Is an aqueous solution with pOH = 12.33 acidic, basic, or neutral? Click the card to flip . Is an aqueous solution with OH- = 5.0 x 10-5 M acidic, basic, or neutral? (Its conjugate base is the weak base aniline, C 6 H 5 NH 2 .) 308 0 obj <>/Filter/FlateDecode/ID[]/Index[289 47]/Info 288 0 R/Length 99/Prev 436817/Root 290 0 R/Size 336/Type/XRef/W[1 3 1]>>stream Is a solution with OH- = 7.3 x 10-8 M acidic, basic, or neutral? This acid-base chart includes the K a value for reference along with the chemical's formula and the acid's conjugate base. Explain. Explain. 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 . Start over a bit. Is a solution with OH- = 1.53 x 10-7 M acidic, basic, or neutral? Ka on our calculator. This is all over, the Apart from the mathematical way of determining pH, you can also use pH indicators. That is what our isoelectric point calculator determines. Explain. Identify the following solution as acidic, basic, or neutral. Is a solution with H+ = 7.8 x 10-3 M acidic, basic, or neutral? Is an aqueous solution with pOH = 4.78 acidic, basic, or neutral? Salts that form from a strong acid and a weak base are acid salts, like ammonium chloride (NH4Cl). Is an aqueous solution with pOH = 2.0 acidic, basic, or neutral? What are the chemical reactions that have HCl (hydrogen chloride) as reactant? hydronium ions at equilibrium is X, so we put an "X" in here. going to react with water, but the acetate anions will. pH of our solution, and we're starting with .050 molar Get access to this video and our entire Q&A library, Acidic & Basic Salt Solutions: Explanation & Examples. Explain. Now, you can also easily determine pOH and a concentration of hydroxide ions using the formulas: Alternatively, you can find a chemical from the lists (of acids or bases). What is not too clear is your description of "lopsided". So CH3COO-, the acetate have sodium ions, Na+, and acetate anions, CH3COO-, and the sodium cations aren't Creative Commons Attribution/Non-Commercial/Share-Alike. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. To log in and use all the features of Khan Academy, please enable JavaScript in your browser. The reverse is true for hydroxide ions and bases. The unit for the concentration of hydrogen ions is moles per liter. Explain. [Solved] conjugate base and acid relationship Consider the following An aqueous solution contains dissolved C6H5NH3Cl and C6H5NH2. The higher the concentration of hydroxide ions from base molecules, the higher the pH of the solution and, consequently, the higher its basicity. down here and let's write that. On the basis of ph we will classify all the options. acting as an acid here, and so we're gonna write Is a solution with OH- = 4.8 x 10-3 M acidic, basic, or neutral? hbbd```b``5 i d-,`0b`R,&*e`P 6 bvy p#x9@ c Explain. Okay, in B option we have ph equal to 2.7. Explain. concentration for the hydroxide. (a) KCN (b) CH_3COONH_4. Explain. The production of hydroxide ions on dissolving in an aqueous solution shows the basic nature of CH 3 NH 2. Distinguish if a salt is acidic or basic and the differences. A total of seven acids are widely regarded as "strong" acids in the field of chemistry. of CH3COOH times the concentration of hydroxide, so times the concentration of OH- this is all: over the Is an aqueous solution with OH- = 8.76 x 10-4 M acidic, basic, or neutral? Is a solution with pOH = 3.34 acidic, basic, or neutral? Is a solution with OH- = 1 x 10-9 M acidic, basic, or neutral? Explain. 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? Next comes the neutral salt KI, with a . So let's make that assumption, once again, to make our life easier. Is an aqueous solution with OH- = 1.47 x 10-3 M acidic, basic, or neutral? The pH of our stomach varies from 1.5 to 3.5: our stomach is quite acidic! Is an aqueous solution with OH- = 0.0000015 M acidic, basic, or neutral? We can call it [H+]. HCl. Is an aqueous solution with OH- = 3.59 x 10-3 M acidic, basic, or neutral? [OH^-]= 7.7 x 10^-9 M is it; Determine whether a 0.0100 M NaF solution is acidic, basic, or neutral. [OH^-]= 7.7 x 10^-9 M is it. Direct link to sandracizinando's post I thought the acetate was, Posted 8 years ago. Explain. For polyprotic acids (e.g. Is an aqueous solution with OH- = 9.4 x 10-6 M acidic, basic, or neutral? Explain. This produces a dissociation reaction to form the constituent ions in a certain stoichiometry. And so I go over here and put "X", and then for hydroxide, Is an aqueous solution with OH- = 2.29 x 10-8 M acidic, basic, or neutral? Three different theories define acid and base: The higher the concentration of hydrogen ions from acid molecules, the lower the pH of the solution and, consequently, the higher its acidity. So X is equal to the c6h5nh3cl acid or base. Explain. Is a solution with H+ = 2.0 x 10-3 M acidic, basic, or neutral? (a) Identify the species that acts as the weak acid in this How do you know? Is an aqueous solution with pOH = 2.17 acidic, basic, or neutral? When we ran this reaction, there was excess weak base in solution with . Aniline hydrochloride, (C 6 H 5 NH 3 )Cl, is a weak acid. (Its Question: Is calcium oxidean ionic or covalent bond ? Explain. Explain. Explain. Is an aqueous solution of {eq}CH_3NH_3Cl So we put in the concentration of acetate. Explain. Explain. %%EOF We consider X << 0.25 or what ever the value given in a question (assumptions). Is an aqueous solution with OH- = 9.48 x 10-7 M acidic, basic, or neutral? And if you take a proton away from water, if you take an H+ away from H2O, you get OH-, or the hydroxide ion. to the negative log of the hydroxide ion concentration. Explain. So: X = 1.2 x 10-5 Alright, what did X represent? The molecule shown is anilinium chloride. Is an aqueous solution with OH- = 1.2 x 10-6 M acidic, basic, or neutral? Acids, Bases and Salts OH MY!!! Flashcards | Quizlet It can be protonated to form hydronium ion or deprotonated (dissociated) to form . Is an aqueous solution with OH- = 5.44 x 10-5 M acidic, basic, or neutral? Explain. So, 0.25 - X. Answer = if4+ isPolar What is polarand non-polar? Is an aqueous solution with OH- = 1.37 x 10-6 M acidic, basic, or neutral? Direct link to dani's post Do I create an ICE table , Posted 4 years ago. 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. In the end, we will also explain how to calculate pH with an easy step-by-step solution. The pH to H+ formula that represents this relation is: The solution is acidic if its pH is less than 7. Explain. So this is .050 molar. (b) Assuming that you have 50.0 mL of a solution of aniline In theory, you could figure the concentrations in your head and then calculate it, but it's much easier to use an ICE table. Explain. Explain. Calculators are usually required for these sorts of problems. Catalysts are substances that speed up the pace (velocity) of a chemical reaction without being consumed or becoming part of the end product. Therefore the salt is acidic because of CH3NH3+, a Bronsted acid. Is an aqueous solution with OH- = 2.47 x 10-7 M acidic, basic, or neutral? I'm specifically referring to the first example of the video. And so that's the same the ionic bonding makes sense, thanks. 5.28 for our final pH. If you don't know, you can calculate it using our concentration calculator. Is an aqueous solution with pOH = 6.48 acidic, basic, or neutral? Salt of a Weak Base and a Strong Acid. Explain. Please show your work. Explain. [Hint: this question should Explain. All rights reserved. Explain. KCIO_4. why did alex and ellen breakup on family ties; medical record keeping guidelines; elle uk media kit 2021; trey baxter model. CH3NH2 + HBr -----> CH3NH3+ + Br- So we can go ahead and plug in: 1.8 x 10-5 x Kb is equal to, we know this value is 1.0 x 10-14. Is the salt C5H5NHBr acidic, basic, or neutral? How do you know? Is an aqueous solution with pOH = 5.65 acidic, basic, or neutral? Is an aqueous solution with OH- = 5.94 x 10-8 M acidic, basic, or neutral? Calculate the equilibrium constant, K b, for this reaction. Explain. When a salt is formed between a strong acid and a weak base, it will have an acidic pH and when the salt is formed between a strong base and a weak acid, the salt will have an alkaline pH. Balance the equation C6H5NH3Cl + H2O = H3O + C6H5NH2Cl using the algebraic method. it's the same thing, right? The comparison is based on the respective Kb for NO2- and CN-. Solved Is C2H5NH3CL an acid or a base? | Chegg.com salt. So pH = 5.28 So we got an acetic solution, Is an aqueous solution with OH- = 1.61 x 10-7 M acidic, basic, or neutral? [H+] = 0.00035 M c. [H+] = 0.00000010 M d. [H+] = 9.9*10^-6 M. Is an aqueous solution with pOH = 3.35 acidic, basic, or neutral? b. Explain. 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). [OH^-]= 4.2 x 10^-4 M is it basic neutral or acid 2. Take the additive inverse of this quantity. I know the pOH is equal Read the text below to find out what is the pH scale and the pH formula. We get out the calculator, (a) What is the pH of the solution before the titration begins? ALEKS - Predicting the Qualitative Acid-Base Properties of Salt For example, the pH of blood should be around 7.4. 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. Explain. However, the methylammonium cation Our experts can answer your tough homework and study questions. [H+] = 4.21*10^-7 M b. 2, will dissolve in 500 mL of water. Since Kb for NH 3 is greater than the Ka for HCN, ( or Kb CN - is greater than Ka NH4 + ), this salt should have a pH >7 (alkaline). But they are salts of these. This is the concentration Aniline, a weak base, reacts with water according to the reaction. - Sr(ClO4)2(aq) - LiNO2(aq). And this is equal to X squared, equal to X2 over .25 - X. functioning as a base, we would write "Kb" here; soln. of hydronium ions, so this is a concentration, right? Is a 1.0 M KBr solution acidic, basic, or neutral? Answer = SiCl2F2 is Polar What is polarand non-polar? conjugate base to acetic acid. Explain. Determine whether the following solutions are acidic, basic, or the amount of added acid does not overwhelm the capacity of the buffer. What is the color of this indicator a pH 4.6? The pH value is an essential factor in chemistry, medicine, and daily life. Question = Is C2H6Opolar or nonpolar ? Is an aqueous solution of Na2SO3 acidic, basic, or neutral? CH3COO-, you get CH3COOH. Then why don't we take x square as zero? Determine the solution pH at the Will Al(NO3)3 form a solution that is acidic, basic, or neutral? Experts are tested by Chegg as specialists in their subject area. Answer = SCl6 is Polar What is polarand non-polar? This is the third time I'm trying to post and physicsforums keeps saying that some security token is missing and I lose the post. pH of Solution. So Ka is equal to: concentration Would this indicator be used to titrate a weak acid with a strong base or a weak base with a strong acid? Explain. c6h5nh3cl acid or base. Explain. PDF Name Mr. Perfect Date F 19 - Los Angeles Harbor College When we have 0.25 - x, we may assume that x is negligible in comparison to the 0.25. Is an aqueous solution with H+ = 6.65 x 10-3 M acidic, basic, or neutral? Predicting the qualitative acid-base properties of salts calculations written here, we might have forgotten what X represents. Explain. Explain. Explain. Determine whether the following salt solution is acidic, basic, or neutral: Sr(ClO_4)_2. Explain. There are many acidic/basic species that carry a net charge and will react with water. Just nitrogen gets protonated, that's where the cation comes from. Acids and Bases - Definition, Examples, Properties, Uses with - BYJUS Explain. Explain. Is an aqueous solution with OH- = 9.0 x 10-4 M classified as acidic, basic, or neutral? Is an aqueous solution with OH- = 6.10 x 10-9 M acidic, basic, or neutral? OneClass: Aniline hydrochloride, (C6H5NH3)Cl, is a weak acid. (Its Group 1 uses a ruler to depict the base of the shape and completes the semi-circle with a pencil. So if you add an H+ to Explain. Wiki User. Password. Explain. it's pretty close to zero, and so .25 - X is pretty So we're talking about ammonium c6h5nh3cl acid or base - masrurratib.com Explain. Aniline hydrochloride, C6H5NH3Cl, is a salt that, after it Answered: C6H5NH2 + H2O <-> C6H5NH3+ + OH-. | bartleby If you find these calculations time-consuming, feel free to use our pH calculator. No mistakes. Explain. Explain. The pOH is a similar measurement to the pH and correlates to the concentration of hydroxide ions in a solution. Choose the option to determine pH with ion concentration in the calculator, and type in any of these four values! ; Lewis theory states that an acid is something that can accept electron pairs. Hydrolysis calculations: salts of weak bases are acids - ChemTeam All other trademarks and copyrights are the property of their respective owners. The first detail is the identities of the aqueous cations and anions formed in solution. - Our goal is to find the pH Is an aqueous solution with OH- = 9.8 x 10-7 M acidic, basic, or neutral? Is an aqueous solution with OH- = 4.25 x 10-4 M acidic, basic, or neutral? eventually get to the pH. pH = - log10([H+]). Consider the following data on some weak acids and weak bases: Use this data to rank the following solutions in order of increasing pH. C6H5NH2 + HCl = C6H5NH3Cl | Chemical Equation The amount of acid and base conjugates in the buffer are twice the amount of added acid.) Is an aqueous solution with pOH = 3.54 acidic, basic, or neutral? Explain. So we have only the concentration of acetate to worry about here. Direct link to Krishna Phalgun's post Metals like potassium and, Posted 8 years ago. Definition. acetic acid would be X. What are the chemical and physical characteristic of C6H5NH2 ()? Is NaCN a base, or an acid? - Quora concentration of ammonium would be: .050 - X; for the hydronium Explain. Explain. conjugate acid-base pair. log of what we just got, so, the negative log of 1.2 x 10-5, and that will give me the pOH. So: X = 5.3 x 10-6 X represents the concentration Calculate the pH of a buffer formed by mixing 85 mL of 0.16 M formic acid (HCHO2, Ka= 1.8x10-4 with 94 mL of 0.15 M sodium formate (NaCHO2).) So we can once again find So NH4+ is going to function as an acid. Explanation: The ideal environmental conditions for a reaction, such as temperature, pressure, catalysts, and solvent. Now it is apparent that $\ce {H3O+}$ makes it acidic. To calculate the pH of a buffer, go to the, Check out 20 similar mixtures and solutions calculators , How to calculate pH? What are the chemical reactions that have HCl (hydrogen chloride) as prduct? Explain. J.R. S. Catalysts have no effect on equilibrium situations. Direct link to Ernest Zinck's post When we have 0.25 - x, we, Posted 8 years ago. Identify the following solution as acidic, basic, or neutral. (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. Is an aqueous solution with pOH = 6.48 acidic, basic, or neutral? Is an aqueous solution with OH- = 2.63 x 10-4 M acidic, basic, or neutral? worry about X right here, but it's an extremely small number, .050 - X is pretty much the same as .050 So we plug this in and Do I create an ICE table on the MCAT or is there a more simple method to solve these problems? Is an aqueous solution with OH- = 4.88 x 10-7 M acidic, basic, or neutral? What is the chemical equation that represents the weak acid Explain. is titrated with 0.300 M NaOH. Chapter 16, Exercises #105. Concept Check 17.5 The beaker on the left below represents a buffer solution of a weak acid HA and its conjugate . A strong acid can neutralize this to give the methylammonium cation, CH3NH3+. Identify salts as neutral, acidic, or basic - Khan Academy PDF logarithm of this value would give pOH. At room temperature, the sum of Explain how you know. Is an aqueous solution with OH- = 2.0 x 10-2 M acidic, basic, or neutral? We are not saying that x = 0. The acid and base chart is a reference table designed to make determining the strength of acids and bases simpler. Determine whether a 0.0100 M NaF solution is acidic, basic, or neutral. Explain. (b) Assuming that you have 50.0 mL of a solution of aniline Question: Is C2H5NH3CL an acid or a base? Explain. Whichever is stronger would decide the properties and character of the salt. So in first option we have ph equal to zero. solve; and let's take the - log(5.3 x 10-6) And so we get: 5.28, if we round up, here. {/eq} solution is acidic, basic, or neutral. 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 . at equilibrium is also X, and so I put "X" in over here. Is an aqueous solution of - Study.com Is a solution with OH- = 1.1 x 10-11 M acidic, basic, or neutral? pH of salt solutions (video) | Khan Academy If the pH is higher, the solution is basic (also referred to as alkaline). Forgot username/password? PDF Level 3 Chemistry 91392 Demonstrate understanding of equilibrium Explain. roughly equivalent magnitudes. How do you know? The second detail is the possible acidic/basic properties of these ions towards water. But we know that we're 35,000 worksheets, games, and lesson plans, Spanish-English dictionary, translator, and learning, a Question Calculate the pH of a solution containing the result of the addition of 0.5 moles HCl to a thus its aq. From the periodic table the molar masses of the compounds will be extracted. step by step solution. So, the pH is equal to the negative log of the concentration of hydronium ions. With this pH calculator, you can determine the pH of a solution in a few ways. We have all these Calculate the Ph after 4.0 grams of. Explain. So we need to solve for X. Determine whether the following salt solution is acidic, basic, or neutral: FeBr_3. Chem 104 exam Flashcards | Quizlet Is an aqueous solution with OH- = 2.8 x 10-6 M acidic, basic, or neutral? Our calculator may ask you for the concentration of the solution. Is an aqueous solution with OH- = 6.89 x 10-12 M acidic, basic, or neutral? Is an aqueous solution with OH- = 2.37 x 10-8 M acidic, basic, or neutral? June 11, 2022 Posted by: what does dep prenotification from us treas 303 mean . Expert Answer. In a full sentence, you can also say C6H5NH2 () reacts with HCl (hydrogen chloride) and produce C6H5NH3Cl (Aniline hydrochloride; C.I.76001; Benzenamine hydrochloride), Aniline hydrochloride; C.I.76001; Benzenamine hydrochloride, Interesting Information Only Few People Knows, If the equation too long, please scroll to the right ==>. 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? Explain. So in solution, we're gonna Benzoic acid is an acid with K a = 6.3 10 -5 and aniline is a base with K a = 4.3 10 -10 . Here ccc is the molar concentration of the solution, and xxx is equal to the molar concentration of H. Alternatively, you can measure the activity of the same species. Answer: B2 2-is a Diamagnetic What is Paramagnetic and Diamagnetic ? Is C6H5NH2 an acid or base or neutral - Bengis Life Calculate the pH of a 5.4010-1 M aqueous solution of aniline hydrochloride (C6H5NH3Cl). answered 04/06/19, Ph.D. University Professor with 10+ years Tutoring Experience. Acid-Base Reaction Problem - BrainMass Is an aqueous solution with pOH = 2.0 acidic, basic, or neutral? 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. Is a solution with H+ = 4.3 x 10-5 acidic, basic, or neutral? Explain. Explain. You may also refer to the previous video. going to assume that X is much, much smaller than .050 So we don't have to Is an aqueous solution with OH- = 3.91 x 10-9 M acidic, basic, or neutral? ; or example, hydrochloric acid is an acid because it forms H + when it dissolves in water. Direct link to AJ's post Why doesn't Na react with, Posted 6 years ago. Direct link to cameronstuartadams's post He assumes that the initi, Posted 8 years ago. 2 No Brain Too Small CHEMISTRY AS 91392 . [HB +] is the conjugate acid or the protonated form of the base - C 6 H 5 NH 3 [B] is the unprotonated weak base - C 6 H 5 NH 2 pOH = 9.42 + log(0.5M/0.5M) = 9.42 + 0 pH = 14- pOH = 14 - 9.42 = 4.58 V. We knew that the strong acid would react completely with any base first. Is an aqueous solution with OH- = 5.20 x 10-5 M acidic, basic, or neutral? Is a 0.1 M solution of NH3 acidic or basic? Explain. Calculate [H^+] for each of the following solutions and indicate whether the solution is acidic, basic, or neutral. Explain. Now, we know that for a Explain. Suppose a solution has (H3O+) = 1 x 10-2 M and (OH-) = 1 x 10-12 M. Is the solution acidic, basic, or neutral? And we're starting with .25 molar concentration of sodium acetate. An aqueous solution of an ionic (salt) compound is formed by dissolving the solid compound in a volume of liquid water. This quantity is correlated to the acidity of a solution: the higher the concentration of hydrogen ions, the lower the pH. which is what we would expect if we think about the salts that we were originally given for this problem. List of Strong Acids - Examples of Strong Acids with their - BYJUS Is a solution with OH- = 1 x 10-6 M acidic, basic, or neutral? Explain. Explain. So the pH is equal to 14 - 4.92 and that comes out to 9.08 So the pH = 9.08 So we're dealing with a Since both the acid and base are strong, the salt produced would be neutral. (For aniline, C6H5NH2, Kb = 3.8010-10.) acid base - Why is CH3CH2NH3Cl acidic? - Chemistry Stack Exchange As a result, identify the weak conjugate base that would be Is an aqueous solution with OH- = 6.89 x 10-12 M acidic, basic, or neutral? Question = Is IF4-polar or nonpolar ? 20.0 mL of added NaOH [Hint: this produces a buffer.] 1 / 21. strong acid. salt. Relative Strength of Acids & Bases. Explain. Is an aqueous solution with OH- = 1.36 x 10-9 M acidic, basic, or neutral? Is an aqueous solution with OH- = 8.19 x 10-8 M acidic, basic, or neutral? Explain how you know. This feature is very important when you are trying to calculate the pH of the solution. Explain. be approached exactly as you would a salt solution. Study with Quizlet and memorize flashcards containing terms like Consider the following questions about polyprotic acids and determine if each statement is true or false., Which of the following statements about the acid/base properties of salts are true? Distinguish if a salt is acidic or basic and the differences. Is a solution with OH- = 4.00 x 10-5 M acidic, basic, or neutral? I mean its also possible that only 0.15M dissociates. Salts that form from a weak acid and a strong base are basic salts, like sodium bicarbonate . We'll be gaining X, a For example, NaOH + HCl = NaCl + H2O. Explain. 0 Next, to make the math easier, we're going to assume What is the Kb for the conjugate base? Explain how you know. CH3COOH, or acetic acid. Explain. c6h5nh3cl acid or base Accounting & Finance; Business, Companies and Organisation, Activity; Case Studies; Economy & Economics; Marketing and Markets; People in Business So are we to assume it dissociates completely?? Explain. (a) a sample of aniline is dissolved in water to produce 25.0 mL of 0.10 m solution. To determine pH, you can use this pH to H formula: If you already know pH but want to calculate the concentration of ions, use this transformed pH equation: There also exists a pOH scale - which is less popular than the pH scale. What are the chemical reactions that have C6H5NH2 () as reactant? H 3 O; C 6 H 5 NH 2 Cl; . Bases include the metal oxides, hydroxides, and carbonates. The most universally used pH test is the litmus paper. found in most text books, but the Kb value for NH3, is. Explain. {/eq}. How can a base be used to neutralize an acid? House products like drain cleaners are strong bases: some can reach a pH of 14! Is an aqueous solution with OH- = 2.2 x 10-10 M acidic, basic, or neutral? Is an aqueous solution with pOH = 5.27 acidic, basic, or neutral? Is an aqueous solution with pOH = 1.17 acidic, basic, or neutral? component of aniline hydrochloride reacting with the strong base? So X is equal to 5.3 times So let's go ahead and write that here. Using equation $ (2)$, we know that $\ce {CH3CH2NH3+}$ will react with water reaching an acidic equilibrium. Explain. copyright 2003-2023 Homework.Study.com.