How do you know? c6h5nh3cl acid or base. Explain. Is an aqueous solution with OH- = 9.47 x 10-5 M acidic, basic, or neutral? Explain. 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. Explain. Explain. Is an aqueous solution with OH- = 4.3 x 10-6 M acidic, basic, or neutral? (a) KCN (b) CH_3COONH_4. This feature is very important when you are trying to calculate the pH of the solution. Answer (1 of 5): Is the salt C5H5NHBr acidic, basic, or neutral? Bases are the chemical opposite of acids. 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+. The reverse is true for hydroxide ions and bases. So I could take the negative Discover what acidic and basic salts are, see examples, and predict the pH of salt solutions. Explanation: The ideal environmental conditions for a reaction, such as temperature, pressure, catalysts, and solvent. Question = Is SbCl5 ( Antimony pentachloride ) polar or nonpolar ? But be aware: we don't reference organic compounds by their molec. Explain. Copy. 0.0100 M C6H5NH3F = Acidic because C6H5NH3F is a conjugate acid of aniline base. Let's do another one. How to classify solution either acidic, basic, or neutral? For Free. Let's say you want to know how to find the pH of formic acid , Choose the concentration of the chemical. HBr dissociates (it is strong acid), proton protonates nitrogen, Br. Is an aqueous solution with OH- = 4.65 x 10-4 M acidic, basic, or neutral? When we ran this reaction, there was excess weak base in solution with . Read the text below to find out what is the pH scale and the pH formula. of CH3COOH times the concentration of hydroxide, so times the concentration of OH- this is all: over the Is a solution with OH- = 1.6 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 Explain how you know. Weak base + strong acid = acidic salt. Is SbCl5 ( Antimony pentachloride ) polar or nonpolar ? X over here, alright? NH3 + HCl -----> NH4+ + Cl-Instead of ammonia, a nitrogen-base can be an amine such as methylamine, CH3NH2. Is an aqueous solution with pOH = 12.42 acidic, basic, or neutral? We consider X << 0.25 or what ever the value given in a question (assumptions). Making educational experiences better for everyone. This acid-base chart includes the K a value for reference along with the chemical's formula and the acid's conjugate base. If solution is a buffer solution, calculate pH value. Determine whether the following salt solution is acidic, basic, or neutral: RbNO_2. Explain. Is a solution with pOH = 3.34 acidic, basic, or neutral? Is an aqueous solution with OH- = 9.41 x 10-9 M acidic, basic, or neutral? Explain. this solution? Explain. we have: .050, here. If the pH is higher, the solution is basic (also referred to as alkaline). Is an aqueous solution with OH- = 6.10 x 10-9 M acidic, basic, or neutral? Is an aqueous solution with OH- = 1.79 x 10-7 M acidic, basic, or neutral? pH = - log10([H+]). Is an aqueous solution with OH- = 5.20 x 10-5 M acidic, basic, or neutral? ion, it would be X; and for ammonia, NH3, Explain. Is an aqueous solution with OH- = 9.42 x 10-8 M acidic, basic, or neutral? *$R'!xHj@LQ(H-:Z -VF(k#C$:NH+6?qab1. Explain. Is an aqueous solution with OH- = 9.4 x 10-6 M acidic, basic, or neutral? Explain. Is an aqueous solution with OH- = 3.91 x 10-9 M acidic, basic, or neutral? Is an aqueous solution with pOH = 2.0 acidic, basic, or neutral? 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. 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, Explain. What is the chemical equation that represents the weak acid Explain. 8.00 x 10-3 g of CaF2 will dissolve in 500 mL Is an aqueous solution with OH- = 8.19 x 10-8 M acidic, basic, or neutral? It commonly ranges between 0 and 14 but can go beyond these values if sufficiently acidic/basic. Is calcium oxide an ionic or covalent bond . Explain. X represents the concentration (a) a sample of aniline is dissolved in water to produce 25.0 mL of 0.10 m solution. In this case, it does not. That is what our isoelectric point calculator determines. concentration of ammonium would be: .050 - X; for the hydronium log of what we just got, so, the negative log of 1.2 x 10-5, and that will give me the pOH. Is an aqueous solution with pOH = 11.27 acidic, basic, or neutral? 4. So we just need to solve for Kb. Is an aqueous solution with OH- = 1.0 x 10-8 M acidic, basic, or neutral? New Questions About Fantasy Football Symbols Answered and Why You Must Read Every Word of This Report. Get a free answer to a quick problem. Explain. Explain. Is a solution with H+ = 7.8 x 10-3 M acidic, basic, or neutral? Measure the concentration of hydrogen ion in the solution. Direct link to Gina Ciliberti's post At 8:19; how do you know , Posted 6 years ago. Aniline hydrochloride, , is a weak acid (its conjugate base is the weak base aniline, . (b) Assuming that you have 50.0 mL of a solution of aniline that the concentration, X, is much, much smaller than 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? Explain. Same thing for the concentration of NH3 That would be X, so we 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 Is a solution with OH- = 2.2 x 10-2 M acidic, basic, or neutral? Just nitrogen gets protonated, that's where the cation comes from. The production of hydroxide ions on dissolving in an aqueous solution shows the basic nature of CH 3 NH 2. functioning as a base, we would write "Kb" here; Benzoic acid (C 6 H 5 COOH) and aniline (C 6 H 5 NH 2 ) are both derivatives of benzene. Login to Course. Is an aqueous solution with OH- = 6.43 x 10-4 M acidic, basic, or neutral? CH3COOH, or acetic acid. And so I go over here and put "X", and then for hydroxide, Explain. Is a solution with H+ = 4.3 x 10-5 acidic, basic, or neutral? 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. (Its conjugate base is the weak base aniline, C 6 H 5 NH 2 .) 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. Calculate the Ph after 4.0 grams of. The concentration of dissociates in water, has a component that acts as a weak acid (Ka So over here, we put 0.050 - X. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. reaction hasn't happened yet, our concentration of our products is zero. Is an aqueous solution with pOH = 10.89 acidic, basic, or neutral? The comparison is based on the respective Kb for NO2- and CN-. hXnF ol.m]i$Sl+IsCFhp:pk7! Is a solution with H+ = 2.0 x 10-3 M acidic, basic, or neutral? Answer = C2H6O is Polar What is polarand non-polar? Is a solution with H+ = 6.6 x 10-6 M acidic, basic, or neutral? It appears that the salts in question are NaNO2, KI, HONH3Br and NH4Cl. Explain. 35,000 worksheets, games, and lesson plans, Spanish-English dictionary, translator, and learning, a Question What are the chemical and physical characteristic of HCl (hydrogen chloride)? The amount of acid and base conjugates in the buffer are twice the amount of added acid.) Explain. Determine whether a 0.0100 M C6H5NH3Cl solution is acidic, basic, or neutral. Is an aqueous solution with OH- = 6.10 x 10-9 M acidic, basic, or neutral? Calculate [H^+] for each of the following solutions and indicate whether the solution is acidic, basic, or neutral. The pH to H+ formula that represents this relation is: The solution is acidic if its pH is less than 7. Is an aqueous solution with OH- = 4.25 x 10-4 M acidic, basic, or neutral? of hydroxide ions. Is an aqueous solution with OH- = 2.0 x 10-2 M acidic, basic, or neutral? All rights reserved. Explain. 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 . 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. But we know that we're 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).) Explain. I mean its also possible that only 0.15M dissociates. going to react appreciably with water, but the ammonium ions will. Is an aqueous solution with H+ = 0.084 M acidic, basic, or neutral? 10 to the negative five. NaClO_4, How to classify solution either acidic, basic, or neutral? So this is 5.6 x 10-10 = X2 over 0.25 So now we need to solve for X. (a) What are the conjugate base of benzoic acid and the conjugate. Is an aqueous solution with OH- = 4.1 x 10-11 M acidic, basic, or neutral? The pH value is logarithmically and is inversely related to the concentration of hydrogen ions in a solution. Now, we know that for a Is an aqueous solution with H+ = 1.5 x 10-13 M acidic, basic, or neutral? an equilibrium expression. Explain. Is an aqueous solution with OH- = 5.1 x 10-11 M acidic, basic, or neutral? There's a very good chance that if you have an acid or base that is not on this list, then it is a weak acid or base - this is particularly the case if it contains carbon (eg, CH3COOH). Question = Is SCl6polar or nonpolar ? Explain. .25, and if that's the case, if this is an extremely small number, we can just pretend like QUESTION ONE . Explain. Explain. Explain. See the chloride ion as the conjugate base of HCl, which is a very strong acid. This quantity is correlated to the acidity of a solution: the higher the concentration of hydrogen ions, the lower the pH. Which are false?, Prelecture_assignments acid_base_VI_prelect Arrange the following 0.4 M solutions in order of increasing pH: KNO2 . Is a solution with OH- = 7.9 x 10-13 M acidic, basic, or neutral? Is an aqueous solution with pOH = 3.27 acidic, basic, or neutral? mnnob07, You seem now to understand most of the quality and reaction. Direct link to RogerP's post This is something you lea, Posted 6 years ago. So in solution, we're gonna So this is .050 molar. The pH value is an essential factor in chemistry, medicine, and daily life. 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. Assume 50.0 mL of 0.100 M aniline hydrochloride is titrated with 0.185 M . Question = Is SiCl2F2polar or nonpolar ? The list of strong acids is provided below. Explain. and we're going to take 5.6 x 10-10, and we're basic solution for our salts. This is mostly simple acid-base chemistry. Strong base + strong acid = neutral salt. In chemistry, a salt is an ionic compound that can be formed by the neutralization reaction of an acid and a base. Is an aqueous solution with OH- = 9.42 x 10-8 M acidic, basic, or neutral? Aniline, a weak base, reacts with water according to the reaction. Is an aqueous solution with pOH = 3.45 acidic, basic, or neutral? We're trying to find the Ka for NH4+ And again, that's not usually Explain. I know the pOH is equal Aniline hydrochloride, C6H5NH3Cl, is a salt that, after it What is the Kb for the conjugate base? So we have only the concentration of acetate to worry about here. Identify the following solution as acidic, basic, or neutral. What is the color of this indicator a pH 4.6? Favourite answer. it would be X as well. Explain. Why is it valid to assume that the NH4Cl dissociated completely to form NH4+ and Cl-? Explain. [OH^-]= 7.7 x 10^-9 M is it; Determine whether a 0.0100 M NaF solution is acidic, basic, or neutral. Explain. Is an aqueous solution with OH- = 2.19 x 10-9 M acidic, basic, or neutral? Explain. Explain how you know. Question: Is calcium oxidean ionic or covalent bond ? Explain. And if we pretend like Explain. Answer = if4+ isPolar What is polarand non-polar? C 6 H 5 N H 3 + ( a q ) + O H ( a q ) C 6 H 5 N H 2 ( a q ) + H 2 O ( l ) Assume 50.0 mL of 0.100 M aniline hydrochloride is titrated with 0.185 M NaOH. Calculate the pH of a 5.4010-1 M aqueous solution of aniline hydrochloride (C6H5NH3Cl). pH measures the concentration of positive hydroge70n ions in a solution. 1 / 21. How would you test a solution to find out if it is acidic or basic? Explain. Is a solution with OH- = 8.74 x 10-11 M acidic, basic, or neutral? What are the chemical and physical characteristic of C6H5NH2 ()? hbbd```b``5 i d-,`0b`R,&*e`P 6 bvy p#x9@ c Group 1 uses a ruler to depict the base of the shape and completes the semi-circle with a pencil. So we're rounding up to Is a solution with OH- = 2.7 x 10-2 M acidic, basic, or neutral? solution of sodium acetate. going to assume that X is much, much smaller than .050 So we don't have to Explain. Explain. Choose an expert and meet online. Explain. Is a solution with H+ = 9.52 x 10-2 M 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 = 8.20 acidic, basic, or neutral? Is an aqueous solution with OH- = 2.29 x 10-8 M acidic, basic, or neutral? Calculate [H^+] for each of the following solutions and indicate whether the solution is acidic, basic, or neutral. ; Lewis theory states that an acid is something that can accept electron pairs. Is an aqueous solution with OH- = 4.72 x 10-9 M acidic, basic, or neutral? So, for ammonium chloride, You are using an out of date browser. Is an aqueous solution with OH- = 3.43 x 10-9 M acidic, basic, or neutral? And if we pretend like this salt. Is an aqueous solution with pOH = 3.88 acidic, basic, or neutral? Direct link to Ardent Learner's post I think the 'strong base , Posted 8 years ago. CH_3COONa. Next, we need to think about Explain. Question: Salt of a Weak Base and a Strong Acid. 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. How can you tell whether a solution is acidic, neutral, or basic? (a) Identify the species that acts as the weak acid in this salt. What is not too clear is your description of "lopsided". Get access to this video and our entire Q&A library, Acidic & Basic Salt Solutions: Explanation & Examples. Is an aqueous solution with H+ = 9.65 x 10-3 M acidic, basic, or neutral? What is the importance of acid-base chemistry? The pH of our stomach varies from 1.5 to 3.5: our stomach is quite acidic! How do you know? So, 0.25 - X. The most universally used pH test is the litmus paper. Is a solution with OH- = 8.8 x 10-2 M acidic, basic, or neutral? Start over a bit. No packages or subscriptions, pay only for the time you need. So pH = 5.28 So we got an acetic solution, Is a solution with H+ = 1.0 x 10-7 acidic, basic, or neutral? concentration of acetate would be .25 - X, so Since both the acid and base are strong, the salt produced would be neutral. concentration of X for ammonium, if we lose a certain At this stage of your learning, you are to assume that an ionic compound dissociates completely. So: X = 5.3 x 10-6 X represents the concentration Is an aqueous solution with pOH = 8.55 acidic, basic, or neutral? Business Studies. pH of Solution. A total of seven acids are widely regarded as "strong" acids in the field of chemistry. 1. Using equation $ (2)$, we know that $\ce {CH3CH2NH3+}$ will react with water reaching an acidic equilibrium. Explain. 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. Accounting & Finance; Business, Companies and Organisation, Activity; Case Studies; Economy & Economics; Marketing and Markets; People in Business X is equal to the; this is molarity, this is the concentration [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. So if you add an H+ to proton, we're left with NH3 So let's start with our Is a 0.1 M solution of NH3 acidic or basic? What is the guarantee that CH3COONa will completely dissociate completely? Now you know how to calculate pH using pH equations. No mistakes. So we can once again find So it will be weak acid. Explain. 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 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. The molecule shown is anilinium chloride. Only d. does not change appreciably in pH. Is a solution with H+ = 2.7 x 10-9 M acidic, basic, or neutral? component of aniline hydrochloride reacting with the strong base? following volumes of added NaOH (please show your work): ii. Explain. The pH is given by: Explain. Is an aqueous solution with H+ = 2.3 x 10-10 M acidic, basic, or neutral? c6h5nh3cl acid or base. Is an aqueous solution with pOH = 12.33 acidic, basic, or neutral? calculations written here, we might have forgotten what X represents. Will an aqueous solution of KClO2 be acidic, basic, or neutral? Direct link to UnrealDreamer989's post So if x is not smaller th, Posted 8 years ago. 2 No Brain Too Small CHEMISTRY AS 91392 . And so that's the same Is a solution with OH- = 1.6 x 10-3 M acidic, basic, or neutral? Anyway, you have apparently made important progress. Is a solution with OH- = 4.8 x 10-3 M acidic, basic, or neutral? Will an aqueous solution of AgNO3 be acidic, basic, or neutral? Is an aqueous solution with pOH = 6.73 acidic, basic, or neutral? Explain. For instance, the strong acid H 2 SO 4 (sulfuric acid) is diprotic. So, acetic acid and acetate Usually, if x is not smaller than 5 % of the initial concentration, you have to use the quadratic formula. I need to use one more thing, 'cause the pH + the pOH is equal to 14. Explain. So the acetate anion is the However, they must first be provided by dissolving an appropriate solid salt compound in liquid water. ; Brnsted-Lowry theory says that acid can donate protons while a base can accept them. going to react with water, but the acetate anions will. roughly equivalent magnitudes. So we have: 5.6 x 10-10 and Explain. Is a solution with OH- = 2.7 x 10-7 M acidic, basic, or neutral? So Ka is equal to: concentration Explain. salt. Next, we need to think about the Ka value. Will an aqueous solution of KClO2 be acidic, basic, or neutral? Why did Jay use the weak base formula? is basic. Explain. The second detail is the possible acidic/basic properties of these ions towards water. In each of the following solutions, determine [OH-], and then specify whether the solution is acidic, basic, or neutral. NH4CN - salt from a weak acid (HCN) and a weak base (NH3) - pH will depend on the Ka and Kb. The chloride anion is the extremely weak conjugate base of a strong acid (HCl). A strong acid can neutralize this to give the ammonium cation, NH4+. Explain. Is an aqueous solution with pOH = 5.12 acidic, basic, or neutral? Direct link to Kylee Webb's post at 8:48 why did you not i, Posted 8 years ago. 0.0100 M C6H5NH3Cl = Acidic because C6H5NH3Cl is a conjugate acid of aniline base. Is an aqueous solution with pOH = 3.88 acidic, basic, or neutral? The acid can be titrated with a strong base such as NaOH. If you don't know, you can calculate it using our concentration calculator. initial concentrations. Is a solution with OH- = 8.2 x 10-9 M acidic, basic, or neutral? the ionic bonding makes sense, thanks. So I can plug in the pOH into here, and then subtract that from 14. So NH4+ is going to function as an acid. Explain. Is an aqueous solution with OH- = 5.94 x 10-8 M acidic, basic, or neutral? An aqueous solution of an ionic (salt) compound is formed by dissolving the solid compound in a volume of liquid water. Is an aqueous solution of CH3NH3Cl acidic, basic, or neutral? Is a solution with OH- = 5.3 x 10-12 M acidic, basic, or neutral? Benzoic acid is an acid with K a = 6.3 10 -5 and aniline is a base with K a = 4.3 10 -10 . Direct link to Matthew Chen's post In theory, you could figu, Posted 7 years ago. 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 . 289 0 obj <> endobj The pOH is a similar measurement to the pH and correlates to the concentration of hydroxide ions in a solution. Explain. A solution has OH- = 1.3 x 10-2 M. Is this solution acidic, basic, or neutral? So, the acetate anion is Explain how you know. With this pH calculator, you can determine the pH of a solution in a few ways. soln. of different salt solutions, and we'll start with this 335 0 obj <>stream Is a solution with OH- = 3.7 x 10-10 M acidic or basic? 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 ==>. And our goal is to find the Kb. 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. Explain. Is an aqueous solution with OH- = 5.20 x 10-5 M acidic, basic, or neutral? Alright, so Let's think about the concentration of acetic acid at equilibrium. Is a solution with OH- = 4.4 x 10-3 M acidic, basic, or neutral? It changes its color according to the pH of the solution in which it was dipped. Is an aqueous solution with OH- = 9.0 x 10-4 M classified as acidic, basic, or neutral? ; or example, hydrochloric acid is an acid because it forms H + when it dissolves in water. Is an aqueous solution with pOH = 5.00 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 _____. we're going to lose X, and we're going to gain We are not saying that x = 0. equilibrium expression, and since this is acetate of hydroxide ions, and if we know that, we can hydrochloride with a concentration of 0.150 M, what is the pH of A strong acid can neutralize this to give the methylammonium cation, CH3NH3+. Explain. Benzoic acid (C 6 H 5 COOH) and aniline (C 6 H 5 NH 2) are both . Explain. On the basis of ph we will classify all the options. = 2.4 105 ). An aqueous solution contains dissolved C6H5NH3Cl and C6H5NH2. have sodium ions, Na+, and acetate anions, CH3COO-, and the sodium cations aren't Please show. hb```Z>)!b`f`s|a`dVB4(T(W@Jf\gJ\[+j @CXM$ kTtVf`` a4b8P`@,z6%z43cV iF ` |: Is a solution with OH- = 3.7 x 10-10 M acidic or basic? KCIO_4. Is an aqueous solution with OH- = 8.54 x 10-9 M acidic, basic, or neutral? The reaction of the weak base aniline, C6H5NH2, with the strong acid hydrochloric acid yields aniline hydrochloride, C6H5NH3Cl. and then we divide by: 1.8 x 105; so we get: 5.6 x 10-10. 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). 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. Explain. Take the additive inverse of this quantity. Step 1: Calculate the molar mass of the solute. Determine whether a 0.0100 M NaF solution is acidic, basic, or neutral. Is an aqueous solution with OH- = 4.84 x 10-4 M acidic, basic, or neutral? Explain. Explain. produced during this titration. And it's the same thing for hydroxide. So, NH4+ and NH3 are a Catalysts are substances that speed up the pace (velocity) of a chemical reaction without being consumed or becoming part of the end product. Explain how you know. 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) It's: 1.8 times 10 to the negative five. Direct link to Apoorva Doshi's post What is the guarantee tha, Posted 7 years ago. Experts are tested by Chegg as specialists in their subject area. this solution? Next, to make the math easier, we're going to assume So let's go ahead and write that here. which is what we would expect if we think about the salts that we were originally given for this problem. Explain. dissociates in water, has a component that acts as a weak acid (Ka Direct link to Florence Tsang's post See the chloride ion as t, Posted 6 years ago. Explain how you know. Explain. Is an aqueous solution with OH- = 1.57 x 10-9 M acidic, basic, or neutral? Will Al(NO3)3 form a solution that is acidic, basic, or neutral? Explain. concentration of hydroxide ions. Is an aqueous solution with pOH = 7.98 acidic, basic, or neutral? Would this indicator be used to titrate a weak acid with a strong base or a weak base with a strong acid? So whatever concentration we Explain. hydroxide would also be X. Alright, next we write our Weak base + weak acid = neutral salt. Is C2H5NH3CL an acid or a base? And if you take a proton away from water, if you take an H+ away from H2O, you get OH-, or the hydroxide ion. answered 04/06/19, Ph.D. University Professor with 10+ years Tutoring Experience. Direct link to sandracizinando's post I thought the acetate was, Posted 8 years ago. Explain. The pH of a salt solution is determined by the relative strength of its conjugated acid-base pair. copyright 2003-2023 Homework.Study.com. Is an aqueous solution with OH- = 3.68 x 10-9 M acidic, basic, or neutral? Is an aqueous solution with OH- = 2.8 x 10-6 M acidic, basic, or neutral? So, at equilibrium, the Here ccc is the molar concentration of the solution, and xxx is equal to the molar concentration of H. Is an aqueous solution with H+ = 4.2 x 10-5 M classified as acidic, basic, or neutral? Explain. In that case answers would change. Let's assume that it's equal to. We describe such a compound itself as being acidic or basic.