c6h5nh3cl acid or base
Explain. Please show. If you're seeing this message, it means we're having trouble loading external resources on our website. Will an aqueous solution of KClO2 be acidic, basic, or neutral? Explain. Explain. HCl. Is an aqueous solution with pOH = 5.12 acidic, basic, or neutral? We're gonna write Ka. 1. hb```Z>)!b`f`s|a`dVB4(T(W@Jf\gJ\[+j @CXM$ kTtVf`` a4b8P`@,z6%z43cV iF ` |: Explain. Next, we need to think about Is an aqueous solution with OH- = 9.48 x 10-7 M acidic, basic, or neutral? Is a solution with OH- = 1.6 x 10-3 M acidic, basic, or neutral? Is a solution with OH- = 1.99 x 10-7 M acidic, basic, or neutral? found in most text books, but the Kb value for NH3, is. So, we could find the pOH from here. Explain. Username. How do you know? acting as an acid here, and so we're gonna write Explain. Discover what acidic and basic salts are, see examples, and predict the pH of salt solutions. KCIO_4. Click the card to flip . Explain. The production of hydroxide ions on dissolving in an aqueous solution shows the basic nature of CH 3 NH 2. Is a solution with OH- = 5.3 x 10-12 M acidic, basic, or neutral? Question = Is if4+polar or nonpolar ? Is an aqueous solution with OH- = 4.84 x 10-4 M acidic, basic, or neutral? Is a 0.1 M solution of NH3 acidic or basic? 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. The total number of stars for this article is: C6H5NH2 + HCl = C6H5NH3Cl | Chemical Equation. CH3NH3Cl is an ionic compound, consisting of CH3NH3+ and Cl- ions. produced during this titration. Explain. Calculate the concentration of C6H5NH3+ in this buffer solution. [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. Explain. Explain. ; or example, hydrochloric acid is an acid because it forms H + when it dissolves in water. Is an aqueous solution with OH- = 2.47 x 10-7 M acidic, basic, or neutral? Explain. In chemistry, a salt is an ionic compound that can be formed by the neutralization reaction of an acid and a base. able to find this in any table, but you can find the Ka for acetic acid. Explain. Explain. This is similar to the reason why the chloride ion (and the sodium ion) in NaCl does not affect the pH of the solution. Is an aqueous solution with OH- = 4.65 x 10-4 M 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. Explain. 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. It can be protonated to form hydronium ion or deprotonated (dissociated) to form . Explain. The first detail is the identities of the aqueous cations and anions formed in solution. Since both the acid and base are strong, the salt produced would be neutral. It's going to donate a proton to H2O. Is an aqueous solution with OH- = 3.43 x 10-9 M acidic, basic, or neutral? ; Brnsted-Lowry theory says that acid can donate protons while a base can accept them. Explain. Explain. Post author By ; qalipu first nation membership list Post date June 11, 2022; white spots on tan skin that won't tan . So in first option we have ph equal to zero. concentration of acetate would be .25 - X, so Due to this we take x as 0. Is an aqueous solution with OH- = 8.0 x 10-10 M acidic, basic, or neutral? we're going to lose X, and we're going to gain Explain. 10 to the negative five. What are the chemical and physical characteristic of C6H5NH2 ()? Okay. The sodium hydroxide, calcium carbonate and potassium oxide are examples of bases. solve; and let's take the - log(5.3 x 10-6) And so we get: 5.28, if we round up, here. b. Our calculator may ask you for the concentration of the solution. What are the chemical reactions that have HCl (hydrogen chloride) as reactant? Is an aqueous solution with H+ = 1.5 x 10-13 M acidic, basic, or neutral? reaction is usually not something you would find Explain. So CH3COO-, the acetate 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? lose for the acetate anion, we gain for acetic acid. Determine whether the following salt solution is acidic, basic, or neutral: NH_4I. Calculate pH by using the pH to H formula: Of course, you don't have to perform all of these calculations by hand! Now it is apparent that $\ce {H3O+}$ makes it acidic. Explain. The question doesn't give any information about CH3NH2+ and I don't see it in the book's appendix, So something-NH2 gets protonated to something-NH3+. Label each compound (reactant or product) in the equation with a variable to . Why did Jay use the weak base formula? Posted 8 years ago. Distinguish if a salt is acidic or basic and the differences. Explain. Is an aqueous solution with pOH = 4.78 acidic, basic, or neutral? .25, and if that's the case, if this is an extremely small number, we can just pretend like It may not display this or other websites correctly. equilibrium expression, and since this is acetate and then we divide by: 1.8 x 105; so we get: 5.6 x 10-10. Explain. Aniline hydrochloride, C6H5NH3Cl, is a salt that, after it dissociates in water, has a component that acts as a weak acid (Ka = 2.4 105 ). Explain. Explain. nothing has reacted, we should have a zero concentration for both of our products, right? So if x is not smaller than 0.25, would you have to use the quadratic formula to solve for x? Step 1: Calculate the molar mass of the solute. Is an aqueous solution with OH- = 6.10 x 10-9 M acidic, basic, or neutral? Is a solution with H+ = 1.2 x 10-4 M acidic, basic, or neutral? And this is equal to X squared, equal to X2 over .25 - X. Explain. Is an aqueous solution with OH- = 1.57 x 10-9 M acidic, basic, or neutral? (Its conjugate base is the weak base aniline, C 6 H 5 NH 2 .) Explain. Is a solution with OH- = 9.00 x 10-8 M acidic, basic, or neutral? Explain. Is an aqueous solution with pOH = 2.0 acidic, basic, or neutral? Explain. Explain. Is a solution with pOH = 3.34 acidic, basic, or neutral? Our goal is to calculate the pH of a .050 molar solution We'll be gaining X, a Explain. All other trademarks and copyrights are the property of their respective owners. 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. eventually get to the pH. Is an aqueous solution with pOH = 1.17 acidic, basic, or neutral? The earliest definition of acids and bases is Arrhenius's definition which states that: An acid is a substance that forms hydrogen ions H + when dissolved in water, and; A base is a substance that forms hydroxide ions OH-when dissolved in water. Is an aqueous solution with OH- = 0.85 M acidic, basic, or neutral? To calculate the pH of a buffer, go to the, Check out 20 similar mixtures and solutions calculators , How to calculate pH? Explain. Is an aqueous solution with OH- = 9.42 x 10-8 M acidic, basic, or neutral? Explain. Answer = C2Cl2 is Polar What is polarand non-polar? So, 1.0 x 10-14 We divide that by 1.8 x 10-5 And so, the Ka value is: 5.6 x 10-10 So if we get some room down here, we say: Ka = 5.6 x 10-10 This is equal to: so it'd Is an aqueous solution with H+ = 6.65 x 10-3 M acidic, basic, or neutral? Is a solution with OH- = 1 x 10-6 M acidic, basic, or neutral? going to react appreciably with water, but the ammonium ions will. What is not too clear is your description of "lopsided". [Hint: this question should Is an aqueous solution with OH- = 5.44 x 10-5 M acidic, basic, or neutral? You and I don't actually know because the structure of the compound is not apparent in the molecular formula. Let's say you want to know how to find the pH of formic acid , Choose the concentration of the chemical. Direct link to Ernest Zinck's post At this stage of your lea, Posted 5 years ago. hydrochloride with a concentration of 0.150 M, what is the pH of So we can once again find CH_3COONa. So let's make that assumption, once again, to make our life easier. That was our original question: to calculate the pH of our solution. We describe such a compound itself as being acidic or basic. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Suppose a solution has (H3O+) = 1 x 10-13 M and (OH-) = 1 x 10-1 M. Is the solution acidic, basic, or neutral? Explain. hydronium ions at equilibrium is X, so we put an "X" in here. Experts are tested by Chegg as specialists in their subject area. Is an aqueous solution with pOH = 10.57 acidic, basic, or neutral? Term. the Kb value for this reaction, and you will probably not be Explain. Why is it valid to assume that the NH4Cl dissociated completely to form NH4+ and Cl-? So it will be weak acid. Explain. No packages or subscriptions, pay only for the time you need. Is a solution with OH- = 3.7 x 10-10 M acidic or basic? Is an aqueous solution with pOH = 3.22 acidic, basic, or neutral? Is an aqueous solution with pOH = 5.27 acidic, basic, or neutral? Explain. Is a solution with H+ = 1.0 x 10-7 acidic, basic, or neutral? 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. So at equilibrium, our Is an aqueous solution with OH- = 9.47 x 10-5 M acidic, basic, or neutral? It can be protonated to form hydronium ion or deprotonated (dissociated) to form hydroxide ion. NH3 + HCl -----> NH4+ + Cl-Instead of ammonia, a nitrogen-base can be an amine such as methylamine, CH3NH2. Is an aqueous solution with OH- = 2.19 x 10-9 M acidic, basic, or neutral? Therefore, it has no effect on the solution pH. Explain. Is an aqueous solution with OH- = 4.1 x 10-11 M acidic, basic, or neutral? proton, we're left with NH3 So let's start with our I have not presented any method yet, I was referring to qualitative description so far. The concentration of Let's assume that it's equal to. Most questions answered within 4 hours. Determine whether a 0.0100 M NaCl solution is acidic, basic, or neutral. Explain. so we write: Kb is equal to concentration of our products over concentration of our reactives. (a) Identify the species that acts as the weak acid in this X is equal to the; this is molarity, this is the concentration Question = Is IF4-polar or nonpolar ? Some species are amphiprotic (both acid and base), with the common example being water. 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. Is an aqueous solution with pOH = 10.89 acidic, basic, or neutral? Is an aqueous solution with OH- = 1.61 x 10-7 M acidic, basic, or neutral? dissociates in water, has a component that acts as a weak acid (Ka June 11, 2022 Posted by: what does dep prenotification from us treas 303 mean . Explain. Explain. Explain. square root of that number and we get: X is equal to, this gives us: X is equal to 1.2 times we're going to multiply that, we're going to multiply that, by .25 And so we get 1.4 x 10-10. Explain. From the periodic table the molar masses of the compounds will be extracted. And so I go over here and put "X", and then for hydroxide, Is an aqueous solution with OH- = 5.0 x 10-5 M acidic, basic, or neutral? Explain. We know Kb is 1.8 x 10-5 This is equal to: 1.0 times 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 . 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 Explain. Is a solution with OH- = 4.8 x 10-3 M acidic, basic, or neutral? Explain. Need Help? 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. As a result, identify the weak conjugate base that would be So we have: 5.6 x 10-10 and put an "X" into here. So X is equal to the Explain. Is an aqueous solution with H+ = 4.2 x 10-5 M classified as acidic, basic, or neutral? So, acetic acid and acetate salt. 289 0 obj <> endobj Explain. So let's go ahead and write that down. CH3COOH, or acetic acid. Explain. Is an aqueous solution with OH- = 1.61 x 10-7 M acidic, basic, or neutral? Is a solution with OH- = 1 x 10-9 M acidic, basic, or neutral? Note that there is no $\ce {OH-}$ to start with (very little in reality), so equation $ (1)$ is not applicable. Is an aqueous solution with OH- = 7.34 x 10-6 M acidic, basic, or neutral? But be aware: we don't reference organic compounds by their molec. Apart from the mathematical way of determining pH, you can also use pH indicators. The second detail is the possible acidic/basic properties of these ions towards water. Is an aqueous solution of Na2SO3 acidic, basic, or neutral? However, they must first be provided by dissolving an appropriate solid salt compound in liquid water. NH_4Br (aq). Select your chemical and its concentration, and watch it do all the work for you. 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. Explain. You can also use the solution dilution calculator to calculate the concentration of ions in a diluted solution. Explain how you know. So in solution, we're gonna Direct link to Florence Tsang's post See the chloride ion as t, Posted 6 years ago. Explain. Is an aqueous solution with pOH = 10.89 acidic, basic, or neutral? why did alex and ellen breakup on family ties; medical record keeping guidelines; elle uk media kit 2021; trey baxter model. Calculate the equilibrium constant, K b, for this reaction. Is an aqueous solution with OH- = 3.84 x 10-7 M acidic, basic, or neutral? Direct link to Gina Ciliberti's post At 8:19; how do you know , Posted 6 years ago. Explain. dissociates in water, has a component that acts as a weak acid (Ka Consider the following data on some weak acids and weak bases: Use this data to rank the following solutions in order of increasing pH. Is an aqueous solution with OH- = 5.1 x 10-11 M acidic, basic, or neutral? Explain. Most bases are minerals which form water and salts by reacting with acids. concentration of our reactants, and once again, we ignore water. going to assume that X is much, much smaller than .050 So we don't have to So we put in the concentration of acetate. Now you know how to calculate pH using pH equations. Answer (1 of 14): NaCN is a neutral salt there lies a triple bond between C and N which facilitates easy removal of sodium in its aqueous soln. Start over a bit. Explain. Explain. So for a conjugate acid-base pair, Ka times Kb is equal to Kw. Only d. does not change appreciably in pH. Explain. An aqueous solution of an ionic (salt) compound is formed by dissolving the solid compound in a volume of liquid water. 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, 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- = 5.20 x 10-5 M acidic, basic, or neutral? = 2.4 105 ). The most universally used pH test is the litmus paper. I need to use one more thing, 'cause the pH + the pOH is equal to 14. (b) Assuming that you have 50.0 mL of a solution of aniline Predict whether the solution is acidic, basic, or neutral, and explain the answer. Next, we think about the change. Just nitrogen gets protonated, that's where the cation comes from. The pH value is logarithmically and is inversely related to the concentration of hydrogen ions in a solution. QUESTION ONE . Is an aqueous solution with pOH = 5.00 acidic, basic, or neutral? I'm specifically referring to the first example of the video. Explain. it's pretty close to zero, and so .25 - X is pretty I think the 'strong base if weak conjugate acid' argument only really works if the conjugate acid is less acidic than water. strong base have completely neutralized each other, so only the Suppose a solution has (H3O+) = 1 x 10-10 M and (OH-) = 1 x 10-4 M. Is the solution acidic, basic, or neutral? much the same thing as 0.25. 2014-03-28 17:28:41. 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. copyright 2003-2023 Homework.Study.com. Is an aqueous solution with OH- = 1.47 x 10-3 M acidic, basic, or neutral? Login to Course. Is an aqueous solution with H+ = 9.65 x 10-3 M acidic, basic, or neutral? So if we lose a certain Explain. Is an aqueous solution with OH- = 9.41 x 10-9 M acidic, basic, or neutral? All rights reserved. Wiki User. The equivalence point [Hint: at this point, the weak acid and Determine whether the following salt solution is acidic, basic, or neutral: RbNO_2. Explain. All other trademarks and copyrights are the property of their respective owners. In each of the following solutions, determine [OH-], and then specify whether the solution is acidic, basic, or neutral. Note: in the first four problems, I give the K a of the conjugate acid (for example, the ammonium ion in Example #1). of CH3COOH times the concentration of hydroxide, so times the concentration of OH- this is all: over the We're trying to find Ka. Hoh Aqua [Oh2] HO Oxidane Pure Water Hydroxic Acid Hydrogen Oxide H2O Molar Mass H2O Oxidation Number. So, the pH is equal to the negative log of the concentration of hydronium ions. Question = Is SbCl5 ( Antimony pentachloride ) polar or nonpolar ? You may also refer to the previous video. 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 Chapter 16, Exercises #105. This is something you learn with experience, although it helps if you can remember the names of the common strong acids (HCl, HBr, Hi, H2SO4, HNO3, HClO4) and strong bases (hydroxides of Group 1 and 2 elements). Explain. Explain. So we have only the concentration of acetate to worry about here. We get out the calculator, That is what our isoelectric point calculator determines. which is what we would expect if we think about the salts that we were originally given for this problem. The acid can be titrated with a strong base such as NaOH. c6h5nh3cl acid or base. 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. Catalysts are substances that speed up the pace (velocity) of a chemical reaction without being consumed or becoming part of the end product. Explain. So if we make the concentration of the acetate anion, X, that reacts Alright, so, X reacts. Label Each Compound With a Variable. For example, the pH of blood should be around 7.4. Answer = IF4- isNonpolar What is polarand non-polar? Is an aqueous solution with pOH = 3.27 acidic, basic, or neutral? (K a for aniline hydrochloride is 2.4 x 10-5). Will an aqueous solution of KClO2 be acidic, basic, or neutral? So pH = 5.28 So we got an acetic solution, It commonly ranges between 0 and 14 but can go beyond these values if sufficiently acidic/basic. Is a solution with OH- = 2.7 x 10-2 M acidic, basic, or neutral? Click the card to flip . Explain. Since a very strong acid has a very weak conjugate base, the chloride ion don't really take protons from water, thus it does not affect the pH of the solution, we thus do not include it into the equation. Balance the equation C6H5NH3Cl + H2O = H3O + C6H5NH2Cl using the algebraic method. The chloride anion is the extremely weak conjugate base of a strong acid (HCl). Is an aqueous solution with pOH = 2.17 acidic, basic, or neutral? In other words, select a '1, ' next to the solution that will have the lowest pH, a '2. ' Direct link to brewbooks's post One "rule of thumb" that , Posted 7 years ago. Determine whether a 0.0100 M NaF solution is acidic, basic, or neutral. {/eq} acidic, basic, or neutral? Alright, so at equilibrium, NaClO_4, How to classify solution either acidic, basic, or neutral? Is an aqueous solution with pOH = 12.42 acidic, basic, or neutral? We can call it [H+]. Explain. What is the Kb for the conjugate base? 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. 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 . Explain. So, the acetate anion is Forgot username/password? Business Studies. The pH of the solution 8.82. But we know that we're c6h5nh3cl acid or base. And then, for the concentration of acetate at equilibrium, concentration of acetate is zero point two five minus X. Direct link to dani's post Do I create an ICE table , Posted 4 years ago. Determine whether the following salt solution is acidic, basic, or neutral: Sr(ClO_4)_2. Is an aqueous solution with OH- = 6.89 x 10-12 M acidic, basic, or neutral? The pH of our stomach varies from 1.5 to 3.5: our stomach is quite acidic! Would an aqueous solution with OH- = 7.4 x 10-12 M be acidic, basic, or neutral? Explain. Explain. Choose the option to determine pH with ion concentration in the calculator, and type in any of these four values! Explain. Use this acids and bases chart to find the relative strength of the most common acids and bases. Is an aqueous solution of Na2SO3 acidic, basic, or neutral? Answer = C2H6O is Polar What is polarand non-polar? 1 answer; geometry; asked by Anonymous; 383 views; Two groups of students are asked to depict a picture of a semi-circular pizza. Is an aqueous solution with OH- = 4.88 x 10-7 M acidic, basic, or neutral? This feature is very important when you are trying to calculate the pH of the solution. Next, we need to think about the Ka value. Measure the concentration of hydrogen ion in the solution. To predict the relative pH of this salt solution you must consider two details. Predict whether the solution of the following will be acidic, basic, or neutral, and explain the answer. Is a solution with OH- = 2.7 x 10-7 M acidic, basic, or neutral? Explain. Explain. Explain. soln. Explain. Explain. Anyway, you have apparently made important progress. Concept Check 17.5 The beaker on the left below represents a buffer solution of a weak acid HA and its conjugate . Explain. Explain. Determine whether a 0.0100 M C6H5NH3F solution is acidic, basic, or neutral. What are the chemical and physical characteristic of HCl (hydrogen chloride)? The concentration of C6H5NH2 is 0.50 and pH is 4.20. a. 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. In the end, we will also explain how to calculate pH with an easy step-by-step solution. An aqueous solution contains dissolved C6H5NH3Cl and C6H5NH2. Relative Strength of Acids & Bases. So it will be a strong acid because as the value of ph decrease, so acidity of the solution will be increased. When we ran this reaction, there was excess weak base in solution with . [OH^-]= 7.7 x 10^-9 M is it; Determine whether a 0.0100 M NaF solution is acidic, basic, or neutral. On the basis of ph we will classify all the options. PH is defined as the negative of the base-ten logarithm of the molar concentration of hydrogen ions present in the solution. Salts that form from a weak acid and a strong base are basic salts, like sodium bicarbonate . Is an aqueous solution with pOH = 3.88 acidic, basic, or neutral? Hydroxylammonium chloride is acidic in water solution. Weak base + strong acid = acidic salt. Explain. Is an aqueous solution with OH- = 1.36 x 10-9 M acidic, basic, or neutral? Is an aqueous solution with pOH = 8.20 acidic, basic, or neutral? salt. Explain. Is an aqueous solution of {eq}CH_3NH_3Cl Is a solution with OH- = 7.9 x 10-13 M acidic, basic, or neutral? Will an aqueous solution of AgNO3 be acidic, basic, or neutral? - Sr(ClO4)2(aq) - LiNO2(aq). Is an aqueous solution with OH- = 9.8 x 10-7 M acidic, basic, or neutral? 1. Is an aqueous solution with pOH = 4.59 acidic, basic, or neutral? Explain. initial concentrations. Is an aqueous solution with pOH = 2.0 acidic, basic, or neutral? With this pH calculator, you can determine the pH of a solution in a few ways. Is an aqueous solution with OH- = 4.3 x 10-6 M acidic, basic, or neutral? Creative Commons Attribution/Non-Commercial/Share-Alike. Suppose a solution has (H3O+) = 1 x 10-9 M and (OH-) = 1 x 10-5 M. Is the solution acidic, basic, or neutral? 0.0100 M C6H5NH3Cl = Acidic because C6H5NH3Cl is a conjugate acid of aniline base. Is an aqueous solution with OH- = 2.63 x 10-4 M acidic, basic, or neutral? [OH^-]= 7.7 x 10^-9 M is it. Is a solution with OH- = 3.7 x 10-10 M acidic or basic? 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). Direct link to Apoorva Doshi's post What is the guarantee tha, Posted 7 years ago. solution of ammonium chloride. AboutTranscript. Is a solution with H+ = 6.6 x 10-6 M acidic, basic, or neutral? thus its aq. hXnF ol.m]i$Sl+IsCFhp:pk7! Direct link to cameronstuartadams's post He assumes that the initi, Posted 8 years ago. Explain. A solution has OH- = 1.3 x 10-2 M. Is this solution acidic, basic, or neutral? Explain. Ks = [Ca2+][F-]2 (b) (i) Calculate the solubility of calcium fluoride in mol L-1, at this temperature. 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? Is an aqueous solution of CH3NH3Cl acidic, basic, or neutral? 8.00 x 10-3. g of . For polyprotic acids (e.g.