Because the hydrogen ion concentration is 1.0 107 M in pure water at 25C, the pH of pure liquid water (and, by extension, of any neutral solution) is, \[ pH = -log[1.0 \times 10^{-7}] = 7.00\]. What specific point does the BrnstedLowry definition address? . It explains how to balance the chemical equation, . Chemistry of buffers and buffers in our blood. When a strong acid dissolves in water, the proton that is released is transferred to a water molecule that acts as a proton acceptor or base, as shown for the dissociation of sulfuric acid: \[ \underset{acid\: (proton\: donor)}{H_2 SO_4 (l)} + \underset{base\: (proton\: acceptor)} {H_2 O(l)} \rightarrow \underset{acid}{H _3 O^+ (aq)} + \underset{base}{HSO_4^- (aq)} \]. Why was it necessary to expand on the Arrhenius definition of an acid and a base? What is the complete ionic equation for each reaction? Strong acid solutions. If organic, identify the compound as a weak base or a weak acid by the presence of an amine or a carboxylic acid group, respectively. In fact, this is only one possible set of definitions. It dissociates completely in an aqueous solution and gives arise to H+ and Cl-. The salt that is formed comes from the acid and base. The reaction of a weak acid and a strong base will go to completion, so it is reasonable to prepare calcium propionate by mixing solutions of propionic acid and calcium hydroxide in a 2:1 mole ratio. The proton and hydroxyl ions combine to Solve Now 10 word . For example, pH paper consists of strips of paper impregnated with one or more acidbase indicatorsAn intensely colored organic molecule whose color changes dramatically depending on the pH of the solution., which are intensely colored organic molecules whose colors change dramatically depending on the pH of the solution. Explain how an aqueous solution that is strongly basic can have a pH, which is a measure of the acidity of a solution. For example, monoprotic acids (a compound that is capable of donating one proton per molecule) are compounds that are capable of donating a single proton per molecule. Ammonia reacts with nitric acid (HNO3) which is a strong acid to yield to slightly acidic salt named ammonium nitrate. We can summarize the relationships between acidity, basicity, and pH as follows: Keep in mind that the pH scale is logarithmic, so a change of 1.0 in the pH of a solution corresponds to a tenfold change in the hydrogen ion concentration. The proton and hydroxyl ions combine to. Write a balanced chemical equation for the reaction of aqueous propionic acid (CH3CH2CO2H) with aqueous calcium hydroxide [Ca(OH)2] to give calcium propionate. . Acid Base Neutralization Reactions & Net Ionic Equations Example: Writing a Molecular Equation for a Neutralisation Reaction. compound that can donate two protons per molecule in separate steps). Classify each compound as a strong acid, a weak acid, a strong base, a weak base, or none of these. Acid-Base Reaction. The reaction between strong hydrochloric acid and strong sodium hydroxide gives out water and NaCl (Table salt). The BrnstedLowry definition of a base, however, is far more general because the hydroxide ion is just one of many substances that can accept a proton. The most common strong bases are ionic compounds that contain the hydroxide ion as the anion; three examples are NaOH, KOH, and Ca(OH)2. Therefore, these reactions tend to be forced, or driven, to completion. Propose a method for preparing the solution. Step 1/3. For example, a 1.0 M solution of a strong monoprotic acid such as HCl or HNO3 has a pH of 0.00: Conversely, adding a base to pure water increases the hydroxide ion concentration and decreases the hydrogen ion concentration. The conjugate acid in a reaction will contain one more H atom and one more + charge than the base. Although these definitions were useful, they were entirely descriptive. Write the balanced chemical equation for each reaction. Write a balanced chemical equation for the reaction of solid sodium acetate with dilute sulfuric acid to give sodium sulfate. \(2CH_3CO_2Na(s) + H_2SO_4(aq) \rightarrow Na_2SO_4(aq) + 2CH_3CO_2H(aq)\). Ammonia (NH3) is a weak base available in gaseous form. The reaction is an acid-base neutralization reaction. \(HClO_4(l) \rightarrow H^+(aq) + ClO_4^-(aq)\), The H+ ion concentration is therefore the same as the perchloric acid concentration. Acids differ in the number of protons they can donate. What is the concentration of commercial vinegar? Again, the double arrow indicates that the reaction does not go to completion but rather reaches a state of equilibrium. For the sake of brevity, however, in discussing acid dissociation reactions, we often show the product as \(H^+_{(aq)}\) (as in Equation \(\PageIndex{7}\) ) with the understanding that the product is actually the\(H_3O^+ _{(aq)}\) ion. Because of its more general nature, the BrnstedLowry definition is used throughout this text unless otherwise specified. If the protective lining of the stomach breaks down, this acid can attack the stomach tissue, resulting in the formation of an ulcer. Because the gaseous product escapes from solution in the form of bubbles, the reverse reaction cannot occur. If we are dealing with a weak acid (or base) then the Ka (or pKa) of the acid must be known. The overall reaction is therefore simply the combination of H+(aq) and OH(aq) to produce H2O, as shown in the net ionic equation: \[ H^+(aq) + OH^-(aq) \rightarrow H_2O(l) \)]. In contrast, only a fraction of the molecules of weak acids (An acid in which only a fraction of the molecules react with water) to producee \(H^+\) and the corresponding anion. Exercise \(\PageIndex{1}\): Acid Strength, The Arrhenius Definition of Acids and Bases, The BrnstedLowry Definition of Acids and Bases, Definition of Strong/Weak Acids & Bases, YouTube (opens in new window), status page at https://status.libretexts.org. If the product had been cesium iodide, what would have been the acid and the base? NaOH is a corrosive white crystalline solid that readily absorbs moisture from the air. The BrnstedLowry definition of an acid is essentially the same as the Arrhenius definition, except that it is not restricted to aqueous solutions. 15 Facts on HI + NaOH: What, How To Balance & FAQs. Acid Base Neutralization Reaction Example Hydrogen bromide donates its proton to potassium hydroxide. Definition of pH. Following are some of the examples which will help you to understand the process and reaction taking place between acid and base which will give the end product as a salt. Because of the limitations of the Arrhenius definition, a more general definition of acids and bases was needed. Because HCl is a strong acid and CO32 is a weak base, the reaction will go to completion. A base that dissociates essentially completely in water) to give \(OH^-\) and the corresponding cation), An acid in which only a fraction of the molecules react with water) to producee, (A base in which only a fraction of the molecules react with water to produce. An antacid tablet reacts with 0.1 M HCl (the approximate concentration found in the human stomach). Balanced chemical equation for hydrochloric acid and sodium hydroxide NaOH (aq) + HCl (aq) NaCl (aq) + H 2O (l) This is an acid-base reaction (neutralization): NaOH is a base, HCl is an acid. An acidic solution and a basic solution react together in a neutralization reaction that also forms a salt. The resulting \(H_3O^+\) ion, called the hydronium ionis a more accurate representation of \(H^+_{(aq)}\). In Equation 4.28, the products are NH 4+, an acid, and OH , a base. Examples include reactions in which an acid is added to ionic compounds that contain the HCO3, CN, or S2 anions, all of which are driven to completion (Figure \(\PageIndex{1}\) ): \[ HCO_3^- (aq) + H^+ (aq) \rightarrow H_2 CO_3 (aq) \], \[ H_2 CO_3 (aq) \rightarrow CO_2 (g) + H_2 O(l) \], \[ CN^- (aq) + H^+ (aq) \rightarrow HCN(g) \], \[ S ^{2-} (aq) + H^+ (aq) \rightarrow HS^- (aq) \], \[ HS^- (aq) + H^+ (aq) \rightarrow H_2 S(g) \]. Using mole ratios, calculate the number of moles of base required to neutralize the acid. What are examples of neutralization reactions - This chemistry video tutorial explains how to predict the products of acid base neutralization reactions. solid strontium hydroxide with hydrobromic acid, aqueous sulfuric acid with solid sodium hydroxide. )%2F04%253A_Reactions_in_Aqueous_Solution%2F4.03%253A_Acid-Base_Reactions, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), A substance with at least one hydrogen atom that can dissociate to form an anion and an, (a substance that produces one or more hydroxide ions (\(OH^-\) and a cation when dissolved in aqueous solution, thereby forming a basic solution), (a compound that is capable of donating one proton per molecule), A compound that can donate more than one proton per molecule is known as a, compound that can donate two protons per molecule in separate steps). Placing a drop of a solution on a strip of pH paper and comparing its color with standards give the solutions approximate pH. We will discuss these reactions in more detail in Chapter 16. The reaction is then said to be in equilibrium (the point at which the rates of the forward and reverse reactions become the same, so that the net composition of the system no longer changes with time). The aluminum metal ion has an unfilled valence shell, so it . Example: HCl (aq) + NaOH (aq) NaCl (aq) + H2O (l) NaCl is the salt is this reaction and you already know water. Ammonia, for example, reacts with a proton to form \(NH_4^+\), so in Equation \(\PageIndex{3}\), \(NH_3\) is a BrnstedLowry base and \(HCl\) is a BrnstedLowry acid. All other polyprotic acids, such as H3PO4, are weak acids. The other product is water. In chemistry, the word salt refers to more than just table salt. Monoprotic acids include HF, HCl, HBr, HI, HNO3, and HNO2. Similarly, strong bases dissociate essentially completely in water to give \(OH^\) and the corresponding cation. . A neutralization reaction (a chemical reaction in which an acid and a base react in stoichiometric amounts to produce water and a salt) is one in which an acid and a base react in stoichiometric amounts to produce water and a salt (the general term for any ionic substance that does not have OH as the anion or H+ as the cation), the general term for any ionic substance that does not have OH as the anion or H+ as the cation. The chemical equation for this reaction is: State whether each compound is an acid, a base, or a salt. acid + carbonate salt + water + carbon dioxide or acid +. One of the key factors affecting reactions that occur in dilute solutions of acids and bases is the concentration of H+ and OH ions. Typically less than 5% of a weak electrolyte dissociates into ions in solution, whereas more than 95% is present in undissociated form. Recall that all polyprotic acids except H2SO4 are weak acids. According to the Arrhenius definition, an acid is a substance like hydrochloric acid that dissolves in water to produce H+ ions (protons; Equation \(\ref{4.3.1}\)), and a base is a substance like sodium hydroxide that dissolves in water to produce hydroxide (OH) ions (Equation \(\ref{4.3.2}\)): \[ \underset{an\: Arrhenius\: acid}{HCl_{(g)}} \xrightarrow {H_2 O_{(l)}} H^+_{(aq)} + Cl^-_{(aq)} \label{4.3.1} \], \[ \underset{an\: Arrhenius\: base}{NaOH_{(s)}} \xrightarrow {H_2O_{(l)}} Na^+_{(aq)} + OH^-_{(aq)} \label{4.3.2} \]. There is no correlation between the solubility of a substance and whether it is a strong electrolyte, a weak electrolyte, or a nonelectrolyte. Most reactions of a weak acid with a weak base also go essentially to completion. When a strong acid and a strong base are mixed, they react according to the following net-ionic equation: HO (aq) + OH (aq) 2HO (l). Examples of the last two are as follows: \[ \underset{strong\: acid}{HCl(aq)} + \underset{weak\: base}{NH_3 (aq)} \rightarrow \underset{salt}{NH_4 Cl(aq)} \], \[ \underset{weak\: acid} {CH_3 CO _2 H(aq)} + \underset{strong\: base}{NaOH(aq)} \rightarrow \underset{salt}{CH _3 CO _2 Na(aq)} + H_2 O(l) \]. Second, and more important, the Arrhenius definition predicted that, none of these; formaldehyde is a neutral molecule. Remember that there is no correlation between solubility and whether a substance is a strong or a weak electrolyte! In fact, this is only one possible set of definitions. (the point at which the rates of the forward and reverse reactions become the same, so that the net composition of the system no longer changes with time). \( H^+ + I^- + Cs^+ + OH^- \rightarrow Cs^+ + I^- + H_2O \), Modified by Joshua Halpern (Howard University). Strong acids react completely with water to produce H3O+(aq) (the hydronium ion), whereas weak acids dissociate only partially in water. Why? Because we want to neutralize only 90% of the acid present, we multiply the number of moles of HCl by 0.90: \((0.015\: mol\: HCl)(0.90) = 0.014\: mol\: HCl\), We know from the stoichiometry of the reaction that each mole of CaCO3 reacts with 2 mol of HCl, so we need, \( moles\: CaCO_3 = 0 .014\: \cancel{mol\: HCl} \left( \dfrac{1\: mol\: CaCO_3}{2\: \cancel{mol\: HCl}} \right) = 0 .0070\: mol\: CaCO_3 \), \( \left( \dfrac{500\: \cancel{mg\: CaCO_3}} {1\: Tums\: tablet} \right) \left( \dfrac{1\: \cancel{g}} {1000\: \cancel{mg\: CaCO_3}} \right) \left( \dfrac{1\: mol\: CaCO_3} {100 .1\: \cancel{g}} \right) = 0 .00500\: mol\: CaCO_ 3 \). Acids differ in the number of protons they can donate. The pH of the perchloric acid solution is thus, \(pH = -log[H^+] = -log(2.1 \times 10^{-2}) = 1.68\). substance formed when a BrnstedLowry acid donates a proton. We are given the pH and asked to calculate the hydrogen ion concentration. How many milliliters of 0.223 M NaOH are needed to neutralize 25.00 mL of this final solution? A compound that can donate more than one proton per molecule is known as a polyprotic acid. Identify the acid and the base in this reaction. The acid-base reaction definition describes the chemical change that occurs in a reaction between acid and base. Thus we need \(\dfrac{0.0070\: \cancel{mol\: CaCO_3}}{0.00500\: \cancel{mol\: CaCO_3}}= 1.4\) Tums tablets. This chemistry video tutorial explains how to predict the products of acid base neutralization reactions. The salt that forms is . According to Brnsted and Lowry, an acid (A substance with at least one hydrogen atom that can dissociate to form an anion and an \(H^+\) ion (a proton) in aqueous solution, thereby forming an acidic solution) is any substance that can donate a proton, and a base (a substance that produces one or more hydroxide ions (\(OH^-\) and a cation when dissolved in aqueous solution, thereby forming a basic solution) is any substance that can accept a proton. Thus \([H^+] = 10^{-3.80} = 1.6 \times 10^{-4}\: M\). Derive an equation to relate the hydrogen ion concentration to the molarity of a solution of a strong monoprotic acid. One was proposed independently in 1923 by the Danish chemist J. N. Brnsted (18791947) and the British chemist T. M. Lowry (18741936), who defined acidbase reactions in terms of the transfer of a proton (H+ ion) from one substance to another. Mathematical equations are a way of representing mathematical relationships between variables. B Next we need to determine the number of moles of HCl present: \( 75\: \cancel{mL} \left( \dfrac{1\: \cancel{L}} {1000\: \cancel{mL}} \right) \left( \dfrac{0 .20\: mol\: HCl} {\cancel{L}} \right) = 0. Pure liquid water contains extremely low but measurable concentrations of H3O+(aq) and OH(aq) ions produced via an autoionization reaction, in which water acts simultaneously as an acid and as a base: \[H_2O(l) + H_2O(l) \rightleftharpoons H_3O^+(aq) + OH^-(aq)\tag{8.7.22}\). Mathematics is a way of dealing with tasks that involves numbers and equations. A Determine whether the compound is organic or inorganic. Acids other than the six common strong acids are almost invariably weak acids. What is the pH of a solution prepared by diluting 25.00 mL of 0.879 M HCl to a volume of 555 mL? acid-base reaction, a type of chemical process typified by the exchange of one or more hydrogen ions, H +, between species that may be neutral ( molecules, such as water, H 2 O; or acetic acid, CH 3 CO 2 H) or electrically charged (ions, such as ammonium, NH 4+; hydroxide, OH ; or carbonate, CO 32 ). It is a pungent-smelling, colorless gas, highly soluble in water and denser than air. The molecular equation reveals the least about the species in solution and is actually somewhat misleading because it shows all the reactants and products as if they were intact undissociated compounds.. General acid-base reactions, also called neutralization reactions can be summarized with the following reaction equation: ACID (aq) + BASE (aq) H 2 O (l) + SALT (aq) or (s) The DRIVING FORCE for a general acid-base reaction is the formation of water. According to the Arrhenius definition, an acid is a substance like hydrochloric acid that dissolves in water to produce H+ ions (protons; Equation \(\PageIndex{1}\) ), and a base is a substance like sodium hydroxide that dissolves in water to produce hydroxide (OH) ions (Equation \(\PageIndex{2}\) ): \[ \underset{an\: Arrhenius\: acid}{HCl_{(g)}} \xrightarrow {H_2 O_{(l)}} H^+_{(aq)} + Cl^-_{(aq)} \], \[ \underset{an\: Arrhenius\: base}{NaOH_{(s)}} \xrightarrow {H_2O_{(l)}} Na^+_{(aq)} + OH^-_{(aq)} \]. A more accurate tool, the pH meter, uses a glass electrode, a device whose voltage depends on the H+ ion concentration. substances can behave as both an acid and a base. The reaction is then said to be in equilibrium (the point at which the rates of the forward and reverse reactions become the same, so that the net composition of the system no longer changes with time). . The BrnstedLowry definition of a base, however, is far more general because the hydroxide ion is just one of many substances that can accept a proton. Using the balanced chemical equation for the acid dissociation reaction and Equation \(\PageIndex{24}\) or \(\PageIndex{25}\), determine [H+] and convert it to pH or vice versa. One example of an acid-base reaction that occurs in everyday life is the reaction between vinegar (acetic acid) and baking soda (sodium bicarbonate). Instead, the solution contains significant amounts of both reactants and products. Acid Base Reaction Example Hydrochloric acid and Sodium hydroxide Hydrochloric acid is a strong acid. When these two substances are mixed, they react to form carbon dioxide gas, water, and sodium acetate. What are examples of neutralization reactions - When a strong acid reacts with a strong base the resultant salt is neither acidic nor basic in nature i.e. Adding an acid to pure water increases the hydrogen ion concentration and decreases the hydroxide ion concentration because a neutralization reaction occurs, such as that shown in Equation 8.7.15. In ancient times, an acid was any substance that had a sour taste (e.g., vinegar or lemon juice), caused consistent color changes in dyes derived from plants (e.g., turning blue litmus paper red), reacted with certain metals to produce hydrogen gas and a solution of a salt containing a metal cation, and dissolved carbonate salts such as limestone (CaCO3) with the evolution of carbon dioxide. If we look at the net ionic equation for this reaction it shows that the driving force for the reaction is the production of water: H+(aq) + OH-(aq) H2O (l) When you react the acid and base, this process is called neutralization. C Calculate the number of moles of base contained in one tablet by dividing the mass of base by the corresponding molar mass. A neutralization reaction is when an acid and a base react to form water and a salt and involves the combination of H+ ions and OH . Occasionally, the same substance performs both roles, as you will see later. acid and a base that differ by only one hydrogen ion. Acid-base definitions. Because of its more general nature, the BrnstedLowry definition is used throughout this text unless otherwise specified. How many Rolaids tablets must be consumed to neutralize 95% of the acid, if each tablet contains 400 mg of NaAl(OH)2CO3? HCl(aq) + KOH(aq . The concentration of hydrogen ions in pure water is only 1.0 107 M at 25C. The most common weak base is ammonia, which reacts with water to form small amounts of hydroxide ion: \[ NH_3 (g) + H_2 O(l) \rightleftharpoons NH_4^+ (aq) + OH^- (aq) \]. If the base is a metal hydroxide, then the general formula for the reaction of an acid with a base is described as follows: Acid plus base yields water plus salt. In general: acid + metal salt + hydrogen The metal needs to be more reactive than hydrogen in the reactivity series for it to. can donate more than one proton per molecule. none of these; formaldehyde is a neutral molecule. The products of an acidbase reaction are also an acid and a base. Before we discuss the characteristics of such reactions, lets first describe some of the properties of acids and bases. The pH scaleA logarithmic scale used to express the hydrogen ion (H+) concentration of a solution, making it possible to describe acidity or basicity quantitatively. If either the acid or the base is in excess, the pH of the resulting solution can be determined from the concentration of excess reactant. We're here for you 24/7. Monoprotic acids include HF, HCl, HBr, HI, HNO3, and HNO2. One was proposed independently in 1923 by the Danish chemist J. N. Brnsted (18791947) and the British chemist T. M. Lowry (18741936), who defined acidbase reactions in terms of the transfer of a proton (H+ ion) from one substance to another. . Acid base reaction products calculator - We'll provide some tips to help you select the best Acid base reaction products calculator for your needs. For example, aspirin is an acid (acetylsalicylic acid), and antacids are bases. First, because acids and bases were defined in terms of ions obtained from water, the Arrhenius concept applied only to substances in aqueous solution. In this reaction, water acts as an acid by donating a proton to ammonia, and ammonia acts as a base by accepting a proton from water. 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\newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), A substance with at least one hydrogen atom that can dissociate to form an anion and an, (a substance that produces one or more hydroxide ions (\(OH^-\) and a cation when dissolved in aqueous solution, thereby forming a basic solution), (a compound that is capable of donating one proton per molecule).