acid base reaction equations examples acid base reaction equations examples

(Assume all the acidity is due to the presence of HCl.) The chemical equation for this reaction is: )%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). The reaction of a strong acid with a strong base is a neutralization reaction, which produces water plus a salt. The aluminum metal ion has an unfilled valence shell, so it . The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. (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). Ammonium nitrate is famous in the manufacture of explosives. There is no correlation between the solubility of a substance and whether it is a strong electrolyte, a weak electrolyte, or a nonelectrolyte. What is the pH of a solution prepared by diluting 25.00 mL of 0.879 M HCl to a volume of 555 mL? As you will learn in a more advanced course, the activity of a substance in solution is related to its concentration. 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. 4.3: Acid-Base Reactions is shared under a CC BY-NC-SA 3.0 license and was authored, remixed, and/or curated by LibreTexts. If 20.0 mL of 0.10 M NaOH are needed to neutralize 15.0 mL of gastric fluid, what is the molarity of HCl in the fluid? Similarly, strong bases dissociate essentially completely in water to give \(OH^\) and the corresponding cation. Acid + Base Water + Salt. Second, and more important, the Arrhenius definition predicted that. 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). substance formed when a BrnstedLowry base accepts a proton. Although these definitions were useful, they were entirely descriptive. Over time, the reaction reaches a state in which the concentration of each species in solution remains constant. Acid-base reactions are essential in both biochemistry and industrial chemistry. 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. What is its hydrogen ion concentration? Neutralization Reaction Definition ,Equation ,Examples Neutralization Reaction Equation: Acid + Base - Salt + Water Examples of Neutralization Reaction: HCl + NaOH - NaCl + H2O How do you balance neutralization Please be sure you are familiar with the topics discussed in Essential Skills 3 (section 4.11")before proceeding to the Numerical Problems. Strong acids and strong bases are both strong electrolytes. When [HA] = [A], the solution pH is equal to the pK of the acid . 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}\). A compound that can donate more than one proton per molecule. By solving an equation, we can find the value of . Conversely, bases that do not contain the hydroxide ion accept a proton from water, so small amounts of OH are produced, as in the following: \( \underset{base}{NH_3 (g)} + \underset{acid}{H_2 O(l)} \rightleftharpoons \underset{acid}{NH_4^+ (aq)} + \underset{base}{OH^- (aq)} \). Before we discuss the characteristics of such reactions, lets first describe some of the properties of acids and bases. Explain your answer. There is no correlation between the solubility of a substance and whether it is a strong electrolyte, a weak electrolyte, or a nonelectrolyte. In Chapter 4.6, we defined acids as substances that dissolve in water to produce H+ ions, whereas bases were defined as substances that dissolve in water to produce OH ions. Multiply the number of moles by the percentage to obtain the quantity of acid that must be neutralized. In Equation \(\PageIndex{12}\), the products are NH4+, an acid, and OH, a base. acids and bases. 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. \(2CH_3CO_2Na(s) + H_2SO_4(aq) \rightarrow Na_2SO_4(aq) + 2CH_3CO_2H(aq)\). Examples of the last two are as follows: \[ \underset{strong\: acid}{HCl(aq)} + \underset{weak\: base}{NH_3 (aq)} \rightarrow \underset{salt}{NH_4 Cl(aq)} \], \[ \underset{weak\: acid} {CH_3 CO _2 H(aq)} + \underset{strong\: base}{NaOH(aq)} \rightarrow \underset{salt}{CH _3 CO _2 Na(aq)} + H_2 O(l) \]. Figure 8.7.2 A Plot of pH versus [H+] for Some Common Aqueous Solutions. State whether each compound is an acid, a base, or a salt. Each of these half-reactions is balanced separately and then combined to give the balanced redox equation. For example, in pure water [H 3 O +] = 1 10 7, with the result that the pH = 7.0. provides a convenient way of expressing the hydrogen ion (H+) concentration of a solution and enables us to describe acidity or basicity in quantitative terms. Example: HCl (aq) + NaOH (aq) NaCl (aq) + H2O (l) NaCl is the salt is this reaction and you already know water. Weak acid vs strong base. 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. Sulfuric acid is unusual in that it is a strong acid when it donates its first proton (Equation \(\PageIndex{8}\) ) but a weak acid when it donates its second proton (Equation 8.7.9) as indicated by the single and double arrows, respectively: \[ \underset{strong\: acid}{H_2 SO_4 (l)} \xrightarrow {H_2 O(l)} H ^+ (aq) + HSO_4 ^- (aq) \], \[ \underset{weak\: acid}{HSO_4^- (aq)} \rightleftharpoons H^+ (aq) + SO_4^{2-} (aq) \]. The only common strong bases are the hydroxides of the alkali metals and the heavier alkaline earths (Ca, Sr, and Ba); any other bases you encounter are most likely weak. HI and NaOH are both strong acid and base respectively. react essentially completely with water to give \(H^+\) and the corresponding anion. For example, aspirin is an acid (acetylsalicylic acid), and antacids are bases. Weak acid equilibrium. B If inorganic, determine whether the compound is acidic or basic by the presence of dissociable H+ or OH ions, respectively. Acid-base reactions are essential in both biochemistry and industrial chemistry. The resulting \(H_3O^+\) ion, called the hydronium ionis a more accurate representation of \(H^+_{(aq)}\). Classify each compound as a strong acid, a weak acid, a strong base, or a weak base in aqueous solution. Moreover, many of the substances we encounter in our homes, the supermarket, and the pharmacy are acids or bases. In chemical equations such as these, a double arrow is used to indicate that both the forward and reverse reactions occur simultaneously, so the forward reaction does not go to completion. Map: Chemistry - The Central Science (Brown et al. How many Rolaids tablets must be consumed to neutralize 95% of the acid, if each tablet contains 400 mg of NaAl(OH)2CO3? Because of the limitations of the Arrhenius definition, a more general definition of acids and bases was needed. Assume that the stomach of someone suffering from acid indigestion contains 75 mL of 0.20 M HCl. In fact, this is only one possible set of definitions. Acid Base Neutralization Reaction Example Hydrogen bromide donates its proton to potassium hydroxide. What are examples of neutralization reactions - This chemistry video tutorial explains how to predict the products of acid base neutralization reactions. H + ( aq) + OH - ( aq ) H 2 O ( l) Acid and bases that ionize completely giving larger hydrogen or hydroxide ions in solutions are called strong acids and bases. A 25.00 mL sample of a 0.9005 M solution of HCl is diluted to 500.0 mL. 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, \( moles\: CaCO_3 = 0 .014\: \cancel{mol\: HCl} \left( \dfrac{1\: mol\: CaCO_3}{2\: \cancel{mol\: HCl}} \right) = 0 .0070\: mol\: CaCO_3 \), \( \left( \dfrac{500\: \cancel{mg\: CaCO_3}} {1\: Tums\: tablet} \right) \left( \dfrac{1\: \cancel{g}} {1000\: \cancel{mg\: CaCO_3}} \right) \left( \dfrac{1\: mol\: CaCO_3} {100 .1\: \cancel{g}} \right) = 0 .00500\: mol\: CaCO_ 3 \). What is the second product? 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. Instead, the solution contains significant amounts of both reactants and products. Weak Acid-Base Calculations Weak acids and bases do not dissociate completely, so while the approach to solving the equations is similar to strong-acid systems, the complication of the Ka is added. In a balanced neutralization equation, the moles of H+ ions supplied by the acid will be equal to the moles of OH- ions supplied by the base. Qualitatively, however, we can state that strong acids (An acid that reacts essentially completely with water) to give \(H^+\) and the corresponding anion. 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. 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. Thus all acidbase reactions actually involve two conjugate acidbase pairsAn acid and a base that differ by only one hydrogen ion. Acids differ in the number of protons they can donate. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. These reactions are exothermic. Moreover, many of the substances we encounter in our homes, the supermarket, and the pharmacy are acids or bases. Strong base 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. B If inorganic, determine whether the compound is acidic or basic by the presence of dissociable H+ or OH ions, respectively. Strong acids and strong bases are both strong electrolytes. Because the negative exponent of [H+] becomes smaller as [H+] increases, the pH decreases with increasing [H+]. with your math homework, our Math Homework Helper is here to help. The equation for the dissociation of acetic acid, for example, is CH3CO2H + H2O CH3CO2 + H3O+. Is the hydronium ion a strong acid or a weak acid? For example, the balanced chemical equation for the reaction between HCl(aq) and KOH(aq) is. What is the complete ionic equation for each reaction? Sulfuric acid is unusual in that it is a strong acid when it donates its first proton (Equation \(\ref{4.3.8}\)) but a weak acid when it donates its second proton (Equation \(\ref{4.3.9}\)) as indicated by the single and double arrows, respectively: \[ \underset{strong\: acid}{H_2 SO_4 (l)} \xrightarrow {H_2 O(l)} H ^+ (aq) + HSO_4 ^- (aq) \label{4.3.8} \], \[ \underset{weak\: acid}{HSO_4^- (aq)} \rightleftharpoons H^+ (aq) + SO_4^{2-} (aq) \label{4.3.9} \]. Substances that can behave as both an acid and a base are said to be amphotericWhen substances can behave as both an acid and a base.. Propose a method for preparing the solution. Strong acid vs weak base. Ammonia reacts with nitric acid (HNO3) which is a strong acid to yield to slightly acidic salt named ammonium nitrate. All carboxylic acids that contain a single CO2H group, such as acetic acid (CH3CO2H), are monoprotic acids, dissociating to form RCO2 and H+. Why was it necessary to expand on the Arrhenius definition of an acid and a base? In BrnstedLowry terms, an acid is a substance that can donate a proton (H+), and a base is a substance that can accept a proton. Because of its more general nature, the BrnstedLowry definition is used throughout this text unless otherwise specified. 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). Even a strongly basic solution contains a detectable amount of H+ ions. Compounds that are capable of donating more than one proton are generally called polyprotic acids. Except for the reaction of a weak acid or a weak base with water, acidbase reactions essentially go to completion. An acid-base reaction is a chemical reaction that occurs between an acid and a base.It can be used to determine pH.Several theoretical frameworks provide alternative conceptions of the reaction mechanisms and their application in solving related problems; these are called the acid-base theories, for example, Brnsted-Lowry acid-base theory. The Arrhenius Definition of Acids and Bases, The BrnstedLowry Definition of Acids and Bases, status page at https://status.libretexts.org, To know the characteristic properties of acids and bases. 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. Autoionization of water. The proton (H +) from the acid combines with the hydroxide (OH -) from the base to make water (H 2 O). For example, H2SO4 can donate two H+ ions in separate steps, so it is a diprotic acid (a compound that can donate two protons per molecule in separate steps) and H3PO4, which is capable of donating three protons in successive steps, is a triprotic acid (a compound that can donate three protons per molecule in separate steps), (Equation \(\ref{4.3.4}\), Equation \(\ref{4.3.5}\), and Equation \(\ref{4.3.6}\)): \[ H_3 PO_4 (l) \overset{H_2 O(l)}{\rightleftharpoons} H ^+ ( a q ) + H_2 PO_4 ^- (aq) \label{4.3.4} \], \[ H_2 PO_4 ^- (aq) \rightleftharpoons H ^+ (aq) + HPO_4^{2-} (aq) \label{4.3.5} \], \[ HPO_4^{2-} (aq) \rightleftharpoons H^+ (aq) + PO_4^{3-} (aq) \label{4.3.6} \]. A more accurate tool, the pH meter, uses a glass electrode, a device whose voltage depends on the H+ ion concentration. While Brnsted theory cannot explain the formation of complex ions with a central metal ion, Lewis acid-base theory sees the metal as the Lewis Acid and the ligand of the coordination compound as a Lewis Base. 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. . A salt and hydrogen are produced when acids react with metals. An acid base neutralization reaction is when an acid reacts with a base to create water and a salt. ), Given: volume and molarity of acid and mass of base in an antacid tablet, Asked for: number of tablets required for 90% neutralization. If we are dealing with a weak acid (or base) then the Ka (or pKa) of the acid must be known. 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. Remember that there is no correlation between solubility and whether a substance is a strong or a weak electrolyte! pH = - log 0.5 = 0.3. H2SO4 + NH3 NH4+ + SO42-. The BrnstedLowry definition of an acid is essentially the same as the Arrhenius definition, except that it is not restricted to aqueous solutions. ; in Equation \(\PageIndex{12}\), they are NH4+/NH3 and H2O/OH. Common weak acids include HCN, H2S, HF, oxoacids such as HNO2 and HClO, and carboxylic acids such as acetic acid. . none of these; formaldehyde is a neutral molecule. substances can behave as both an acid and a base. 15 Facts on HI + NaOH: What, How To Balance & FAQs. All acidbase reactions involve two conjugate acidbase pairs, the BrnstedLowry acid and the base it forms after donating its proton, and the BrnstedLowry base and the acid it forms after accepting a proton. A chemist needed a solution that was approximately 0.5 M in HCl but could measure only 10.00 mL samples into a 50.00 mL volumetric flask. Acidbase reactions are essential in both biochemistry and industrial chemistry. Classify each compound as a strong acid, a weak acid, a strong base, a weak base, or none of these. Calculate the number of tablets required by dividing the moles of base by the moles contained in one tablet. When acid reacts with base, it forms salt and water and the reaction is called as neutralization. Most reactions of a weak acid with a weak base also go essentially to completion. Legal. (a compound that can donate three protons per molecule in separate steps). AboutTranscript. Each carbonate ion can react with 2 mol of H+ to produce H2CO3, which rapidly decomposes to H2O and CO2. Malonic acid is a dicarboxylic acid; propose a structure for malonic acid. An example, using ammonia as the base, is H2O + NH3 OH + NH4+. can donate more than one proton per molecule. First, because acids and bases were defined in terms of ions obtained from water, the Arrhenius concept applied only to substances in aqueous solution. Thus water can act as either an acid or a base by donating a proton to a base or by accepting a proton from an acid. Acid-Base Reactions: Definition, Examples & Equation Chemistry Chemical Reactions Acid-Base Reactions Acid-Base Reactions Acid-Base Reactions Chemical Analysis Formulations Instrumental Analysis Pure Substances Sodium Hydroxide Test Test for Anions Test for Metal Ions Testing for Gases Testing for Ions Chemical Reactions Acid-Base Reactions 015\: mol\: HCl \). Mathematical equations are a way of representing mathematical relationships between variables. acid and a base that differ by only one hydrogen ion. We will discuss these reactions in more detail in Chapter 16. The reactions in Equation \(\PageIndex{21}\) are responsible for the rotten egg smell that is produced when metal sulfides come in contact with acids. If the acid and base are equimolar, the . For dilute solutions such as those we are discussing, the activity and the concentration are approximately the same. (Assume the density of the solution is 1.00 g/mL.). With clear, concise explanations and step-by-step examples, we'll help you master even the toughest math concepts. 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. Under what circumstances is one of the products a gas? Because HCl is a strong acid and CO32 is a weak base, the reaction will go to completion. The same term can be applied to alkaline solutions; thus, in 0.1 molar sodium hydroxide [OH ] = 0.1, [H 3 O +] = Kw / [OH ] = 1 10 14 /0.1 = 10 13, and pH = 13.0. 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.. Most of the ammonia (>99%) is present in the form of NH3(g). 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. In chemistry, the word salt refers to more than just table salt. Examples: Strong acid vs strong base. All acidbase reactions contain two acidbase pairs: the reactants and the products. A Determine whether the compound is organic or inorganic. Acids other than the six common strong acids are almost invariably weak acids. When these two substances are mixed, they react to form carbon dioxide gas, water, and sodium acetate. In contrast, only a fraction of the molecules of weak acids and weak bases react with water to produce ions, so weak acids and weak bases are also weak electrolytes. 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. 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 . The pH of the perchloric acid solution is thus, \(pH = -log[H^+] = -log(2.1 \times 10^{-2}) = 1.68\). 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. The products of an acid-base reaction are also an acid and a base. Although acetic acid is very soluble in water, almost all of the acetic acid in solution exists in the form of neutral molecules (less than 1% dissociates). To relate KOH to NaH2PO4 a balanced equation must be used. Identify the acid and the base in this reaction. 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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).