in many plants and vegetables. What is the resulting pH? 5.34 c. 7.00 d. 4.43 e. 9.54. In three trials a 25.0 mL sample of the phosphoric acid solution required 27... A 45.0 mL sample of 1.0 M HOCl was titrated to the endpoint using standardized 1.150 M NaOH. In a linear graphical representation of a zero-order reaction, what value is represented by the y-intercept of the line drawn from plotting [A] vs. time? The solution required 18.47 mL of NaOH to reach a phenolphthalein endpoint. Their chemical structure typically includes conjugated double bonds. (B) At the stoichiometric point... A 0.5210-g sample of an unknown monoprotic acid was titrated with 9.98 10-2 M NaOH. What is the pH of this final solution? (Hint: assume that one of the products is H2CO3). Given the data in the table below, what is the concentration of the acetic acid solution? 100.0 mL of 0.100 M acetic acid is placed in a flask and is titrated with 0.100 M sodium hydroxide. Which one of the following conditions is always true for a titration of a weak base with a H_2SO_4? Calculate the pH at the halfway point and at the equivalence point for the following titrations. A particular weak acid (HA) with K_a = 2.0 \times 10^{-5} is 75% titrated with a strong base to produce a buffer solution. (B) equal to 7.00. If it took 30.0 mL of 0.50 M NaOH to neutralize 15.0 mL of HNO3, what is the concentration of the HNO3? Based on their compositions and structures and on conjugate acid-base relationships, select the stronger base in each of the following pairs. Show the calculatio... Vinegar is an aqueous solution of acetic acid CH3 OOH. What is the pH of 100 mL of a buffer that is 0.5 M HCNO and 0.5 M CNOâ when 100 mL of a 0.2 M NaOH solution is added? D. is equal to the pKa of the conjugate acid. Which of the following are true regarding indicators employed in acid/base titrations? In a particular spontaneous process the entropy of the system decreases. The acid-dissociation constant for acetic acid is 1.8Ã10â5. Which of the following reactions lies to the right, favoring the formation of products, and which lies to the left, favoring formation of reactants? Acetic acid K_a = 1.8 times 10^{-5} (a) 4.28 (b) 4.45 (c) 4.74 (d) 5.59. Sodium hydroxide is used extensively in acid-base titrations because it is a strong, inexpensive base. (C) greater than 7.00. Select as many as appropriate. Write the balanced chemical equation for the reaction of hydrochloric acid with sodium bicarbonate, NaHCO_3. A 106.8 mL sample of 0.088 M HCl is mixed with 29.2 mL of 0.095 M NH_3. 7.0 b. volume of NaOH solution in the burette at the start (mL): 50.00 mL volume of NaOH solution in the burette at the... A. At what volume will the second equivalence point occur? How do you remove air bubbles from the burette tip? If a 7.0 mL sample of vinegar was titrated to the stoichiometric equivalence point with 7.5 mL of 1.5 M NaOH, what is the mass percent of CH_{3}COOH in the vinegar sample? The density of HNO3 is 1.42 (g/cm3). During a certain reversible process, the surroundings undergo an entropy change, ÎSsurr = - 79 J/K . Explain. A 25.00 mL sample of a solution required 20.35 mL of 0.1175 M NaOH to reach the visual endpoint. How many grams of water can be cooled from 42 âC to 16 âC by the evaporation of 56 g of water? What is the percent by mass of benzoi... 1. If the titration of a 25.0-mL sample of acetic acid requires 40.90 mL of 0.010 M calcium hydroxide, what is the molarity of the acid? Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.200 M HClO (aq) with 0.200 M KOH (aq). A 2.00-gram sample of acetylsalicylic acid, better known as aspirin, is dissolved in 100 mL of water and titrated with 0.200 mol/L NaOH(aq) to the endpoint. After 25.00 mL of the KOH solution is added, the pH in the titrated flask will be. Match the statement with the type of titration it would apply to. If it requires 35.0 mL of Mg(OH)_2 to neutralize the acid, determine the molarity of the base. Identify the types of intermolecular forces present in HSSH. It aims to help students hone their analytical and problem-solving skills by presenting detailed approaches to solving chemical problems. Calculate the pH after the following volumes of titrant have been added. What is the molar concentration of H_2SO_4? She tritiated a 50.0 mL sample of the calcium hydroxide solution with standardized solution of 0.300M nitric acid. Suppose we were given a sample of acetic acid, CH_3COOH (K_a = 1.8 times 10^{-5}) of unknown concentration. You transferred 20 mL of acetic acid solution to an Erlenmeyer flask and added 2 drops of phenolphthalein solution. A solution is prepared by dissolving 22.44 grams of acetic acid in enough water to make 250.0 mL of solution. Calculate the pH of a solution made by mixing 44.0 mL of 0.044 M HCl and 35.0 mL of 0.055 M RbOH. HC2H3O2(aq) + KOH(aq) \rightarrow H2O(l) + KC2H3O2(aq). Calculate the density of sulfur hexafluoride gas at 707 torr and 22 âC. HCl(aq) + NaOH(aq) arrow NaCl(aq) + H2O(l) Which of the following statem... 5 ml of vinegar was in the beaker and 8 ml of NaOH was added to the vinegar solution to turn it pink. If 18.6 mL of the barium hydroxide solution was needed to neutralize a 3.41 mL aliquot of the perchloric acid solution, what is the concentration of the acid? What is the stoichiometric coefficient for H2O in the balanced redox reaction, and is it a reactant or product? What is the molarity of the ammonia solution? What is the concentration of the H2SO4 solution? It takes 12.45 mL of a 0.500 M NaOH solution to titrate 30.0 mL of acetic acid. dentify the types of intermolecular forces present in NH2NH2. (Answer in mL). How many grams of MgCO_3 are required to neutralize 300 mL of stomach acid HCl, which is equivalent to 0.0500 M HCl? What is the normality of the sul... A 0.235-gram sample of a solid that is 92.5% NaOH and 7.5% Ca(OH)2 by mass requires 45.6 mL of an HCl solution for its titration. Calculate the volume of KOH required to reach the equivalence point. A flask is charged with 0.124 md of A and allowed to react to form B according to the reaction A(g) â B(g). Nitrogen and hydrogen gases react to form ammonia gas via the following reaction: The Goodyear blimp contains 5.74Ã106 L of helium at 25âC and 1.00 atm. (The Kb value for pyridine is 1.7Ã10â9), What is the pH of a 0.40 M solution of benzoic acid, C6H5COOH? 2 HCl(aq) + Ba(OH)2(aq) \rightarrow BaCl2(aq) + 2 H2O(l) Select one... What is the pH of a solution that results from the addition of 200 mL of 1 M HCl (a strong acid) with 100 mL of 1 M NaOH (a strong base)? a. Drag the a Observations Soluble or Insoluble The Structural Formula of the Alcohol A. ethanol 1butanol Soluti In each reaction box place the best reagent and conditions from the list below. The inicial buret reading was 1.16 mL. Assume that ÎH and ÎS do not vary with temperature. Complete Solutions Manual General Chemistry Ninth Edition ... - ID:5dcdb97adce08. Carboxylic acid HCOOH(l), formic acid CH3COOH(l), acetic acid CH3COOH (aq) (COOH)2(s), oxalic acid C6H5COOH(s), benzoic acid â255 â875 â ⦠What is the normality of the NaOH solution? What is the pH of a buffer that is 0.6 M HF and 0.2 M NaF? a. Which equation is an expression of the second law of thermodynamics for a spontaneous process? Access the answers to hundreds of Acid–base titration questions that are explained in a way that's easy for you to understand. Use uppercase for the first character in the element and lowercase for the second character. What is the pH at the equivalence point? What is the concentration of the NaOH? Suppose 10.00 mL of NaOH is added to the HF solution. 27.8 mL of 0.156 M solution of HCl was used for the titration of 20 mL of a strong base. A student titrated a 1.0115 g sample of potassium hydrogen phthalate (HKC_8H_4O_4; 204.2285 g/mol, and commonly known as KHP) with sodium hydroxide. How many moles of H^+ were present in the aliquot? What is the net ionic reaction? Uploaded by. The reaction of H2SO4 with NaOH is represented by the equation H2SO4(aq) + 2NaOH(aq) arrow Na2SO4(aq) + 2H2O(l). To balance a chemical equation, enter an equation of a chemical reaction and press the Balance button. A 0.5678 g sample of impure C a ( O H ) 2 is dissolved in 50.00 mL of water. Consider the equilibrium that is established in a saturated solution of silver chloride, Ag+(aq) + Clâ(aq) â AgCl(s). Calculate the: A) initial pH B) pH after adding 10 ml of HCl C) pH at the equivalence point. A volume of 60.0 mL of a 0.390 M HNO_3 solution is titrated with 0.860 M KOH. Given that Kc of the reaction below is 2.2 à 10-3 at a certain temperature, which of the following statements is correct? Get help with your Acid–base titration homework. Which correctly lists the following in order of increasing entropy? a) How many millimoles of HNO3 are present at the start of the titration? What was the concentration of the HCl? If the sodium hydroxide is standardized and found to be 0.1011 M, and 25.65 mL of NaOH is used to titrate a 150.0 mL sample of salad dressing, how many moles of acetic acid were in the salad dressi... A 25.1-mL sample of 0.293 M triethylamine, (C2H5)3N, is titrated with 0.372 M hydroiodic acid. If 3.09 grams of KHP are needed to exactly neutralize 33.8 mL of a barium hydroxide solution, what is the concentration of the base solution? The first-order rate constant for decomposition of a typical insecticide in the environment is 3.43 x 10-2 days-1. A solution is prepared by dissolving 27.7 g of CaCl2 in 375 g of water. The concentration of CaCl2 is ________% by mass. Which solution will have the highest pH? A minimum of 5.0 grams of potassium hydroxide is required. 3. KOH + HCl to KCl + H_2O. If the inside surface of each tube were coated with wax, would the general shape of the water meniscus change? Suggest a suitable indicator for each of the following titrations. What is the molarity of the KOH solution? Can't find the question you're looking for? Which of the following correct pairs an acid with its conjugate base? Suppose that you are going to do a titration experiment to determine the solubility of calcium hydroxide using a hydrochloric acid solution. What is the pH range of most buffer systems? Calculate the molarity of a HCl solution if 34.21 mL of 0.0431 M NaOH neutralizes 25.00 mL of the acid solution.
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