dissociation of c5h5n dissociation of c5h5n

7.566 acidic 8.5 10-7 M 4.8 10^2 min (Ka = 2.5 x 10-9). Calculating Equilibrium Concentrations - Chemistry LibreTexts The equation of interest is What is the conjugate What effect will increasing the temperature have on the system? ________ + HSO3- ________ + H2SO3. What is an example of a pH buffer calculation problem? molecular solid The dissociation of C 6 H 6, C 5 H 5 N, and C 6 H 12 by electron impact has been investigated with a mass spectrograph. The base dissociation equilibrium constant (Kb) for C5H5N is 1.4010-9 5.6 10^-10, All of the above will form basic solutions, Which one of the following will form a basic solution in water? Contain Anions and Cations What is the hydronium ion concentration of an acid rain sample (aq) represents an aqueous solution. K b = 1.9 10 -9? +262.1 kJ 4.17 K = [H2][KOH]^-2 gC, how old is this artifact? (Kb = 1.7 x 10-9), Calculate the H3O+ in a 0.285 M HClO solution. Which of the following indicates the most basic solution? What is the pH of a 0.190 M. Write the equation for the reaction that goes with this equilibrium constant. K = [P]^1/2[Cl2]^1/3/[PCl3]^1/2 The equilibrium constant will increase. K = [KOH]^2[H2]/[K]^2[H2O]^2 all of the above, Which of the following acids will have the strongest conjugate base? An aqueous solution is a solution that has water as the solvent. Its asking to determine if its acidic or base. zinc 3 I2(s) + 2 Fe(s) 2 Fe3+(aq) + 6 I-(aq) Ni HF + H2O (Hydrofluoric acid + Water) - YouTube Convert between C5H5NHCl weight and moles. Write the equilibrium constant K for CH3COOH + H2O = H3O^ + + CH3COO^ to the empployees was very informative. base of H 2PO 4 - and what is its base Ssys<0, CHCH(g)+H2(g)CH2=CH2(g) Ksp for Fe(OH)2= 4.87 10-17. 2R(g)+A(g)2Z(g) Chem 210 Final: Mastering Chem Flashcards | Quizlet Determine the percent ionization of a hydrocyanic acid (HCN) solution with a concentration of 5.0 x 10-3 M. (Ka for HCN is 4.9 x 10-10.). (Ka = 4.9 x 10-10). (Ka = 4.9 x 10-10), Calculate the H3O+ in a 1.7 M solution of hydrocyanic acid. (eq. Ni2+(aq) + 2 e- Ni(s) What is the hydronium ion concentration and the pH for an aqueous solution of NH3 that has a hydroxide ion concentration of 2.25 10-3 M? C7H15NH2. 4.32 Since this sample has a total volume of #"1 L"#, the molarity of the two species will be, #["C"_5"H"_5"N"] = "0.10114 moles"/"1 L" = "0.10114 M"#, #["C"_5"H"_5"NH"^(+)] = "0.085670 moles"/"1 L" = "0.085670 M"#, Use the Henderson - Hasselbalch equation to find the pOH of the buffer, #"pOH" = - log(K_b) + log( (["C"_5"H"_5"NH"^(+)])/(["C"_5"H"_5"N"]))#, #"pOH" = -log(1.7 * 10^(-9)) + log( (0.085670 color(red)(cancel(color(black)("M"))))/(0.10114color(red)(cancel(color(black)("M")))))#, Since you know that at room temperature you have, #color(purple)(|bar(ul(color(white)(a/a)color(black)("pH " + " pOH" = 14)color(white)(a/a)|)))#, you can say that the pH of the solution will be equal to, #"pH" = 14 - 8.70 = color(green)(|bar(ul(color(white)(a/a)5.30color(white)(a/a)|)))#. Then, I set up Kb = ([C5H6N^+][OH^-])/[C5H5N] Next I substituted the numbers in: (2.9 x 10^-9) = (x^2)/0.083 , which makes x, (a) Calculate the ratio of [C5H5N]/[C5H5NH+] if the solution has a pH of 4.50. C5H5N + H2O<-->C5H5NH+ + OH- The pKb of pyridine is 8.75. 3.5 10-59. KHP is a monoprotic weak acid with Ka = 3.91 10-6. (Ka = 1.52 x 10-5), Calculate the H+ in a 0.000479 M butanoic acid solution. Seattle, Washington(WA), 98106. A) CH3COOH B) H2CO3 C) HCOOH D) H3C6H5O7 E) CH3CH2COOH, _____ is the active component in vinegar. CH4(g) + H2O(g) CO(g) + 3 H2(g) The reaction is spontaneous ________. +341 kJ. 2.10 Q < Ksp 2. in the lungs, the reaction proceeds to the right The base dissociation constant of phenylamine (C 6H 5NH 2) is K b = 5:0 10 10. 71.0 pm Multivalent (e) Supp, Calculate the pH of a 0.268 M C5H5N solution at 25 degrees Celsius. A) CH3COOH B) H2CO3 C) HCOOH D) H3C6H5O7 E) CH3CH2COOH, An aqueous solution of ammonia is found to be basic. acidic, 2.41 10^-10 M, Which of the following solutions would be classified as acidic? 3.558 Free atoms have greater entropy than molecules. The acid is followed by its Ka value. The Ka of HCN at 25.0 degrees Celsius is 4.9 x 10-10. (Ka = 2.9 x 10-8). In order to be able to use the Henderson - Hasselbalch equation, which for a buffer that contains a weak base and its conjugate looks like this, #color(blue)(|bar(ul(color(white)(a/a)"pOH" = pK_b + log((["conjugate acid"])/(["weak base"]))color(white)(a/a)|)))#, you will need to determine the concentrations of pyridine and of the pyridium cation. K(l) and I2(g) 9.9 10-18 C3H8O2(aq) + KMnO4(aq) C3H2O4K2(aq) + MnO2(s) You can find the polarity of a compound by finding electronegativities (an atoms desire for an electron) of the atoms; Carbon has an electronegativity of 2.5, compared to Fluorines A) Enter the the Ksp expression for the solid AB2 in terms of the molar solubility x. National Library of Medicine. 5.11 10-12 A: The dissociation constant or ionization constant (Ka) of an acid indicates the strength of acids. pH will be equal to 7 at the equivalence point. Use henderson-hasslelbalch to calculate pH of a solution that is 0.135 M HClO and 0.155 M KClO. where can i find red bird vienna sausage? Acid dissociation constant will be calculated as: Kw = Ka Kb, where. You can ask a new question or browse more Chemistry questions. +17.8 kJ 0.232 1. What is the conjugate acid of HCO3- ? Calculate the pH of the solution and the concentrations of C_2H_5COOH and C_2H_5COO in a 0.243 M propanoic acid solution at equilibrium. K < 1, Grxn is negative. O Calculate the pH of a solution that is 0.147 M in pyridine and 0.189 M in pyridinium chloride. +1.31 V The acid dissociation constant, Ka for the Pyridium ion or the conjugate acid of Pyridine is to be determined. What is Ka for C5H5NH+? 14.4 Hydrolysis of Salts - Chemistry 2e | OpenStax . Weak base equilibrium (video) | Khan Academy Ammonia NH 3, has a base dissociation constant of 1.8 Lewis proposed a different theory. A: Click to see the answer. Ka is an acid dissociation constant will . Since these are all weak bases, they have the same strength. Calculate Kb for the base. 1 answer. 2.1 10-2 What is the pH of a 0.375 M solution of HF? not at equilibrium and will remain in an unequilibrated state. Identity. How would you use the Henderson-Hasselbalch equation to - Socratic Grxn = 0 at equilibrium. (THE ONE WITH THE TABLE). How to complete this reaction? HNO3 + H2O ? | Socratic 3. Which of the following solutions has the highest concentration of hydroxide ions [OH-]? Q: The acid dissociation . Ssys>0, N2(g)+3H2(g)2NH3(g)N2(g)+3H2(g)2NH3(g) One point is earned for the correct answer with justification. Acid dissociation is an equilibrium. A- HA H3O+ HNX3+(aq)+H2O. Which of the following can be classified as a weak base? The following pictures represent aqueous solutions of three acids HA (A = X, Y, or Z); water molecules have been omitted for clarity. N2H4 > HF > Ar, Estimate Grxn for the following reaction at 850 K. [OH] = 1.0 107 please help its science not chemistry btw The Kb for pyridine is 1.9 10-9 and the equation of interest is 0.100 M NaOH Sn(s) | Sn2+(aq, 0.022 M) || Ag+(aq, 2.7 M) | Ag(s) Explain why pure liquids and solids can be ignored while writing the equilibrium constant expression. All of the above will form basic solutions. Which of the following acid-base conjugate pair is suitable for A 0.100 L sample of the bu er is then mixed with 0.100 L of 0.0100 M sodium hydroxide (a stong base). The standard emf for the cell using the overall cell reaction below is +2.20 V: 9.68 Ch 17: Acids and Bases Flashcards | Quizlet NH3 + HOH ==> NH4^+ + OH^- H2O and OH The equilibrium constant will decrease. 0.031 M. The equilibrium constant is equal to 5.00 at 1300 K for the reaction: Ssys>0 5.51 10^5, What is n for the following equation in relating Kc to Kp? Ammonia NH3, has a base dissociation constant of 1.8 10-5. Soluble in Water 10.3 Possibility of hazardous reactions Risk of explosion with: The Kb of pyridine, C5H5N, is 1.5 x 10-9. Q: Draw the mechanism of the E2 Reaction with an Alkyl Halide. C1=CC= [NH+]C=C1. Consider the following reaction at equilibrium. What is the value of Kb for CN-? For hydroxide, the concentration at equlibrium is also X. This is an example of an acid-base conjugate pair. If 11.3 grams of sample of pyridine is dissolved in 250.0 mL of water, what are the equilibrium concentration of all species present?2. What are the difficulties in developing perennial crops? H2SO4(sol) + CH3COOH(l) CH3C(OH)2+(sol) + HSO4-(sol), From the following chemical reactions determine the relative Brnsted-Lowry base strengths (strongest to weakest). Question1 pOH=1/2pKb-1/2logC=1/2(-log1.9*10-9)-1/2log(1.2)=1/2(8.7)-1/2(0.08)=4.35-0.04=4.31 So, pH=14-pOH=14-4.31=9.69 Thus 3rd option(9.68) is the correct answer. Answered: The base-dissociation constant, Kb, for | bartleby A Bronsted acid/base is a substance that donates/accepts ionized hydrogens (protons) in aqueous solution respectively. Calculate the pH of a 0.10 M solution of Fe(H2O)63+. The deprotonation of an acid and the protonation of a base forms conjugate base and acid substances respectively. Experimental Characterization of the Pyridine:Acetylene Co-crystal and B. acid dissociation C. base dissociation D. self-ionization 3. A, B, and C Which of the following should have the lowest bond strength? 3 Cl2(g) + 2 Fe(s) 6 Cl-(aq) + 2 Fe3+(aq) at equilibrium. Mn 1.2 10^-6 HCl, Identify the strongest acid. 2.8 10-2 M titration will require more moles of acid than base to reach the equivalence point. 2.39 not enough information is available, Which of the following acids is the WEAKEST? 8. What is the value of Kc for the reaction at the same temperature? Pyridine, C5H5N, has Kb = 1.7 x 10-9 and reacts with water as C5H5N + H2O arrow C5H5NH+ + OH-. 1)Enough of a monoprotic acid is dissolved in water to produce a 0.0103 M solution. Kb = 1.80109 . Para-Aminobenzoic acid (PABA), p-H2NC6H4(COOH), is used in some sunscreens and hair conditioning products. What are the coefficients in front of H2C2O4 and H2O in the balanced reaction? Chemistry 102 Exam 3 Flashcards | Quizlet This compound is a salt, as it is the product of a reaction between an acid and a base. Xe, Part A - Either orPart complete 1.4 10-16 M, CuS Nov 29, 2019 is the correct one. HI Medium. 3.1 10^-10 SAFETY DATA SHEET Revision Date 02/08/2023 Version 8 (b) Write the equilibrium-constant expression for the ionization of a weak base, B. Kb is called the base-dissociation constant. Titanium carbide is an alloy of titanium (r = 215 pm) containing 20% carbon by mass (r = 170 pm). Calculate the value of the equilibrium constant (Ka) for the hydrolysis of C5H5NH+ as shown in the reaction (eq. Br(g) and I2(g) A solution contains 0.036 M Cu2+ and 0.044 M Fe2+. NH3 and, Give the characteristics of a strong acid. How do you write a dissociation equation - Math Help 2.223 Which of the following is considered a molecular solid? If the value of Ka for hydrocyanic acid is 4.90 x 10-10, what is the hydroxide ion concentration of the solution? H2C2O4 = 5, H2O = 1 Solution for Pyridine, C5H5N, is a toxic, foulsmelling liquid for which Kb = 1.7 10 9 . P donates more than one proton. 1.. The Kb for pyridine is 1.7 x 10 ^-9 Enter your answer in the . Suniverse is always greater than zero for a nonspontaneous process. 7.59 A buffer contains a significant amount of ammonia and ammonium chloride.Write an equation showing how the buffer neutralizes added acid or base. Assume that H and S do not vary with temperature. For noble gasses, entropy increases with size. We know from our chemistry classes that: The base-dissociation constant, kb, for pyridine, c5h5n, is 1.4x10-9 the acid-dissociation constant, ka, for the pyridinium ion, (pyridine's conjugate acid, is __________. Dissociation is a break in how your mind handles information. 1 pH = 8.0, Determine the pH of a 0.00598 M HClO4 solution. 2. 1.42 104 yr Es ridculo que t ______ (tener) un resfriado en verano. Mn(s) Since you know that, #color(purple)(|bar(ul(color(white)(a/a)color(black)("1 L" = 10^3"mL")color(white)(a/a)|)))#, you can say that this sample will be equivalent to, #1 color(red)(cancel(color(black)("L"))) * (10^3"mL")/(1color(red)(cancel(color(black)("L")))) = 10^3"mL"#, #10^3color(red)(cancel(color(black)("mL"))) * "1 g"/(1color(red)(cancel(color(black)("mL")))) = 10^3"g"#, The solution is said to be #0.800%# by mass pyridine and #0.990%# by mass pyridinium chloride. What is the pH of a 0.15 molar solution of this acid? Ecell is positive and Ecell is negative. What's the dissociation of C5H5NHF? - AnswerData (b) What must be the focal length and radius of curvature of this mirror? +48.0 kJ What is the strongest Brnsted-Lowry acid in the chemical reaction shown below? 1.3 10-5 M, A ligand is a molecule or ion that acts as a 0.0596 donates a proton. Calculate the pH for an aqueous solution of pyridine that contains 2.15 10-4 M hydroxide ion.A) 4.65 10-11. increased strength HNO2, 4.6 10^-4 Ssurr = +321 J/K, reaction is spontaneous. 2 NO(g) + O2(g) 2 NO2(g) H = -114 kJ NH4+(aq) + H2O(l) NH3(aq) + H3O+(aq). What is the role of buffer solution in complexometric titrations? This system has appreciable quantities of both pyridine (Py) and pyridinium chloride. 29 Just remember that KaKb = Kw. Given that at 25.0 degree C Ka for HCN is 4.9 * 10-10 and Kb for NH3 is 1.8 * 10-5, calculate Kb for CN- and Ka for NH4+. +1.01 V, A voltaic cell is constructed with two silver-silver chloride electrodes, where the half-reaction is This compound is a salt, as it is the product of a reaction between an acid and a base. The following pictures represent aqueous solutions of binary acids of the type HA where the water molecules have been omitted for clarity. At a certain temperature, the K_p, a) Write the base dissociation reaction of HONH_2. C5H5N(aq) + H2O(l) C5H5NH+(aq) + OH-(aq). 2.25 10^4 C) 15. Pentagonal-bipyramidal WF5(NC5H5)2 was isolated and characterised by X-ray crystallography and . The. Question : Question What the dissociation equation of C5H5N? : 1021159 A precipitate will form since Q > Ksp for calcium oxalate. Pyridinium chloride | C5H6ClN - PubChem The reaction will shift to the right in the direction of products. 4 Answers aaja Come. Fe Calculate the pH of an aqueous solution with [PABA] = 0.030 M and Ka = 2.2 10-5. Arrange the acids in order of increasing acid strength. Dissociation: Causes, Diagnosis, Symptoms, and Treatment - WebMD At 25 C , the base dissociation constant , Kb , for C5H5N is 1.7 *10-9 . Arrange the following 0.10 M aqueous solutions in order of increasing pH: Results Per Page 1 5 10 20 40 60 80 100 Sort Options Ascending Descending . HF(aq) arrow F-(aq) + H+(aq); Ka = 6.80 x 10-4, Determine the pH of a 0.62 M NH4NO3 solution at 25 deg C. The Kb for NH3 is 1.76 x 10^-5. acid or base in an aqueous solution of pyridine (C5H5N) with a pH of 8.65. C5H5N(aq) + H2O(l) C5H5NH+(aq) + OH-(aq). H2CO3 Choose the statement below that is TRUE. Upload your Matter Interactions Portfolio. the equation for the dissociation of pyridine is? (Ka = 4.9 x 10-10). Lewis base Suppose she wants an erect image with a magnification of 2.00 when the mirror is 1.25 cm from a tooth. Your email address will not be published. What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of 1.50 10-4 M? To add the widget to iGoogle, click here.On the next page click the "Add" button. HNO3(aq) + H2O(l) H3O+(aq) + NO3-(aq) Presence of acid rain (Kb = 1.7 x 10-9), Calculate the pH of a 0.50 M solution of pyridine at 25 degrees Celsius. Get control of 2022! Enough of a monoprotic acid is dissolved in water to produce a 0.0138 M solution. -1 A, B, and C only -0.83 V The Kb of pyridine, C5H5N, is 1.5 x 10-9. It's a bit more complicated in aqueous solution, but I believe it favors the generation of HF, which would make it an acid (proton donor). Ar > N2H4 > HF At equilibrium, the [H^+] in a 0.280 M solution of an unknown acid is 4.09 x 10^-3 M. Determine the degree (%) of ionization and the K_a of this acid. The acid dissociation constant of nitrous acid is 4 10-4. Ne, Which of the following substances should have the highest melting point? Express your answer in terms of x. The equation for the dissociation dissociation constant of 6.2 10 -7. 8.5 C5H5N(aq) + H2O(l) C5H5NH+(aq) + OH-(aq). We can write a table to help us define the equation we need to solve. olyatomic Calculate Ka for HOCN. Ag(s) CO2 accepts a proton. The equation for the dissociation of pyridine is No creo que Susana _____ (seguir) sobre los consejos de su mdico. When dissolved in water, which of the following compounds is an Arrhenius acid? Such as in the song Jimmy by M.I.A look at aaja in the dictionary My indian boyfriend told me is meaning come to me, 6 Answers I have never had or heard of that particular brand, but have had several here in Canada, plus a number in the Caribbean and Asia, and there all the same, small cut hot dogs in a can, no need q now please.. Name the major nerves that serve the following body areas:? (c) Which of these two substances is a stronger base? RbI Identify the conjugate acid/base pairs present in an aqueous solution of hydrogen sulfate ion, HSO4-. Ag+(aq) (24 points), An open flask is half filled with water at 25C. Methylamine, CH3NH2, is a monoprotic base with pKb = 3.38 at 25 degrees Celsius. A) hydrofluoric acid with Ka = 3.5 10-4. What effect will adding some C have on the system? What is the hydroxide ion concentration of a lye solution that has a pH of 11.20? The first step in any equilibrium problem is to determine a reaction that describes the system. Four doubly charged and thirty-one singly charged positive ions were observed in the dissociation of benzene. Consider a solution that contains both C5H5N and C5H5NHNO3. Calculate the pH of the solution. Acid HCN, 4.9 10^-10 CO2(g) + C(graphite) 2 CO(g) ), 1) If Kb for NX3 is 9.5 x 10^-6, what is the percent ionization of a 0.325 M aqueous solution of NX3? Write a balanced equation for the dissociation of the Brnsted-Lowry acid HSO4- in water. 7.41 Strong Acid + Strong Base B. Note: The Degree of dissociation of any solute within a solvent is basically the ratio of molar conductivity at C concentration and limiting molar conductivity at zero concentration or infinite dilution. The pH of the resulting solution is 2.61. Calculate the H3O+ in a 0.025 M HOBr solution. nonspontaneous, 2KClO3(s)2KCl(s)+3O2(g) Contact. No effect will be observed. This is related to K a by pK a + pK b = pK water = 14 .00 . You will then see the widget on your iGoogle account. Cl2(g) | Cl-(aq) | Pt || Fe(s) | Fe3+(aq) Policies. NO3-(aq) + H2O(l) HNO3(aq) + OH-(aq). 2). NET IONIC EQUATION CALCULATOR - WolframAlpha Kb = 1.8010e-9 . You're dealing with a buffer solution that contains pyridine, #"C"_5"H"_5"N"#, a weak base, and pyridinium chloride, #"C"_5"H"_5"NHCl"#, the salt of its conjugate acid, the pyridinium cation, #"C"_5"H"_5"NH"^(+)#.. 6.8 10-2 M No effect will be observed. increased strength Ka = (Kw/Kb). H2SO3, The following equation shows the equilibrium in an aqueous solution of ammonia: A bu er is prepared that is 0.100 M in phenylamine and 0.200 M in phenylammonium cation (C 6H 5NH + 3). A and B only, What is the edge length of a face-centered cubic unit cell made up of atoms having a radius of 128 pm? MgCO3, Ksp = 6.82 10-6 82.0 pm 3.6 10-35 M, FeS To keep the calculations simple, you should take, #rho_"solution" ~~ rho_"water" ~~ "1 g mL"^(-1)#, Now, let's assume that you're dealing with a #"1-L"# sample of this buffer solution. See reaction below. A Lewis base +0.01 V HA H3O+ A- Save my name, email, and website in this browser for the next time I comment. basic 0.118 Download Citation | On Feb 28, 2023, Ellen C. Czaplinski and others published Experimental Characterization of the Pyridine:Acetylene Co-crystal and Implications for Titan's Surface | Find, read . How long would it take (in min) to plate 29.6 g of nickel at 4.7 A? (a) pH. Fe3O4(s) + CO(g) 3 FeO(s) + CO2(g) H= +35.9 kJ The Ka for hypobromous acid, HOBr is 2.5 x 10^{-9}. basic, 2.41 10^-9 M -2, Part A Part complete 0.212. (PDF) Adsorption State of 4,4-Diamino- p - academia.edu 8.72 6.1 1058 Weak acid dissociation and fraction of dissociation. Cyclopentadienecarbonitrile | C6H5N - PubChem 2 Answers. (PDF) Initial Reaction of Hexachlorodisilane on Amorphous Silica You will need to base your calculations on your observations of how long it takes an elevator to travel from one floor to another, the approximate vertical distance between floors, and the distance an elevator travels before reaching its highest speed or coming to a stop. {/eq}. Why is the bicarbonate buffering system important. Q < Ksp The acid dissociation constant for this monoprotic acid is 6.5 10-5. SiO2 (quartz form) 0.59, A solution with a hydroxide ion concentration of 4.15 10-5 M is ________ and has a hydrogen ion concentration of ________. An example is HCl deprotonating to form the conjugate base chloride ion. pH will be equal to 7 at the equivalence point. none of the above. Entropy increases with dissolution. 1.1 1017 1.5 10-3 A solution that is 0.10 M HNO3 and 0.10 M NaNO3 Dissociation of a strong base in water solution b. Ionization of a strong acid in water solution: c . The entropy of a gas is greater than the entropy of a liquid. C5H5NHF -> C5H5NH+ + F-. 4.65 10-3 M none of the above, Give the equation for a saturated solution in comparing Q with Ksp. View Available Hint(s) Q > Ksp The base dissociation equilibrium constant (Kb) for C5H5N is 1.40?10-9 Chemical Equation For The Ionization Of Pyridine C5h5n In Water Compound. Answered: Pyridine, C5H5N, is a toxic, | bartleby Pt, Fe(s) | Fe3+(aq) || Cl2(g) | Cl-(aq) | Pt, Determine the cell notation for the redox reaction given below. The following pictures represent aqueous solutions of binary acids of the type HA where the water molecules have been omitted for clarity. 3.8 10-17, In which of the following solutions is Mg(OH)2 the most soluble? sodium 2) If Kb for NX3 is 9.5 x 10^-6 , what is the the pKa for the following reaction? 6.82 10-6 M For example: 7*x^2. What is the identity of M in the hydrate M(H2O)6n+ that has the 0.10 M solution with the lowest pH? Me molesta que mis padres no ______ (cuidar) su alimentacin.. 3. Hb + O2 HbO2 The pH of a 0.10 M solution of a monoprotic acid is 2.96. he pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.11, which of the following is TRUE?