: an acid is an electron pair acceptor. Explain. Kb for ammonium hydroxide is 1.8 x 10-5 according to the following reaction. H3PO4 is a weak acid, so it does not fully ionise in water. (a) What is the K_a for ammonium ion? Example: What is the pH of a 0.400 M KBr solution? At 7, neutral. Determine if the following salt is neutral, acidic or basic. Will ammonium nitrate give an acidic, basic, or neutral solution when dissolved in water? Ka. The pH of this solution will be greater than 7. The [H3O+] from water is negligible. Calculate [OH-] in a solution that has [H3O+] = 6.7 x 10-2 M. Is the solution acidic or basic? Reason: If neutral, write only NR. {/eq} is dissolved in water, it gives ammonium hydroxide {eq}\rm \left( {N{H_4}OH} \right) The solution contains a significant concentration of the weak base CN-. A Bronsted-Lowry base is a proton . Perhaps they gain the characteristic of their dominant parent: the acid or base. Antacids, which combat excess stomach acid, are comprised of bases such as magnesium hydroxide or sodium hydrogen . Select all the statements that correctly describe this system. Show your work. Neutral. It goes under complete dissociation. The H+ ion is not an isolated ion, but interacts strongly with H2O to produce the ion, which has the formula H3O+. Explain. Relationship between Ka and Kb of Conjugate Acid-Base Pairs. A solution with a pH of 11.0 is _______ ? Ba (OH)2 An acid can be defined as a substance that loses one or more H+ ions when dissolved in water. Although the pH values of many familiar solutions fall between 0 and 14, in reality pH values can fall outside this range. Is the solution of NH_4C_2H_3O_2 acidic, basic or neutral? The relative acidity (basicity) of an aqueous solution can be determined using the relative acid (base) equivalents. Because Ka for a weak acid HA is ______, we can assume [HA]equilibrium [HA]initial. Question = Is if4+polar or nonpolar ? weaker; left; reactants Therefore, a soluble acetate salt, such as sodium acetate will release The hydrated cation is the ______. Explain. A weak acid is a weak electrolyte. forms H3O+ ions in aqueous solution How does a conjugate acid differ from its conjugate base? The percent dissociation of a weak acid increases as the initial concentration of the acid decreases. The stronger the acid, the _____ the [H3O+] at equilibrium and the _____ the value of Ka. Rank the three different definitions for acids and bases from the least to the most inclusive. So we know that acids and Select all that apply. Direct link to mondirapaul26's post could someone please redi. Arrange the following acids in order of greatest (at the top of the list) to least (at the bottom of the list) amount of H3O+ produced in solution. Is the resulting solution basic, acidic, or neutral? NaNO 2 - basic (NO 2-is a weak base - the conjugate base of a weak acid,HNO 2) NO 2-+ H2 O X HNO 2 + OH-NH 4 Cl - acidic (NH 4 + is a weak acid - the conjugate acid of a weak base, NH 3) NH 4 + + H 2 O X H 3 O + + NH 3 Li 2 SO 4 - basic (SO 4 2-is a weak base - the conjugate base of a weak acid,HSO 4 I'll tell you the Acid or Base list below. salt, the equation for the interaction of the ion with the water, the equilibrium Problem: Acetic acid, HC2H3O2, is a weak acid that is in equilibrium in the following given reaction: HC2H3O2(aq) + H2O(l) H3O+(aq) + CH3CO2-(aq) a. KH2PO4 will generate OH- ions when disolved in water (therefore pH is rising), because is a salt derived from a strong alkali (KOH) and a weak acid (H3PO4). Blank 1: electron Blank 2: proton, hydron, or cation BASE ( wikipedia) It is considered an acid because it sometimes dissipates into ions in water, one of which is a H+ ion. Which of the following compounds can be classified as bases according to the Arrhenius definition? The percent composition of a sample of 20.0 g oleic acid will be (higher, lower or the same) as a sample of 50.0 g oleic acid. NaOH). An acid is any hydrogen-containing substance that is capable of donating a proton (hydrogen ion) to another substance. Explain. .Salts are composed of related numbers of cations (positively charged ions) and anions (negative ions) so that the product is electrically neutral (without a net charge). Show your work. Solutions for Acids and Bases Questions 2. a. Fe(NO3)3 b. NH4I c. NaNO2. C5H5NHClO4 The weak conjugate acid of the weak base pyridine is pyrridinium ion. Acidic. ion functions as a weak acid, the equilibrium constant is given the label reacting with a weak base to give us this salt. Now the next step is to find out what is the nature of acid and base. - a strong acid or base is fully dissociated - a weak acid or base is partially dissociated. The pH scale tells you how acidic or basic a substance is. A higher pKa value (which corresponds to a smaller Ka value) indicates a weaker acid. Arrange the following compounds in order of increasing acid strength (weakest at the top to strongest at the bottom of the list). A salt consisting of the anion of a weak _____ and the cation of a strong _____ yields a basic solution. Ammonium hypochlorite, NH_4ClO, is the salt of ammonia, NH_3, and hypochlorous acid, HClO. Direct link to pipipipipikatchu's post should we always add wate, Posted 3 years ago. How do you know? that are basic. donates an electron pair. Direct link to rahulram05's post Is there any chart which , Posted 3 years ago. NH 4 + and CH 3-COO-are not a conjugate acid/base pair, which means that they do not constitute a . Show your work. See, to understand this The cation has no impact on the pH of the solution. Select all that apply. HOWEVER! A monoprotic acid has ionizable proton(s), whereas a diprotic acid has ionizable proton(s). Now if you have tried it, let's see. Posted 3 years ago. This solution could be neutral, but this is dependent on the nature of their dissociation constants. Select the correct descriptions of the leveling (limiting) effect of water on strong acids and strong bases. Select ALL the strong bases from the following list. The base in the forward reaction is CH3NH2. The number of O atoms attached to the central nonmetal atom. The relationship between Ka and Kb for any conjugate acid-base pairs What is the pH of a 0.509 M solution? 4) Is the solution of CH3NH3CN acidic, basic or neutral? Which of the following common household substances are bases? If you're seeing this message, it means we're having trouble loading external resources on our website. This is the most wide-ranging of the three (i.e. What Kind Of Breast Pain Indicates Pregnancy, Starbucks Barista Salary Philippines Reddit. down and give us ions, sodium ion and hydroxide ion. (this only works with monoprotic (having one mol of proton/H+/H3O+ per mol of acid) acids and bases) Reuben Asare Badu For example, for NH4C2H3O2. {/eq} is described as a salt of weak acid that is acetic acid {eq}\rm \left( {C{H_3}COOH} \right) Is a solution of the salt NH4NO3 acidic, basic, or neutral? Reason: Example: The Ka for acetic acid is 1.7 x 10-5. A 0.15 M solution of butanoic acid, CH3CH2CH2COOH, contains 1.51 x 10-3 M H3O+. The pH of an aqueous solution of 0.340 M methylamine (a weak base with the formula CH_3NH_2) is _____. Soluble hydroxides are strong bases. What is the only step that is necessary in the calculation of pH of a weak base and not a weak acid? What is the pH of a solution that is 0.0260 M in CH_3NH_3NO_3 at 25^\circ C? Use this acids and bases chart to find the relative strength of the most common acids and bases. nature of the acid and base, I can comment on what will be the nature of this salt, right? Select all that apply. The latter reaction proceeds forward only to a small extent, the equilibrium Select all that apply. With reference to the table of Ka values provided, select all the equilibrium acid-base reactions that will favor the products. Is a 0.1 M solution of NH4Cl acidic or basic? In terms of the Arrhenius definition of acids and bases, neutralization is described as _______. And then, the third step was, from this nature, find out Answer = CLO3- (Chlorate) is Polar What is polarand non-polar? Which of the following are products of the reaction between the strong acid HCl and the strong base NaOH? pH OF ACID SALT SOLUTIONS An acid salt is one that still contains H as part of the anion (HSO 4-, H 2PO 4-, HCO 3-, etc) Will the solution of such a salt be acidic due to the reaction: HCO 3-+ H 2O CO 3 2-+ H 3O + Ka2 = 4.7 x 10-11 Or will it be basic due to the reaction: HCO 3-+ H 2O H 2CO 3 + OH-Kb= K w = 1.0 x 10-14 Ka1 4.2x10-7 = 2.4 x 10-8 HF + OCl- F- + HOCl, Acidic solution If the pH paper turns red, is the substance acidic, basic, or neutral? Therefore, a soluble acetate salt, such as sodium acetate will release acetate ions into the solution, which a few of these will interact with water, forming unionized acetic acid and the hydroxide ion. Blank 1: base Which of the following are valid assumptions used in solving weak-acid equilibria problems? CN- will behave as a base when it reacts with water. Safety goggles. An acid can be defined as a substance that loses one or more H+ ions when dissolved in water. answered by DrBob222. Okay, if you already are aware of this, let's move ahead. Reason: And how to find out the raise 10 to the power of the negative pH value. NH4^+ + H2O ==> NH3 + H3O^+. it should be base. Both NH4+ and CN- will hydrolyze (react with water) in aqueous solution. Suppose some ammonium sulfate was mixed with water. Well to do that, first of all I'll have to find out what acid and base would have reacted to give me this salt. A) ammonium chloride (NH_4CI) B) sodium chloride (N. Is an aqueous solution with H+ = 5.7 x 10-8 M classified as acidic, basic, or neutral? Is an aqueous solution with OH- = 9.0 x 10-4 M classified as acidic, basic, or neutral? Processing of production orders is as follows: At the end of each week, the production planning department prepares a master production schedule (MPS) that lists which shoe styles and quantities are to be produced during the next week. Our experts can answer your tough homework and study questions. If you continue to use this site we will assume that you are happy with it. acidic and basic as well. Bronsted-Lowry acid bases, when they react, they neutralize each other's effect. One method of preparing elemental mercury involves roasting cinnabar (HgS) in quicklime (CaO) at 600.C600 .^{\circ} \mathrm{C}600.C followed by condensation of the mercury vapor. Select all that apply. Would a 0.1 M aqueous solution of CuSO4 be acidic, basic, or neutral? Oxoacids where the number of O atoms exceeds the number of ionizable H atoms by 2 or more: HNO3, H2SO4, and HClO4. Hydrated cation acts as an acid. Now let's exchange the ions to get the acid and base. Will an aqueous solution of Li2S be acidic, basic, or neutral? An example is sulfurous acid: A solution of sulfurous acid is dominated by molecules of H 2 SO 3 with relatively scarce H 3 O + and ions. Usually only the first dissociation is taken into account in calculations involving polyprotic acids. Now this means that not all the molecules of this acid are going to dissociate. Answer and Explanation: Ammonium acetate (N H4C2H3O2) ( N H 4 C 2 H 3 O 2) is described as a salt of weak acid that is acetic acid (CH3COOH) ( C H 3 C O O H) and a weak base . The net ionic equation for the hydrolysis of NaC2H3O2 is the following: C2H3O2^- + HOH ==> HC2H3O2 + OH^-. a. 2) Is the solution of NH4NO2 acidic, basic or Is NaCN acidic, basic, or neutral? https://www.thinglink.com/scene/636594447202648065 ACID ( wikipedia) An acid is a molecule or ion capable of donating a hydron (proton or hydrogen ion H+), or, alternatively, capable of forming a covalent bond with an electron pair (a Lewis acid). So we know that ions of acids and bases, they exchange position and HCN is therefore weaker than H2CO3, and the reaction will favor the reactants. a) Acidic, NH_4Cl is the salt of a weak base. Whichever is stronger would decide the properties and character of the salt. Since two . A solution where (H+) = 1 x 10-13 M is: a) Basic b) Neutral c) Acidic d) Strongly acidic e) Two of these; Write a net ionic equation for the reaction that occurs, when aqueous solutions of hypochlorous acid and barium hydroxide are combined. Is NH4NO3 an acid, a base, or a salt? The pH scale is a logarithmic scale, meaning that a solution with a pH of 1.00 has a concentration of hydronium (H3O+) _____ times _____ than a solution with a pH of 3.00. This is our base. partially, okay? A pH level of 7 is a neutral substance which is water. ions of salt with water. Direct link to Mahaty's post Perhaps they gain the cha, Posted 3 years ago. Each new production order is added to the open production order master file stored on disk. Which one of the following 0.1 M salt solutions will be basic? Will the salt ammonium iodide be acidic, basic, or neutral in a water solution? Blank 2: Kb, base-dissociation constant, base dissociation constant, or pKb. Answer: B2 2-is a Diamagnetic What is Paramagnetic and Diamagnetic ? Weak acids and weak bases are weak electrolytes. - aci. Now let's write down the There are 7 hydrogen atoms. Durable sneakers will save a single shoe repair expenses. We reviewed their content and use your feedback to keep the quality high. Acids accept electron pairs. Each day, parts department clerks review the open production orders and the MPS to determine which materials need to be released to production. neutral? Which of the following options correctly describe a solution with a pH = 8.00? D. Strongly basic . [OH-] = Kw[H3O+]Kw[H3O+] = 1.010141.5. The reaction will always favor the formation of the _____ acid and base. For solutions with the same initial concentration of acid HA, the smaller the value of Ka, the _____ the % dissociation and thus the _____ the acid. Consider the acid-base nature of ammonium chloride , NH4Cl, when it is dissolved in water. Kb for ammonium hydroxide is 1.8 x 10-5 according to the following reaction.. The pH of a solution of NH4C2H3O2 is approximately 7. The solution will be basic. show that a buffer system will maintain a relatively fixed pH Write the net-ionic equation for the reaction of HCl with NH4C2H3O2 Acid. A base is an electron pair donor. Direct link to Pi|GLA's post It is considered an acid , Posted 3 years ago. To tell if (NH4)2SO4 (Ammonium sulfate) forms an acidic, basic (alkaline), or neutral solution we can use these three simple rules along with the neutralization reaction that formed (NH4)2SO4 .. And if you have a question (mumbles), how are these things happening. What is the pH of a 0.808 M KOBr solution if the Ka of HOBr is 2.0 10-9? {/eq}, both are acid and base. Which of the following anions will produce a neutral solution in water? Question: Is ammonium acetate (NH4C2H3O2) acidic, basic, or neutral in pH? Select all that apply. Explain the Lewis model of acid-base chemistry. Place the least inclusive definition at the top of the list and the most inclusive definition at the bottom of the list. C_2H_3O_2^- + H_2O ]rightleftharpoons HC_2H_3O_2 - OH^-;\;\;\;\textit{K}_b = 5.7\times 10^{-10} the complete reaction of all H+ ions from the acid with all the OH- ions from the base. The pH value of 11.951 therefore has 3 significant figures. b. But see, one thing to note over here is that HCl, this is a strong acid, and NaOH, this is a strong base. Best custom paper writing service. May 10, 2008. If the Ka of the cation is greater than the Kb of the anion, a solution of the salt will be ______. {/eq}. One way to determine the pH of a buffer is by using . Select all that apply. now, then don't worry. Become a Study.com member to unlock this answer! The pH of a solution is a logarithmic value. Direct link to Pi|GLA's post We write it like that so , Posted 2 years ago. A Lewis acid absorbs an electron pair from a Lewis base, resulting in the formation of a coordinate covalent bond. - basic, because of the ionization of CH3NH2. In this equation, [HA] and [A] refer to the equilibrium concentrations of the Conjugate acid-base pairs (video) - Khan Academy acid-base pair used to create the buffer solution.Aug 24, 2021 488 Math Tutors Now if you have tried it, let's see. Will an aqueous solution of calcium acetate [Ca(C_2H_3O_2)_2] be acidic, basic or neutral? Blank 3: amphoteric or amphiprotic. In this video we saw that salts could be acidic, basic, or neutral in nature. Kb ammonia = 1.8 x 10-5. In the reaction of boric acid with water, we have B(OH) 3 + H 2 O B(OH)-4 + H +. Baking soda and ammonia, common household cleaners, are a. All rights reserved. HCl, this is a strong acid. base, we get the salt NaCl, NaCl salt, and this is a neutral salt, meaning when we put NaCl in functions as a weak base, the equilibrium constant is given the label Kb. Is NH4CN acidic, basic, or neutral? 3. Like how is it that a strong acid reacts with a weak base to give me an acidic salt? Some species can act as either an acid or a base depending on the other species present. Will a solution of the salt NH4Cl be acidic, basic, or neutral? Now if you have thought D) The salt is a product of a strong acid and a strong base. Ammonium acetate is formed from weak acid and weak base. it works for everything). Is it difficult to write an admission paper, From Zero to Fluent: Tips for Finding the Right Korean Lesson Near You, Predict whether an aqueous solution of each of the following salts will be acidic, basic, or neutral. For each, state whether the solution is acidic, basic, or neutral. So let's begin. How many atoms of mercury are present in the mercury vapor at 300.C300 .^{\circ} \mathrm{C}300.C if the reaction is conducted in a closed 15.0-L container? The scale goes from 0 to 14. H2S is a _____ acid than HCl because S is _____ electronegative than Cl, while HBr is a _____ acid than HCl because the H-Cl bond is shorter and has _____ strength than the H-Br bond. If yes, kindly write it. The conjugate acid has one more H than its conjugate base. going to be basic in nature. Explain. If the pH value is equal to 7, then the compound will be neutral, and if the pH value is greater than seven, then the compound will be basic. An acid-base reaction occurs when one species loses a proton and another species simultaneously gains a proton. Acid Base Properties of Salts Recommended for Chapter(s): 7 Demo #025 Materials NOT in box 1. This lesson focuses on acids and bases, how to identify them, and the characteristics they have. Few ions B and D are a conjugate acid-base pair. Select all that apply. The latter reaction proceeds forward only to a small extent; the equilibrium Will ammonium bromide give an acidic, basic, or neutral solution when dissolved in water? NH4NO3 is acidic, strong acid and weak base NH4C2H3O2 is made up of a weak acid and a weak base, so we must look at the Ka and Kb, The Kb is larger than the Ka, so it's more basic. Share this. Which of the following is NOT a conjugate acid-base pair? Polyprotic acids are generally weak acids. 4) Is the solution of CH3NH3CN acidic, basic or neutral. Since acetate Ka of HClO = 3.0 10-8. Which of the following options correctly describe the structural characteristics of strong and weak bases? Classify the following salt solutions as acidic, neutral, or basic. A base is an acids chemical opposite.. 1) KNO_3 2) NaClO 3) NH_4Cl. b. With so many stars in our solar system, the night sky is a beautiful sight. The anion, A-, of a weak acid is a(n) ______ because anions react with solvent water to produce HA and OH-. Calculate the Ka value for the anilium ion (C6H5NH3+) if Kb for aniline (C6H5NH2) is 4.0 x 10-10. {/eq}, both are acid and base. In an organic acid such as CH3CH2COOH, the ionizable H atoms is/are ______. What Is ammonium acetate (NH_4C_2H_3O_2) acidic, basic, or neutral? about this, let's see. Classify an aqueous solution with OH- = 7.4 x 10-4 M as acidic, basic, or neutral. Explain. Ignore the use of any superscripts or subscripts in your answers. ion formed to determine whether the salt is an acidic, basic, or neutral Then, depending on the Ammonium ion is the conjugate acid of the weak base, ammonia with a Kb = 1.8 x 10^-5, and formate ion is the conjugate base of the weak acid fo. So see, the first step was, from the given salt, try to find out the acid and the base that could have reacted upon this. NH3 is a weak base, therefore, the NH4^+ hydrolyzes. Select all that apply. The ______ of dissociated HA molecules increases as a weak acid solution is diluted. [HA] at equilibrium is approximately equal to [HA]init. Neutral. Best sights of the knowledge base for you. Which of the following factors will affect the relative strength of oxoacids? The equilibrium expression for this reaction Acidic substances are usually identified by their sour taste. A 0.10 M solution of KCN will be acidic, neutral, or basic? that resists the change in pH when limited amounts of acid or Write the net-ionic equation for the reaction of HCl with NH4C2H3O2 475 Math Consultants 84% . Select all that apply. In this case, since both acetic acid and NH4OH have about the same Ka (or Kb), then the NH4C2H3O2 is about neutral. NH4C2H3O2: NH4 is a weak acid, so it has a strong conjugate base. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Bases react with acids to produce a salt and water 6. Strong acid molecules are not present in aqueous solutions. Select all that apply. So let's do that. Most compounds that contain nitrogen are weak electrolytes. participate readily in proton-transfer reactions. Blank 2: acids. Molecular Examples HF - hydrofluoric acid CH 3 CO 2 H - acetic acid NH 3 - ammonia H 2 O - water (weakly dissociates in itself) Nonelectrolytes Since pH is a logarithmic value, the digits before the decimal are not significant. So the strong parent is the acid. Lewis acid neutral? Sodium hydroxide is found in drain cleaner. can combine with OH-, this will go with OH-, and I'll get NH4OH and this is going to be a base. nature of this salt, whether this is acidic, basic, or neutral? For example, NH3 is the base, and NH4+ is the conjugate acid (the ionic form), so there is no involvement of hydroxide ions (those occur in strong bases, e.g. Explain. Note a salt may have low solubility in water, yet still be a strong electrolyte because the amount that does dissolve completely ionizes in water. [H3O+] = [A-] [HA]init UNIVERSIDADE FEDERAL DA PARABA CENTRO DE CINCIAS EXATAS E DA NATUREZA DEPARTAMENTO DE QUMICA PROGRAMA DE PS-GRADUAO EM QUMICA TESE DE DOUTORADO AVALIAO DA CAPACI the nature of the salt? Metal cations act like ______ when dissolved in water. Calculate the pH and [H3O+] of a 0.080 M solution of NaOH. copyright 2003-2023 Homework.Study.com. could someone please redirect me to the other videos which explain how and why the salts take on their dominant parent's properties? H-A is a covalent bond, so that can exist in solution. Weak electrolytes include weak acids, weak bases, and a variety of other compounds. That means our salt is also Learn about acids and bases. binary molecular compounds. It exists as all ions. KOH is a strong base while H2S is a weak acid. 2003-2023 Chegg Inc. All rights reserved. Reason: Instructions, Select all the factors that affect the ease with which a proton is released from a nonmetal hydride (represented by the general formula E-H.), The strength of the E-H bond 0.00010 M So let's see. A base is a substance that will accept the acids hydrogen atom . {/eq}. Direct link to Shweta Sharma's post CH3COOH it has a OH so wh, Posted 3 years ago. Neutral. It is a white solid and can be derived from the reaction of ammonia and acetic acid." (Assume a solution is neutral if its pH is 7.00 plus-minus 0.05). The acid and base chart is a reference table designed to make determining the strength of acids and bases simpler. Explain. Molecules with electron deficient central atoms. . Blank 2: OH-, hydroxide, hydroxide ion, or HO- Question = Is CLO3-polar or nonpolar ? In contrast, strong acids, strong bases, and salts are strong electrolytes. All hydrohalic acids in Period 3 or below, Correctly order the steps necessary to solve weak-acid equilibria problems. The last machine in each work cell prints a bar-code label that the worker affixes to the box. Instructions. constant K is very small. Calculate [H3O+] in a solution with a [OH-] = 3.0 10-4 M. Is the solution acidic or basic? Blank 3: leveling or levelling. We get p H = ( 4.76 + 9.25) / 2 = 7.005 7 (only one significant figure is given, since you have stated the concentration as 1 M ). Which of the following species usually act as weak bases? The dissociation constant of the weak base is: a) 1.39 * 10^{-5} b) 1.39 * 10^{-4} c) 1.45 * 10^{-10} d) 1.65 * 10^{-5}, why ammonium acetate completely dissociates in water(aq): CH3COONH4 + aq -> CH3COO-+ NH4+. Question = Is C2Cl2polar or nonpolar ? Examples of Lewis bases include NO2-, NH3, and H2O. - basic, because of the hydrolysis of CH3NH3^+ ions. Bases have a pH between 7 and 14. https://en.wikipedia.org/wiki/Base_(chemistry), https://en.wikipedia.org/wiki/Salt_(chemistry), https://en.wikipedia.org/wiki/Neutralization_(chemistry). Which of the following statements accurately describe Bronsted-Lowry acid-base reactions? When making a buffer by adding a conjugate acid/base pair to water, one ingredient is the reactant and the other is the product (and there is . Which of the following choices correctly depicts the net ionic equation for the reaction of a strong acid (HNO3) with a strong base (KOH)? The compound ammonium acetate is a strong electrolyte. Mixture 2, reaction of a strong base and weak acid, also goes to completion. Explain. So we have found out the parent acid and base for the given So the ions of our salt will be CH3COO-, or acetate ion and the sodium plus sign, Question = Is SbCl5 ( Antimony pentachloride ) polar or nonpolar ? Select ALL the strong acids from the following list. Answer = IF4- isNonpolar What is polarand non-polar? New Questions About Fantasy Football Symbols Answered and Why You Must Read Every Word of This Report. Although physically she is recovering quite well from the procedure, you note that she is becoming more despondent and depressed. Question: Is B2 2-a Paramagnetic or Diamagnetic ? Blank 4: acid. Reason: In calculations involving polyprotic acids, we generally only take into account H3O+ formed from the first dissociation.