Each new production order is added to the open production order master file stored on disk. called the how of this. If the pH value of a solution of the compound is less than seven, then the compound will be acidic. In this reaction, NH 3 has a lone pair of electrons and BF 3 has an incomplete octet, since boron doesn't have enough electrons around it to form an octet. Classify the salt as acidic, basic, or neutral. Determine if the following salt is neutral, acidic or basic. Blank 4: covalent or sigma. Since there is no transfer of hydrogen atoms here, it is clear that this is a Lewis acid-base reaction. can be used to estimate the pH of the salt solution. Direct link to Shweta Sharma's post CH3COOH it has a OH so wh, Posted 3 years ago. [H3O+] = [OH-]. is the ionization constant for the base form of the pair, and Kw is the
BASE ( wikipedia) increases NH4 is a weak acid, so it has a strong conjugate base. H3PO4 is a weak acid, so it does not fully ionise in water. A production order preparation program accesses the MPS and the operations list (stored in a permanent disk file) to prepare a production order for each shoe style that is to be manufactured. Basic solution Is an aqueous solution of NaCNO acidic, basic, or neutral? Will ammonium nitrate give an acidic, basic, or neutral solution when dissolved in water? Hydrohalic acids: HCl, HBr, and HI Direct link to Shivani's post At 2:42,why is Na put aft, Posted 2 years ago. Question = Is if4+polar or nonpolar ? And if you have a question (mumbles), how are these things happening. C2H3O2 is the strong conjugate base of a weak acid. Blank 1: H or hydrogen It is probably a bit alkaline in solution. The Periodic Table Lesson for Kids: Structure & Uses. In order to determine whether a solution of NH4C2H3O2 is acidic, basic, or neutral, what two values could be compared? An acid is a molecule or ion capable of donating a, In chemistry, bases are substances that, in aqueous solution, are slippery to the touch, taste astringent, change the color of, In chemistry, a salt is an ionic compound that can be formed by the neutralization reaction of an acid and a base. 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. And we have also seen that NH4OH, ammonium hydroxide, for x will be very small as well, thus the term (0.500 - x) is equal to
Like how is it that a strong acid reacts with a weak base to give me an acidic salt? Which of the following statements correctly describes the behavior of strong acids, HA, in aqueous solution? Explain. Blank 3: amphoteric or amphiprotic. Now let's write down the Is CaH2 acidic, basic, or neutral? NH4C2H3O2: NH4 is a weak acid, so it has a strong conjugate base. CH3COOH is a weaker acid than HF. A monoprotic acid has _____ ionizable proton(s). What is the pH of a 0.25 M solution of ethanolamine (Kb = 3.2 x 10-5)? Get access to this video and our entire Q&A library. Neutral. Whichever is stronger would decide the properties and character of the salt. 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. Most molecules of the weak acid remain undissociated at equilibrium. (b) What is the K_b for hypochlorite ion? hydrofluoric acid HF, phosphoric acid H 3 PO 4, carbonic acid H 2 CO 3, acetic acid HC 2 H 3 O 2 Weak means very little ionized like 1-5%. Is a solution with a pH of 4 extremely acidic, moderately acidic, slightly basic, extremely basic, neutral? The anion is the conjugate base of a weak acid. Ka for HCN is 5.8 x 10-10. Are you looking for the best essay writers offering their assistance on the web? If your blood is buffered to a pH of 7.4, is your blood acidic, basic, or neutral? Sodium hydroxide is found in drain cleaner. Salts can be formed from the reaction of a strong acid and a strong base, a strong acid and a weak base, a weak acid and a strong base or a weak acid and a weak base. According to the Arrhenius definition, an acid is a substance like hydrochloric acid that dissolves in water to produce H + ions (protons; Equation 4.3.1 ), and a base is a substance like sodium hydroxide that dissolves in water to produce hydroxide (OH ) ions (Equation 4.3.2 ): HCl ( g) anArrheniusacid H2O ( l) H + ( aq) + Cl ( aq) Although physically she is recovering quite well from the procedure, you note that she is becoming more despondent and depressed. . From water I will get 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. A salt consisting of the anion of a _____ acid and the cation of a _____ base yields an acidic solution. Rank the following compounds in order of decreasing acid strength (strongest at the top to weakest at the bottom of the list). A(n) acid is one that dissociates only slightly in water, whereas a(n) acid dissociates completely into ions. - basic, because of the hydrolysis of CH3NH3^+ ions. In this video we saw that salts could be acidic, basic, or neutral in nature. Complete the following table. Which of the following species is present in the greatest concentration in a 1.0 M solution of CH3COOH? pH = -0.18 - acidic, because of the hydrolysis of CH3NH3^+ ions. (this only works with monoprotic (having one mol of proton/H+/H3O+ per mol of acid) acids and bases) Reuben Asare Badu 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 ). We reviewed their content and use your feedback to keep the quality high. And on the other hand, when we have a weak acid Select the two types of strong acids. Salts of Weak Acid-Weak Base Reactions: such as NH4C2H3O2, NH4CN, NH4NO2, etc.. According to the Bronsted-Lowry definition, an acid donates H+ to a base. Consider the acid-base nature of ammonium chloride , NH4Cl, when it is dissolved in water. K2S is the salt of KOH and H2S. Sodium acetate is therefore essential in an aqueous medium. {/eq}. For example, the acetate ion is the conjugate base of acetic acid, a weak
Only a few molecules of this will break into its' ions, okay? Blank 1: Ka, acid-dissociation constant, acid dissociation constant, or pKa 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 Weak electrolytes include weak acids, weak bases, and a variety of other compounds. Is H_3O^+ = 1 \times 10^{-10}; OH^- = 1 \times 10^{-4} M acidic, basic, or neutral? {/eq}, both are acid and base. It will be hydrolyzed to produce an acidic solution. weaker; left; reactants bases, when they react, they neutralize each other's effect. NH4+ is an acidic ion and Cl- is a neutral ion; solution will be acidic. Calculate [H3O+] in a solution with a [OH-] = 3.0 10-4 M. Is the solution acidic or basic? 2) Is the solution of NH4NO2 acidic, basic or The pH of a solution is a measure of its _____ concentration. Show your work. be the nature of salt if the acid and base both are strong, and what will be the nature if one of them is strong and the other is weak. NaOH, sodium hydroxide. salt. Blank 3: electrons Such a species is described as being . Which of the following is not true for a solution at 25C that has a hydroxide concentration of 2.5 10-6 M? Experts are tested by Chegg as specialists in their subject area. Bases are molecules that can split apart in water and release hydroxide ions. The pH of a solution is a logarithmic value. neutral? Above 7, the substance is basic. Createyouraccount. It is a white solid and can be derived from the reaction of ammonia and acetic acid." Pour 60 mL of each of the solutions into separate 100 mL beakers. all of these natures, and if you can't, then don't worry. A solution having a pH of 8.6 would be described as: a. distinctly basic b. slightly basic c. neutral d. slightly acidic e. distinctly acidic. 3.3 10-11 M So let's begin. 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 . And how to find out the it works for everything). Hello, my query is that, is there a way to remember which acid is strong and which base is weak? In contrast, strong acids, strong bases, and salts are strong electrolytes. Acidic b. The strongest acid in an aqueous solution is the hydronium ion. New Questions About Fantasy Football Symbols Answered and Why You Must Read Every Word of This Report. In a Bronsted-Lowry acid-base reaction, equilibrium will favor the _____ if the reacting acid and base are strong. Although the pH values of many familiar solutions fall between 0 and 14, in reality pH values can fall outside this range. This equation is used to find either
In general the stronger an acid is, the _____ its conjugate base will be. Question = Is SiCl2F2polar or nonpolar ? Question = Is if4+ polar or nonpolar ? Which of the following mathematical relationships are correct for an aqueous solution at 25oC? [{Blank}] (acidic, ba. Explain. Reason: 0.00010 M Acid, base, and neutral compounds can be identified easily with the help of pH values and their dissociation constants. HCN is therefore weaker than H2CO3, and the reaction will favor the reactants. Our experts can answer your tough homework and study questions. Bases have a pH between 7 and 14. By definition, a buffer consists of a weak acid and its conjugate weak base. Water I will write it as HOH. In this video, we are Now this means that all the If you're seeing this message, it means we're having trouble loading external resources on our website. are strong and weak. Select all that apply. So we know that acids and We'll also see some examples, like, when HCl reacts with NaOH We can derive a . If a pH is closer to 13, is the substance more acidic or basic? Blank 2: lone , nonbonded, nonbonding, non-bonding, non-bonded, unshared, or unbonded If the pH value is less than seven, then the compound will be acidic, 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 considered as a base. It is considered an acid because it sometimes dissipates into ions in water, one of which is a H+ ion. With reference to the table of Ka values provided, select all the equilibrium acid-base reactions that will favor the products. Blank 2: lone, nonbonded, unbonded, non-bonded, or unshared [H2O] is not included in the Ka expression for a particular acid. A strong acid dissociates completely into ions in water. Explain. Now if you have tried it, let's see. Neutral. Instructions. The solution of a strong acid will have extremely few to no undissociated HA molecules. NH3 is a weak base (Kb = 1.8\times10-5) and so the salt NH4Cl acts as a weak acid. Ammonium hydroxide is a weak base. 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. What is the pH of a solution that is 0.040 M in NH4Cl at 25 C? Does the acetic acid/sodium acetate solution buffer in the acidic, basic, or neutral range? Consider two solutions of the weak acid HCN, one with concentration 0.10 M and one with concentration 0.010 M. Select the statements that correctly describe these solutions. x = 1.1 x 10-5 M which is the H3O+ concentration. Does (NH4)2SO4 when dissolved in water create a solution that is acidic, basic, or neutral? Which of the following factors will affect the relative strength of oxoacids? NH3 or C2H7NO2). 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 . Blank 1: base What is the Ka of butanoic acid? Which of the following options correctly describe a solution with a pH = 8.00? This results in the system automatically collecting data identifying who produced each pair of shoes and how much time it took to make them. water, forming unionized acetic acid and the hydroxide ion. Select all that apply. C5H5NHClO4 The weak conjugate acid of the weak base pyridine is pyrridinium ion. The direction of an acid-base equilibrium depends on the relative strengths of the acids and bases involved. Strong acid molecules are not present in aqueous solutions. In this video we will take up some salts and try to identify their nature based on this table. D. Strongly basic . C2H3O2 is the strong conjugate base of a weak acid. 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. Which of the following statements correctly describes a characteristics of polyprotic acids? The net ionic equation for the hydrolysis of NaC2H3O2 is the following: C2H3O2^- + HOH ==> HC2H3O2 + OH^-. Explain your answer. CH_3COONa. Neutral solution, [H3O+] > [OH-] If you are given a pH and asked to calculate [H+], you would _______. Soluble salts that contain anions derived from weak acids form solutions
{/eq} is dissolved in water, it gives ammonium hydroxide {eq}\rm \left( {N{H_4}OH} \right) participate readily in proton-transfer reactions. 1. ______ metal ions are acidic in aqueous solution because their hydrated form can transfer an H+ to water. So can you pause the video and do all the three steps, and then figure out what is the answer? Na2HPO4 is amphoteric: write the two reactions. Acids accept electron pairs. this is a weak base. Is an aqueous solution of CH3NH3Cl acidic, basic, or neutral? 4) Is the solution of CH3NH3CN acidic, basic or neutral? constant K is very small. 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). [H3O+] = Kw[OH]Kw[OH-] = 1.010143.0104. What is the [H3O+] in a 0.60 M solution of HNO2? For each, state whether the solution is acidic, basic, or neutral. Acidic solutions have a _____ pOH than basic solutions. {/eq} is described as a salt of weak acid that is acetic acid {eq}\left( {C{H_3}COOH} \right) Is ammonium acetate (NH4C2H3O2) acidic, basic, or neutral in pH? Is CH3COOH a strong acid, strong base, weak acid, or weak base? So the strong parent is the acid. Will the soliutions of these salts be acidic, basic or neutral? 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 H+ ion is a hydrogen atom that has lost a (n) and is therefore just a (n) . expression for this interaction and the Ka or Kb value. Calculate [OH-] in a solution that has [H3O+] = 6.7 x 10-2 M. Is the solution acidic or basic? The electronegativity of the central atom (E). What
Select all the statements that correctly describe this system. Select the correct statements describing a solution containing a salt composed of the cation of a strong base and the anion of a polyprotic acid. This For example, NaOH + HCl = NaCl + H2O Since both the acid and base are strong, the salt produced would be neutral. donates an H+. Ammonium hypochlorite, NH_4ClO, is the salt of ammonia, NH_3, and hypochlorous acid, HClO. Direct link to Shresth's post Hello, my query is that, , Posted 3 years ago. now, then don't worry. The reaction of an acid and a base in aqueous solution, in which all H+ ions from the acid react with all the OH- ions from the base is called . The relative strength of an acid or base depends on how high its k a or k b value is, in this case, the k a value is far lower than the k b value, so the ammonia is more strongly basic than ammonium is acidic. All other trademarks and copyrights are the property of their respective owners. Explain. And the equivalence point may move slightly acid, to neutral, to slightly basic, depending upon Ka and Kb of the acid/base system. How Can I See Expired, Disappearing Photos On Instagram? Select ALL the weak acids from the following list. Blank 1: H3O+, hydronium, hydronium ion, or H+ The buffering range covers the weak acid pK a 1 pH unit. Kb for ammonium hydroxide is 1.8 x 10-5 according to the following reaction. An aqueous solution of ammonium acetate acts as a buffer solution. Is HCN acidic, basic or neutral when dissolved in water? Calculate the Ka value for the anilium ion (C6H5NH3+) if Kb for aniline (C6H5NH2) is 4.0 x 10-10. So over here we have a weak acid but a strong base. to be acidic in nature. Select all that apply. All strong acids and bases appear equally strong in H2O. A salt consisting of the anion of a weak _____ and the cation of a strong _____ yields a basic solution. Answer = C2Cl2 is Polar What is polarand non-polar? The chemical formula of ammonium acetate is CH3COONH4. Explain. Is a soft drink with a pH of 3.2 classified as acidic, basic, or neutral? Which of the following are products of the reaction between the strong acid HCl and the strong base NaOH? .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). Consider the reaction below : H2O + HF \rightarrow Generates hydroxide when it reacts with water. Blank 4: acid. we will have to talk about many more concepts so only digits after the decimal point are significant. Now if you have tried it, let's see. Explain. Perbromic acid is unstable and cannot be formed by displacement of chlorine from perchloric acid, as periodic acid is prepared; it can only be made by protonation of the perbromate ion. You can go back and watch the video again. Answer = IF4- isNonpolar What is polarand non-polar? If the Ka of the cation is greater than the Kb of the anion, a solution of the salt will be ______. Select all that apply. Is H_2PO_4^- an Arrhenius acid, an Arrhenius base, a Br\varnothing. Baking soda and ammonia, common household cleaners, are a. Select all that apply. A short quiz will follow. First, write the equation for the dissolving process, and examine each
nature of this salt, whether this is acidic, basic, or neutral? See, to understand this Thus the conjugate base Cl- is _____ because its conjugate acid HCl is strong. I hope you can remember raise 10 to the power of the negative pH value. Is the solution of NH_4C_2H_3O_2 acidic, basic or neutral? (0.500). 1 . {/eq} acidic, basic, or neutral? For the NH4^+, it is much easier to write BOTH as half reactions. A Lewis acid absorbs an electron pair from a Lewis base, resulting in the formation of a coordinate covalent bond. A Bronsted-Lowry base is a proton . 2) Is the solution of NH4NO2 acidic, basic or Example: What is the pH of a 0.400 M KBr solution? Metal cations act like ______ when dissolved in water. So see, we have seen earlier H+ and hydroxide, OH-. An acid donates a proton to form its conjugate , which therefore has one less atom and one more charge than its acid. Acidic. A species that contains one or more atoms as well as one or more electron pairs can act as either an acid or a base, depending on the reaction. Water is usually add, Posted 10 days ago. water, forming ammonia and the hydronium ion. englewood section 8 housing. Make an "ICE" chart to aid in the solution. While you may have never heard of darmstadtium, believe it or not, it has something in common with gold, oxygen, and lead. NH3 is a weak base (Kb = 1.8\times10-5) and so the salt NH_4Cl acts as a weak acid. Question = Is C2Cl2polar or nonpolar ? ions of both of these. 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? What is the pH of a solution that is 0.0260 M in CH_3NH_3NO_3 at 25^\circ C? Mixture 2, reaction of a strong base and weak acid, also goes to completion. Which of the following common household substances are acids? This solution could be neutral, but this is dependent on the nature of their dissociation constants. Example: The Kb for aniline is 3.8 x 10-10. If something shiny has ever caught your eye, chances are it was made of metal! Which of the following statements accurately describe Bronsted-Lowry acid-base reactions? Which of the following options correctly reflect the steps required to calculate the pH of a solution containing 0.150 M KCN? Kb = 5.9 x 10-10. What
Earn Transferable Credit & Get your Degree, Get access to this video and our entire Q&A library. Will the salt ammonium iodide be acidic, basic, or neutral in a water solution? HSO3- is the conjugate acid of SO32-. Which of the following anions will produce a neutral solution in water? The solution contains a significant concentration of the weak base CN-. Because Ka for a weak acid HA is ______, we can assume [HA]equilibrium [HA]initial. salt that gets formed takes the nature of the strong parent. Is an aqueous solution of KBrO4 acidic, basic, or neutral? Which of the following species are Lewis acids? Select all that apply. All materials are barcoded. Blank 2: base Weak . HF + OCl- F- + HOCl, Acidic solution The 0.10 M solution will have a higher [H3O+]. An acid is any hydrogen-containing substance that is capable of donating a proton (hydrogen ion) to another substance. What is the pH of a solution that is 0.029 M in NH_4Cl at 25 C? This means that CH3COO- is a ______ base than F-. Direct link to Mahaty's post Perhaps they gain the cha, Posted 3 years ago. b) Neutral because there is no hydrolysis. Second, write the equation for the reaction of the ion with water and the
It will dissociate to NH4+ and C2H3O2- both are a weak acid (NH4) and weak base (C2H3O2) so Ka of NH4 is ~ to the Kb of acetate (C2H3O2) anion so overall the pH value wouldclose to7.00or. So in aqueous medium, K2S will be basic in nature. For nonmetal hydrides, acid strength increases from left to right across a period and increases down a group. HOWEVER, Ka = Kb, so the solution is neutral. If yes, kindly write it. 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. Will NH4NO3 form an acidic, basic, or neutral solution when dissolved in water? NH4NO3 is the conjugate acid of the weak base ammonium hydroxide (NH4OH) and the strong acid nitric acid (HNO3). So let's do that. Anion has no effect on pH b/c they're the conjugate bases of strong acids. - aci. NH4NO3 is the conjugate acid of the weak base ammonium hydroxide (NH4OH) and the strong acid nitric acid (HNO3). For example, the acetate ion is the conjugate base of acetic acid, a weak acid. Soluble salts that contain cations derived from weak bases form solutions
Reason: Salts can be characterized from the type of acid and base which combine in the neutralization reaction. So this time I have the salt Bronsted-Lowry acid Since two . Factory workers work individually at specially designed U-shaped work areas equipped with several machines to assist them in completely making a pair of shoes. Kb for ammonium hydroxide is 1.8 x 10-5 according to the following reaction.. c. Basic. Which of the following species could act as EITHER an acid OR a base? Molecules with electron deficient central atoms. ion functions as a weak acid, the equilibrium constant is given the label
HCN is a _____ acid than acetic acid and will therefore have a _____ pKa value. We use cookies to ensure that we give you the best experience on our website. Hydrogen cyanide (HCN) is a weak acid with Ka = 6.2 10-10. Write the following chart on the board Color PH . is as follows: Where Ka is the ionization constant of the acid form of the pair, Kb
An acid-base reaction can therefore be viewed as a proton- process. The electronegativity of the central nonmetal atom The simplified proton balance will be true only at a p H that is exactly in the middle of the two p K a -values. Sodium acetate, CHCOONa. c. Basic. Share this. Is an aqueous solution of CoF2 acidic, basic, or neutral? Pause the video and think about this. The equilibrium expression for this reaction
Now the second step was to find out the nature of the base and acid, right? the nature of the salt. This is the most wide-ranging of the three (i.e. Select all that apply. Since "x" represents the hydroxide
So this is the first step. Hence, H2PO4- can be treated as a weak, base as it is the conjugate base of a weak acid. We will make the assumption that since Kb is so small that the value
Acidic. Ammonium acetate is an ammonium salt obtained by reaction of ammonia with acetic acid. Indicate whether the following salts will produce basic, acidic, or neutral pH when dissolved in water. So you have NH. Answer = SiCl2F2 is Polar What is polarand non-polar? 2. Since acetate
ionization constant for water. Select all that apply. Start with the first step at the top of the list. Is NH4CN acidic, basic, or neutral? Direct link to mondirapaul26's post could someone please redi. All hydrohalic acids in Period 3 or below, Correctly order the steps necessary to solve weak-acid equilibria problems. In terms of the Arrhenius definition of acids and bases, neutralization is described as _______. So this is the salt that is given. What are the species that will be found in an aqueous solution of NH4OH? 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. Which of the following statements does NOT describe a type of weak acid? Oxoacids where the number of O atoms exceeds the number of ionizable H atoms by 2 or more: HNO3, H2SO4, and HClO4. KOH is a strong base while H2S is a weak acid. In this case, since both acetic acid and NH4OH have about the same Ka (or Kb), then the NH4C2H3O2 is about neutral. Is NaCN acidic, basic, or neutral? K+ is a neutral ion and CN- is a basic ion. Example: Calculate the pH of a 0.500 M solution of KCN. Select all that apply. 2. The cation is the conjugate acid of a weak base. We can derive a general buffer equation by considering the following reactions for a weak acid, HA, and the soluble salt of its conjugate weak Exp 16 Buffer solution Sp07. Classify an aqueous solution with H+ = 9.8 x 10-12 M as acidic, basic, or neutral. Classify an aqueous solution with OH- = 5.0 x 10-10 M as acidic, basic, or neutral. A Bronsted-Lowry acid is a proton _____ and must therefore contain at least one ionizable _____ atom in its formula. 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). For solutions with the same initial concentration of acid HA, the smaller the value of Ka, the _____ the % dissociation and thus the _____ the acid. [{Blank}] (acidic, basic, neutral) (2) What are the acid-base properties of the anion? Which of the protons depicted in the structure of acetic acid is considered acidic or ionizable?