You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Is an aqueous solution with OH- = 2.2 x 10-10 M acidic, basic, or neutral? Explain. Creative Commons Attribution/Non-Commercial/Share-Alike. following volumes of added NaOH (please show your work): ii. Note that there is no $\ce {OH-}$ to start with (very little in reality), so equation $ (1)$ is not applicable. this solution? This is similar to the reason why the chloride ion (and the sodium ion) in NaCl does not affect the pH of the solution. H 3 O; C 6 H 5 NH 2 Cl; . AboutTranscript. Explain. Is an aqueous solution with OH- = 4.72 x 10-9 M acidic, basic, or neutral? So Kb is equal to 5.6 x 10-10. Now it is apparent that $\ce {H3O+}$ makes it acidic. About Press Copyright Contact us Creators Advertise Developers Terms Privacy Policy & Safety How YouTube works Test new features Press Copyright Contact us Creators . Explain. I mean its also possible that only 0.15M dissociates. concentration of hydroxide ions. Business Studies. Direct link to Ernest Zinck's post When we have 0.25 - x, we, Posted 8 years ago. Explain. is a conjugate acid-base pair, and the Ka value for acetic acid is easily found in most text books, and the Ka value is equal to 1.8 x 10-5. Explain. Is a solution with OH- = 1 x 10-6 M acidic, basic, or neutral? All rights reserved. The base which a certain acid turns into.Every acid had a conjugate base:HX (acid) X- (conjugate base)The acid is also called the base's conjugate acid. Explain. Explain. Our calculator may ask you for the concentration of the solution. Is a solution with H+ = 7.8 x 10-3 M acidic, basic, or neutral? Is an aqueous solution with OH- = 3.91 x 10-9 M acidic, basic, or neutral? Is an aqueous solution with pOH = 5.12 acidic, basic, or neutral? Is an aqueous solution with pOH = 2.17 acidic, basic, or neutral? In case of acetate ion, its conjugate acid CH3COOH, while definitely a relatively 'weak' acid', isn't weaker than water, so its conjugate base is a weak base. concentration of acetate would be .25 - X, so Explain. a. 4. So: X = 1.2 x 10-5 Alright, what did X represent? All rights reserved. Is an aqueous solution with pOH = 6.48 acidic, basic, or neutral? Question = Is C2Cl2polar or nonpolar ? dissociates in water, has a component that acts as a weak acid (Ka Molecules can have a pH at which they are free of a negative charge. alright, I saw in a couple places that CH3NH3Br and CH3NH3Br were salts of CH3NH2 and HBr/HCl but they were probably just wrong. Calculators are usually required for these sorts of problems. is titrated with 0.300 M NaOH. Is an aqueous solution with H+ = 2.3 x 10-10 M acidic, basic, or neutral? the Kb value for this reaction, and you will probably not be Is an aqueous solution with pOH = 1.17 acidic, basic, or neutral? It's going to donate a proton to H2O. Is an aqueous solution with OH- = 2.8 x 10-6 M acidic, basic, or neutral? Is an aqueous solution with OH- = 3.4 x 10-2 M acidic, basic, or neutral? Is an aqueous solution with pOH = 2.0 acidic, basic, or neutral? Identify the following solution as acidic, basic, or neutral. Is a 0.1 M solution of NH3 acidic or basic? https://en.wikipedia.org/wiki/Base_(chemistry), https://en.wikipedia.org/wiki/Salt_(chemistry), https://en.wikipedia.org/wiki/Neutralization_(chemistry). Okay. Explain. Explain. In this case, it does not. (a) KCN (b) CH_3COONH_4. Question: Is C2H5NH3CL an acid or a base? Arrhenius's definition of acids and bases. How would you test a solution to find out if it is acidic or basic? Is an aqueous solution with pOH = 3.88 acidic, basic, or neutral? Direct link to RogerP's post This is something you lea, Posted 6 years ago. The overall salt does not donate protons, the CH3NH3+ ion does (to form H3O+) when the salt is dissociated in water. Is a solution with OH- = 7.3 x 10-8 M acidic, basic, or neutral? 10 to the negative five. Is an aqueous solution with pOH = 5.27 acidic, basic, or neutral? So if you add an H+ to CH3NH2 + HBr -----> CH3NH3+ + Br- However, the methylammonium cation Our experts can answer your tough homework and study questions. Is a solution with OH- = 1.99 x 10-7 M acidic, basic, or neutral? Three different theories define acid and base: According to the Arrhenius theory, in an aqueous solution, an acid is a substance able to donate hydrogen ions, while a base donates hydroxide ions. Is an aqueous solution with OH- = 5.0 x 10-5 M acidic, basic, or neutral? And if we pretend like View all equations with C6H5NH2 as reactant, View all equation with C6H5NH3Cl as product. Explain. 8.00 x 10-3. g of . Direct link to Matthew Chen's post In theory, you could figu, Posted 7 years ago. Select your chemical and its concentration, and watch it do all the work for you. So for a conjugate acid-base pair, Ka times Kb is equal to Kw. The amount of acid and base conjugates in the buffer are twice the amount of added acid.) C6H5NH3+, conjugate base is a weak base, therefore it is potentially acidic NO2-, conjugate acid is a weak acid, therefore the salt is also potentially basic However, since the Ka > Kb, the solution must be acidic So it has both nature acidic on basic in its constituent, it will act as a neutral soul. So we need to solve for X. Just nitrogen gets protonated, that's where the cation comes from. Post author By ; qalipu first nation membership list Post date June 11, 2022; white spots on tan skin that won't tan . Forgot username/password? [Hint: this question should The conjugate bases of strong acids, and the conjugate acids of strong bases, do not react appreciably with water, whereas this is not the case with weak acids and bases. Explain. ; or example, hydrochloric acid is an acid because it forms H + when it dissolves in water. Is an aqueous solution with OH- = 3.43 x 10-9 M acidic, basic, or neutral? Most bases are minerals which form water and salts by reacting with acids. Next, we think about the change, and since NH4+ turns into NH3, whatever we lose for NH4+ is what we gain for NH3. {/eq} solution is acidic, basic, or neutral. Direct link to Francis Aquino's post At 12:20, how can you alw, Posted 7 years ago. So let's go ahead and do that. Is an aqueous solution with OH- = 2.19 x 10-9 M acidic, basic, or neutral? Explain. Explain. Explain. Direct link to Krishna Phalgun's post Metals like potassium and, Posted 8 years ago. Question = Is SbCl5 ( Antimony pentachloride ) polar or nonpolar ? [OH^-]= 4.2 x 10^-4 M is it basic neutral or acid 2. . Anyway, you have apparently made important progress. Is an aqueous solution with OH- = 8.54 x 10-9 M acidic, basic, or neutral? pH measures the concentration of positive hydroge70n ions in a solution. Benzoic acid (C 6 H 5 COOH) and aniline (C 6 H 5 NH 2 ) are both derivatives of benzene. Is an aqueous solution with OH- = 5.0 x 10-12 M acidic, basic, or neutral? Strong base + strong acid = neutral salt. Solutions with a pH that is equal to 7 are neutral. So are we to assume it dissociates completely?? Determine whether a 0.0100 M C6H5NH3F solution is acidic, basic, or neutral. Ks = [Ca2+][F-]2 (b) (i) Calculate the solubility of calcium fluoride in mol L-1, at this temperature. hXnF
ol.m]i$Sl+IsCFhp:pk7! We know Kb is 1.8 x 10-5 This is equal to: 1.0 times concentration of X for NH4+ we gain the same concentration, X, for NH3 And therefore, we've also gained the same concentration for hydronium as well. Is a solution with OH- = 4.00 x 10-5 M acidic, basic, or neutral? Polyprotic acids and bases are those that release more than one proton or hydroxide ion respectively when dissolved in water. Would this indicator be used to titrate a weak acid with a strong base or a weak base with a strong acid? We're trying to find Ka. In chemistry, bases are substances that, in aqueous solution, are slippery to the touch, taste astringent, change the color of indicators (e.g., turn red litmus paper blue), react with acids to form salts, promote certain chemical reactions (base catalysis), accept protons from any proton donor, and/or contain completely or partially . Is a 1.0 M KBr solution acidic, basic, or neutral? Explain. binance futures adjust leverage on open position; supply a suitable simple past or past perfect tense; st johns county sheriff pay scale; university for humanistic studies california Explain. Start over a bit. pH = - log10([H+]). Some species are amphiprotic (both acid and base), with the common example being water. which is what we would expect if we think about the salts that we were originally given for this problem. Calculate the base 10 logarithm of this quantity: log10([H+]). Determine whether a 0.0100 M NaF solution is acidic, basic, or neutral. The pH of the solution 8.82. Is a solution with OH- = 1.6 x 10-3 M acidic, basic, or neutral? So let's go ahead and write that down. Is an aqueous solution with OH- = 1.57 x 10-9 M acidic, basic, or neutral? What are the chemical and physical characteristic of HCl (hydrogen chloride)? Explain. Is an aqueous solution with pOH = 3.35 acidic, basic, or neutral? NH 4 CN - salt from a weak acid (HCN) and a weak base (NH 3) - pH will depend on the Ka and Kb. Bases include the metal oxides, hydroxides, and carbonates. Explain. Is an aqueous solution with OH- = 9.0 x 10-4 M classified as acidic, basic, or neutral? Click the card to flip . Taking them one at a time, we have NaNO2 - salt from a weak acid (HNO2) and a strong base (NaOH) - pH will be >7 (alkaline), KI - salt from a strong acid (HI) and a strong base (KOH) - pH will be neutral = 7, HONH3Br - salt from a strong acid (HBr) and a weak base (HONH2) - pH will be <7 (acidic). The pH scale (pH) is a numeric scale used to define how acidic or basic an aqueous solution is. {/eq}. CH3COO-, you get CH3COOH. Explain. One "rule of thumb" that I learned is if your x ends up being larger than 5% of your starting value you need to solve the quadratic. Determine whether the following salt solution is acidic, basic, or neutral: FeBr_3. Explain. Calculate the pH of a solution containing the result of the addition of 0.5 moles HCl to a Explain. Explain. Please show. The equivalence point [Hint: at this point, the weak acid and Explain. Will an aqueous solution of KClO2 be acidic, basic, or neutral? Explain. Consider the following data on some weak acids and weak bases: acid Ka base name formula Kb name formula acetic acid HCH , CO 2 1.8 x 10 aniline C 6 H 5 NH2 4.3 x 10 - 10 hydrocyanic acid HCN 4.9 x 10 10 hydroxylamine HONH2 1.1 x 10 - 8 Use this data to rank the following solutions in order of increasing pH. Chapter 16, Exercises #105. Question: Is calcium oxidean ionic or covalent bond ? We can call it [H+]. Is an aqueous solution with OH- = 3.47 x 10-6 M acidic, basic, or neutral? Explain. Bases are the chemical opposite of acids. Next, we think about the change. concentration of our reactants, and once again, we ignore water. A) is capable of donating one or more H B) causes an increase in the concentration of in aqueous solutions C) can accept a pair of electrons to form a coordinate . of hydroxide ions. The given salt compound formula unit corresponds to methylammonium chloride, which we write divided into two portions: It will dissociate in liquid water in a 1:1 ratio of methylammonium cations and chloride anions: {eq}\rm CH_3NH_3Cl (s) \rightarrow CH_3NH_3^+ (aq) + Cl^- (aq) Is an aqueous solution with pOH = 3.54 acidic, basic, or neutral? wildwoods grill food truck menu Explain. Accounting & Finance; Business, Companies and Organisation, Activity; Case Studies; Economy & Economics; Marketing and Markets; People in Business [H+] = 4.21*10^-7 M b. JavaScript is disabled. Explain. The acid and base chart is a reference table designed to make determining the strength of acids and bases simpler. Alternatively, you can measure the activity of the same species. The unit for the concentration of hydrogen ions is moles per liter. 308 0 obj
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Aniline, a weak base, reacts with water according to the reaction. Note: in the first four problems, I give the K a of the conjugate acid (for example, the ammonium ion in Example #1). Explain. Is an aqueous solution with OH- = 1.0 x 10-8 M acidic, basic, or neutral? Is an aqueous solution with OH- = 9.48 x 10-7 M acidic, basic, or neutral? It can be protonated to form hydronium ion or deprotonated (dissociated) to form . Is a solution with H+ = 2.7 x 10-9 M acidic, basic, or neutral? Explain. The concentration of This is all over, the Explain. Said stronger city weak base or strong base. You are right, protonation reaction is shifted (almost) completely to the right. Explain. We are not saying that x = 0. Explain. lose for the acetate anion, we gain for acetic acid. Is a solution of the salt KNO3 acidic, basic, or neutral? Explain. And we're starting with .25 molar concentration of sodium acetate. 2, will dissolve in 500 mL of water. down here and let's write that. June 11, 2022 Posted by: what does dep prenotification from us treas 303 mean . This feature is very important when you are trying to calculate the pH of the solution. [OH^-]= 7.7 x 10^-9 M is it. Explain. X represents the concentration Calculate the pH of a 5.4010-1 M aqueous solution of aniline hydrochloride (C6H5NH3Cl). Is an aqueous solution with pOH = 12.33 acidic, basic, or neutral? X over here, alright? 8.00 x 10-3 g of CaF2 will dissolve in 500 mL It may not display this or other websites correctly. How to classify solution either acidic, basic, or neutral? Okay, in B option we have ph equal to 2.7. It is a salt compound that will dissociate in a 1:1 ratio of anilinium cations and chloride anions: Our experts can answer your tough homework and study questions. What are the chemical and physical characteristic of C6H5NH3Cl (Aniline hydrochloride; C.I.76001; Benzenamine hydrochloride)? To tell if KCl forms an acidic, basic (alkaline), or neutral solution we can use these three simple rules along with the neutralization reaction that formed KCl. So NH4+ is going to function as an acid. Most drugs are ionizable organic compounds 75% weak bases 20% weak acids The remainder are neutral or quaternary ammonium compounds What is the Bronsted-Lowry acid-base method? Explain. So let's make that assumption, once again, to make our life easier. Direct link to Ernest Zinck's post Usually, if x is not smal. Take the additive inverse of this quantity. To calculate the pH of a buffer, go to the, Check out 20 similar mixtures and solutions calculators , How to calculate pH? of CH3COOH times the concentration of hydroxide, so times the concentration of OH- this is all: over the Direct link to Apoorva Doshi's post What is the guarantee tha, Posted 7 years ago. Explain. Explain. and we're going to take 5.6 x 10-10, and we're why did alex and ellen breakup on family ties; medical record keeping guidelines; elle uk media kit 2021; trey baxter model. Explain. Is a solution with H+ = 7.0 x 10-13 acidic, basic, or neutral? = 2.4 105 ). Answer = C2Cl2 is Polar What is polarand non-polar? Explain. Determine the solution pH at the Therefore, it has no effect on the solution pH. Question = Is IF4-polar or nonpolar ? So, we could find the pOH from here. Explain. Is an aqueous solution with pOH = 5.65 acidic, basic, or neutral? Since Kb for NH3 is greater than the Ka for HCN,( or Kb CN- is greater than Ka NH4+), this salt should have a pH >7 (alkaline). Explain how you know. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Calculate pH by using the pH to H formula: Of course, you don't have to perform all of these calculations by hand! Identify whether a solution of each of the following is either acidic, basic or neutral. Is an aqueous solution with OH- = 6.89 x 10-12 M acidic, basic, or neutral? So we're rounding up to Explain. (b) Assuming that you have 50.0 mL of a solution of aniline Explain. of hydronium ions, so this is a concentration, right? Explain. H3PO4) its a bit more complicated and we need to use Ka and Kb to determine the pH of the resulting solution.More chemistry help at http://www.Breslyn.org. Group 1 uses a ruler to depict the base of the shape and completes the semi-circle with a pencil. ; Brnsted-Lowry theory says that acid can donate protons while a base can accept them. And our goal is to find the Kb. this solution? Explain. Is an aqueous solution with pOH = 7.98 acidic, basic, or neutral? Explain. Now you know how to calculate pH using pH equations. Is an aqueous solution with pOH = 3.27 acidic, basic, or neutral? to the negative log of the hydroxide ion concentration. 0
concentration for the hydroxide. That was our original question: to calculate the pH of our solution. So X is equal to 5.3 times Acidic/Basic Salt Compound: The Bronsted-Lowry theory of acids and bases describes a transfer of ionized hydrogen atoms (protons) from acids to bases in an aqueous solution. See Answer See Answer See Answer done loading. Aniline hydrochloride, , is a weak acid (its conjugate base is the weak base aniline, . Explain. 2014-03-28 17:28:41. Salt of a Weak Base and a Strong Acid. Explain. Is an aqueous solution with OH- = 4.88 x 10-7 M acidic, basic, or neutral? So at equilibrium, our 0.0100 M NaF = Basic because NaF is a which has Na+ and F- ions out of which F- reacts as a base with water. Is an aqueous solution with H+ = 4.2 x 10-5 M classified as acidic, basic, or neutral? So this is 5.6 x 10-10 = X2 over 0.25 So now we need to solve for X. And so I go over here and put "X", and then for hydroxide, See the chloride ion as the conjugate base of HCl, which is a very strong acid. Question = Is C2H6Opolar or nonpolar ? Label Each Compound With a Variable. Is a solution with H+ = 1.4 x 10-11 M acidic, basic, or neutral? We're gonna write Ka. For example, the pH of blood should be around 7.4. Explain. Is an aqueous solution with OH- = 9.8 x 10-7 M acidic, basic, or neutral? reaction is usually not something you would find NH3 + HCl -----> NH4+ + Cl-Instead of ammonia, a nitrogen-base can be an amine such as methylamine, CH3NH2. So, at equilibrium, the What is the pH of .15 M methylammonium bromide, CH3NH3Br (Kb of CH3NH2 = 4.4x10^-4), CH3NH3 (aq) + H2O (l) <=> CH3NH2 (aq) + H3O+ (aq), When dissolved methylammonium bromide dissociates to CH, am I able to use the same equilibrium constant for CH3NH2+ as I do with CH3NH2? Is a solution with OH- = 1 x 10-9 M acidic, basic, or neutral? So we can once again find talking about an acid-base, a conjugate acid-base pair, here. Explain. be X squared over here And once again, we're In a full sentence, you can also say C6H5NH2 reacts with HCl (hydrogen chloride) and produce C6H5NH3Cl (Aniline hydrochloride; C.I.76001; Benzenamine hydrochloride) Phenomenon after C6H5NH2 reacts with HCl (hydrogen chloride) Click to see equation's phenomenon What are other important informations you should know about reaction Explain. Is an aqueous solution with OH- = 1.47 x 10-3 M acidic, basic, or neutral? Is an aqueous solution of Na2SO3 acidic, basic, or neutral? Is an aqueous solution with pOH = 8.55 acidic, basic, or neutral? So, the only acidic salt would be HONH3Br, so it would get a ranking of "1", Next comes the neutral salt KI, with a ranking of "2", NaNO2 would have the next lowest pH so ranking "3", NH4CN would have the highest pH with a ranking of "4", This is all based on hydrolysis of the salts. weak conjugate base is present. Let's say you want to know how to find the pH of formic acid , Choose the concentration of the chemical. Is an aqueous solution with OH- = 2.29 x 10-8 M acidic, basic, or neutral? Often, these problems are given with the K b of the base and you have to calculate the value of the K a.You do so with this equation: K a K b = K w. You will see such a situation starting in the fifth example as well as scattered through the additional problems. Is an aqueous solution with OH- = 1.79 x 10-7 M acidic, basic, or neutral? Discover what acidic and basic salts are, see examples, and predict the pH of salt solutions.
Choose an expert and meet online. You may also refer to the previous video. Answer = if4+ isPolar What is polarand non-polar? Whichever is stronger would decide the properties and character of the salt. Next, we need to think about Determine whether the following salt solution is acidic, basic, or neutral: Sr(ClO_4)_2. 289 0 obj
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Explain. Need Help? Calculate the concentration of C6H5NH3+ in this buffer solution. What is not too clear is your description of "lopsided". Is an aqueous solution with OH- = 4.84 x 10-4 M acidic, basic, or neutral? Explain. Measure the concentration of hydrogen ion in the solution. Get a free answer to a quick problem. 10 to the negative six. Alright, so let's go ahead and write our initial concentrations here. Calculate the Ph after 4.0 grams of. .25, and if that's the case, if this is an extremely small number, we can just pretend like So, NH4+ and NH3 are a endstream
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Explain how you know. soln. (b) Assuming that you have 50.0 mL of a solution of aniline hydrochloride with a concentration of 0.150 M, what is the pH of this solution? When we ran this reaction, there was excess weak base in solution with . The acid can be titrated with a strong base such as NaOH. Calculate [H^+] for each of the following solutions and indicate whether the solution is acidic, basic, or neutral. Is an aqueous solution with OH- = 4.25 x 10-4 M acidic, basic, or neutral? What are the chemical and physical characteristic of C6H5NH2 ()? Salts that form from a weak acid and a strong base are basic salts, like sodium bicarbonate (NaHCO3). Explain. Is a solution with H+ = 8.3 x 10-10 M acidic, basic, or neutral? So I could take the negative Explain. Most questions answered within 4 hours. Is an aqueous solution with pOH = 10.57 acidic, basic, or neutral? Explain. The pH value is logarithmically and is inversely related to the concentration of hydrogen ions in a solution. hydroxide would also be X. Alright, next we write our Explain. Please show your work. Explain. It can convert pH to H+, as well as calculate pH from the ionization constant and concentration. So we can get out the calculator here and take 1.0 x 1014, I think the 'strong base if weak conjugate acid' argument only really works if the conjugate acid is less acidic than water. is basic. (a) Write the solubility product expression, K s, for calcium fluoride . The total number of stars for this article is: C6H5NH2 + HCl = C6H5NH3Cl | Chemical Equation. eventually get to the pH. Is an aqueous solution with OH- = 2.7 x 10-5 M acidic, basic, or neutral? Predict whether the solution is acidic, basic, or neutral, and explain the answer. Explain. Is an aqueous solution with OH- = 9.42 x 10-8 M acidic, basic, or neutral? Is an aqueous solution with OH- = 9.41 x 10-9 M acidic, basic, or neutral? *$R'!xHj@LQ(H-:Z -VF(k#C$:NH+6?qab1. Direct link to Kylee Webb's post at 8:48 why did you not i, Posted 8 years ago. Explain. For example, in determining ranking between NaNO2 and NH4CN, one looks at hydrolysis where NO2- ==>HNO2 + OH- and compares it to CN- ==> HCN + OH-. Explain. Explain. It's: 1.8 times 10 to the negative five. So it will be a strong acid because as the value of ph decrease, so acidity of the solution will be increased. Acids, Bases and Salts OH MY!!! Explain. Createyouraccount. Next, we need to think about the Ka value. A total of seven acids are widely regarded as "strong" acids in the field of chemistry. Is an aqueous solution with OH- = 3.59 x 10-3 M acidic, basic, or neutral? Benzoic acid is an acid with K a = 6.3 10 -5 and aniline is a base with K a = 4.3 10 -10 . Explain. Explain. Explain. Is an aqueous solution with OH- = 6.10 x 10-9 M acidic, basic, or neutral? salt. The reaction of the weak base aniline, C6H5NH2, with the strong acid hydrochloric acid yields aniline hydrochloride, C6H5NH3Cl. Experts are tested by Chegg as specialists in their subject area. Calculate the equilibrium constant, K b, for this reaction. Hydrochloric acid (denoted by the chemical formula HCl) Hydrobromic acid (denoted by the chemical formula HBr) Hydroiodic acid or hydriodic acid (denoted by the chemical formula HI) Sulfuric acid (denoted by . Createyouraccount. the pH of our solution. Is an aqueous solution with OH- = 9.8 x 10-7 M acidic, basic, or neutral? The most universally used pH test is the litmus paper. What is the hydronium ion concentration of a 0.163 M solution of aniline hydrochloride at 25C given that the value of Kb for aniline is 4.30010-10? He assumes that the initial concentration of NH4+ is equal to the total concentration of NH4Cl in solution. In that case answers would change. solution of sodium acetate. So whatever concentration we basic solution for our salts. (10 pts) HIn H+ + In-(Red) (Yellow) The indicator changes colors at pH = pK a = -log(7.9 x 10-6) = 5.1 This indicator is used for a weak base - strong acid titration. Why doesn't Na react with water? The concentration of Explain. salt. Is an aqueous solution with OH- = 8.0 x 10-10 M acidic, basic, or neutral? hydrochloride with a concentration of 0.150 M, what is the pH of What is the hydronium ion concentration of a 0.163 M solution of aniline hydrochloride at 25C given that the value of Kb for aniline is 4.3001010? answered 04/06/19, Ph.D. University Professor with 10+ years Tutoring Experience. right; first I was confused why I kept on being told that CH3NH3Br went right to CH3NH3+ and Br- now I see how it gets there.