kb of na3po4

C) 9. Rated by 1 million+ students Get app now Login. I dont know why I was thinking it was going to loose that other hydrogen to become PO43- Got it now! Report your answer as 10 POH. T=iK bm, where i = van Hoff's factor, K b = boiling point elevation constant, m = molality. 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. 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. Policies. Abase ionization constant (Kb)is the equilibrium constant for the ionization of a base. HHS Vulnerability Disclosure. Many compounds of pharmaceutical interest are formulated in sodium phosphate buffers. Potassium Nitrite Calculate the pH of 0.10 M KNO2 solution. We can calculate its basic dissociation constant (Kb) using the following expression. What Are The Ka And Kb Values For .1M Na2HPO4, NaH2PO4, And Na3PO4? 'days' : 'day' }} Not sure about the ice thing, but SQ means square root. Calculate the pH of a 0.300 M Na3PO4 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. 'months' : 'month' }} (Kb > 1, pKb < 1). 1.62 g/cm. Calculate the pH of a 0.0798 M H3PO4 solution. 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? 1 Answer. 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. 'months' : 'month' }}, {{ nextFTS.remaining.days }} Done on a Dell Dimension laptop computer with a Wacom digital tablet (Bamboo). Chemistry(Please help, thank you!!!) Solution: Osmosis and osmotic pressure are related. The simplifying assumption is that. The anion is phosphate, PO4^-3 and (it has a charge of -3). Monosodium phosphate | NaH2PO4 or H2NaO4P | CID 23672064 - structure, chemical names, physical and chemical properties, classification, patents, literature . Requested URL: byjus.com/chemistry/sodium-phosphate/, User-Agent: Mozilla/5.0 (Windows NT 10.0; Win64; x64) AppleWebKit/537.36 (KHTML, like Gecko) Chrome/103.0.5060.114 Safari/537.36 Edg/103.0.1264.62. Conjugate Acid-Base Pairs. Click here to review boiling of pure liquids. 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. TSP is used as a cleaning agent, builder, lubricant, food additive, stain remover, and degreaser. Contact. [12] The United States Food and Drug Administration lists sodium phosphates as generally recognized as safe.[13][14]. The solvent used here is water. E) 8. In the polymerization of ethane-1,2-diol and butanedioic acid, is it an addition or a condensation reaction? You seem very solid on your sciences! Thanks a ton guys.. If I had it I could calculate Ka and get my pH. Non-Zwitterionic Buffer Compound Formula MW Solubility pKa at 20 C g/100 mL of H2O at 20 C 1 2 3 Boric Acid H3BO3 61.8 6.4 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 ionization for a general weak acid, HA, can be written as follows: Because the acid is weak, an equilibrium expression can be written. CHEBI:37583. This will give you the Kb. They are all defined in the help file accompanying BATE. A lower pKb value indicates a stronger base. Molecular Weight/ Molar Mass. 1. 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. You must log in or register to reply here. 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? The larger the value of pKa, the smaller the extent of dissociation. Calculate the pH of a solution of 0.100 M Na3PO4. D The overall dissolution of LiCl is exothermic; this is indicated by the temperature of the water rising. Na3PO4 molecular weight. You can create your own Flashcards and upload decks These values are usually not measured but calculated from thermodynamical data and should not be treated too seriously. solvent. FOIA. Astrong baseis a base, which ionizes completely in an aqueous solution. . A large Kb value indicates the high level of dissociation of a strong base. Unless otherwise stated, pKa and pKb was measured at STP. 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 . Ky75, Page 5 24. * Compiled from Appendix 5 Chem 1A, B, C Lab Manual and Zumdahl 6th Ed. Therefore, the numerical value of. {{ nextFTS.remaining.months }} You have the the following six independent equations in order to specify the unknown concentrations of six species as present in an aqueous solution consisting of $\pu{0.1 M}$ $\ce{H3PO4}$ and $\pu{0.05M}$ $\ce{Na3PO4}$: {{ nextFTS.remaining.months > 1 ? As a result of the EUs General Data Protection Regulation (GDPR). Kb is the molal boiling point elevation constant, and kcabwalc sdliug . 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. Molecular weight calculation: 22.98977*3 + 30.973761 + 15.9994*4. 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. As someone who has to write intricate Excel worksheets for preparing buffers at our company, this program [Buffer Maker] seems amazing. Given that HPO is a triprotic acid for which Ka1 = 7.2 10, Ka2 = 6.3 10 and Ka3 = 4.2 10, the Kb for HPO is 1.6 10. For the reactions of dissociation of acid: stepwise dissociation constants are defined as. Ka and pKa. The pH of a solution is a measure of the molar concentration of hydrogen `(H^+)` , or hydronium `(H_3O^+)` ions of the solution. In the Western world, phosphate usage has declined owing to ecological problems with the damage to lakes and rivers through eutrophication. National Center for Biotechnology Information. Astrong acidis an acid which is completely ionized in an aqueous solution. For that to be the case, the energy released during when the ion-dipole attractions form has . TABLE OF CONJUGATE ACID-BASE PAIRS Acid Base K a (25 oC) HClO 4 ClO 4 - H 2 SO 4 HSO 4 - HCl Cl- HNO 3 NO 3 - H 3 O + H 2 O H 2 CrO 4 HCrO 4 - 1.8 x 10-1 H 2 C 2 O 4 (oxalic acid) HC 2 O 4 - 5.90 x 10-2 [H 2 SO 3] = SO 2 (aq) + H2 O HSO 2003-2023 Chegg Inc. All rights reserved. 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. 'Starts Today' : 'remaining' }} {\displaystyle {\ce {Na3PO4.1/4NaOCl.11H2O}}} Answer to: Which of the following compounds can be combined with Na3PO4 to make a buffer solution? [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. This compound is also known as Trisodium Phosphate. 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, Answer Save. E) None of the above. pKa and pKb are the logarithmic scales of Ka and Kb. 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. What is the pH of a 0.01 M Na3PO4 solution? 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. You will be notified when your spot in the Trial Session is available. Use table search to locate desired compound in database. Ka and pKa The Ksp's for CuCl, AgCl . Convert grams Na3PO4 to moles or moles Na3PO4 to grams. Phosphate ions are used as a buffer because there are three protonated forms (H3PO4, H2PO4-, and HPO42-) that have pKa in the correct . C) Weak acid vs. strong base. 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 (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). im sorry to be a bit slow on this, but why couldnt you use k1 for this problem? Click hereto get an answer to your question What is the pOH of a 0.5 M Na3PO4 solution ? Try It Now, You can create your own Flashcards and upload decks Answer: E. A 1 L buffer solution is 0 M in HF and 0 M in LiF. 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 strong acid is an acid which is completely . By clicking Buy Now! 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. 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 . Consider an aqueous 1.00 m solution of Na3PO4, a compound with useful detergent properties (kb = 0.51 degree C m-1). 4 Ka=[H+][Al(OH)+2]/[Al+3] operating systems: XP, Vista, 7, 8, 10 single user license price: 24.95 - approximately $33 Buy Now! In this case find and write both names as found on the Common Ion Table.-----------------------------For a complete tutorial on naming and formula writing for compounds, like Sodium phosphate and more, visit:http://www.breslyn.org/chemistry/namingDrawing/writing done in InkScape. Spark, {{ nextFTS.remaining.months }} Acid pH = Base Hydrolysis Reaction Ka Kb 2.4E-02 pka E pKb Calculations: 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. Remember. 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. Then divide 1x10^-14/Ka2. A) Strong acid vs. strong base. 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 . Equilibrium: The state of a reaction in which the rates of the forward and reverse reactions are equal. 3.5 b. More. CCRIS 7086. The Kb for NH3 is 1 10-5. 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. Osmosis is the flow of a solvent into a solution through a semipermeable membrane. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Calculate the pH of the solution after the addition of 0 moles of solid LiOH. pH = Conjugate Acid Base Hydrolysis Reaction Kb c pka E pKb 10.66 Calculations: 58 'days' : 'day' }}, {{ nextFTS.remaining.months }} PO43- + H2O HPO42- + OH- ; Kb (PO4-3) = 2.4 10-2. 100% (1 rating) ka Kb=10-14/Ka Phosphori . T = Kbm. (from highest freezing point to lowest freezing poinT) Thanks. Density. In this video we'll write the correct name for Na3PO4.To write the name for Na3PO4 we'll use the Periodic Table and follow some simple rules. {{ nextFTS.remaining.days }} B) Strong acid vs. weak base. : A quantitative measure of the strength of an acid in solution; a weak acid has a pKa value in the approximate range 2 to 12 in water and a strong acid has a pKa value of less than about 2. H2ONH4Cl(2)A.NH3KbB.NH3KbC.pHD.pH . Finally, calculate the freezing point depression. A) 9. a: Na3PO4 and AgNO3 b: K2SO4 and Na2CO3 C: Pb(NO3)2 and Na2CO3 d: BaCl2 and KOH. As we can see in the second step, HPO is the conjugate base of HPO. {{ nextFTS.remaining.days }} I dont know why I can't the right answer but any help would be great! Acid with values less than one are considered weak. [citation needed] This mixture is particularly effective for removing mildew, but is less effective at removing mold. When a solute is added to a solvent, the vapor pressure of the solvent (above the resulting solution) is less than the vapor pressure above the pure solvent. Because these reactions occur in aqueous solutions, water is not included in the equation even though it is part of the reaction. Sodium phosphate (Na3PO4) Sodium orthophosphate, tertiary. pKa and pKb values have been taken from various books and internet sources. For a better experience, please enable JavaScript in your browser before proceeding. (Ka=6.2x10^-10) is quite lower than the the Kb of NH4OH (Kb=1.8x10^-5). The figures below illustrate how the vapor pressure of water is affected by the addition of the non-volatile solute, NaCl. Equation or enables us to calculate the base constant of a conjugate base from the acid constant of the acid, and vice versa. 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. Weak Base Calculations Sodium Phosphate Conjugate Calculate the pH of 0.10 M Na3PO4 solution. -3.7^@"C" Your strategy here will be to determine the van't Hoff factor for sodium iodide, "NaI" calculate the molality of the solution calculate the freezing-point depression of the solution The idea is that the freezing point of a solution is lower than the freezing point of the pure solvent, which for water is 0^@"C" at normal pressure. Is it because it wont dissociate to form either a base or an acid? pKa: A quantitative measure of the strength of an acid in solution; a weak acid has a pKa value in the approximate range 2 to 12 in water and a strong acid has a pKa value of less than about 2. We are not permitting internet traffic to Byjus website from countries within European Union at this time. Products sold as TSP substitutes, containing soda ash and zeolites, are promoted as direct substitutes. m is the molal concentration of the solute in the solution. B) 9. Molar mass of Na3PO4 = 163.940671 g/mol. Because Na3PO4 . SQ is square rootthat's basically a shortcut formula to what you would get if you did the ICE box. 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). The normal freezing point of water is 0.0C. H I think that is what you call it. Name the metal (the cation) as it appears on the Periodic Table. Expert Answer. 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. Polyprotic acids are those with more than one acidic proton. For the definitions of Kan constants scroll down the page. BPP Marcin Borkowskiul. It may not display this or other websites correctly. Base ionization constant (Kb): The equilibrium constantfor theionizationof abase. 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). 1 x 10-14 = K a*Kb Ka = 1x10-14/1.8x10-5 = 5.6 x 10-10 (or look up in table) So, So, no basic action either. 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. Acid pH = Base Hydrolysis Reaction Ka Kb 2.4E-02 pka E pKb Calculations: 'days' : 'day' }}. The acid ionization represents the fraction of the original acid that has been ionized in solution. While TSP is not toxic per se, it is severely irritating to gastric mucosa unless used as part of a buffered solution. Therefore the solution will be neutral. 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+. you must have since you knew your 5 was wrong, right? As with acids, bases can either be strong or weak, depending on their extent of ionization. We had trouble validating your card. Then, calculate the molality of the solution. Higher T will have a higher boiling point. Table 2. nKa Values / Acid-Salts Sodium Hypochlorite Calculate the pH of 0.10 M NaClO solution. {{ nextFTS.remaining.days > 1 ? Calculate the hydronium ion concentration and pH for a 0.043 M solution of sodium format, NaHCO_2. (Kb > 1, pKb < 1). A scientist wants to make a solution of tribasic sodium phosphate,Na3PO4 , for a laboratory experiment. 163.94 g/mol. Sodium Phosphate. For the definitions of Kbn constants scroll down the page. For the reactions of dissociation of base: Next dissociation steps are trated the same way. did you know that the right answer was 10 all along? Trisodium phosphate solution. {{ nextFTS.remaining.days > 1 ? 8600 Rockville Pike, Bethesda, MD, 20894 USA. So you can only have three significant figures for any given phosphate species. ], Sodium phosphates including monosodium phosphate, disodium phosphate, and trisodium phosphate are approved as food additives in the EU. Kb and Ka are also related through the ion constant for water, Kw, by the relationship Kw = Kb x Kb=a. Depending on the source pKa for HCl is given as -3, -4 or even -7. Conjugate acids (cations) of strong bases are ineffective bases. Given the acid constant for a weak acid . 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. Note that the normal boiling point of water increases as the concentration of sucrose increases. Other names - Trisodium phosphate, Sodium orthophosphate, Tribasic sodium phosphate. For which type of titration will the pH be basic at the equivalence point? So elevation in boiling point will be above a boiling point of water for all solutions. Note that ammonia and most organic bases release OH- ions due to hydrolysis, not dissociation. Please remember that only some of them are included in the trial version database, but you can always enter them manually for calculations. What is the percent CsCl by mass in a 0.711 M CsCl solution that has a density of 1.091 Weak acids with relatively higherKavalues are stronger than acids with relatively lowerKavalues. 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. = 141.98 g/mol) that has been dissolved in a 250 mL volumetric flask and diluted to the mark. NaCl is added slowly to a solution that is 0.010 M each in Cu+, Ag+, and Au+. 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? D) 4. 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. For the definitions of Kan constants scroll down the page. Therefore, the numerical value ofKais a reflection of the strength of the acid. It usually results in a bowel movement after 30 minutes to 6 hours. speed set mortar working time of thinset; best choice products jeep parts; zulu social aid and pleasure club posters Diprotic Acids. 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? Aweak baseis a base that ionizes only slightly in an aqueous solution. 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. However, for simplicity, only non-volatile solutes will be considered here. Now, the difference between the freezing point of the . K_b for the reaction of HCO_2^- ion with water is 5.6 times 10^{-11}. In the U.S., trisodium phosphate is an approved flux for use in hard soldering joints in medical-grade copper plumbing. When this acid donates an H + ion to water . 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. Solution is formed by mixing known volumes of solutions with known concentrations. 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. Department of Health and Human Services. Still have questions? 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. Besides, difference between pKa=-1 and pKa=-10 starts to influence calculation results for the solutions with very high ionic strengths, such calculations are dubious in any case. 2. LIVE Course for free. The disodium hydrogen phosphate is reacted with sodium hydroxide to form trisodium phosphate and water. Since HT-Na3PO4 possesses a fully occupied cation sublattice (no vacancies), it has been proposed that cation transport and anion . Explanation: The molar mass of sodium phosphate is M r = (3 23) + 31+ (4 16) = 164g/mol. {{ nextFTS.remaining.days > 1 ? This shows sodium phosphate to be about 42.07% sodium by mass. What is the pH of 1.0 M Na3PO4 in aqueous solution ? Acids. An equilibrium expression can be written for the reactions of weak bases with water. 'months' : 'month' }}, {{ nextFTS.remaining.days }} Na Write the balanced, complete, and net ionic equations for each precipitation reaction. Done on a Dell Dimension laptop computer with a Wacom digital tablet (Bamboo). 'months' : 'month' }} Assuming equal concentrations, rank these aqueous solutions by their freezing point: LiSO4, Li3PO4, SnCl4, NH4Br. 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)? Toggle mobile menu. Aweak acidis an acid that ionizes only slightly in an aqueous solution. Previous question Next question. State whether the following aqueous solutions are expected to be acidic, basic or neutral Dissociation can be also described by overall constants, as well as base dissociation constants or protonation constants. 11 what is the Kb of Na3PO4. in these problems, being on the wrong side of neutral is the red flag that you picked the wrong direction (gaining/losing a proton). Get Answer. Note that the molal boiling point elevation constant, K b, has a specific value depending on the identity of the solvent. C) Weak acid vs. strong base. 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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