#$I{8fNV~g"1M d1/0shBNp6+7Q/ap\*=i<6(XoKOzW^lo/3GfHwc:%IGR_O \hg:bHM|l:,N-] NhRmp;{2o>owTk['`phaG9*VB9G/& h34fm\Jk]I&1JT"p%X>'rYwq.MhV;qcB50a!+OVdj*#45evZcVy; \6"d~p%s^. (i) What is meant by the term buffer solution? Phillips, Theresa. pH = answer 4 ( b ) (I) Add To Classified 1 Mark c) H2CO3 and NaHCO3 are also an acid/base conjugate pair and they will make an excellent buffer. A buffer contains significant amounts of ammonia and ammonium chloride. A buffer contains significant amounts of ammonia and ammonium chloride. A. WebWhat are the chemical reactions that have NaH2PO4 (Sodium dihydrogen phosphate; Primary sodium phosphate; Phosphoric acid dihydrogen sodium salt; Monobasic sodium phosphate; Sodium phosphate) as product? a. You're correct in recognising monosodium phosphate is an acid salt. In the Henderson-Hasselbalch equation, pH = pKa + log ( [salt] / [acid]), the salt is Na2HPO4 and the acid is NaHzPO4. Then dilute the buffer as desired. Identify all of the. Sometimesfor example, in an ion exchange ionic-strength gradient elutionit is required to have a gradient of, say, [NaC1] superimposed on the buffer. A. OWE/ The requirement is for a 0.1 M Na-phosphate buffer, pH 7.6. Write equations to show how this buffer behaves when (a) HCL is added and (b) NaOH is add, This problem has been solved! A buffer contains significant amounts of acetic acid and sodium acetate. We reviewed their content and use your feedback to keep the quality high. (Only the mantissa counts, not the characteristic.) Predict whether the equilibrium favors the reactants or the products. See the answer 1. All other trademarks and copyrights are the property of their respective owners. A buffer is made with HNO2 and NaNO2. If a law is new but its interpretation is vague, can the courts directly ask the drafters the intent and official interpretation of their law? How can I explain to my manager that a project he wishes to undertake cannot be performed by the team? }{/eq} and Our experts can answer your tough homework and study questions. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Here is where the answer gets fuzzy. Write an equation showing how this buffer neutralizes an added base. If YES, which species would need to be in excess? What is the balanced equation for NaH2PO4 + H2O? WebNa2HPO4 () + H3PO4 (Sonac; Phosphoric acid; Orthophosphoric acid; Phosphoric acid hydrogen) = NaH2PO4 (Sodium dihydrogen phosphate; Primary sodium phosphate; Phosphoric acid dihydrogen sodium salt; Monobasic sodium phosphate; Sodium phosphate) | Balanced Chemical Reaction Equation Home Na2HPO4 H3PO4 = NaH2PO4 | Become a Study.com member to unlock this answer! directly helping charity project in Vietnam building shcools in rural areas. [Na+] + [H3O+] = WebThe problem is, that your protein may not like it and you should keep the formula as "clean" as possible. A buffer is prepared from NaH2PO4 and WebThe Henderson-Hasselbalch equation enables determination of a buffer solution's pH when the pKa is known. Web1. How do you make a buffer with NaH2PO4? Write the acid base neutralization reaction between the buffer and the added HCl. Which of these is the charge balance equation for the buffer? Write a net ionic equation that occurs in a Na2HPO4/NaH2PO4 buffer solution when: A) a small amount of HCl is added (2 points) B) a small amount of sodium hydroxide is added (2 points) 2 See answers Advertisement Write equations to show how this buffer neutralizes added H^+ and OH^-. [HPO42-] + [OH-], D.[Na+] + [H3O+] = Create a System of Equations. To make your phosphate buffer, you'll need the following materials: Before making a buffer, you should first know what molarity you want it to be, what volume to make, and what the desired pH is. b) NaH2PO4 and Na2HPO4 are an acid/base conjugate pair. H2O is indicated. Let "x" be the concentration of the hydronium ion at equilibrium. Calculate the pH of a buffer solution made by mixing 100 cm3 of 0.5 mol dm3 Na2HPO4 and 100 cm3 of 0.3 mol dm3 NaH2PO4. Write equations for the reaction of the PO_4/H_2PO_4 buffer reacting with an acid and a base. Cross out that which you would use to make a buffer at pH 3.50. B. aNa3PO4 + bNaH2PO4 = cNa2HPO4 Create a System of Equations In a buffer system of {eq}\rm{Na_2HPO_4 when A-/HA=1, Calculating pH of reaction mixture of silver nitrate and ascorbic acid. WebA buffer must have an acid/base conjugate pair. Henderson-Hasselbalch Equation and Example, Calculating the Concentration of a Chemical Solution. Write an equation to show how the buffer neutralizes any added acid ({eq}H_3O^+ Since phosphoric acid is a weak acid and NaH2PO4 is its salt (differing with one H+) and it has a common anion i.e. Create a System of Equations. What is the activity coefficient when = 0.024 M? A. You have a buffer system made up of equimolar amounts of carbonic acid, H_2OCO_3, and sodium bicarbonate, NaHCO_3. calculate the number of N, C, O, and H atoms in 1.78*10^4g of urea. WebYou'll get a detailed solution from a subject matter expert that helps you learn core concepts. If the buffer contains 1.05 M of B and 0.750M conjugate acid and has a pH of 9.50, what is the pH af, Write two equations showing how the HC_2H_3O_2/NaC_2H_3O_2 buffer uses up added. Explanation: The ideal environmental conditions for a reaction, such as temperature, pressure, catalysts, and solvent. You can specify conditions of storing and accessing cookies in your browser, 5. Find more information about "Net ionic equation" here: (A) As we know that HCl is a strong acid and when it is added to an aqueous solution then it leads to increase in the concentration of hydrogen ions. Which equation is NOT required to determine the pH of 0.10 M solution of weak acid, HA? Create a System of Equations. Explain. (Select all that apply.) Why is a buffer solution best when pH = pKa i.e. (Only the mantissa counts, not the characteristic.) Find another reaction Write an equation showing how this buffer neutralizes added base NaOH. Create a System of Equations. [Na+] + [H3O+] = [H2PO4-] + 2 [HPO42-] + 3 [PO43-] + [OH-] B. WebNa2HPO4 () + H3PO4 (Sonac; Phosphoric acid; Orthophosphoric acid; Phosphoric acid hydrogen) = NaH2PO4 (Sodium dihydrogen phosphate; Primary sodium phosphate; Phosphoric acid dihydrogen sodium salt; Monobasic sodium phosphate; Sodium phosphate) | Balanced Chemical Reaction Equation Home Na2HPO4 H3PO4 = NaH2PO4 | "How to Make a Phosphate Buffer." However if you want to account for 99.99999999999% of the species (12 significant figures), then you're going to have to consider all four phosphate species. a KH 2 PO 4 + b NaOH = c Na 2 HPO 4 + d K 2 HPO 4 + f H 2 O. Write a chemical equation that shows how this buffer neutralizes small amounts of acid, H^+. Find another reaction [Na+] + [H3O+] = [H2PO4-] + 2 [HPO42-] + 3 [PO43-] + [OH-] B. NaH2PO4 + NaOH Na2HPO4 + H2O Sodium dihydrogen phosphate reacts with acid like hydrochloric acid results in the formation of phosphoric acid and sodium chloride. Explain how the equilibrium is shifted as buffer reacts w, Write the chemical equation showing dihydrogen phosphate and hydrogen phosphate conjugate acid-base relationship. 2. c) H2CO3 and NaHCO3 are also an acid/base conjugate pair and they will make an excellent buffer. & To adjust for these, we apply the Debye-Huckel equation using A at 0.509 and calculating I by assuming that half of the buffer strength is divided between the conjugate acid and A buffer is made by dissolving HC_2H_3O_2 and NaC_2H_3O_2 in water. You are handed a buffer solution that contains equal concentrations of a weak acid and its conjugate base. You're correct in recognising monosodium phosphate is an acid salt. Time arrow with "current position" evolving with overlay number. The three pKa values for phosphoric acid (from the CRC Handbook of Chemistry and Physics) are 2.16, 7.21, and 12.32. A buffer is most effective at Explain how this combination resists changes in pH when small amounts of acid or base are added. aNa3PO4 + bNaH2PO4 = cNa2HPO4 Create a System of Equations HUn0+(L(@Qni-Nm'i]R~H Let "x" be the concentration of the hydronium ion at equilibrium. Ka = 1.8 105 for acetic acid. Experts are tested by Chegg as specialists in their subject area. Which of these is the charge balance equation for the buffer? 0000007740 00000 n To prepare the buffer, mix the stock solutions as follows: o i. a solution that resists / minimises a change in its pH or helps maintain its pH.. (NOT any of: "maintains pH"; "keeps pH constant"; "no change in pH"), ..when small amounts of acid / H+ or base / OH are added (both acid and, (ii) Write equations to show how the hydrogencarbonate ion, HCO3. (c) Write the reactio. 0000006970 00000 n 2. ThoughtCo. Once the desired pH is reached, bring the volume of buffer to 1 liter. Silver phosphate, Ag3PO4, is sparingly soluble in water. What is the net ionic equation for the reaction that occurs when a small amount of hydrochloric acid is added to the Na2HPO4/NaH2PO4 buffer solution? H2O is indicated. 'R4Gpq] A buffer is made by dissolving HF and NaF in water. What is "significant"? Error: equation can be balanced in an infinite number of ways: this is a combination of two different reactions. Create a System of Equations. ThoughtCo, Aug. 9, 2021, thoughtco.com/how-to-make-a-phosphate-buffer-in-8-steps-375497. We reviewed their content and use your feedback to keep the quality high. What are the chemical and physical characteristic of H3PO4 (Sonac; Phosphoric acid; Orthophosphoric acid; Phosphoric acid hydrogen)? Write an equation that shows how this buffer neut. The following equilibrium is present in the solution. Web2 Mark s (iii) A solution containing both Na2HPO4 and NaH2PO4 is commonly used as a buffer solution. NaH2PO4 + HCl H3PO4 + NaCl A buffer is made by dissolving H_3PO_4 and NaH_2PO_4 in water. Which of the following mixtures could work as a buffer and why? WebSodium phosphate monobasic monohydrate = H 4 NaO 5 P or - or - expressed more "normally": NaH 2 PO 4. 0000001625 00000 n Is it NaH2PO4 + H2O ----> PO4^3- + H3O^+ + 2Na^+ ? For 50 mL: 38.5 mL of Na2HPO42H2O and 11.5 mL of NaH2PO4H2O. WebBalance the equation Na3PO4 + NaH2PO4 = Na2HPO4 using the algebraic method. Explain the answer. What could be added to a solution of hydrofluoric acid to prepare a buffer? Buffer prepared by mixing 40ml of 0.01M NaH2PO4 with 100ml 0.01M Na2HPO4. By If it is a buffer, write an equilibrium equation for the conjugate acid/base pair. Write a net ionic equation that occurs in a Na2HPO4/NaH2PO4 buffer solution when: A) a small amount of HCl is added (2 points) B) a small amount of sodium hydroxide is added (2 points) 2 See answers Advertisement For a 1 M buffer, [Base] + [Acid] = 1 and [Base] = 1 - [Acid]. WebBalance the equation Na3PO4 + NaH2PO4 = Na2HPO4 using the algebraic method. All of the following are TRUE for activities and activity coefficients, except: For Ag+ when = 0.01 M, = 0.898 and when = 0.05, = 0.80. What is the net ionic equation for the reaction that occurs when a small amount of hydrochloric acid is added to the Na2HPO4/NaH2PO4 buffer solution? There are only three significant figures in each of these equilibrium constants. You're correct in recognising monosodium phosphate is an acid salt. WebNa_2HPO_4 + NaH_2PO_4 Calculate the pH of 1.00 L of a buffer that is 0.100 M HNO_2 and 0.170 M NaNO_2 What is the pH of the same buffer after the addition of 1.00 mL of 12.0 M HCI. Given a 6 M solution of NH3 (Kb = 1.78 * 10-5) and 6 M HNO3: Part A: If a buffer were prepared, what species would be the acid in the buffer? Phillips, Theresa. A buffer contains significant amounts of ammonia and ammonium chloride. ________________ is a measure of the total concentration of ions in solution. a.) Popular Answers (1) Dissolve 35.61 g of Na2HPO42H2O and 27.6 g of NaH2PO4H2O separately in H2O. (a) NaHSO_4/Na_2SO_4 (b) HNO_2/NaNO_2 (c) HCl/NaOH (d) NaH_2PO_4/Na_2HPO_4. The charge balance equation for the buffer is which of the following? H2PO4^- so it is a buffer For 1 liter of buffer, NaH2PO4.2H20 (15.60 g) and NaC1 (58.44 g) are dissolved in about 950 ml of distilled H20, titrated to pH 7.6 with a fairly concentrated NaOH solution (but of arbitrary concentration) and made up to 1 liter. Web2 Mark s (iii) A solution containing both Na2HPO4 and NaH2PO4 is commonly used as a buffer solution. WebWhat are the chemical reactions that have NaH2PO4 (Sodium dihydrogen phosphate; Primary sodium phosphate; Phosphoric acid dihydrogen sodium salt; Monobasic sodium phosphate; Sodium phosphate) as product? The net ionic equation, if a small amount of HCl is added: b) On adding small amount of sodium hydroxide into the solution then there will occur an increase in concentration of hydroxide ions into the solution. Ksp = units: (ii) The numerical value of Ksp is 1.25 1020 at 298 K. Use this value to calculate [Ag+(aq)] in, [Ag+(aq)] = .. mol dm3, The half-equation for the redox reaction between phosphoric(III) acid and phosphoric(V) acid is, Find suitable data from the Data Booklet to write an equation for the reaction between H3PO3. WebNote that the change in pH (up or down) produced by adding equivalent amounts of strong acid or strong base are equal. Question: What is the net ionic equation for the reaction that occurs when a small amount of hydrochloric acid is added to the Na2HPO4/NaH2PO4 buffer solution? When mixed in equal concentration, will a combination of CH3COOH(aq) and NaNO3(aq) produce a buffer? In this case, you just need to observe to see if product substance 3. If more hydrogen ions are incorporated, the equilibrium transfers to the left. Find another reaction An acid added to the buffer solution reacts. Which of the statements below are INCORRECT for mass balance and charge balance? WebAnswer (1 of 2): A buffer is a solution of any weak acid and its salt having common ions.or a solution of any weak base and its salt having common ions. 0000004875 00000 n Can I tell police to wait and call a lawyer when served with a search warrant? C. It forms new conjugate pairs with the added ions. Buffer 1: a solution containing 0.50 F NH_4Cl and 1.00 F NH_3. To prepare the buffer, mix the stock solutions as follows: o i. Making this buffer is a bit more complicated than making TAE and TBE buffers, but the process is not difficult and should take only about 10 minutes. In the Henderson-Hasselbalch equation, pH = pKa + log ( [salt] / [acid]), the salt is Na2HPO4 and the acid is NaHzPO4. In Henderson equation for acidic buffer we will use pKa3 because Na2HPO4 acting as weak acid and Na3PO4 as its salt with strong base. By clicking Post Your Answer, you agree to our terms of service, privacy policy and cookie policy. [H2PO4-] + 2 Create an equation for each element (K, H, P, O, Na) where each term represents the number of atoms of the element in each reactant or equation for the buffer? 3. When an acid is introduced into this buffer, which of H2CO3 and HCO3- reacts with the acid to maintain the pH of the solution? The addition of a strong base to a weak acid in a titration creates a buffer solution. b.Show the net ionic equation for the reaction that oc, Write the chemical equation showing dihydrogen phosphate and hydrogen phosphate conjugate acid-base relationship. Adjust the volume of each solution to 1000 mL. Browse other questions tagged, Start here for a quick overview of the site, Detailed answers to any questions you might have, Discuss the workings and policies of this site. a KH 2 PO 4 + b NaOH = c Na 2 HPO 4 + d K 2 HPO 4 + f H 2 O. Write a chemical equation showing what happens when H+ is added to this buffer solution. How do you make a buffer with NaH2PO4? Create an equation for each element (K, H, P, O, Na) where each term represents the number of atoms of the element in each reactant or Label Each Compound With a Variable. NaH2PO4 is much more acidic than Na2HPO4, hence NaH2PO4 acts as an acid while Na2HPO4 acts a salt of NaH2PO4 with a strong base NaOH. Explain. If you look at the pKa values for phosphoric acid, Wikipedia lists pKa1 = 2.148, pKa2 = 7.198, and pKa3 = 12.319. The following equilibrium is present in the solution. Create a System of Equations. Part A Write an equation showing how this buffer neutralizes added acid (HI). 0000004068 00000 n Explain. A buffer contains significant amounts of ammonia and ammonium chloride. 685 0 obj <> endobj Connect and share knowledge within a single location that is structured and easy to search. Chemistry Stack Exchange is a question and answer site for scientists, academics, teachers, and students in the field of chemistry. WebError: same compound(s) should not be present in both products and reagents: Na2HPO4. If more hydroxide ions were incorporated,then it would result in the transfer to be to the right . Hence, net ionic equation will be as follows. Sodium hydroxide - diluted solution. Write an equation that shows how this buffer neutralizes a small amount of acids. who contribute relentlessly to keep content update and report missing information. Adjust the volume of each solution to 1000 mL. Write an equation to show how the A buffer solution is made by mixing Na2HPO4 with NaH2PO4. rev2023.3.3.43278. Can HF and HNO2 make a buffer solution? Most of the entries in the NAME column of the output from lsof +D /tmp do not begin with /tmp. What is a buffer and how does it relate to the Henderson-Hasselbalch equation? Donating to our cause, you are not only help supporting this website going on, but also Calculate the pH of a buffer solution made by mixing 100 cm3 of 0.5 mol dm3 Na2HPO4 and 100 cm3 of 0.3 mol dm3 NaH2PO4. endstream endobj 686 0 obj<>/Metadata 32 0 R/PieceInfo<>>>/Pages 31 0 R/PageLayout/OneColumn/StructTreeRoot 34 0 R/Type/Catalog/LastModified(D:20061204104744)/PageLabels 29 0 R>> endobj 687 0 obj<>/ProcSet[/PDF/Text]/ExtGState<>>>/Type/Page>> endobj 688 0 obj<> endobj 689 0 obj<> endobj 690 0 obj<> endobj 691 0 obj<>stream It prevents an acid-base reaction from happening. WebHomework Equations pH=pHa+log( [A-]/[HA]) The Attempt at a Sodium hydrogen phosphate react with hydrogen chloride to produce phosphoric acid and sodium chloride. WebThe problem is, that your protein may not like it and you should keep the formula as "clean" as possible. Express your answer as a chemical equation. [PO43-]. {/eq}. W e. Use equations to explain how a buffer system, such as HNO_2 \cdot NO_2,reacts with H_3O and OH? Predict whether the equilibrium favors the reactants or the products. A buffer contains significant amounts of ammonia and ammonium chloride. Use the pKa value nearest your desired pH; the ratio refers to the acid-base conjugate pair that corresponds to that pKa. WebSodium dihydrogen phosphate reacts with bases like sodium hydroxide resulting in the formation of sodium hydrogen phosphate and water. The molarity of the buffer is determined by the mass of the acid, NaH2PO4, which is weighed out, and the final volume to which the solution is made up. Asking for help, clarification, or responding to other answers. Could a combination of HI and H3PO4 be used to make a buffer solution? why we need to place adverts ? This means that addition of buffer into the given solution will not cause much change in the concentration of in large amount. Store the stock solutions for up to 6 mo at 4C. It's easy! https://www.thoughtco.com/how-to-make-a-phosphate-buffer-in-8-steps-375497 (accessed March 4, 2023). 2. What is the Difference Between Molarity and Molality? Theresa Phillips, PhD, covers biotech and biomedicine. Write the net Bronsted equation and determine the equilibrium constant for the acid-base reaction that occurs when aqueous solutions of H2CO3 and KHS are mixed. Phillips, Theresa. Adjust the volume of each solution to 1000 mL. WebError: same compound(s) should not be present in both products and reagents: Na2HPO4. NaH2PO4 is much more acidic than Na2HPO4, hence NaH2PO4 acts as an acid while Na2HPO4 acts a salt of NaH2PO4 with a strong base NaOH. Identify the acid and base. Write an equation showing how this buffer neutralizes added acid (HNO3). b) Write the equation for the reaction that occurs. Web1. Which equation is NOT required to determine the molar solubility of AgCN? Which equation is NOT required to determine the pH of 0.10 M solution of weak acid. Use a pH probe to confirm that the correct pH for the buffer is reached. How do the relative and absolute concentrations of an acid and its conjugate base in a buffer affect its effectiveness in resisting pH changes upon the addition of a strong acid and a strong base? a. Na_2HPO_4 + NaH_2PO_4 b. Na_2HPO_4 c. H_2O d. NaH_2PO_4. Could a combination of HI and LiOH be used to make a buffer solution? What is a buffer? WebLabel each compound (reactant or product) in the equation with a variable to represent the unknown coefficients. 3 [Na+] + [H3O+] = To learn more, see our tips on writing great answers. Catalysts have no effect on equilibrium situations. Explain why or why not. If HC1 is used, the reaction will be: yielding NaC1, of an indeterminate concentration, which is not wanted in the buffer. A buffer solution is made by mixing Na2HPO4 with NaH2PO4. The HH equation states that the ratio of salt to acid, rather than their absolute concentrations, determines the pH. NaH2PO4 is much more acidic than Na2HPO4, hence NaH2PO4 acts as an acid while Na2HPO4 acts a salt of NaH2PO4 with a strong base NaOH. The concentration of the NaOH is of no concern, so any arbitrary concentration can be used. Interesting Information Only Few People Knows, This system is delivered to you by Vietnamese students and teachers WebSodium dihydrogen phosphate reacts with bases like sodium hydroxide resulting in the formation of sodium hydrogen phosphate and water. Check the pH of the solution at Which of these is the charge balance equation for the buffer? }{/eq} and {eq}\rm{NaH_2PO_4 (a) pH = 7.0, because the acid and base neutralize each other (b) pH < 7 b. WebFirst, write the equation for the ionization of the ammonium ion and the related K a expression solved for the hydronium ion concentration. Why is a buffer able to resist drastic changes to pH upon the addition of an acid or a base? Write a net ionic equation that occurs in a Na2HPO4/NaH2PO4 buffer solution when: A) a small amount of HCl is added (2 points) B) a small amount of sodium hydroxide is added (2 points) 2 See answers Advertisement 0000000016 00000 n Monosodium phosphate and its conjugate base, disodium phosphate, are usually used to generate buffers of pH values around 7, for biological applications, as shown here. :D. What are the chemical and physical characteristic of Na2HPO4 ()? [Na+] + [H3O+] = For 50 mL: 38.5 mL of Na2HPO42H2O and 11.5 mL of NaH2PO4H2O. Thanks for contributing an answer to Chemistry Stack Exchange! Please correct your reaction or click on one of the suggestions below: Na2HPO4 + HCl = NaCl + NaH2PO4 Na2HPO4 + HCl = H3PO4 + NaCl Select a substance that could be added to sulfurous acid to form a buffer solution. WebNote that the change in pH (up or down) produced by adding equivalent amounts of strong acid or strong base are equal. From the equation it is clear that if the [salt] > [acid], the pH will be greater than the pKa, and if [salt] < [acid], the pH will be less than the pKa. NaH2PO4 (Sodium dihydrogen phosphate; Primary sodium phosphate; Phosphoric acid dihydrogen sodium salt; Monobasic sodium phosphate; Sodium phosphate), appearing at the end of the reaction. a Na 3 PO 4 + b NaH 2 PO 4 = c Na 2 HPO 4. Why? Write the equation for the reaction that occurs when strong acid (H3O+) is added to the buffer. Buffer 2: a solutio. endstream endobj 699 0 obj<>/Size 685/Type/XRef>>stream Adjust the volume of each solution to 1000 mL. Question: What is the net ionic equation for the reaction that occurs when a small amount of hydrochloric acid is added to the Na2HPO4/NaH2PO4 buffer solution? What is the balanced equation for NaH2PO4 + H2O? If the pH and pKa are known, the amount of salt (A-) A = 0.0004 mols, B = 0.001 mols WebNote that the change in pH (up or down) produced by adding equivalent amounts of strong acid or strong base are equal. You can adjust your cookie settings, otherwise we'll assume you're okay to continue. Label Each Compound With a Variable Label each compound (reactant or product) in the equation with a variable to represent the unknown coefficients. WebThough both NaH2PO4 and Na2HPO4 has acidic hydrogen but first one has two and second one has one acidic hydrogen respectively. Label each compound (reactant or product) in the equation with a variable to represent the unknown coefficients. 4. I just updated the question. Which of these is the charge balance equation for the buffer? It only takes a minute to sign up. pH = answer 4 ( b ) (I) Add To Classified 1 Mark If the pH and pKa are known, the amount of salt (A-) Explain why or why not. For phosphoric acid the three pKa's are different enough so that only two phosphate species will have a "significant" concentration at whatever pH the solution is at. For simplicity, this sample calculation creates 1 liter of buffer. A buffer is most effective at its pKa, which is the point where [salt] = [acid]. Write a net ionic equation showing how this buffer neutralizes added base (Ba(OH)2). Explain. 2. Also see examples of the buffer system. xb```b``e`a`` @1V X0g UU9B)lsW;0qy: t40xt00[t0@yXl//FFo -Yj0L0e9`t0Ymgb1I@A|E4#) 76+5 (Only the mantissa counts, not the characteristic.) Check the pH of the solution at xbbc`b``3 1x4>Fc` g

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