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Boiling Point Elevation - Purdue University Welcome to Sarthaks eConnect: A unique platform where students can interact with teachers/experts/students to get solutions to their queries.
(Kb = 1.3 10) Due to high demand and limited spots there is a waiting list. JavaScript is disabled.
How to calculate pH of solution made of H3PO4 and Na3PO4? FOIA. Calculate the pH of the solution containing 3.875g of Na 2 HPO 4 (MW. 1 x 10-14 = K a*Kb Ka = 1x10-14/1.8x10-5 = 5.6 x 10-10 (or look up in table) So, It is a white, granular or crystalline solid, highly soluble in water, producing an alkaline solution. 100% (1 rating) ka Kb=10-14/Ka Phosphori . Click here to review boiling of pure liquids. The simplifying assumption is that. Astrong baseis a base, which ionizes completely in an aqueous solution. 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,
T=iK bm, where i = van Hoff's factor, K b = boiling point elevation constant, m = molality. KCl is neutral because KOH is a strong base and HCl is a strong acid. * Compiled from Appendix 5 Chem 1A, B, C Lab Manual and Zumdahl 6th Ed. The 3 Month (100 Day) MCAT Study Schedule Guide: 2022 Edition, All resources are student and donor supported. PO Error: equation KI+Na3PO4=KNa+IPO4 is an impossible reaction Please correct your reaction or click on one of the suggestions below: KI + Na3PO4 = K3PO4 + NaI KI + Na3PO4 = KPO4 + Na3I Instructions and examples below may help to solve this problem You can always ask for help in the forum Why aluminium nitride AlN has higher melting point than Lithium oxide? Weak Base Calculations Sodium Phosphate Conjugate Calculate the pH of 0.10 M Na3PO4 solution. PO43 + H2OHPO42 + OH ; Kb = 2.4 102. 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 . For the reactions of dissociation of base: Next dissociation steps are trated the same way. National Center for Biotechnology Information.
A weak acid has a pKa value in the approximate range of -2 to 12 in water. Astrong acidis an acid which is completely ionized in an aqueous solution. Osmosis is the flow of a solvent into a solution through a semipermeable membrane. Molarity = moles of solute/Liters of solution 0.300 M Na3PO4 = moles Na3PO4/2.50 Liters = 0.75 moles Na3PO4 Answer to: Consider an aqueous 1.00 m solution of Na3PO4, a compound with useful detergent properties (kb = 0.51 C m-1). PO43- + H2O HPO42- + OH- ; Kb (PO4-3) = 2.4 10-2. pH = Conjugate Acid Base Hydrolysis Reaction Kb c pka E pKb 10.66 Calculations: 58
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. Strong acids are listed at the top left hand corner of the table and have Ka values >1 2. Finally, calculate the freezing point depression. Because strong acids are essentially 100% ionized, the concentration of the acid in the denominator is nearly zero and theKavalue approaches infinity. 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 .
Phosphoric acid, h3po4, is a triprotic acid, for which ka1 = 7.2 10 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. C) Weak acid vs. strong base. Table of Acids with Ka and pKa Values* CLAS * Compiled . For reference or additional information, please contact websupport@aatbio.com, Click here to see all available distributors, https://www.aatbio.com/data-sets/pka-and-pkb-reference-table, (nitrilotris(methylene))triphosphonic Acid, 1(2h)-Pyrimidinecarboxamide, 5-Fluoro-3,4-Dichlo, 1(2h)-Pyrimidinecarboxamide, 5-Fluoro-3,4-Dihydr. Unless otherwise stated, pKa and pKb was measured at STP. LIVE Course for free. Weak acids with relatively higherKavalues are stronger than acids with relatively lowerKavalues.
Trisodium phosphate | Na3PO4 - PubChem 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). 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. What is the pH of 1.0 M Na3PO4 in aqueous solution ? m is the molal concentration of the solute in the solution. 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. Many compounds of pharmaceutical interest are formulated in sodium phosphate buffers. Department of Health and Human Services. When this acid donates an H + ion to water . The disodium hydrogen phosphate is reacted with sodium hydroxide to form trisodium phosphate and water.
Arrange the following aqueous solutions in order of decreasing freezing Previous question Next question. Note that the normal boiling point of water increases as the concentration of sucrose increases. Thus, Na 3PO 4 has the highest boiling point. Answer: E. A 1 L buffer solution is 0 M in HF and 0 M in LiF. Jawaban - Manakah diantara berikut titik beku yang paling tinggi nh4c1 0,1 m na3po4 0,1m al2(so) 0,1m co(nh2)2 0,1m - jawaban-sekolah.com I dont know why I can't the right answer but any help would be great! Calculate the pH of a 0.0798 M H3PO4 solution. For H3PO4, Ka1 = 7.5 103, Ka2 = 6.2 108, and Ka3 = 4.2 1013., What is the pH of a solution that has 0.250 M HF and 0.250 M HClO? Weak Base Calculations Sodium Phosphate Conjugate Calculate the pH of 0.10 M Na3PO4 solution. {{ nextFTS.remaining.days > 1 ? For the definitions of Kan constants scroll down the page.
PDF Worksheet 20 - Polyprotic Acids and Salt Solutions The larger the value of pKa, the smaller the extent of dissociation. Kb is the molal boiling point elevation constant, and
31P and 23Na Solid-State NMR Studies of Cation Dynamics in HT-Sodium pH = Conjugate Acid Base Hydrolysis Reaction Kb c pka E pKb 10.66 Calculations: 58 Table 2. nKa Values / Acid . Now let's try some numbers. D) All of the above. For reference or additional information, please contact websupport@aatbio.com pKa and pKb values have been taken from various books and internet sources.
Calculating pH of a Na2HPO4 solution - Student Doctor Network 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. pH = Conjugate Acid Base Hydrolysis Reaction Kb c pka E pKb 10.66 Calculations: 58
What is the freezing point of a solution that contains 0.5 moles of Nal did you know that the right answer was 10 all along? It may not display this or other websites correctly.
Calculate the pH of 0.5 M Na3PO4 in aqueous solution H2ONH4Cl(2)A.NH3KbB.NH3KbC.pHD.pH . 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. Name the metal (the cation) as it appears on the Periodic Table. We had trouble validating your card. 31 164 100 = 18.9%P. Contact. The figure below shows a microscopic view of the surface of pure water. pKa (HNO3)=-1.4 so Ka (HNO3)=25.119. From the molecular equation find the overall ionic and net ionic: Molecular: H3PO4 (aq) + 3NaOH (aq) --> Na3PO4 (aq) + 3H2O (l) Write the balanced molecular, complete ionic, and net ionic equations for the reactions that occur when the following are mixed. The Kb for NH3 is 1 10-5. 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. How many moles of sodium ions are present in 2.50 L of 0.300 M Na3PO4? Calculate the pH of the solution after the addition of 0 moles of solid LiOH. Phosphate ions are used as a buffer because there are three protonated forms (H3PO4, H2PO4-, and HPO42-) that have pKa in the correct . Table 2. nKa Values / Acid-Salts Sodium Hypochlorite Calculate the pH of 0.10 M NaClO solution. 2003-2023 Chegg Inc. All rights reserved. This will give you the Kb. Acids and bases exist as conjugate acid-base pairs.The term conjugate comes from the Latin stems meaning "joined together" and refers to things that are joined, particularly in pairs, such as Brnsted acids and bases.. Every time a Brnsted acid acts as an H +-ion donor, it forms a conjugate base.Imagine a generic acid, HA. 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 . 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. In the U.S., trisodium phosphate is an approved flux for use in hard soldering joints in medical-grade copper plumbing. Conjugate acids (cations) of strong bases are ineffective bases. Higher T will have a higher boiling point. For the reactions of dissociation of acid: stepwise dissociation constants are defined as. To show that they are dissolved in water we can write (aq) after each. Equation or enables us to calculate the base constant of a conjugate base from the acid constant of the acid, and vice versa. The following graph shows the normal boiling point for water (solvent) as a function of molality in several solutions containing sucrose (a non-volatile solute). As for pKb values of strong bases - NaOH, KOH, LiOH, Ca(OH)2 - pleas read the explanation in our FAQ section. Ka and pKa Now consider 1 mole of N a3P O4 which has a mass of 164g: 3 23 = 69g is sodium, 31g is phosphorous, 4 16 = 64g is oxygen. NaCl is added slowly to a solution that is 0.010 M each in Cu+, Ag+, and Au+. Answer Save. 1.62 g/cm. {{ nextFTS.remaining.days }} Step 2: Solve. 1 Answer.
Acid-Base Pairs, Strength of Acids and Bases, and pH - Purdue University {{ nextFTS.remaining.days > 1 ? On the contrary inorganic bases - like NaOH, KOH, LiOH, Ca(OH)2 - increase pH dissociating. 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 . HHS Vulnerability Disclosure. So, no basic action either. Then, calculate the molality of the solution. Density. 3.5 b. For the definitions of Kan constants scroll down the page. Because these reactions occur in aqueous solutions, water is not included in the equation even though it is part of the reaction. 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 . Base ionization constant (Kb): The equilibrium constantfor theionizationof abase. A lower pKb value indicates a stronger base. Molecular Weight/ Molar Mass. Now, the difference between the freezing point of the . A) 9. Assume no volume change upon the addition of base. Na+ = Sodium Mg2+ = Magnesium Al3+ = Aluminum2.Find the polyatomic ion on the Common Ion Table and write the name.Note: It is possible to have two polyatomic ions such as NH4NO3. What is the percent CsCl by mass in a 0.711 M CsCl solution that has a density of 1.091 Consider an aqueous 1.00 m solution of Na3PO4, a compound with useful detergent properties (kb = 0.51 degree C m-1). The Kb value for ammonia is 1.8 x 10 a. O What's something you just don't understand? (Kb > 1, pKb < 1). Ka2 = 6.34 x 10 ^ -8. You must log in or register to reply here. Note that ammonia and most organic bases release OH- ions due to hydrolysis, not dissociation. Operating systems: XP, Vista, 7, 8, 10, 11. Acid with values less than one are considered weak. kcabwalc sdliug . Calculate the pH of a solution of 0.100 M Na3PO4. 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? 11 what is the Kb of Na3PO4. Try It Now. Science Chemistry Pls solve this question correctly in 5 min i will give u like for sure You have the following chemicals available: NaH2PO4 (s), Na2HPO4 2H2O (s), Na3PO4 (s), 6.00 M HCl, and 6.00 M NaOH. Solution: Osmosis and osmotic pressure are related.
Explanation: The molar mass of sodium phosphate is M r = (3 23) + 31+ (4 16) = 164g/mol. How To Remove Scratches From Chrome Plating. Dissociation can be also described by overall constants, as well as base dissociation constants or protonation constants. 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. Ky75, Page 5 24.
Equation for Na3PO4 + H2O (Sodium phosphate - YouTube Manakah diantara berikut titik beku yang paling tinggi By clicking Buy Now! One example is arsenic acid, H 3AsO 4, a triprotic acid.It has three equilibrium expressions associated with its reaction with water: H 3AsO 4 + H 2O ' H 2AsO 4-+ H3O + K a1 = 5.0 x 10-3 H 2AsO 4 Acids are classified as either strong or weak, based on their ionization in water. It usually results in a bowel movement after 30 minutes to 6 hours. 'days' : 'day' }} For which type of titration will the pH be basic at the equivalence point? solvent. 'Starts Today' : 'remaining' }} {{ nextFTS.remaining.months }}
kb of na3po4 The site owner may have set restrictions that prevent you from accessing the site. Click hereto get an answer to your question What is the pOH of a 0.5 M Na3PO4 solution ? Acids are classified as either strong or weak, based on their ionization in water.
Which of the following aqueous solutions has the highest boiling point? The boiling point of a solution, then, will be greater than the boiling point of the pure solvent because the solution (which has a lower vapor pressure) will need to be heated to a higher temperature in order for the vapor pressure to become equal to the external pressure (i.e., the boiling point). This compound is also known as Trisodium Phosphate. They are all defined in the help file accompanying BATE. Get Answer. 163.94 g/mol. The (aq) shows that they are aqueous dissolved in water.The equation for Na3PO4 ( Sodium phosphate and H2O sometimes isnt considered a chemical reaction since it is easy to change the Na + and PO4 3- back to Na3PO4 (just let the H2O evaporate). Aweak baseis a base that ionizes only slightly in an aqueous solution. As with acids, bases can either be strong or weak, depending on their extent of ionization. 4 What is the pOH of a .22 M NaOH solution? 1 Tri-Sodium Phosphate.
Values of dissociation constants pKa and pKb for acids and bases Policies. Given the acid constant for a weak acid . remaining 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.
14.7: Conjugate Acid-Base Pairs and pH - Chemistry LibreTexts State whether the following aqueous solutions are expected to be acidic, basic or neutral We reviewed their content and use your feedback to keep the quality high. How do you arrange these aqueous solutions in order of decreasing freezing point: 0.10 m Na3PO4, 0.35 m NaCl, 0.20 m MgCl2, 0.15 m C6H12O6, and CH3OOH? So you can only have three significant figures for any given phosphate species. Please contact your card provider or customer support. 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.
Molecular weight of Na3PO4 - Convert Units Done on a Dell Dimension laptop computer with a Wacom digital tablet (Bamboo). View the full answer. Potassium Nitrite Calculate the pH of 0.10 M KNO2 solution.
Cracking The Ap Chemistry Exam [PDF] [2b77bebs6vog] Toggle mobile menu. For example: CH3COOH pKa=4.76 c=0.1 HCl pKa=-10 c=0.1 Case 2. Because Na3PO4 . SQ is square rootthat's basically a shortcut formula to what you would get if you did the ICE box.
Answered: What is the percent ionization of | bartleby I dont know why I was thinking it was going to loose that other hydrogen to become PO43- Got it now! Not exactly infinity, huh. Kb and Ka are also related through the ion constant for water, Kw, by the relationship Kw = Kb x Kb=a. 11.22 b. Kb for PO4 3- + H2O --> HPO4 2- + OH - is 4.5 X 10 3 A) 2.2 B) 1.82 C) 11.8 D) 12.2 a. Trisodium phosphate has gained a following as a nutritional supplement that can improve certain parameters of exercise performance. Use table search to locate desired compound in database. 'months' : 'month' }}, {{ nextFTS.remaining.days }} Molecular weight calculation: 22.98977*3 + 30.973761 + 15.9994*4. Therefore, the numerical value of. 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.
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. a: Na3PO4 and AgNO3 b: K2SO4 and Na2CO3 C: Pb(NO3)2 and Na2CO3 d: BaCl2 and KOH.
Solved Weak Base Calculations Sodium Phosphate Conjugate | Chegg.com (Ka=6.2x10^-10) is quite lower than the the Kb of NH4OH (Kb=1.8x10^-5).
Homework 2 with Answer - Broward College, South Campus Homework 2 CHM A scientist wants to make a solution of tribasic sodium phosphate,Na3PO4 , for a laboratory experiment.
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.
Solved What are the Ka and Kb values for .1M Na2HPO4, - Chegg Table 2. nKa Values / Acid-Salts Sodium. Therefore, since the freezing point decreases by 24.0C, the freezing point of the solution is -24.0C. . Polyprotic acids are those with more than one acidic proton. Na 3 PO 4. A) Strong acid vs. strong base. Na3PO4 ==> 3Na^+ + PO4^-3. The solvent used here is water.
kb of na3po4 - rakantrading.net Sodium Phosphate (Na3PO4) - Molecular Mass, Structure, Properties and Uses Nov 23, 2010. At the same time, the Na3PO4 is a very different substance than Na + and PO4 3-.If you need to know how to balance chemical reactions, see my complete tutorial on balancing all types of chemical equations:Balancing Equations in 5 Easy Steps: https://youtu.be/zmdxMlb88FsMore Practice Balancing: https://youtu.be/Qci7hiBy7EQDrawing/writing done in InkScape. While TSP is not toxic per se, it is severely irritating to gastric mucosa unless used as part of a buffered solution. D) 4. {{ nextFTS.remaining.months > 1 ? We can calculate its basic dissociation constant (Kb) using the following expression. pH calculator program - Base Acid Titration and Equilibria - dissociation constants pKa and pKb. 2.
What is the pH of a 0.01 M Na3PO4 solution? So elevation in boiling point will be above a boiling point of water for all solutions. Kb and pKb [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. 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. If I had it I could calculate Ka and get my pH. Convert grams Na3PO4 to moles or moles Na3PO4 to grams. It is considered the solvent in these reactions, so the concentration stays essentially constant. 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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