c) Evaluate the maximum temperature of part (b) for monatomic hydrogen gas (H). And, when an acid or base is added to a solution then any resistance by the solution in changing the pH of the solution is known as a buffer. A buffer is made with HNO2 and NaNO2. In the Henderson-Hasselbalch equation, pH = pKa + log ( [salt] / [acid]), the salt is Na2HPO4 and the acid is NaHzPO4. 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. Identify which of the following mixed systems could function as a buffer solution. Hence, net ionic equation will be as follows. 3. a. Th, Which combination of an acid and a base can form a buffer solution? buffer How to react to a students panic attack in an oral exam? why we need to place adverts ? Label each compound (reactant or product) in the equation with a variable to represent the unknown coefficients. (iii) A solution containing both Na2HPO4 and NaH2PO4 is commonly used as a buffer solution. This same buffer can be diluted to create buffers of 0.5 M, 0.1 M, 0.05 M, or anything in between. Balance each of the following equations by writing the correct coefficient on the line. It should, of course, be concentrated enough to effect the required pH change in the available volume. NaH2PO4 c) H2CO3 and NaHCO3 are also an acid/base conjugate pair and they will make an excellent buffer. Phosphate Buffer A buffer contains significant amounts of acetic acid and sodium acetate. A = 0.0004 mols, B = 0.001 mols a. NH3 b. Cl- c. NH4+, A buffer can be made using a mixture of Na2CO3 (aq) and NaHCO3 (aq) . Could a combination of HI and CH3NH2 be used to make a buffer solution? Na2HPO4 Why are Suriname, Belize, and Guinea-Bissau classified as "Small Island Developing States"? Chapter 17 For 50 mL: 38.5 mL of Na2HPO42H2O and 11.5 mL of NaH2PO4H2O. Donating to our cause, you are not only help supporting this website going on, but also NaOH is a suitable base because it maintains sodium as the cation: Once the solution has been titrated to the correct pH, it may be diluted (at least over a small range, so that deviation from ideal behavior is small) to the volume that will give the desired molarity. 3 [Na+] + [H3O+] = [H2PO4-] + [HPO42-] + Question: A buffer is prepared from NaH2PO4 and Na2HPO4. Na2HPO4 There are only three significant figures in each of these equilibrium constants. Explain. What is the charge on the capacitor? Write two equations showing how the NH_3/NH_4Cl buffer uses up added. aNa3PO4 + bNaH2PO4 = cNa2HPO4 Create a System of Equations What is "significant"? Write an equation showing how this buffer neutralizes an added base. Which of the statements below are INCORRECT for mass balance and charge balance? 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 buffer contains significant amounts of acetic acid and sodium acetate. WebNote that the change in pH (up or down) produced by adding equivalent amounts of strong acid or strong base are equal. b. 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 Sodium methanoate, NaHCOO, and methanoic acid, HCOOH, can be used to make a buffer solution. See Answer. A phosphate buffer solution is especially useful for biological applications,which are especially sensitive to pH changes since it is possible to prepare a solution near any of three pH levels. Chapter 17 copyright 2003-2023 Homework.Study.com. A blank line = 1 or you can put in the 1 that is fine. WebBalance the equation Na3PO4 + NaH2PO4 = Na2HPO4 using the algebraic method. In the Henderson-Hasselbalch equation, pH = pKa + log ([salt] / [acid]), the salt is Na2HPO4 and the acid is NaHzPO4. %PDF-1.4 % What is the activity coefficient when = 0.024 M? Y@ 4b b/>`WjE!(r\J|AT7EpsDH\s$55S%}xD(iAvF`QA*Z$+>QtC _^O!40_:a3 Two buffers are then required, for the two chambers of the gradient generator: the starting buffer (that is, the equilibration buffer, without added NaC1, or with the starting concentration of NaC1) and the finishing buffer, which is the same as the starting buffer but which additionally contains the finishing concentration of NaC1. 0000000016 00000 n A. a) 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. WebBalance the equation Na3PO4 + NaH2PO4 = Na2HPO4 using the algebraic method. H2O is indicated. The following equilibrium is present in the solution. Which statement below is NOT correct for the pH of a 0.01 M NaCl solution versus the pH of a 0.01 M in FeSO4 solution? A buffer is prepared from NaH2PO4 and Na2HPO4. Would a solution of NaNO2 and HNO2 constitute a buffer? Can I tell police to wait and call a lawyer when served with a search warrant? 2 [HPO42-] + 3 The K_a of a buffer does not change when any amount of an acid is added to the buffer solution. 0000003227 00000 n Explain how the equilibrium is shifted as the buffer r, Which buffer would be better able to hold a steady pH on the addition of strong acid, buffer 1 or buffer 2? 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. buffer Catalysts have no effect on equilibrium situations. 0000004875 00000 n Write out an acid dissociation reacti. NaH2PO4 and Na2HPO4 mixture form a buffer solution This equation does not have any specific information about phenomenon. Copyright ScienceForums.Net 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? 2. There are two ionisable hydrogen atom in H2PO4-, so there should be stepwise hydrogen dissociation. A buffer contains significant amounts of ammonia and ammonium chloride. xref It bonds with the added H^+ or OH^- in solution. How does a buffer work? To subscribe to this RSS feed, copy and paste this URL into your RSS reader. Equation for added acid: Equation for added base: Sh, Consider a buffer solution whose acid component is acetic acid, CH3COOH. xb```b``e`a`` @1V X0g UU9B)lsW;0qy: t40xt00[t0@yXl//FFo -Yj0L0e9`t0Ymgb1I@A|E4#) 76+5 Suppose a small amount of a strong acid is added to an aniline buffer system (C6H5NH2/C6H5NH3 +). The following equilibrium is present in the solution. {/eq}). Since phosphoric acid is a weak acid and NaH2PO4 is its salt (differing with one H+) and it has a common anion i.e. pH = answer 4 ( b ) (I) Add To Classified 1 Mark 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. Bio Lab Assignment #3- Acids, bases, and pH buffers (i) Write an expression for the solubility product, Ksp, of Ag3PO4, and state its units. For simplicity, this sample calculation creates 1 liter of buffer. 0000000616 00000 n Which of the following is NOT true for pH? Since phosphoric acid is a weak acid and NaH2PO4 is its salt (differing with one H+) and it has a common anion i.e. Explain why or why not. Use a pH probe to confirm that the correct pH for the buffer is reached. We no further information about this chemical reactions. Find another reaction A $27-\mu \mathrm{F}$ capacitor has an electric potential difference of 45 V across it. By clicking Accept all cookies, you agree Stack Exchange can store cookies on your device and disclose information in accordance with our Cookie Policy. WebNote that the change in pH (up or down) produced by adding equivalent amounts of strong acid or strong base are equal. NaH2PO4 The relative amounts depend on the 3 equilibrium equations, and the total concentration of all of the phosphate species. How much heat will be released when 8.21 g of sulfur reacts with excess O, according to the following equation? A) Write an equation that shows how this buffer neutralizes added acid. In the Henderson-Hasselbalch equation, pH = pKa + log ( [salt] / [acid]), the salt is Na2HPO4 and the acid is NaHzPO4. If the pH and pKa are known, the amount of salt (A-) If you look at the pKa values for phosphoric acid, Wikipedia lists pKa1 = 2.148, pKa2 = 7.198, and pKa3 = 12.319. Explain how this combination resists changes in pH when small amounts of acid or base are added. Explain why or why not. Find the pK_a value of the equation. Here are two examples of how a phosphate buffer can be calculated, as described by Clive Dennison, Department of Biochemistry at the University of Natal, South Africa. Chapter 8 Analytical Chemistry How to prove that the supernatural or paranormal doesn't exist? Theresa Phillips, PhD, covers biotech and biomedicine. b) Write the equation for the reaction that occurs. The charge balance equation for the buffer is which of the following? Buffer 2: a solutio. In this reaction, the only by-product is water. Bio Lab Assignment #3- Acids, bases, and pH buffers [HPO42-] +. The requirement is for an ionic-strength gradient finishing buffer, 0.1 M Na-phosphate buffer, pH 7.6, containing 1.0 M NaCl. H2PO4^- so it is a buffer Write a equilibrium equation for the conjugate acid/base pair if it is a buffer: i) KF/HF ii) NH_3/NH_4Br iii) KNO_3/HNO_3 iv) Na_2CO_3/NaHCO_3, A buffer contains significant amounts of sodium cyanide and cyanic acid. 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? Stack Exchange network consists of 181 Q&A communities including Stack Overflow, the largest, most trusted online community for developers to learn, share their knowledge, and build their careers. Then dilute the buffer as desired. WebA buffer is prepared from NaH2PO4 and Na2HPO4. , Calculate the grams of O2 required for the combustion of 25.9 g of ethylcyclopentane. Is it NaH2PO4 + H2O ----> PO4^3- + H3O^+ + 2Na^+ ? WebBalance the equation Na3PO4 + NaH2PO4 = Na2HPO4 using the algebraic method. WebThough both NaH2PO4 and Na2HPO4 has acidic hydrogen but first one has two and second one has one acidic hydrogen respectively. WebA buffer is prepared from NaH2PO4 and Na2HPO4. Is it NaH2PO4 + H2O ----> PO4^3- + H3O^+ + 2Na^+ ? Buffers - Purdue University 0000006970 00000 n A buffer contains significant amounts of ammonia and ammonium chloride. Write an equation to show how the buffer neutralizes any added acid ({eq}H_3O^+ ionic equation Rating NaCl + H3PO4 = HCl + NaH2PO4 | Chemical Equation The total number of stars for this article is: 5 in 1 review Rating: 5 / 5 Please correct your reaction or click on one of the suggestions below: Na2HPO4 + HCl = NaCl + NaH2PO4 Na2HPO4 + HCl = H3PO4 + NaCl Find another reaction 0000001625 00000 n 0000000905 00000 n Adjust the volume of each solution to 1000 mL. We have placed cookies on your device to help make this website better. Not knowing the species in solution, what can you predict about the pH? equation a. 1.Write an equation showing how this buffer neutralizes added base (NaOH). Adjust the volume of each solution to 1000 mL. a KH 2 PO 4 + b NaOH = c Na 2 HPO 4 + d K 2 HPO 4 + f H 2 O. rev2023.3.3.43278. Write equations to show how this buffer neutralizes added H^+ and OH^-. 1) A buffer consists of NH_4^(+) and NH_3 (ammonia). A. 'R4Gpq] If the pH and pKa are known, the amount of salt (A-) WebA buffer is prepared from NaH2PO4 and Na2HPO4. WebThough both NaH2PO4 and Na2HPO4 has acidic hydrogen but first one has two and second one has one acidic hydrogen respectively. Cross out that which you would use to make a buffer at pH 3.50. 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. Store the stock solutions for up to 6 mo at 4C. }{/eq} and Our experts can answer your tough homework and study questions. a KH 2 PO 4 + b NaOH = c Na 2 HPO 4 + d K 2 HPO 4 + f H 2 O. Dissolve 35.61 g of Na2HPO42H2O and 27.6 g of NaH2PO4H2O separately in H2O. 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. Calculate the pOH of a 0.010 M HCl solution with an ionic strength of 0.10 M. H+ = 0.83, OH = 0.76. This is only the case when the starting pH of buffer is equal to the pKa of weak acid. Sodium hydroxide - diluted solution. A. (Only the mantissa counts, not the characteristic.) b) Write an equation that shows how this buffer neutralizes added base? Predict whether the equilibrium favors the reactants or the products. Phosphate Buffer NaH2PO4 b. xbbc`b``3 1x4>Fc` g Does the concentration of a buffer impact how the buffer solution responds to the addition of an acid or base? Write equations to show how this buffer behaves when (a) HCL is added and (b) NaOH is add, This problem has been solved! 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? 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? W e. Use equations to explain how a buffer system, such as HNO_2 \cdot NO_2,reacts with H_3O and OH? c) H2CO3 and NaHCO3 are also an acid/base conjugate pair and they will make an excellent buffer. H2O is indicated. Connect and share knowledge within a single location that is structured and easy to search. No information found for this chemical equation. It prevents added acids or bases from dissociating. [H2PO4-] + 2 Note that: Note that it is not correct to weigh out the "salt" (Na2HPO4) in the first instance, as this gives an unwanted by-product. In chemistry, a buffer solution serves to maintain a stable pH when a small amount of acid or base is introduced into a solution. Write the chemical equations showing the reactions that take place when: (a) H^+ ions are added to the buffer solution. Chapter 8 Analytical Chemistry Determine the Ratio of Acid to Base. 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. Retrieved from https://www.thoughtco.com/how-to-make-a-phosphate-buffer-in-8-steps-375497. Why assume a neutral amino acid is given for acid-base reaction? pH_problems - University of Toronto Scarborough Write an equation that shows how this buffer neutralizes added acid. Explain. The charge balance equation for the buffer is which of the following? Which of these is the charge balance B. Adjust the volume of each solution to 1000 mL. (Only the mantissa counts, not the characteristic.) This is only the case when the starting pH of buffer is equal to the pKa of weak acid. If you look at the pKa values for phosphoric acid, Wikipedia lists pKa1 = 2.148, pKa2 = 7.198, and pKa3 = 12.319. H3PO4 (Sonac; Phosphoric acid; Orthophosphoric acid; Phosphoric acid hydrogen), disappearing. (b) Write the reaction that takes place when a small amount of OH- is introduced to this buffer solution. Which equation is NOT required to determine the pH of 0.10 M solution of weak acid, HA? A buffer is most effective at [PO43-]. 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 As both the buffer components are salt then they will remain dissociated as follows. 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 | 3 [Na+] + [H3O+] = [H2PO4-] + [HPO42-] + Question: A buffer is prepared from NaH2PO4 and Na2HPO4. 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. Why pH does not change? Write the chemical equation showing the dihydrogen phosphate and hydrogen phosphate conjugate acid-base relationship. Error: equation can be balanced in an infinite number of ways: this is a combination of two different reactions. a. Na_2HPO_4 + NaH_2PO_4 b. Na_2HPO_4 c. H_2O d. NaH_2PO_4. Which of these is the charge balance equation for the buffer? What are the chemical and physical characteristic of NaH2PO4 (Sonac; Phosphoric acid; Orthophosphoric acid; Phosphoric acid hydrogen)? 4. The simplifying assumption is that $$\ce{[H3PO4] + [H2PO4^-] << [HPO4^{2-}] + [PO4^{3-}]}$$. 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? Is it NaH2PO4 + H2O ----> PO4^3- + H3O^+ + 2Na^+ ? WebError: same compound(s) should not be present in both products and reagents: Na2HPO4. A buffer contains significant amounts of ammonia and ammonium chloride. Explain why or why not. ionic equation When mixed in equal concentration, will a combination of HCl(aq) and NaCl(aq) produce a buffer? WebFirst, write the equation for the ionization of the ammonium ion and the related K a expression solved for the hydronium ion concentration. 685 0 obj <> endobj Predict the acid-base reaction. 700 0 obj<>stream Label Each Compound With a Variable. In reality there is another consideration. 0000004068 00000 n Label Each Compound With a Variable Label each compound (reactant or product) in the equation with a variable to represent the unknown coefficients. The requirement is for a 0.1 M Na-phosphate buffer, pH 7.6. #$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^. "How to Make a Phosphate Buffer." Write an equation for each of the following buffering action. }{/eq}, the acid and base components are {eq}\rm{H_2PO_4^- She has worked as an environmental risk consultant, toxicologist and research scientist. b) NaH2PO4 and Na2HPO4 are an acid/base conjugate pair. 2003-2023 Chegg Inc. All rights reserved. [HPO42-] + [OH-], E.[Na+] = [H2PO4-] + Create a System of Equations. Calculating the pH of a mixture of Na2HPO4 and Na3PO4? Can a solution with equal amounts of a weak acid and its conjugate base be used as a buffer? But then due to the presence of buffer there will occur not much change in concentration and the acid will get converted into salt. Store the stock solutions for up to 6 mo at 4C. pH = answer 4 ( b ) (I) Add To Classified 1 Mark Explain. (2021, August 9). a. 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. The reaction implies that only a simple calculation of molarity and a single weighing is required: only one solution needs to be made up, and all of the material weighed out is used in the bufferthat is, there is no waste. Is it plausible for constructed languages to be used to affect thought and control or mold people towards desired outcomes? Which of these is the charge balance equation for the buffer? NaH2PO4 + HCl H3PO4 + NaCl Write an equation showing how this buffer neutralizes added HCl. equation NaH2PO4 + H2O NaH2PO4 Sodium hydroxide - diluted solution. Na2HPO4 A buffer solution is made by mixing {eq}Na_2HPO_4 Popular Answers (1) Dissolve 35.61 g of Na2HPO42H2O and 27.6 g of NaH2PO4H2O separately in H2O. 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. The requirement is for a 0.1 M Na-phosphate buffer, pH 7.6. The best answers are voted up and rise to the top, Not the answer you're looking for? Explain why or why not. How does the added acid affect the buffer equilibrium? Chemistry Stack Exchange is a question and answer site for scientists, academics, teachers, and students in the field of chemistry. Which of these is the charge balance a Na 3 PO 4 + b NaH 2 PO 4 = c Na 2 HPO 4. buffer 0000006364 00000 n HH Equation: pH = pKa + log ([Base] / [Acid]), For a buffer of pH 6.9, [Base] / [Acid] = 0.4898, Substitute for [Acid] and Solve for [Base]. NaH2PO4 A. To learn more, see our tips on writing great answers. Which of the four solutions is the best buffer against the addition of acid or base? [OH-] NaH2PO4 (Sodium dihydrogen phosphate; Primary sodium phosphate; Phosphoric acid dihydrogen sodium salt; Monobasic sodium phosphate; Sodium phosphate), appearing at the end of the reaction. 0000002411 00000 n 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. Consider how to prepare a buffer solution with pH = 7.23 (using one of the weak acid/conjugate base systems shown here) by combining 1.00 L of a 0.483 M solution of weak acid with 0.399 M potassium hydroxide. Dissolve 35.61 g of Na2HPO42H2O and 27.6 g of NaH2PO4H2O separately in H2O. What are the chemical reactions that have Na2HPO4 () as reactant? The three pKa values for phosphoric acid (from the CRC Handbook of Chemistry and Physics) are 2.16, 7.21, and 12.32. WebSodium phosphate monobasic monohydrate = H 4 NaO 5 P or - or - expressed more "normally": NaH 2 PO 4. Describe how the pH is maintained when small amounts of acid or base are added to the combination. Create a System of Equations. If more hydroxide ions were incorporated,then it would result in the transfer to be to the right . C. It prevents an acid or base from being neutraliz. Write an equation for the primary equilibrium that exists in the buffer. M phosphate buffer (Na2HPO4-NaH2PO4 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. The compression and rarefaction associated with a sound wave propagating in a gas are so much faster than the flow of heat in the gas that they can be treated as adiabatic processes. 2003-2023 Chegg Inc. All rights reserved. a KH 2 PO 4 + b NaOH = c Na 2 HPO 4 + d K 2 HPO 4 + f H 2 O. Buffer prepared by mixing 40ml of 0.01M NaH2PO4 with 100ml 0.01M Na2HPO4. Chapter 8 Analytical Chemistry Write a chemical equation showing what happens when H+ is added to this buffer solution. Can a solution with equal amounts of a strong acid and a weak acid be used as a buffer? To prepare the buffer, mix the stock solutions as follows: o i. WebBalance the equation Na3PO4 + NaH2PO4 = Na2HPO4 using the algebraic method. Store the stock solutions for up to 6 mo at 4C. WebSodium dihydrogen phosphate reacts with bases like sodium hydroxide resulting in the formation of sodium hydrogen phosphate and water. NaH2PO4 + NaOH Na2HPO4 + H2O Sodium dihydrogen phosphate reacts with acid like hydrochloric acid results in the formation of phosphoric acid and sodium chloride. A buffer contains significant amounts of ammonia and ammonium chloride. NaH2PO4 Write equations for the reaction of the PO_4/H_2PO_4 buffer reacting with an acid and a base. pH = answer 4 ( b ) (I) Add To Classified 1 Mark Learn what a buffer system is in chemistry, as well as the classification, preparation, and purpose of a buffer. NaH2PO4 Let "x" be the concentration of the hydronium ion at equilibrium. buffer nah2po4 and na2hpo4 buffer equation When mixed in equal concentration, will a combination of CH3COOH(aq) and NaNO3(aq) produce a buffer? NaH2PO4 equation for the buffer? How do you make a buffer with NaH2PO4? a. Popular Answers (1) Dissolve 35.61 g of Na2HPO42H2O and 27.6 g of NaH2PO4H2O separately in H2O. Write reactions equations to explain how acetic acid acetate buffer reacts with an acid and how it reacts with a base. A buffer is most effective at By substituting this into the ratio equation, from step 2, you get: Using the equation: [Base] = 1 - [Acid], you can calculate that: After you've used the Henderson-Hasselbalch equation to calculate the ratio of acid to base required for your buffer, prepare just under 1 liter of solution using the correct amounts of monosodium phosphate and disodium phosphate. H*(aq) + OH(aq) H2001 H2PO4 (aq) + H20(1 HPO42-(aq) + H30*(aq) HPO42-(aq) + H2O(l) H2PO4 (aq) + OH(aq) HPO42-(aq) + H3O+ (aq) H2PO4 (aq) + H2O(1) HPO4(aq) + H2O(aq) H2PO4(aq) + H2O1 Question 2 1 pts Given the Ko's of three weak bases and the K's of two weak acids choose the one that could be used as one of the components of a buffer solution with a pH of 10.35.