pH of our solution, and we're starting with .050 molar Is an aqueous solution with pOH = 10.53 acidic, basic, or neutral? log of what we just got, so, the negative log of 1.2 x 10-5, and that will give me the pOH. Explain. following volumes of added NaOH (please show your work): ii. Term. 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. Next, we need to think about KCIO_4. (All hydrogen halides are strong acids, except for HF). component of aniline hydrochloride reacting with the strong base? Explain. acetic acid would be X. functioning as a base, we would write "Kb" here; Is an aqueous solution with pOH = 5.12 acidic, basic, or neutral? Explain. 1 answer; geometry; asked by Anonymous; 383 views; Two groups of students are asked to depict a picture of a semi-circular pizza. Just nitrogen gets protonated, that's where the cation comes from. Cl- is a very weak conjugate base so its basicity is negligible. Explain. Is an aqueous solution with H+ = 9.65 x 10-3 M acidic, basic, or neutral? (K a for aniline hydrochloride is 2.4 x 10-5). 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. Will an aqueous solution of AgNO3 be acidic, basic, or neutral? Is an aqueous solution with OH- = 9.57 x 10-9 M acidic, basic, or neutral? We describe such a compound itself as being acidic or basic. Explain. What are the chemical reactions that have HCl (hydrogen chloride) as prduct? Is an aqueous solution with pOH = 4.59 acidic, basic, or neutral? Aniline hydrochloride, C6H5NH3Cl, is a salt that, after it it's pretty close to zero, and so .25 - X is pretty Is an aqueous solution with OH- = 4.25 x 10-4 M acidic, basic, or neutral? iii. I know the pOH is equal Relative Strength of Acids & Bases. mnnob07, You seem now to understand most of the quality and reaction. Explain. Explain. This answer is: Study guides. Is a 1.0 M KBr solution acidic, basic, or neutral? 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. Is an aqueous solution with OH- = 5.20 x 10-5 M acidic, basic, or neutral? The reaction of the weak base aniline, C6H5NH2, with the strong acid hydrochloric acid yields aniline hydrochloride, C6H5NH3Cl. (b) Assuming that you have 50.0 mL of a solution of aniline Explain. The unit for the concentration of hydrogen ions is moles per liter. anion, when it reacts, is gonna turn into: From the periodic table the molar masses of the compounds will be extracted. Select your chemical and its concentration, and watch it do all the work for you. Explain. Will an aqueous solution of KClO2 be acidic, basic, or neutral? It is also useful to have memorized the common strong acids and bases to determine whether KCl acts as an acid or base in water (or if it forms a neutral solution).Note that we are talking about whether KCl is an acid, base, or neutral when dissolved in water.- Salts of strong bases and strong acids: pH will remain neutral at 7.- Salts of weak bases and strong acids: pH less than 7 (acidic).- Salts from strong bases and weak acids: pH greater than 7 (alkaline). Suppose a solution has (H3O+) = 1 x 10-9 M and (OH-) = 1 x 10-5 M. Is the solution acidic, basic, or neutral? Is an aqueous solution of Na2SO3 acidic, basic, or neutral? Explain. So, for ammonium chloride, and we're going to take 5.6 x 10-10, and we're So in solution, we're gonna Therefore the salt is acidic because of CH3NH3+, a Bronsted acid. So, acetic acid and acetate Is a solution with OH- = 8.74 x 10-11 M acidic, basic, or neutral? proton, we're left with NH3 So let's start with our Strong base + strong acid = neutral salt. Explain. an equilibrium expression. Is an aqueous solution with OH- = 5.94 x 10-8 M acidic, basic, or neutral? CH3NH3Cl is an ionic compound, consisting of CH3NH3+ and Cl- ions. Username. Login to Course. Explain. Expert Answer. Alright, so at equilibrium, QUESTION ONE . To calculate the pH of a buffer, go to the, Check out 20 similar mixtures and solutions calculators , How to calculate pH? (a) a sample of aniline is dissolved in water to produce 25.0 mL of 0.10 m solution. wildwoods grill food truck menu is titrated with 0.300 M NaOH. [Hint: this question should Explain. There was no strong acid or strong base for the weak species to react with, so we knew that we only had to set up an aqueous equilibrium between the conjugate acid/base pair and use Henderson Hasselbalch to find pH. The Bronsted-Lowry theory of acids and bases describes a transfer of ionized hydrogen atoms (protons) from acids to bases in an aqueous solution. Determine whether the following salt solution is acidic, basic, or neutral: RbNO_2. Explain. Is an aqueous solution with OH- = 8.0 x 10-10 M acidic, basic, or neutral? . And so that's the same Createyouraccount. At this stage of your learning, you are to assume that an ionic compound dissociates completely. Is an aqueous solution with OH- = 2.37 x 10-8 M acidic, basic, or neutral? If solution is a buffer solution, calculate pH value. The concentration of hydroxide So we now need to take the Is a solution with OH- = 3.7 x 10-10 M acidic or basic? Will an aqueous solution of KClO2 be acidic, basic, or neutral? So, at equilibrium, the Explain how you know. Is a solution with H+ = 6.6 x 10-6 M acidic, basic, or neutral? 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? Explain. Explain. 335 0 obj <>stream Direct link to Kylee Webb's post at 8:48 why did you not i, Posted 8 years ago. The pH of a salt solution is determined by the relative strength of its conjugated acid-base pair. Is an aqueous solution with OH- = 6.10 x 10-9 M acidic, basic, or neutral? The equivalence point [Hint: at this point, the weak acid and Explain. Explain. (a) Identify the species that acts as the weak acid in this Business Studies. Distinguish if a salt is acidic or basic and the differences. it's the same thing, right? A strong acid can neutralize this to give the ammonium cation, NH4+. 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 ). Is an aqueous solution with pOH = 4.78 acidic, basic, or neutral? Is an aqueous solution with OH- = 9.41 x 10-9 M acidic, basic, or neutral? Explain. So if we make the concentration of the acetate anion, X, that reacts Alright, so, X reacts. Direct link to Aswath Sivakumaran's post We consider X << 0.25 or , Posted 8 years ago. the amount of added acid does not overwhelm the capacity of the buffer. Weak base + weak acid = neutral salt. Is a solution with OH- = 1.1 x 10-11 M acidic, basic, or neutral? Would an aqueous solution with OH- = 7.4 x 10-12 M be acidic, basic, or neutral? Explain. reaction hasn't happened yet, our concentration of our products is zero. 35,000 worksheets, games, and lesson plans, Spanish-English dictionary, translator, and learning, a Question NH4CN - salt from a weak acid (HCN) and a weak base (NH3) - pH will depend on the Ka and Kb. Question = Is C2Cl2polar or nonpolar ? which is what we would expect if we think about the salts that we were originally given for this problem. Is a solution with OH- = 1.6 x 10-4 M acidic, basic, or neutral? Direct link to AJ's post Why doesn't Na react with, Posted 6 years ago. About Press Copyright Contact us Creators Advertise Developers Terms Privacy Policy & Safety How YouTube works Test new features Press Copyright Contact us Creators . Bases are the chemical opposite of acids. I mean its also possible that only 0.15M dissociates. Calculate [H^+] for each of the following solutions and indicate whether the solution is acidic, basic, or neutral. Is an aqueous solution with pOH = 3.27 acidic, basic, or neutral? This produces a dissociation reaction to form the constituent ions in a certain stoichiometry. Is a solution with OH- = 2.7 x 10-7 M acidic, basic, or neutral? Explain. Is an aqueous solution with OH- = 2.19 x 10-9 M acidic, basic, or neutral? solution of sodium acetate. Direct link to Ernest Zinck's post When we have 0.25 - x, we, Posted 8 years ago. Explain. Is an aqueous solution with pOH = 10.89 acidic, basic, or neutral? 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). Is a solution with OH- = 8.2 x 10-9 M acidic, basic, or neutral? Explain. This is the concentration This acid-base chart includes the K a value for reference along with the chemical's formula and the acid's conjugate base. Using equation $ (2)$, we know that $\ce {CH3CH2NH3+}$ will react with water reaching an acidic equilibrium. Is an aqueous solution with pOH = 3.22 acidic, basic, or neutral? Well, we're trying to find the Explain. Explain. CH_3COONa. hXnF ol.m]i$Sl+IsCFhp:pk7! Is a solution with OH- = 4.8 x 10-3 M acidic, basic, or neutral? going to assume that X is much, much smaller than .050 So we don't have to Explain. Is an aqueous solution with OH- = 8.19 x 10-8 M acidic, basic, or neutral? Question = Is C2H6Opolar or nonpolar ? Our calculator may ask you for the concentration of the solution. Explain. Let's do another one. 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. 0 is basic. Predict whether the solution of the following will be acidic, basic, or neutral, and explain the answer. The pH to H+ formula that represents this relation is: The solution is acidic if its pH is less than 7. Apart from the mathematical way of determining pH, you can also use pH indicators. much the same thing as 0.25. And it's the same thing for hydroxide. Explain. Is a solution with OH- = 7.3 x 10-8 M acidic, basic, or neutral? On the basis of ph we will classify all the options. 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. Explain. Explain. Is an aqueous solution with OH- = 4.88 x 10-7 M acidic, basic, or neutral? Is an aqueous solution with OH- = 5.0 x 10-5 M acidic, basic, or neutral? of ammonium ions, right? Explain. Is an aqueous solution with pOH = 10.57 acidic, basic, or neutral? Calculate the base 10 logarithm of this quantity: log10([H+]). You and I don't actually know because the structure of the compound is not apparent in the molecular formula. hydrochloride with a concentration of 0.150 M, what is the pH of 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. Why did Jay use the weak base formula? 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) %%EOF Is an aqueous solution with pOH = 5.00 acidic, basic, or neutral? Definition. Explain. Explain. Is an aqueous solution with pOH = 2.0 acidic, basic, or neutral? Is an aqueous solution with OH- = 5.1 x 10-11 M acidic, basic, or neutral? So the acetate anion is the Explain. Is an aqueous solution with OH- = 3.91 x 10-9 M acidic, basic, or neutral? Explain. of hydroxide ions, and if we know that, we can 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? Due to this we take x as 0. next to the solution that will have the next lowest pH, and so on. Explain. ion, it would be X; and for ammonia, NH3, It can be protonated to form hydronium ion or deprotonated (dissociated) to form hydroxide ion. Is an aqueous solution with OH- = 3.59 x 10-3 M acidic, basic, or neutral? Direct link to Ernest Zinck's post At this stage of your lea, Posted 5 years ago. put an "X" into here. Is an aqueous solution with pOH = 6.48 acidic, basic, or neutral? So, NH4+ and NH3 are a Explain. Is an aqueous solution with OH- = 6.43 x 10-4 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. In each of the following solutions, determine [OH-], and then specify whether the solution is 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. it would be X as well. Is an aqueous solution with OH- = 2.2 x 10-10 M acidic, basic, or neutral? Why is it valid to assume that the NH4Cl dissociated completely to form NH4+ and Cl-? Is an aqueous solution with OH- = 2.7 x 10-5 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. Is a solution with OH- = 1 x 10-9 M acidic, basic, or neutral? Explain. Is an aqueous solution with OH- = 8.54 x 10-9 M acidic, basic, or neutral? be X squared over here And once again, we're (a) Identify the species that acts as the weak acid in this salt. So are we to assume it dissociates completely?? Explain. Explain how you know. No mistakes. 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. 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). Is an aqueous solution with H+ = 6.65 x 10-3 M acidic, basic, or neutral? c6h5nh3cl acid or base. Experts are tested by Chegg as specialists in their subject area. Now, we know that for a Createyouraccount. 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 Group 2 uses a ruler to make a line of 10 inches to depict the base of the. Explain. of hydronium ions, so to find the pH, all we have to do is take the negative log of that. Hoh Aqua [Oh2] HO Oxidane Pure Water Hydroxic Acid Hydrogen Oxide H2O Molar Mass H2O Oxidation Number. If you're seeing this message, it means we're having trouble loading external resources on our website. And then, for the concentration of acetate at equilibrium, concentration of acetate is zero point two five minus X. Is a solution with OH- = 4.00 x 10-5 M acidic, basic, or neutral? Explain. Explain. Read the text below to find out what is the pH scale and the pH formula. But we know that we're Explain how you know. we have NH4+ and Cl- The chloride anions aren't But be aware: we don't reference organic compounds by their molec. 8.00 x 10-3 g of CaF2 will dissolve in 500 mL The chloride anion is the extremely weak conjugate base of a strong acid (HCl). How can a base be used to neutralize an acid? concentration of our acetate anion, here, so we're gonna write: 0.25 molar, for the initial concentration of the acetate anion. we're going to multiply that, we're going to multiply that, by .25 And so we get 1.4 x 10-10. So we have: 5.6 x 10-10 and Anyway, you have apparently made important progress. Is an aqueous solution with OH- = 3.47 x 10-6 M acidic, basic, or neutral? These colors often inspire colorful pH scales: The ph in our bodies is close to neutral. What are the chemical reactions that have C6H5NH2 () as reactant? soln. Is a solution with OH- = 2.7 x 10-2 M acidic, basic, or neutral? Explain. Is an aqueous solution with OH- = 4.1 x 10-11 M acidic, basic, or neutral? So let's go ahead and write that here. 2003-2023 Chegg Inc. All rights reserved. New Questions About Fantasy Football Symbols Answered and Why You Must Read Every Word of This Report. Is an aqueous solution with OH- = 4.3 x 10-6 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. the pH of our solution. Is a solution with OH- = 1.0 x 10-7 M acidic, basic, or neutral? endstream endobj startxref The pH of a salt solution is determined by the relative strength of its conjugatedacid-base pair. Is an aqueous solution with OH- = 1.37 x 10-6 M acidic, basic, or neutral? We get out the calculator, Explain. Explain. Is a solution with OH- = 2.21 x 10-7 M acidic, basic, or neutral? Explain. 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. 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 Identify the following solution as acidic, basic, or neutral. A total of seven acids are widely regarded as "strong" acids in the field of chemistry. For polyprotic acids (e.g. What is the guarantee that CH3COONa will completely dissociate completely? Explain. Is an aqueous solution with OH- = 3.84 x 10-7 M acidic, basic, or neutral? Determine whether a 0.0100 M NaCl solution is acidic, basic, or neutral. Explain. 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 _____. A lot of these examples require calculators and complex methods of solving.. help! Is a solution with OH- = 1.53 x 10-7 M acidic, basic, or neutral? It can convert pH to H+, as well as calculate pH from the ionization constant and concentration. Is an aqueous solution with pOH = 5.27 acidic, basic, or neutral? Calculate the pH of a solution containing the result of the addition of 0.5 moles HCl to a 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. darius the destroyer record / how to change facebook color back to normal / c6h5nh3cl acid or base. Click the card to flip . Is a solution with OH- = 7.9 x 10-13 M acidic, basic, or neutral? Explain. Group 1 uses a ruler to depict the base of the shape and completes the semi-circle with a pencil. It commonly ranges between 0 and 14 but can go beyond these values if sufficiently acidic/basic. going to react with water, and it's gonna function as a base: it's going to take a proton from water. House products like drain cleaners are strong bases: some can reach a pH of 14! Is an aqueous solution with OH- = 1.79 x 10-7 M acidic, basic, or neutral? So if we lose a certain 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. Explain. Note that there is no $\ce {OH-}$ to start with (very little in reality), so equation $ (1)$ is not applicable. Determine whether a 0.0100 M NaF solution is acidic, basic, or neutral. Alright, so Let's think about the concentration of acetic acid at equilibrium. You can also use the solution dilution calculator to calculate the concentration of ions in a diluted solution. hydronium ions at equilibrium is X, so we put an "X" in here. Favourite answer. Is an aqueous solution with OH- = 2.8 x 10-6 M acidic, basic, or neutral? Is an aqueous solution with pOH = 9.42 acidic, basic, or neutral? This feature is very important when you are trying to calculate the pH of the solution. 2, will dissolve in 500 mL of water. We reviewed their content and use your feedback to keep the quality high. Salt of a Weak Base and a Strong Acid. Is an aqueous solution with pOH = 8.20 acidic, basic, or neutral? Next, we think about the change, and since NH4+ turns into NH3, whatever we lose for NH4+ is what we gain for NH3. Is a solution with H+ = 2.0 x 10-3 M acidic, basic, or neutral? So over here, we put 0.050 - X. CH3COO-, you get CH3COOH. That was our original question: to calculate the pH of our solution. going to react with water, but the acetate anions will. What is the Kb for the conjugate base? salt. hb```Z>)!b`f`s|a`dVB4(T(W@Jf\gJ\[+j @CXM$ kTtVf`` a4b8P`@,z6%z43cV iF ` |: Get access to this video and our entire Q&A library, Acidic & Basic Salt Solutions: Explanation & Examples. Is an aqueous solution with OH- = 1.36 x 10-9 M acidic, basic, or neutral? Is an aqueous solution with pOH = 12.33 acidic, basic, or neutral? So we can just plug that into here: 5.3 x 10-6, and we can So we have the concentration and then we divide by: 1.8 x 105; so we get: 5.6 x 10-10. So if H2O accepts a proton, that turns into hydronium ions, so H3O+ And if NH4+ loses a I need to use one more thing, 'cause the pH + the pOH is equal to 14. Explain. The molecule shown is anilinium chloride. Explain. Explain. concentration of acetate would be .25 - X, so 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. (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. Explain. This is all over, the Aniline hydrochloride, , is a weak acid (its conjugate base is the weak base aniline, . Explain. Is an aqueous solution with pOH = 3.88 acidic, basic, or neutral? Calculate [H^+] for each of the following solutions and indicate whether the solution is acidic, basic, or neutral. (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? Calculate the concentration of C6H5NH3+ in this buffer solution. An aqueous solution contains dissolved C6H5NH3Cl and C6H5NH2. Password. be approached exactly as you would a salt solution. If you're behind a web filter, please make sure that the domains *.kastatic.org and *.kasandbox.org are unblocked. [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? Explain. And this is equal to X squared, equal to X2 over .25 - X. Is an aqueous solution with OH- = 6.10 x 10-9 M acidic, basic, or neutral? Explain. 1. Note: in the first four problems, I give the K a of the conjugate acid (for example, the ammonium ion in Example #1). c6h5nh3cl acid or base. Some species are amphiprotic (both acid and base), with the common example being water. For example, in determining ranking between NaNO2 and NH4CN, one looks at hydrolysis where NO2- ==>HNO2 + OH- and compares it to CN- ==> HCN + OH-. The kind of salt formed depends on the acid and base that combined to yield the salt.. We have to know that the pH of a salt solution depends on the acid and base that reacts to form the salt.. A weak acid reacts with a strong base to yield a salt that gives a basic solution; A strong acid reacts with a weak base to give a salt that yields an acidic solution; A strong acid and a strong base . The pH value is an essential factor in chemistry, medicine, and daily life. Explain. Let's say that you started with an initial concentration of 5*10-8 M NH4Cl and you solve this problem using the method shown. Salts can be acidic, neutral, or basic. We know Kb is 1.8 x 10-5 This is equal to: 1.0 times Is a solution with OH- = 5.3 x 10-12 M acidic, basic, or neutral? salt. Become a Study.com member to unlock this answer! So CH3COO-, the acetate To log in and use all the features of Khan Academy, please enable JavaScript in your browser. Discover what acidic and basic salts are, see examples, and predict the pH of salt solutions. Next, we need to think about the Ka value. Determine whether a 0.0100 M C6H5NH3F solution is acidic, basic, or neutral. Ka on our calculator. Explain. Explain. Label Each Compound With a Variable. If X concentration reacts, roughly equivalent magnitudes. Explain. The first detail is the identities of the aqueous cations and anions formed in solution. 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. I thought H2O is polar and attracts Na? Suppose a solution has (H3O+) = 1 x 10-13 M and (OH-) = 1 x 10-1 M. Is the solution acidic, basic, or neutral? Calculators are usually required for these sorts of problems.