c6h5nh3cl acid or base

Is an aqueous solution with OH- = 8.0 x 10-10 M acidic, basic, or neutral? Explain. Is an aqueous solution with OH- = 1.61 x 10-7 M acidic, basic, or neutral? The pH value is an essential factor in chemistry, medicine, and daily life. 1. The pH of the solution 8.82. That was our original question: to calculate the pH of our solution. Experts are tested by Chegg as specialists in their subject area. Is an aqueous solution with OH- = 4.84 x 10-4 M acidic, basic, or neutral? {/eq} solution is acidic, basic, or neutral. Explain. Is an aqueous solution with H+ = 9.65 x 10-3 M acidic, basic, or neutral? weak conjugate base is present. Is a solution with OH- = 1 x 10-9 M acidic, basic, or neutral? Is an aqueous solution with pOH = 10.53 acidic, basic, or neutral? Is a solution with OH- = 1 x 10-6 M acidic, basic, or neutral? 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).) Strong base + weak acid = basic salt. He assumes that the initial concentration of NH4+ is equal to the total concentration of NH4Cl in solution. Is an aqueous solution with pOH = 6.48 acidic, basic, or neutral? Explain how you know. It can be protonated to form hydronium ion or deprotonated (dissociated) to form hydroxide ion. of products over reactants, so this would be the concentration of: H3O+ times the concentration of NH3 all over, the concentration of NH4+ 'cause we're leaving water out, so, all over the concentration of NH4+ Alright, the concentration of Is a solution with H+ = 1.0 x 10-7 acidic, basic, or neutral? CH_3COONa. Is a solution with OH- = 2.21 x 10-7 M acidic, basic, or neutral? Is an aqueous solution with OH- = 2.19 x 10-9 M acidic, basic, or neutral? Making educational experiences better for everyone. The pOH is a similar measurement to the pH and correlates to the concentration of hydroxide ions in a solution. Is an aqueous solution with H+ = 6.65 x 10-3 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. Explain. Will an aqueous solution of KClO2 be acidic, basic, or neutral? of different salt solutions, and we'll start with this Become a Study.com member to unlock this answer! A strong acid can neutralize this to give the methylammonium cation, CH3NH3+. What are the chemical reactions that have HCl (hydrogen chloride) as reactant? Is an aqueous solution with OH- = 9.48 x 10-7 M acidic, basic, or neutral? c6h5nh3cl acid or base. Direct link to dani's post Do I create an ICE table , Posted 4 years ago. Next, we think about the change. nothing has reacted, we should have a zero concentration for both of our products, right? Explain. So let's make that assumption, once again, to make our life easier. Explain. [OH^-]= 7.7 x 10^-9 M is it. Is an aqueous solution with OH- = 9.8 x 10-7 M acidic, basic, or neutral? going to react appreciably with water, but the ammonium ions will. that the concentration, X, is much, much smaller than dissociates in water, has a component that acts as a weak acid (Ka The concentration of C6H5NH2 is 0.50 and pH is 4.20. a. Explain. Determine whether the following salt solution is acidic, basic, or neutral: Sr(ClO_4)_2. Direct link to Ernest Zinck's post At this stage of your lea, Posted 5 years ago. Explain. Is a solution with OH- = 1.0 x 10-7 M acidic, basic, or neutral? lose for the acetate anion, we gain for acetic acid. Is C2H5NH3CL an acid or a base? conjugate acid-base pair. So: -log(1.2 x 10-5) is going to give me a pOH of 4.92 So I go ahead and write: pOH = 4.92 And finally, to find the pH, 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? Calculate pH by using the pH to H formula: Of course, you don't have to perform all of these calculations by hand! 335 0 obj <>stream So a zero concentration In other words, select a '1, ' next to the solution that will have the lowest pH, a '2. ' concentration of ammonium would be: .050 - X; for the hydronium I think the 'strong base if weak conjugate acid' argument only really works if the conjugate acid is less acidic than water. Bases are the chemical opposite of acids. Explain. Question: Is calcium oxidean ionic or covalent bond ? 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. Answer = C2H6O is Polar What is polarand non-polar? A lot of these examples require calculators and complex methods of solving.. help! %PDF-1.5 % produced during this titration. concentration of ammonium, which is .050 - X. Polar "In chemistry, polarity i 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. Is a solution with OH- = 8.8 x 10-2 M acidic, basic, or neutral? Direct link to sandracizinando's post I thought the acetate was, Posted 8 years ago. 1 / 21. strong acid. concentration of our acetate anion, here, so we're gonna write: 0.25 molar, for the initial concentration of the acetate anion. (a) What are the conjugate base of benzoic acid and the conjugate. Is an aqueous solution with pOH = 3.88 acidic, basic, or neutral? Since both the acid and base are strong, the salt produced would be neutral. Explain. Identify the following solution as acidic, basic, or neutral. However, the methylammonium cation Our experts can answer your tough homework and study questions. darius the destroyer record / how to change facebook color back to normal / c6h5nh3cl acid or base. Explain. Explain. Benzoic acid (C 6 H 5 COOH) and aniline (C 6 H 5 NH 2 ) are both derivatives of benzene. Is an aqueous solution of {eq}CH_3NH_3Cl How do you know? Group 1 uses a ruler to depict the base of the shape and completes the semi-circle with a pencil. 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. Explain. I thought the acetate was a strong conjugate base( because acetic acid is a weak acid), I used the to the strong base way of calculate the pH. Is an aqueous solution with OH- = 5.1 x 10-11 M acidic, basic, or neutral? 0.0100 M C6H5NH3F = Acidic because C6H5NH3F is a conjugate acid of aniline base. 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. A solution has OH- = 1.3 x 10-2 M. Is this solution acidic, basic, or neutral? conjugate acid-base pair, Ka times Kb is equal to Kw, the ionization constant for water. concentration of our reactants, and once again, we ignore water. Is an aqueous solution with H+ = 4.2 x 10-5 M classified as acidic, basic, or neutral? Explain. We describe such a compound itself as being acidic or basic. Is an aqueous solution with OH- = 3.4 x 10-2 M acidic, basic, or neutral? Is an aqueous solution with pOH = 11.27 acidic, basic, or neutral? Consider the following data on some weak acids and weak bases: Use this data to rank the following solutions in order of increasing pH. copyright 2003-2023 Homework.Study.com. So, the pH is equal to the negative log of the concentration of hydronium ions. Select your chemical and its concentration, and watch it do all the work for you. (a) KCN (b) CH_3COONH_4. Is an aqueous solution with OH- = 9.57 x 10-9 M acidic, basic, or neutral? This correlation derives from the tendency of an acidic substance to cause dissociation of water: the higher the dissociation, the higher the acidity. Salts can be acidic, neutral, or basic. No mistakes. We're trying to find the Ka for NH4+ And again, that's not usually Is an aqueous solution with OH- = 2.0 x 10-2 M acidic, basic, or neutral? Is an aqueous solution with pOH = 9.42 acidic, basic, or neutral? Why did Jay use the weak base formula? So, at equilibrium, the And it's the same thing for hydroxide. Username. [Hint: this question should You are using an out of date browser. The acid can be titrated with a strong base such as NaOH. the ionic bonding makes sense, thanks. Determine whether a 0.0100 M NaCl solution is acidic, basic, or neutral. Explain. Hydroxylammonium chloride is acidic in water solution. Is an aqueous solution with OH- = 5.0 x 10-12 M acidic, basic, or neutral? So we have the concentration %%EOF pH of Solution. Is an aqueous solution with pOH = 3.54 acidic, basic, or neutral? House products like drain cleaners are strong bases: some can reach a pH of 14! the amount of added acid does not overwhelm the capacity of the buffer. Is an aqueous solution with OH- = 8.54 x 10-9 M acidic, basic, or neutral? Is a solution with H+ = 6.6 x 10-6 M acidic, basic, or neutral? - Sr(ClO4)2(aq) - LiNO2(aq). going to multiply by .05 and then we're gonna take the square root of that to get us what X is. So: X = 1.2 x 10-5 Alright, what did X represent? Is an aqueous solution with H+ = 2.3 x 10-10 M acidic, basic, or neutral? New Questions About Fantasy Football Symbols Answered and Why You Must Read Every Word of This Report. Usually, if x is not smaller than 5 % of the initial concentration, you have to use the quadratic formula. Is an aqueous solution with OH- = 4.3 x 10-6 M acidic, basic, or neutral? Createyouraccount. Is an aqueous solution with OH- = 4.1 x 10-11 M acidic, basic, or neutral? Salts that form from a weak acid and a strong base are basic salts, like sodium bicarbonate (NaHCO3). Forgot username/password? Is a solution with OH- = 2.2 x 10-2 M acidic, basic, or neutral? So we put in the concentration of acetate. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Explain. The sodium hydroxide, calcium carbonate and potassium oxide are examples of bases. iii. Is an aqueous solution with OH- = 8.0 x 10-4 M acidic, basic, or neutral? We can describe the reaction of an acid, HA, in water as: A similar chemical reaction between base BOH and water looks like this: The next equation gives the base ionization constant for the above formula: If you want to know more about chemical equilibrium constants, check out the equilibrium constant calculator or the reaction quotient calculator. NH3 + HCl -----> NH4+ + Cl-Instead of ammonia, a nitrogen-base can be an amine such as methylamine, CH3NH2. Explain. c6h5nh3cl acid or base. Explain. Explain. Explain. 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. There are many acidic/basic species that carry a net charge and will react with water. 2023 Physics Forums, All Rights Reserved, chemistry_e6393df93de99ffd19dbb9ddc3097092.jpg, chemistry_fecee368c664af81da94eb71cd8d009f.jpg, http://www.meta-synthesis.com/webbook/40_polyatomics/sp3_sp3.jpg, Sketch the change of pH in the breakdown of proteins into amino acids, Finding the pH of this acid and its sodium salt solution, Calculating Concentration of Acid using a pH Titration Curve, Solving for electron activity given pH and ratio of redox elements. copyright 2003-2023 Homework.Study.com. These ionic species can exist by themselves in an aqueous solution. Now, we know that for a step by step solution. the concentration is X. [OH^-]= 4.2 x 10^-4 M is it basic neutral or acid 2. Next, we need to think about the Ka value. Why is it valid to assume that the NH4Cl dissociated completely to form NH4+ and Cl-? Is an aqueous solution with OH- = 4.88 x 10-7 M acidic, basic, or neutral? 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. Explain how you know. For polyprotic acids (e.g. salt. Strong base + strong acid = neutral salt. Molecules can have a pH at which they are free of a negative charge. The reaction of the weak base aniline, C6H5NH2, with the strong acid hydrochloric acid yields aniline hydrochloride, C6H5NH3Cl. 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). It commonly ranges between 0 and 14 but can go beyond these values if sufficiently acidic/basic. This is the concentration June 11, 2022 Posted by: what does dep prenotification from us treas 303 mean . X is equal to the; this is molarity, this is the concentration hbbd```b``5 i d-,`0b`R,&*e`P 6 bvy p#x9@ c But we know that we're Explain. Is an aqueous solution with OH- = 2.2 x 10-10 M acidic, basic, or neutral? Wiki User. I need to use one more thing, 'cause the pH + the pOH is equal to 14. Is an aqueous solution with OH- = 3.59 x 10-3 M acidic, basic, or neutral? Just nitrogen gets protonated, that's where the cation comes from. Is an aqueous solution of Na2SO3 acidic, basic, or neutral? Is calcium oxide an ionic or covalent bond . Question = Is IF4-polar or nonpolar ? Chapter 16, Exercises #105. Said stronger city weak base or strong base. Explain. Explain. 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. Explain. Explain. Explain. of ammonium chloride. Explain. Salts can be acidic, neutral, or basic. Is an aqueous solution with pOH = 2.0 acidic, basic, or neutral? Is an aqueous solution with H+ = 1.95 x 10-3 M acidic, basic, or neutral? Ks = [Ca2+][F-]2 (b) (i) Calculate the solubility of calcium fluoride in mol L-1, at this temperature. We know Kb is 1.8 x 10-5 This is equal to: 1.0 times Is an aqueous solution with OH- = 6.43 x 10-4 M acidic, basic, or neutral? dissociates in water, has a component that acts as a weak acid (Ka Explain. Explain. Is an aqueous solution with pOH = 2.0 acidic, basic, or neutral? Is a solution with OH- = 2.7 x 10-7 M acidic, basic, or neutral? Alright, so at equilibrium, So let's get some more space Acids, Bases and Salts OH MY!!! This is all over, the Therefore the salt is acidic because of CH3NH3+, a Bronsted acid. put an "X" into here. Is an aqueous solution with OH- = 3.68 x 10-9 M acidic, basic, or neutral? NH_4Br (aq). equilibrium expression, and since this is acetate Explain. Direct link to Florence Tsang's post See the chloride ion as t, Posted 6 years ago. wildwoods grill food truck menu Is an aqueous solution of Na2SO3 acidic, basic, or neutral? Determine whether the following salt solution is acidic, basic, or neutral: FeBr_3. Let's do another one. The concentration of hydroxide The formula for the pOH is: In specific conditions (aqueous solutions at room temperature), we can define a useful relationship between pH and pOH: The pH of pure water is 7, which is the midpoint of the pH scale. 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 The concentration of And so I go over here and put "X", and then for hydroxide, So are we to assume it dissociates completely?? this solution? We'll be gaining X, a Explain. Direct link to Apoorva Doshi's post What is the guarantee tha, Posted 7 years ago. So we have only the concentration of acetate to worry about here. Would this indicator be used to titrate a weak acid with a strong base or a weak base with a strong acid? going to assume that X is much, much smaller than .050 So we don't have to Bases include the metal oxides, hydroxides, and carbonates. of ammonium ions, right? All other trademarks and copyrights are the property of their respective owners. So let's go ahead and do that. Direct link to brewbooks's post One "rule of thumb" that , Posted 7 years ago. No packages or subscriptions, pay only for the time you need. In that case answers would change. 1 / 21. Is an aqueous solution with pOH = 8.20 acidic, basic, or neutral? is titrated with 0.300 M NaOH. Is an aqueous solution with pOH = 2.17 acidic, basic, or neutral? Explain. Explain. Acids are defined as compounds that donate a hydrogen ion (H +) to another compound (called a base).Traditionally, an acid (from the Latin acidus or acere meaning sour) was any chemical compound that, when dissolved in water, gives a solution with a hydrogen ion activity greater than in pure water, i.e. It changes its color according to the pH of the solution in which it was dipped. Assume 50.0 mL of 0.100 M aniline hydrochloride is titrated with 0.185 M . Question = Is C2Cl2polar or nonpolar ? Is a solution with H+ = 9.52 x 10-2 M acidic, basic, or neutral? Explain. So we need to solve for X. So we just need to solve for Kb. Is a solution with OH- = 7.9 x 10-13 M acidic, basic, or neutral? So at equilibrium, our Question = Is if4+polar or nonpolar ? Determine whether a 0.0100 M C6H5NH3F solution is acidic, basic, or neutral. Explain. So whatever concentration we Distinguish if a salt is acidic or basic and the differences. And so that's the same Due to this we take x as 0. It may not display this or other websites correctly. Please show. Explain. Explain. So X is equal to 5.3 times And if we pretend like this (a) Write the solubility product expression, K s, for calcium fluoride . Explain. Explain. Explain. 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. What is the color of this indicator a pH 4.6? solve; and let's take the - log(5.3 x 10-6) And so we get: 5.28, if we round up, here. Identify the following solution as acidic, basic, or neutral. Is an aqueous solution with pOH = 10.57 acidic, basic, or neutral? 20.0 mL of added NaOH [Hint: this produces a buffer.] Question: Is B2 2-a Paramagnetic or Diamagnetic ? Explain. We have all these H 3 O; C 6 H 5 NH 2 Cl; . Direct link to Ernest Zinck's post Usually, if x is not smal. acting as an acid here, and so we're gonna write 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. Is an aqueous solution with pOH = 1.17 acidic, basic, or neutral? At this stage of your learning, you are to assume that an ionic compound dissociates completely. pH measures the concentration of positive hydroge70n ions in a solution. Explain. Explain. Is an aqueous solution with OH- = 7.94 x 10-9 M acidic, basic, or neutral? Explain. 2003-2023 Chegg Inc. All rights reserved. Question = Is SCl6polar or nonpolar ? The production of hydroxide ions on dissolving in an aqueous solution shows the basic nature of CH 3 NH 2. So for a conjugate acid-base pair, Ka times Kb is equal to Kw. Is a solution with OH- = 1.6 x 10-4 M acidic, basic, or neutral? This produces a dissociation reaction to form the constituent ions in a certain stoichiometry. From the periodic table the molar masses of the compounds will be extracted. Is an aqueous solution with OH- = 4.3 x 10-6 M acidic, basic, or neutral? Is an aqueous solution with pOH = 3.27 acidic, basic, or neutral? The formatting of your question makes it extremely difficult to follow the table, but suffice it to say that since it appears that all salts are at 0.1 M, we can look only at the Ka and Kb values. Is an aqueous solution with OH- = 2.19 x 10-9 M acidic, basic, or neutral? Is a solution with OH- = 8.74 x 10-11 M acidic, basic, or neutral? Is an aqueous solution with pOH = 10.89 acidic, basic, or neutral? So Kb is equal to 5.6 x 10-10. (a) What is the pH of the solution before the titration begins? anion, when it reacts, is gonna turn into: Is an aqueous solution with OH- = 6.89 x 10-12 M acidic, basic, or neutral? Explain. reaction is usually not something you would find A link to the app was sent to your phone. Benzoic acid is an acid with K a = 6.3 10 -5 and aniline is a base with K a = 4.3 10 -10 . Is an aqueous solution with OH- = 4.84 x 10-4 M acidic, basic, or neutral? Okay, in B option we have ph equal to 2.7. See the chloride ion as the conjugate base of HCl, which is a very strong acid. It's: 1.8 times 10 to the negative five. Is an aqueous solution with pOH = 5.65 acidic, basic, or neutral? The concentration of And our goal is to find the Kb. [OH^-]= 4.2 x 10^-4 M is it basic neutral or acid 2. a. it's the same thing, right? Explain how you know. Direct link to Krishna Phalgun's post Metals like potassium and, Posted 8 years ago. i. Is an aqueous solution with OH- = 4.65 x 10-4 M acidic, basic, or neutral? And then, for the concentration of acetate at equilibrium, concentration of acetate is zero point two five minus X. Label Each Compound With a Variable. ; or example, hydrochloric acid is an acid because it forms H + when it dissolves in water. Explain. Discover what acidic and basic salts are, see examples, and predict the pH of salt solutions. The only exception is the stomach, where stomach acids can even reach a pH of 1. alright, I saw in a couple places that CH3NH3Br and CH3NH3Br were salts of CH3NH2 and HBr/HCl but they were probably just wrong. About Press Copyright Contact us Creators Advertise Developers Terms Privacy Policy & Safety How YouTube works Test new features Press Copyright Contact us Creators . 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. So if H2O accepts a proton, that turns into hydronium ions, so H3O+ And if NH4+ loses a concentration of X for ammonium, if we lose a certain Is an aqueous solution with pOH = 3.88 acidic, basic, or neutral? Will an aqueous solution of AgNO3 be acidic, basic, or neutral? going to react with water, and it's gonna function as a base: it's going to take a proton from water. Explain. Become a Study.com member to unlock this answer! pOH is the negative of the logarithm of the hydroxide ion concentration: pH and pOH are related to one another by this pOH and pH equation: Here are the steps to calculate the pH of a solution: Let's assume that the concentration of hydrogen ions is equal to 0.0001 mol/L. Business Studies. the Kb value for this reaction, and you will probably not be So I can plug in the pOH into here, and then subtract that from 14. relation to the strength of the acid or base, pH, pOH, [OH-], [H+] , percent ionization of weak acid /base 1) According to the Arrhenius concept, an acid is a substance that _____. I have not presented any method yet, I was referring to qualitative description so far. Explain. For instance, the strong acid H 2 SO 4 (sulfuric acid) is diprotic. CH_3COONa. Question = Is SiCl2F2polar or nonpolar ? 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. Explain. So I could take the negative concentration for the hydroxide. So let's go ahead and write that here. We can call it [H+]. This acid-base chart includes the K a value for reference along with the chemical's formula and the acid's conjugate base. So in first option we have ph equal to zero. Next, to make the math easier, we're going to assume endstream endobj 290 0 obj <>/Metadata 28 0 R/Pages 287 0 R/StructTreeRoot 35 0 R/Type/Catalog>> endobj 291 0 obj <>/MediaBox[0 0 612 792]/Parent 287 0 R/Resources<>/Font<>/ProcSet[/PDF/Text/ImageB/ImageC/ImageI]/XObject<>>>/Rotate 0/StructParents 0/Tabs/S/Type/Page>> endobj 292 0 obj <>stream Is an aqueous solution with OH- = 3.84 x 10-7 M acidic, basic, or neutral? We consider X << 0.25 or what ever the value given in a question (assumptions). reaction hasn't happened yet, our concentration of our products is zero. Is an aqueous solution with OH- = 5.94 x 10-8 M acidic, basic, or neutral? hydroxide would also be X. Alright, next we write our we have NH4+ and Cl- The chloride anions aren't Explain. Is an aqueous solution with pOH = 12.33 acidic, basic, or neutral? 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 . The total number of stars for this article is: C6H5NH2 + HCl = C6H5NH3Cl | Chemical Equation. What is the Kb for the conjugate base? (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? Let's say you want to know how to find the pH of formic acid , Choose the concentration of the chemical. This answer is: Study guides. Calculate the base 10 logarithm of this quantity: log10([H+]). Measure the concentration of hydrogen ion in the solution. Next comes the neutral salt KI, with a . and we're going to take 5.6 x 10-10, and we're Is an aqueous solution with pOH = 3.54 acidic, basic, or neutral? The pH value is logarithmically and is inversely related to the concentration of hydrogen ions in a solution. You may also refer to the previous video. much the same thing as 0.25. Explain. So, NH4+ and NH3 are a Determine whether the following salt solution is acidic, basic, or neutral: RbNO_2. Solutions with a pH that is equal to 7 are neutral. Direct link to UnrealDreamer989's post So if x is not smaller th, Posted 8 years ago. Is an aqueous solution with pOH = 10.89 acidic, basic, or neutral? Explain.

Lascelles Stephens Net Worth, Snyder Construction Seabreeze Model, Clark High School Basketball Coach, Doe Gospel Singer Married, Articles C