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Due to high demand and limited spots there is a waiting list. National Institutes of Health. Calculate the pH of a 0.300 M Na3PO4 solution. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. National Center for Biotechnology Information. {{ nextFTS.remaining.months > 1 ? The three equilibria values for H 3 PO 4, H 2 PO 4-, and HPO 42- are: Ka1 = 7.11 x 10 ^ -3. CHEBI:37583. Molecular Weight/ Molar Mass. 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. Therefore the solution will be neutral. 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. H2ONH4Cl(2)A.NH3KbB.NH3KbC.pHD.pH . Answer: E. A 1 L buffer solution is 0 M in HF and 0 M in LiF. Dissociation: the process by which compounds split into smaller constituent molecules, usually reversibly. For this reason,Kavalues are generally reported for weak acids only. Phosphates are available from a number of other sources that are much milder than TSP. Therefore, the numerical value of. It may not display this or other websites correctly. Since HT-Na3PO4 possesses a fully occupied cation sublattice (no vacancies), it has been proposed that cation transport and anion . Department of Health and Human Services. Because these reactions occur in aqueous solutions, water is not included in the equation even though it is part of the reaction. * Compiled from Appendix 5 Chem 1A, B, C Lab Manual and Zumdahl 6th Ed. 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. CHEM 1412. Review for Test 1 (chapter 13, 14, 15). Done on a Dell Dimension laptop computer with a Wacom digital tablet (Bamboo). For reference or additional information, please contact websupport@aatbio.com -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. National Library of Medicine. Calculate the hydronium ion concentration and pH for a 0.043 M solution of sodium format, NaHCO_2. Starts Today, By clicking Sign up, I agree to Jack Westin's. Report your answer as 10 POH. Ka and pKa A) Strong acid vs. strong base. 2003-2023 Chegg Inc. All rights reserved. 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. Base ionization constant (Kb): The equilibrium constantfor theionizationof abase. Conjugate acids (cations) of strong bases are ineffective bases. 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. 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. Explanation: The molar mass of sodium phosphate is M r = (3 23) + 31+ (4 16) = 164g/mol. {{ nextFTS.remaining.months > 1 ? 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. 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. Monosodium phosphate | NaH2PO4 or H2NaO4P | CID 23672064 - structure, chemical names, physical and chemical properties, classification, patents, literature . Click hereto get an answer to your question What is the pOH of a 0.5 M Na3PO4 solution ? 100% (1 rating) ka Kb=10-14/Ka Phosphori . {{ nextFTS.remaining.months > 1 ? Therefore, the numerical value ofKais a reflection of the strength of the acid. Acid pH = Base Hydrolysis Reaction Ka Kb 2.4E-02 pka E pKb Calculations: While TSP is not toxic per se, it is severely irritating to gastric mucosa unless used as part of a buffered solution. Acids are classified as either strong or weak, based on their ionization in water. The Ksp's for CuCl, AgCl . 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 (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). A large Kb value indicates the high level of dissociation of a strong base. 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^+. Still have questions? 'days' : 'day' }}, {{ nextFTS.remaining.months }} Acids with a pKa value of less than about -2 are said to be strong acids. 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. (Kb = 1.3 10) Done on a Dell Dimension laptop computer with a Wacom digital tablet (Bamboo). D) All of the above. Sodium Phosphate. For which type of titration will the pH be basic at the equivalence point? Note that the molal boiling point elevation constant, Kb, has a specific value depending on the identity of the solvent. Table 2. nKa Values / Acid-Salts Sodium Hypochlorite Calculate the pH of 0.10 M NaClO solution. 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. 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 More. Welcome to Sarthaks eConnect: A unique platform where students can interact with teachers/experts/students to get solutions to their queries. Toggle mobile menu. 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. A) 9. 'months' : 'month' }} : 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. Kb is the molal boiling point elevation constant, and Acid with values less than one are considered weak. Use table search to locate desired compound in database. The Kb for NH3 is 1 10-5. Try It Now. Calculate the pH of a solution of 0.100 M Na3PO4. Because Na3PO4 . 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. 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? Ky75, Page 5 24. For that to be the case, the energy released during when the ion-dipole attractions form has . (from highest freezing point to lowest freezing poinT) Thanks. ], Sodium phosphates including monosodium phosphate, disodium phosphate, and trisodium phosphate are approved as food additives in the EU. {{ notification.creator.name }} For a better experience, please enable JavaScript in your browser before proceeding. It is considered the solvent in these reactions, so the concentration stays essentially constant. 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. {{ nextFTS.remaining.months }} Phosphate ions are used as a buffer because there are three protonated forms (H3PO4, H2PO4-, and HPO42-) that have pKa in the correct . [12] The United States Food and Drug Administration lists sodium phosphates as generally recognized as safe.[13][14]. The molarity of the solution is x 10^-2. Not exactly infinity, huh. 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. Equation or enables us to calculate the base constant of a conjugate base from the acid constant of the acid, and vice versa. E) 8. E) None of the above. us from charging the card. 'months' : 'month' }}, {{ nextFTS.remaining.days }} Describe two different ways to prepare 500.0 mL of a pH 7.40 buffer where the base concentration if 0.100 M. What Are The Ka And Kb Values For .1M Na2HPO4, NaH2PO4, And Na3PO4? 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. 11 what is the Kb of Na3PO4. {{ nextFTS.remaining.days > 1 ? 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). B) 9. By clicking Buy Now! What is the percent CsCl by mass in a 0.711 M CsCl solution that has a density of 1.091 BPP Marcin Borkowskiul. the boiling point of the NaCl solution will be greater than the boiling point of pure water. Note that ammonia and most organic bases release OH- ions due to hydrolysis, not dissociation. pH = Conjugate Acid Base Hydrolysis Reaction Kb c pka E pKb 10.66 Calculations: 58 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. As for pKb values of strong bases - NaOH, KOH, LiOH, Ca(OH)2 - pleas read the explanation in our FAQ section. [citation needed] This mixture is particularly effective for removing mildew, but is less effective at removing mold. 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 . It is a white, granular or crystalline solid, highly soluble in water, producing an alkaline solution. The Kb value for ammonia is 1.8 x 10 a. O What's something you just don't understand? C) Weak acid vs. strong base. Architektw 1405-270 MarkiPoland. Weak Base Calculations Sodium Phosphate Conjugate Calculate the pH of 0.10 M Na3PO4 solution. 4 What is the pOH of a .22 M NaOH solution? 'days' : 'day' }}. The anion is phosphate, PO4^-3 and (it has a charge of -3). {{ nextFTS.remaining.days > 1 ? What is the pH of a 0.01 M Na3PO4 solution? An equilibrium expression can be written for the reactions of weak bases with water. 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. Try It Now, You can create your own Flashcards and upload decks {{ nextFTS.remaining.days > 1 ? Diprotic Acids. Name the metal (the cation) as it appears on the Periodic Table. Note the interface between liquid water (below) and water vapor (above). [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. 'months' : 'month' }} I need to find the pH of a solution containing 50 grams of Na3PO4. Then divide 1x10^-14/Ka2. name. The pKa values for organic acids can be found in Appendix II of Bruice 5th Ed. H I think that is what you call it. Get Answer. For the definitions of Kan constants scroll down the page. Starts Today. Ka2 = 6.34 x 10 ^ -8. you must have since you knew your 5 was wrong, right? So elevation in boiling point will be above a boiling point of water for all solutions. Potassium Nitrite Calculate the pH of 0.10 M KNO2 solution. The pH of a solution is a measure of the molar concentration of hydrogen `(H^+)` , or hydronium `(H_3O^+)` ions of the solution. The figure below shows a microscopic view of the surface of pure water. 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, Solution: Osmosis and osmotic pressure are related. 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 . 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! T=iK bm, where i = van Hoff's factor, K b = boiling point elevation constant, m = molality. If I had it I could calculate Ka and get my pH. (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: pH calculator program - Base Acid Titration and Equilibria - dissociation constants pKa and pKb. You can create your own Flashcards and upload decks 1 Tri-Sodium Phosphate. View the full answer. 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? christopher clarke missing; what is walter mittys fourth daydream; June 8, 2022 kb of na3po4 T = Kbm. pKa and pKb values have been taken from various books and internet sources. 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. Rated by 1 million+ students Get app now Login. 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)? 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 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. On the contrary inorganic bases - like NaOH, KOH, LiOH, Ca(OH)2 - increase pH dissociating. The disodium hydrogen phosphate is reacted with sodium hydroxide to form trisodium phosphate and water. in these problems, being on the wrong side of neutral is the red flag that you picked the wrong direction (gaining/losing a proton). 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+. 1.62 g/cm. 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. Click here to review boiling of pure liquids. Register; Test; JEE; NEET; . 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. Answer to: Consider an aqueous 1.00 m solution of Na3PO4, a compound with useful detergent properties (kb = 0.51 C m-1). 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? 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 $\pu{0.05M}$ $\ce{Na3PO4}$: Boiling Point. C) Weak acid vs. strong base. Calculate the pH of the solution after the addition of 0 moles of solid LiOH. The figures below illustrate how the vapor pressure of water is affected by the addition of the non-volatile solute, NaCl. 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 PO43 + H2OHPO42 + OH ; Kb = 2.4 102. Equilibrium: The state of a reaction in which the rates of the forward and reverse reactions are equal. Step 2: Solve. B) Strong acid vs. weak base. {{ nextFTS.remaining.days }} What is the pH of 1.0 M Na3PO4 in aqueous solution ? For the definitions of Kan constants scroll down the page. Dissociation can be also described by overall constants, as well as base dissociation constants or protonation constants. No tracking or performance measurement cookies were served with this page. remaining pH = Conjugate Acid Base Hydrolysis Reaction Kb c pka E pKb 10.66 Calculations: 58 Policies. Na3PO4 molecular weight. Hydrochloric acid (HCl), acetic acid (CH 3 CO 2 H or HOAc), nitric acid (HNO 3), and benzoic acid (C 6 H 5 CO 2 H) are all monoprotic acids. (Kb > 1, pKb < 1). 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. A scientist wants to make a solution of tribasic sodium phosphate,Na3PO4 , for a laboratory experiment. 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. Answer to: Consider an aqueous 1.00 m solution of Na3PO4, a compound with useful detergent properties (kb = 0.51 C m-1). Because strong acids are essentially 100% ionized, the concentration of the acid in the denominator is nearly zero and theKavalue approaches infinity. {{ nextFTS.remaining.days }} Abase ionization constant (Kb)is the equilibrium constant for the ionization of a base. 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. Acids. Trisodium phosphate solution. FOIA. 1. When this acid donates an H + ion to water . a: Na3PO4 and AgNO3 b: K2SO4 and Na2CO3 C: Pb(NO3)2 and Na2CO3 d: BaCl2 and KOH. Calculate the pH of a 0.0798 M H3PO4 solution. Acid pH = Base Hydrolysis Reaction Ka Kb 2.4E-02 pka E pKb Calculations: It usually results in a bowel movement after 30 minutes to 6 hours. Rock - if you dont mind me asking what was your DAT score? You are using an out of date browser. Many compounds of pharmaceutical interest are formulated in sodium phosphate buffers. Please contact your card provider or customer support. Depending on the source pKa for HCl is given as -3, -4 or even -7. 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). {{ nextFTS.remaining.days > 1 ? Calculate the pH of a 0.20 M Na3PO4 solution. 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. Why is a sodium phosphate buffer used for the pH 6.24 buffer? The solvent used here is water. Then, calculate the molality of the solution. As someone who has to write intricate Excel worksheets for preparing buffers at our company, this program [Buffer Maker] seems amazing. Use table search to locate desired compound in database. As with acids, bases can either be strong or weak, depending on their extent of ionization. Study with Quizlet and memorize flashcards containing terms like What is the pH of a 6.00 M H3PO4 solution? Molar mass of Na3PO4 = 163.940671 g/mol. 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. 2. Solution is formed by mixing known volumes of solutions with known concentrations. 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. Weak Base Calculations Sodium Phosphate Conjugate Calculate the pH of 0.10 M Na3PO4 solution. NaCl is added slowly to a solution that is 0.010 M each in Cu+, Ag+, and Au+. {{ nextFTS.remaining.months > 1 ? m is the molal concentration of the solute in the solution. Given the acid constant for a weak acid . Nov 23, 2010. 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. Unless otherwise stated, pKa and pKb was measured at STP. PO43- + H2O HPO42- + OH- ; Kb (PO4-3) = 2.4 10-2. This compound is also known as Trisodium Phosphate. Na3PO4 ==> 3Na^+ + PO4^-3. For example: CH3COOH pKa=4.76 c=0.1 HCl pKa=-10 c=0.1 Case 2. LIVE Course for free. im sorry to be a bit slow on this, but why couldnt you use k1 for this problem? We are not permitting internet traffic to Byjus website from countries within European Union at this time. C) 9. Thanks a ton guys.. D) 4. The larger the value of pKa, the smaller the extent of dissociation. Calculate the pH of the solution containing 3.875g of Na 2 HPO 4 (MW. In the Western world, phosphate usage has declined owing to ecological problems with the damage to lakes and rivers through eutrophication. 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. Therefore, since the freezing point decreases by 24.0C, the freezing point of the solution is -24.0C. Conjugate Acid-Base Pairs. 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. Aweak baseis a base that ionizes only slightly in an aqueous solution. 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. We can calculate its basic dissociation constant (Kb) using the following expression. 8600 Rockville Pike, Bethesda, MD, 20894 USA. Anacid ionizationconstant (Ka)is the equilibrium constant for the ionization of an acid. Strong acids are listed at the top left hand corner of the table and have Ka values >1 2. Trisodium phosphate is produced by neutralization of phosphoric acid using sodium carbonate, which produces disodium hydrogen phosphate. Osmosis is the flow of a solvent into a solution through a semipermeable membrane. Density. speed set mortar working time of thinset; best choice products jeep parts; zulu social aid and pleasure club posters The normal freezing point of water is 0.0C. Disclaimer - accuracy of the values shown, especially for the strong acids, is questionable. You will be notified when your spot in the Trial Session is available. Table 2. nKa Values / Acid-Salts Sodium. asked Sep 28, 2022 in Chemistry by lolitkumarsingh ( 58.3k points) some basic concepts of chemistry Astrong acidis an acid which is completely ionized in an aqueous solution. Is it because it wont dissociate to form either a base or an acid? This will give you the Kb. 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. Assume no volume change upon the addition of base. The logarithmic constant (pKa) is equal to -log10(Ka).