Therefore, since the freezing point decreases by 24.0C, the freezing point of the solution is -24.0C. H I think that is what you call it. PDF TABLE OF CONJUGATE ACID-BASE PAIRS Acid Base Ka (25 C) - umb.edu 1 Answer. Assuming equal concentrations, rank these aqueous solutions by their freezing point: LiSO4, Li3PO4, SnCl4, NH4Br. pH of KNO3 in water? - The Student Room PDF Chapter 17 A scientist wants to make a solution of tribasic sodium phosphate,Na3PO4 , for a laboratory experiment. Done on a Dell Dimension laptop computer with a Wacom digital tablet (Bamboo). Table 2. nKa Values / Acid-Salts Sodium Hypochlorite Calculate the pH of 0.10 M NaClO solution. christopher clarke missing; what is walter mittys fourth daydream; June 8, 2022 kb of na3po4 PO43- + H2O HPO42- + OH- ; Kb (PO4-3) = 2.4 10-2. Therefore the percentage composition of each element is: 69 164 100 = 42.1%N a. Conjugate acids (cations) of strong bases are ineffective bases. Na Write the balanced, complete, and net ionic equations for each precipitation reaction. Kb and Ka are also related through the ion constant for water, Kw, by the relationship Kw = Kb x Kb=a. Diprotic Acids. Still have questions? Chemistry(Please help, thank you!!!) Department of Health and Human Services. In this video we will describe the equation Na3PO4 + H2O and write what happens when Na3PO4 is dissolved in water.When Na3PO4 is dissolved in H2O (water) it will dissociate (dissolve) into Na + and PO4 3- ions. For reference or additional information, please contact [email protected] More. The pH of a solution is a measure of the molar concentration of hydrogen `(H^+)` , or hydronium `(H_3O^+)` ions of the solution. Calculate the pH of 0.5 M Na3PO4 in aqueous solution 'months' : 'month' }}, {{ nextFTS.remaining.days }} What is the pH of a 0.01 M Na3PO4 solution? Contact. H2ONH4Cl(2)A.NH3KbB.NH3KbC.pHD.pH . As we can see in the second step, HPO is the conjugate base of HPO. Therefore, the numerical value ofKais a reflection of the strength of the acid. The pKa values for organic acids can be found in Appendix II of Bruice 5th Ed. Weak acid: one that dissociates incompletely, donating only some of its hydrogen ions into solution, Weak base: a proton acceptor that does not ionize fully in an aqueous solution. Note that the normal boiling point of water increases as the concentration of sucrose increases. However, for simplicity, only non-volatile solutes will be considered here. Calculate the pH of a 0.20 M Na3PO4 solution. - Study.com 1 x 10-14 = K a*Kb Ka = 1x10-14/1.8x10-5 = 5.6 x 10-10 (or look up in table) So, You'll get a detailed solution from a subject matter expert that helps you learn core concepts. The 3 Month (100 Day) MCAT Study Schedule Guide: 2022 Edition, All resources are student and donor supported. us from charging the card. Molecular weight calculation: 22.98977*3 + 30.973761 + 15.9994*4. = 141.98 g/mol) that has been dissolved in a 250 mL volumetric flask and diluted to the mark. Nov 23, 2010. you must have since you knew your 5 was wrong, right? What is the percent CsCl by mass in a 0.711 M CsCl solution that has a density of 1.091 You must log in or register to reply here. Weak Base Calculations Sodium Phosphate Conjugate Calculate the pH of 0.10 M Na3PO4 solution. So we start with 0.090 mol of both NH4 + and NH 3.After complete reaction with 0.0010 mol NaOH the resulting amounts of each are: 0.090 0.0010 = 0.089 mol NH4 0.090 + 0.0010 = 0.091 mol NH3 To use Henderson-Hasselbalch equation we need to know the pKa value. Study with Quizlet and memorize flashcards containing terms like What is the pH of a 6.00 M H3PO4 solution? speed set mortar working time of thinset; best choice products jeep parts; zulu social aid and pleasure club posters How many moles of sodium ions are present in 2.50 L of 0.300 M Na3PO4? 1. D) All of the above. 31P and 23Na Solid-State NMR Studies of Cation Dynamics in HT-Sodium 'days' : 'day' }}, {{ nextFTS.remaining.months }} As with acids, bases can either be strong or weak, depending on their extent of ionization. How many grams of Na3PO4 will be needed to produce 575mL of a solution that has a concentration of Na^+ ions of 1.40 M? Not sure about the ice thing, but SQ means square root. National Institutes of Health. Convert grams Na3PO4 to moles or moles Na3PO4 to grams. Trisodium phosphate | Na3PO4 - PubChem By the end of the 20th century, many products that formerly contained TSP were manufactured with TSP substitutes, which consist mainly of sodium carbonate along with various admixtures of nonionic surfactants and a limited percentage of sodium phosphates. Register; Test; JEE; NEET; . K_b for the reaction of HCO_2^- ion with water is 5.6 times 10^{-11}. Therefore the solution will be neutral. Thus, Na 3PO 4 has the highest boiling point. Here are some of the values of weak and strong acids and bases dissociation constants used by BATE when calculating pH of the solution and concetrations of all ions present. {\displaystyle {\ce {Na3PO4.1/4NaOCl.11H2O}}} Answer to: Which of the following compounds can be combined with Na3PO4 to make a buffer solution? 2003-2023 Chegg Inc. All rights reserved. Equilibrium Constants Ka and Kb: pKa, pKb - Jack Westin The anion is phosphate, PO4^-3 and (it has a charge of -3). Calculate the pH of a solution of 0.100 M Na3PO4. The Kb for NH3 is 1 10-5. Use table search to locate desired compound in database. If 0.50 mole of BaCl2 is mixed with 0.20 mole of Na3PO4 , the maximum number of moles of Ba3 (PO4)2 that can be formed is . {{ nextFTS.remaining.months }} Acid-Base Pairs, Strength of Acids and Bases, and pH - Purdue University Na 3 PO 4. Acid with values less than one are considered weak. Because these reactions occur in aqueous solutions, water is not included in the equation even though it is part of the reaction. By clicking Buy Now! The Ksp's for CuCl, AgCl . {{ nextFTS.remaining.days }} Values of dissociation constants pKa and pKb for acids and bases It may not display this or other websites correctly. What Are The Ka And Kb Values For .1M Na2HPO4, NaH2PO4, And Na3PO4? asked Sep 28, 2022 in Chemistry by lolitkumarsingh ( 58.3k points) some basic concepts of chemistry How many grams of Na3PO4 will be needed to produce 450 mL of a solution that has a concentration of Na+ ions of 0.700 M; A scientist wants to make a solution of tribasic sodium phosphate,Na3PO4 , for a laboratory experiment. The high-temperature phases of sodium orthophosphate, HT-Na3PO4, and of the solid solutions (Na2SO4)x(Na3PO4)1-x are characterized by their plastic crystalline state with dynamically disordered PO43- and SO42- anions and a remarkably high cation conductivity. So we start with 0.090 mol of both NH4 + and NH 3.After complete reaction with 0.0010 mol NaOH the resulting amounts of each are: 0.090 - 0.0010 = 0.089 mol NH4 0.090 + 0.0010 = 0.091 mol NH3 To use Henderson-Hasselbalch equation we need to know the pKa value. For the definitions of Kbn constants scroll down the page. To show that they are dissolved in water we can write (aq) after each. An equilibrium expression can be written for the reactions of weak bases with water. Other names - Trisodium phosphate, Sodium orthophosphate, Tribasic sodium phosphate. Monosodium phosphate | NaH2PO4 - PubChem For the definitions of Kan constants scroll down the page. {{ nextFTS.remaining.days === 0 ? Sodium Phosphate (Na3PO4) - Molecular Mass, Structure, Properties and Uses Calculate the pH of the solution after the addition of 0 moles of solid LiOH. Name the metal (the cation) as it appears on the Periodic Table. TSP is used as a cleaning agent, builder, lubricant, food additive, stain remover, and degreaser. A large Kb value indicates the high level of dissociation of a strong base. I need to find the pH of a solution containing 50 grams of Na3PO4. Explanation: The molar mass of sodium phosphate is M r = (3 23) + 31+ (4 16) = 164g/mol. Molecular Weight/ Molar Mass. Equation or enables us to calculate the base constant of a conjugate base from the acid constant of the acid, and vice versa. The acid ionization represents the fraction of the original acid that has been ionized in solution. kb of na3po4 Assume no volume change upon the addition of base. Students (upto class 10+2) preparing for All Government Exams, CBSE Board Exam, ICSE Board Exam, State Board Exam, JEE (Mains+Advance) and NEET can ask questions from any subject and get quick answers by subject teachers/ experts/mentors/students. Kb is the molal boiling point elevation constant, and (K. = 7.5 x 10-3, Ka, = 6.2 x 10-8, K, = 4 x 10-13) What is the poth, 0.5 m Na solution Paperport your answer a: Molecular weight of Na3PO4 - Convert Units Calculate the pH of a 0.0798 M H3PO4 solution. Answer: E. A 1 L buffer solution is 0 M in HF and 0 M in LiF. B) Strong acid vs. weak base. Remember. 31 164 100 = 18.9%P. In this video we will describe the equation Na3PO4 + H2O and write what happens when Na3PO4 is dissolved in water.When Na3PO4 is dissolved in H2O (water) it . Aweak acidis an acid that ionizes only slightly in an aqueous solution. Now let's try some numbers. Relevance. Answered: What is the percent ionization of | bartleby What is the pH of 1.0 M Na3PO4 in aqueous solution ? The solvent used here is water. Calculating pH of a Na2HPO4 solution - Student Doctor Network For example: CH3COOH pKa=4.76 c=0.1 HCl pKa=-10 c=0.1 Case 2. Thanks a ton guys.. Equation for Na3PO4 + H2O (Sodium phosphate - YouTube What is the osmotic pressure of a solution prepared by adding 13.65 g of sucrose (C 12 H 22 O 11) to enough water to make 250 mL of solution . Molarity = moles of solute/Liters of solution 0.300 M Na3PO4 = moles Na3PO4/2.50 Liters = 0.75 moles Na3PO4 pH = Conjugate Acid Base Hydrolysis Reaction - ka Kb 7.52 E pka pkb Calculations: Experts are tested by Chegg as specialists in their subject area. did you know that the right answer was 10 all along? The larger the value of pKa, the smaller the extent of dissociation. . Since HT-Na3PO4 possesses a fully occupied cation sublattice (no vacancies), it has been proposed that cation transport and anion . Anacid ionizationconstant (Ka)is the equilibrium constant for the ionization of an acid. National Center for Biotechnology Information. Diprotic and Triprotic Acids and Bases - Purdue University {{ nextFTS.remaining.months }} How to calculate pH of solution made of H3PO4 and Na3PO4? 4 What is the pOH of a .22 M NaOH solution? The acid equilibrium problems discussed so far have focused on a family of compounds known as monoprotic acids.Each of these acids has a single H + ion, or proton, it can donate when it acts as a Brnsted acid. The figures below illustrate how the vapor pressure of water is affected by the addition of the non-volatile solute, NaCl. {{ nextFTS.remaining.days > 1 ? there are fewer water molecules in the vapor (i.e., lower vapor pressure) above the NaCl solution than in the vapor above pure water, and. PDF Table of Acids with Ka and pKa Values* CLAS - UC Santa Barbara Unless otherwise stated, pKa and pKb was measured at STP. Abase ionization constant (Kb)is the equilibrium constant for the ionization of a base. (Ka=6.2x10^-10) is quite lower than the the Kb of NH4OH (Kb=1.8x10^-5). Is it because it wont dissociate to form either a base or an acid? Potassium Nitrite Calculate the pH of 0.10 M KNO2 solution. It usually results in a bowel movement after 30 minutes to 6 hours. Polyprotic acids are those with more than one acidic proton. 'months' : 'month' }} Previous question Next question. {{ nextFTS.remaining.months > 1 ? As someone who has to write intricate Excel worksheets for preparing buffers at our company, this program [Buffer Maker] seems amazing. C) 9. FOIA. CHEM 1412. Review for Test 1 (chapter 13, 14, 15). Ky75 Kb and pKb What is the pH of a 0.05 M solution of formic acid? (Ka = 1.8 10^-4) CHEM 1172 EXAM 3 [CH 15 16 + 17] Flashcards | Quizlet In the Western world, phosphate usage has declined owing to ecological problems with the damage to lakes and rivers through eutrophication. 1.62 g/cm. What is the freezing point of a solution that contains 0.5 moles of Nal 'months' : 'month' }}, {{ nextFTS.remaining.days }} remaining double check my worki just did this on a napkin and wolfram haha you're lucky i'm bored out of my mind at workhaven't typed up a solution like that in a long time Find the molarity first. (from highest freezing point to lowest freezing poinT) Thanks. Screen capture done with Camtasia Studio 4.0. Note that ammonia and most organic bases release OH- ions due to hydrolysis, not dissociation. For which type of titration will the pH be basic at the equivalence point? The site owner may have set restrictions that prevent you from accessing the site. Phosphoric acid is a triprotic acid, ionizing in the following sequential steps: Kal 7.11 x 10-3 Ko= 6.34 x 10-8 Kg = 4.22 x 10-13 What is the value of Kb for the base sodium phosphate (Na3PO4)? The boiling point of the solvent above a solution changes as the concentration of the solute in the solution changes (but it does not depend on the identity of either the solvent or the solute(s) particles (kind, size or charge) in the solution). On the contrary inorganic bases - like NaOH, KOH, LiOH, Ca(OH)2 - increase pH dissociating. Equilibrium: The state of a reaction in which the rates of the forward and reverse reactions are equal. National Library of Medicine. CCRIS 7086. Calculate the pH of a 0.20 M Na3PO4 solution. Conjugate Acid-Base Pairs. Solution is formed by mixing known volumes of solutions with known concentrations. Rock - if you dont mind me asking what was your DAT score? Experimentally, we know that the change in boiling point of the solvent above a solution from that of the pure solvent is directly proportional to the molal concentration of the solute: T is the change in boiling point of the solvent, SQ is square rootthat's basically a shortcut formula to what you would get if you did the ICE box. im sorry to be a bit slow on this, but why couldnt you use k1 for this problem? Higher T will have a higher boiling point. pKa (HNO3)=-1.4 so Ka (HNO3)=25.119. Architektw 1405-270 MarkiPoland. Again the answer is Kw/Ka (HNO3), and since Ka (HNO3) is taken as around infinity if HNO3 is a strong acid, then this Kb is (around) 0. When this acid donates an H + ion to water . So you can only have three significant figures for any given phosphate species. Ka and pKa Is Na3PO4 acidic, basic, or neutral? - ECHEMI Recently Asked Questions (1.0000x10^1) mL aliquots of a phosphoric acid solution with an unknown concentration is titrated with some (2.99x10^-1) mol/L sodium hydroxide solution.The; A solution turnsmethyl redred andbromocresol greengreen.What is a possible pH of the solution? Arrange the following aqueous solutions in order of decreasing freezing Weak acids with relatively higherKavalues are stronger than acids with relatively lowerKavalues. Acid pH = Base Hydrolysis Reaction Ka Kb 2.4E-02 pka E pKb Calculations: Potassium Nitrite Calculate the pH of 0.10 M KNO2 solution. Molar mass of Na3PO4 = 163.940671 g/mol. Expert Answer. HHS Vulnerability Disclosure. Depending on the source pKa for HCl is given as -3, -4 or even -7. For the reactions of dissociation of base: Next dissociation steps are trated the same way. I dont know why I was thinking it was going to loose that other hydrogen to become PO43- Got it now! Here are some of the values of weak and strong acids and bases dissociation constants used by BATE when calculating pH of the solution and concetrations of all ions present. Thus the product of the acid constant for a weak acid and the base constant for the conjugate base must be Kw, and the sum of p Ka and p Kb for a conjugate acid-base pair is 14. Aweak baseis a base that ionizes only slightly in an aqueous solution. The molarity of the solution is x 10^-2. * Compiled from Appendix 5 Chem 1A, B, C Lab Manual and Zumdahl 6th Ed. Density. The three equilibria values for H 3 PO 4, H 2 PO 4-, and HPO 42- are: Ka1 = 7.11 x 10 ^ -3. Due to high demand and limited spots there is a waiting list. Dissociation: the process by which compounds split into smaller constituent molecules, usually reversibly. Calculating the pH of a mixture of Na2HPO4 and Na3PO4? Calculate the pH of the salt solution of Ca (OOCCH_3)_2, 0.1 M. Calculate the pH of the salt solution of AlCl, 0.1 M, K=10^+. You are using an out of date browser. The acid dissociation constant (Ka) is a quantitative measure of the strength of an acid in solution while the base dissociation constant (Kb) is a measure of basicitythe base's general strength. Ka the acid dissociation constant and Kb the base dissociation constant are measures of the extend of dissociation of a weak acid or base in equilibrium. This shows sodium phosphate to be about 42.07% sodium by mass. We are not permitting internet traffic to Byjus website from countries within European Union at this time. Cracking The Ap Chemistry Exam [PDF] [2b77bebs6vog] Calculate the pH of a 0.300 M Na3PO4 solution. 'months' : 'month' }} Ka and pKa. What is the osmotic pressure of a solution prepared by adding 13.65 g of sucrose (C 12 H 22 O 11) to enough water to make 250 mL of solution at 25 C? Rated by 1 million+ students Get app now Login. {{ nextFTS.remaining.months > 1 ? How to Write the Name for Na3PO4 - YouTube A weak acid has a pKa value in the approximate range of -2 to 12 in water. For the reactions of dissociation of acid: stepwise dissociation constants are defined as. Homework 2 with Answer - Broward College, South Campus Homework 2 CHM The logarithmic constant (pKa) is equal to -log10(Ka). Acids with a pKa value of less than about -2 are said to be strong acids. Phosphoric acid, h3po4, is a triprotic acid, for which ka1 = 7.2 10 {{ notification.creator.name }} It's possible your card provider is preventing [citation needed], Although it is still the active ingredient in some toilet bowl-cleaning tablets, TSP is generally not recommended for cleaning bathrooms because it can stain metal fixtures and can damage grout. What is the dissociation of Na3PO4? - Answers Done on a Dell Dimension laptop computer with a Wacom digital tablet (Bamboo). {{ nextFTS.remaining.months > 1 ? 1 x 10-14 = K a*Kb Ka = 1x10-14/1.8x10-5 = 5.6 x 10-10 (or look up in table) So, [10], With the formula The item of commerce is often partially hydrated and may range from anhydrous Na3PO4 to the dodecahydrate Na3PO412H2O. Base ionization constant (Kb): The equilibrium constantfor theionizationof abase. So, no basic action either. Therefore, the numerical value of. Calculate the pH of the solution containing 3.875g of Na 2 HPO 4 (MW. Because Na3PO4 . Table of Acid and Base Strength - University of Washington We can calculate its basic dissociation constant (Kb) using the following expression. Dissociation can be also described by overall constants, as well as base dissociation constants or protonation constants. I dont know why I can't the right answer but any help would be great! The cation is Na^+ (it has a charge of +1) and there are three of them. D) 4. Given the acid constant for a weak acid . Ka of HF = 3.5 104 and Ka of HClO = 2.9 108, What is the pH of a solution that has 0.200 M HF and 0.200 M HCN? Welcome to Sarthaks eConnect: A unique platform where students can interact with teachers/experts/students to get solutions to their queries. Astrong acidis an acid which is completely ionized in an aqueous solution. Solved What are the Ka and Kb values for .1M Na2HPO4, - Chegg CHEBI:37583. So, to three significant figures, for any sort of mixture of N a X 2 H P O X 4 and N a X 3 P O X 4 salts you'll need to consider both p K a 2 and p K a 3 and you'll end up with a quadratic equation to solve. 3.5 b. [12] The United States Food and Drug Administration lists sodium phosphates as generally recognized as safe.[13][14]. Boiling Point. 163.94 g/mol. If 0.50 mole of BaCl2 is mixed with 0.20 mole of Na3PO4 , the maximum number of moles of Ba3 (PO4)2 that can be formed is . 2. Acid pH = Base Hydrolysis Reaction Ka Kb 2.4E-02 pka E pKb Calculations: Answer Save. NaCl is added slowly to a solution that is 0.010 M each in Cu+, Ag+, and Au+. In this video we'll write the correct name for Na3PO4.To write the name for Na3PO4 well use the Periodic Table and follow some simple rules. Table 2. nKa Values / Acid-Salts Sodium. pH = Conjugate Acid Base Hydrolysis Reaction Kb c pka E pKb 10.66 Calculations: 58 Describe two different ways to prepare 500.0 mL of a pH 7.40 buffer where the base concentration if 0.100 M. So elevation in boiling point will be above a boiling point of water for all solutions. . A) Strong acid vs. strong base. Na3PO4 is the reaction product of the complete neutralisation of H3PO4 ( a weak acid) with NaOH(a strong base) The salt Na3PO4 will be basic salt. Na3PO4 molecular weight. This is a recorded trial for students who missed the last live session. Calculate the pH of a solution formed by mixing 250 mL of 0 M NH4Cl with 100. mL of 0 M NH3. What is the pH of 1.0 M Na3PO4 in aqueous solution - Sarthaks 100% (1 rating) ka Kb=10-14/Ka Phosphori . a.h2co3b.h2oc.h2po4-d.po43-_ Products sold as TSP substitutes, containing soda ash and zeolites, are promoted as direct substitutes. Solution: Osmosis and osmotic pressure are related. Boiling Point Elevation - Purdue University Potassium Nitrite Calculate the pH of 0.10 M KNO2 solution. If 0.50 mole of BaCl2 is mixed with 0.20 mole of Na3PO4 , the maximum number of moles of Ba3 (PO4)2 that can be formed is . Each unit of Na3PO4 that dissociates produces three Na+ ions, which means that there are one-third as many units of Na3PO4 as there are of Na+. 'days' : 'day' }}. These values are usually not measured but calculated from thermodynamical data and should not be treated too seriously. Unless otherwise stated, pKa and pKb was measured at STP. For that to be the case, the energy released during when the ion-dipole attractions form has . Calculate the pH of an aqueous solution with OH- = 1.57 x 10-9 M. Calculate the pH of an aqueous solution with OH- = 2.63 x 10-4 M. State whether the following aqueous solutions are expected to be acidic, basic or neutral You will be notified when your spot in the Trial Session is available. Phosphates are available from a number of other sources that are much milder than TSP. kb of na3po4 - ASE Click hereto get an answer to your question What is the pOH of a 0.5 M Na3PO4 solution ? 14.7: Conjugate Acid-Base Pairs and pH - Chemistry LibreTexts The Kb value for ammonia is 1.8 x 10 a. O What's something you just don't understand? The boiling point of the solvent above a solution will be greater than the boiling point of the pure solvent whether the solution contains a non-volatile solute or a volatile solute. Operating systems: XP, Vista, 7, 8, 10, 11. Solution for What is the percent ionization of HNNH in a solution with a concentration of a 0.580 M? the boiling point of the NaCl solution will be greater than the boiling point of pure water. Acid pH = Base Hydrolysis Reaction Ka Kb 2.4E-02 pka E pKb Calculations: If 0.5 mole of BaCl2 is mixed with 0.2 mole of Na3PO4 the maximum number of mole of Ba3(PO4)2 that can be formed is, Identify coagulant with highest power for coagulating positive colloids: FeCl3; Na3SO4; C6H12O6; Na3PO4, 100 mL of Na3PO4 solution contains 3.45 g of sodium. The acid dissociation constant (Ka) is a quantitative measure of the strength of an acid in solution while the base dissociation constant (Kb) is a measure of basicitythe bases general strength. pH = Conjugate Acid Base Hydrolysis Reaction Kb c pka E pKb 10.66 Calculations: 58 Table 2. nKa Values / Acid . 1(2h)-Pyrimidinecarboxamide, N-Butyl-5-Fluoro-3, 1h-Imidazole, 4,5-Dihydro-2-(phenylmethyl)-, 1h-Purine-2,6-Dione, 3,9-Dihydro-1,3-Dimethyl-, 2,2-Bis(4-Hydroxy-3,5-Dibromophenyl)propane, 2,3-Butanediol, 1,4-Dimercapto-, (r-(r*,r*))- (9, 2,4-Pyrimidinediamine, 5-(3,4-Dichlorophenyl)-6-, 2,8,9-Triisobutyl-2,5,8,9-tetraaza-1-phosphabicyclo[3.3.3]undecane, 2,8,9-Trimethyl-2,5,8,9-tetraaza-1-phosphabicyclo[3.3.3]undecane, 2-((4-(dimethylamino)phenyl)azo)benzoic Acid, 2-(2,4-Dimethoxyphenyl)-5-Methylbenzimidazole, 2-(2,4-Dimethylphenyl)-5-Nitrobenzimidazole, 2-(4-Aminophenylmethyl)-5-Chlorobenzimidazole, 2-(4-Bromophenylmethyl)-5-Chlorobenzimidazole, 2-(4-Chlorophenyl)-Imidazo[4,5-B]pyridine, 2-(4-Chlorphenylmethyl)-5-Chlorobenzimidazole, 2-(4-Fluorophenyl)-Imidazo[4,5-B]pyridine, 2-(4-Methoxyphenylmethyl)-5-Nitrobenzimidazole, 2-(4-Methylphenyl)-Imidazo[4,5-B]pyridine, 2-(4-Methylphenylmethyl)-5-Chlorobenzimidazole, 2-(4-t-Butylphenyl)-Imidazo[4,5-B]pyridine, 2-Furansulfonamide, 4-(4-Methoxybenzoyl)-, 2-Furansulfonamide, 4-[(4-Hydroxyphenyl)sulfonyl, 2-Furansulfonamide, 4-[(4-Methoxyphenyl)sulfonyl, 2-Furansulfonamide, 4-[(4-Methylphenyl)sulfonyl], 2-Methyl-3-Chloromethylhydrochlorothiazide, 2-Piperidinecarboxamide, N-(2,6-Dimethylphenyl)-, 2-Propenoic Acid, 3-(2-Methoxyphenyl)-, (e)-, 2-Propenoic Acid, 3-(2-Methoxyphenyl)-, (z)-, 2-Propenoic Acid, 3-(3,4-Dihydroxyphenyl)-, (e)-, 2-Propenoic Acid, 3-(3-Methoxyphenyl)-, (e)-, 2-Propenoic Acid, 3-(4-Hydroxyphenyl)-, (e)-, 2-Pyrimidinecarboxylic Acid, Methyl Ester, 2-Thiophenesulfonamide, 4-(4-Hydroxybenzoyl)-, 2-Thiophenesulfonamide, 4-(4-Methoxybenzoyl)-, 2-Thiophenesulfonamide, 4-(4-Methylbenzoyl)-, 2-Thiophenesulfonamide, 4-[(3-Hydroxyphenyl)sulf, 2-Thiophenesulfonamide, 4-[(4-Hydroxyphenyl)sulf, 2-Thiophenesulfonamide, 4-[(4-Methoxyphenyl)sulf, 2-Thiophenesulfonamide, 4-[(4-Methylphenyl)sulfo, 2-Thiophenesulfonamide, 5-[(3-Hydroxypropyl)sulf, 2-Thiophenesulfonamide, 5-[(3-Hydroxypropyl)thio, 2-Thiophenesulfonamide, 5-[(4-Hydroxybutyl)sulfo, 2-Thiophenesulfonamide, 5-[(4-Hydroxybutyl)thio], 2-Thiophenesulfonamide, 5-[[3-(methoxyacetyl)oxy, 2-tert-Butyl-1,1,3,3-tetramethylguanidine, 2-tert-Butylimino-2-diethylamino-1,3-dimethylperhydro-1,3,2-diazaphosphorine, 3-((4-(dimethylamino)phenyl)azo)benzoic Acid, 3-Methyl-4h-Pyrido[2,3-E]-1,2,4-Thiadiazine 1,1-, 3-Methyl-4h-Pyrido[3,2-E]-1,2,4-Thiadiazine 1,1-, 3-Methyl-4h-Pyrido[4,3-E]-1,2,4-Thiadiazine 1,1-, 4-((4-(dimethylamino)phenyl)azo)benzoic Acid, 4-Chloro-2-Methylbenzenamine Hydrochloride, 4-Nitro-((4-(n-Dimethyl)aminophenyl)azo)benzene, 4h-Pyran-4-One, 5-Hydroxy-2-(hydroxymethyl)-, 5-(2-Chlorophenyl)oxymethyl-2-Amino-2-Oxazoline, 5-(2-Ethoxyphenyl)oxymethyl-2-Amino-2-Oxazoline, 5-(2-Methoxyphenyl)oxymethyl-2-Amino-2-Oxazoline, 5-(2-Methylphenyl)oxymethyl-2-Amino-2-Oxazoline, 5-(3-Dimethylaminophenyl)oxymethyl-2-Amino-2-Oxa, 5-(3-Nitrophenyl)oxymethyl-2-Amino-2-Oxazoline, 5-(4-Chlorophenyl)oxymethyl-2-Amino-2-Oxazoline, 5-(4-Methoxyphenyl)oxymethyl-2-Amino-2-Oxazoline, 5-(4-Methylphenyl)oxymethyl-2-Amino-2-Oxazoline, 5-(4-Nitrophenyl)oxymethyl-2-Amino-2-Oxazoline, 5-(4-n-Morpholinophenyl)oxymethyl-2-Amino-2-Oxaz, 6-Nh2-5-(n-Methylformylamino)-1,3-Dimethyluracil, 6-Nh2-5-(n-Methylformylamino)-3-Methyluracil, Acetic Acid, 2-[[5-(aminosulfonyl)-2-Thienyl]sul, Acetic Acid, 3-[4-(aminosulfonyl)phenyl]propyl E, Acetic Acid, 3-[[5-(aminosulfonyl)-2-Thienyl]sul, Acetic Acid, 5-[4-(aminosulfonyl)phenyl]pentyl E, Benzamide, 5-Bromo-2-Hydroxy-N,3-Dimethyl-, Benzeneacetic Acid, .alpha.-Hydroxy-.alpha.-Meth, Benzeneacetic Acid, 4-(1,1-Dimethylethyl)-, Benzenemethanol, .alpha.-(1-Aminoethyl)-, (r*,r*, Benzenemethanol, _-[1-(dimethylamino)ethyl]-, (r, Benzenesulfonamide, 3-Amino-4-[(2-Hydroxyethyl)s, Benzenesulfonamide, 3-Amino-4-[(3-Hydroxypropyl), Benzenesulfonamide, 3-Chloro-4-[(3-Hydroxypropyl, Benzenesulfonamide, 3-Fluoro-4-[(2-Hydroxyethyl), Benzenesulfonamide, 3-Fluoro-4-[(3-Hydroxypropyl, Benzenesulfonamide, 3-Fluoro-4-[(4-Hydroxybutyl), Benzenesulfonamide, 4-[(2-Hydroxyethyl)sulfonyl], Benzenesulfonamide, 4-[(2-Hydroxyethyl)thio]-, Benzenesulfonamide, 4-[(2-Hydroxyethyl)thio]-3-n, Benzenesulfonamide, 4-[(3-Hydroxypropyl)sulfonyl, Benzenesulfonamide, 4-[(3-Hydroxypropyl)thio]-, Benzenesulfonamide, 4-[(3-Hydroxypropyl)thio]-3-, Benzenesulfonamide, 4-[(4-Hydroxybutyl)sulfonyl], Benzenesulfonamide, 4-[(4-Hydroxybutyl)thio]-, Benzenesulfonamide, 4-[(5-Hydroxypentyl)thio]-, Benzenesulfonamide, 4-[3-Hydroxy-3-Methylbutyl)s, Benzenesulfonamide, 4-[3-Hydroxy-3-Methylbutyl)t, Benzenesulfonamide, 4-[[2-[(2-Methylpropyl)amino, Benzoic Acid, 2,3,5,6-Tetrafluoro-4-Methyl-, Benzoic Acid, 5-(aminosulfonyl)-2-[(2-Hydroxyeth, Benzoic Acid, 5-(aminosulfonyl)-2-[(3-Hydroxypro, Butanamide, 2-Amino-n-(2,6-Dimethylphenyl)-, Cinnamic Acid, 4-Hydroxy-3-Methoxy-, (e)-, Ethanamine, N,n-Dimethyl-2-[5-Methyl-2-(1-Methyl, Hydrazinecarboxamide, 2-(phenylmethylene)-, Imidazo[5,1-B]quinazolin-9(2h)-One, 1,3-Dihydro-, Imidazo[5,1-B]quinazolin-9(2h)-One, 2-Butyl-1,3-, Phenol, 2,2'-((1-Methyl-1,2-Ethanediyl)bis(nitri, Piperidine, 1-(4,4-Dimethyl-1-Phenylcyclohexyl)-, Propanoic Acid, 2-(2,4-Dichlorophenoxy)-, (r)-, Thieno[2,3-B]furan-2-Sulfonamide, 5-(4-Morpholin, Thieno[2,3-B]furan-2-Sulfonamide, 5-[[(2-Fluoroe, Thieno[2,3-B]thiophene-2-Sulfonamide, 5-[[(2-Hyd, Thieno[2,3-B]thiophene-2-Sulfonamide, 5-[[(2-Met, Thieno[2,3-B]thiophene-2-Sulfonamide, 5-[[[2-(me, Thieno[3,2-B]thiophene-2-Sulfonamide, 5-[[(2-Met.
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