The curve around the equivalence point will be relatively steep and smooth when working with a strong acid and a strong base. The equilibrium will therefore lie to the right, favoring the formation of the weaker acidbase pair: \[ \underset{\text{stronger acid}}{NH^+_{4(aq)}} + \underset{\text{stronger base}}{PO^{3-}_{4(aq)}} \ce{<=>>} \underset{\text{weaker base}}{NH_{3(aq)}} +\underset{\text{weaker acid}} {HPO^{2-}_{4(aq)}} \nonumber \]. Consider, for example, the ionization of hydrocyanic acid (\(HCN\)) in water to produce an acidic solution, and the reaction of \(CN^\) with water to produce a basic solution: \[HCN_{(aq)} \rightleftharpoons H^+_{(aq)}+CN^_{(aq)} \label{16.5.6} \], \[CN^_{(aq)}+H_2O_{(l)} \rightleftharpoons OH^_{(aq)}+HCN_{(aq)} \label{16.5.7} \]. The curve around the equivalence point will be relatively steep and smooth when working with a strong acid and a strong . Because \(pK_a\) = log \(K_a\), we have \(pK_a = \log(1.9 \times 10^{11}) = 10.72\). Click here for more Density-Concentration Calculators. According to Table \(\PageIndex{1}\), HCN is a weak acid (pKa = 9.21) and \(CN^\) is a moderately weak base (pKb = 4.79). An important note is in order. The fully protonated species is always the strongest acid because it is easier to remove a proton from a neutral molecule than from a negatively charged ion. Calculate the ionization constant for each of the following acids or bases from the ionization constant of its conjugate base or conjugate acid: F . This tells us that there is a nitric acid solution of 65% w/v. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. 32 ounces = 1 quart, 128 ounces = 1 gallon, 3.785 liters = 1 gallon, 2.2046 pounds = 1 kilogram. The odd H3PO3 When different volumes of an identical solution are added together, the final volume will always be exactly the sum of the individual portions added. The endpoint can be determined potentiometrically or by using a pH indicator. Nitric acid is HNO3, and nitric acid reacts with water to form hydronium, H3O plus, and nitrate, NO3 minus, which is the conjugate base 2HNO3. Partial List of Strong Acids: Hydrochlroic acid (HCl), Nitric Acid (HNO3), Perchloric Acid (HClO4), Sulfuric Acid (H2SO4), Partial List of Strong Bases: Sodium Hydroxide (NaOH), Barium Hydroxide (Ba(OH)2), Calcium Hydroxide (Ca(OH)2), Lithium Hydroxide (LiOH) (Hydroxides of Group I and II elements are generally strong bases), Partial List of Weak Acids: Acetic Acid (CH3COOH), Carbonic Acid (H2CO3), Phosphoric Acid (H3PO4), Partial List of Weak Bases: Ammonia (NH3), Calcium Carbonate (CaCO3), Sodium Acetate (NaCH3COO). Identify the conjugate acidbase pairs in each reaction. The hydrogen ion concentration decreases by a factor of 10, so the pH increases by 1 . Workers may be harmed from exposure to nitric acid. Volume Before Dilution (V1) Concentration After Dilution (C2) %. HCL, 37% - 12.2 Molar Strength = 36.5-38%, Density = 1.185, Molecular Weight = 36.5 . Acid-base titration calculations help you identify a solution's properties (such as pH) during an experiment or what an unknown solution is when doing fieldwork. are hidden by default. This test method is suitable for concentrations between approximately 50 and 70 %, calculated as nitric acid. HSO 4-Hydrogen sulfate ion. [3] White fuming nitric acid, also called 100% nitric acid or WFNA, is very close to anhydrous nitric acid. It is both extremely corrosive and toxic. The main industrial use of nitric acid is for the production of fertilizers. Similarly, Equation \(\ref{16.5.10}\), which expresses the relationship between \(K_a\) and \(K_b\), can be written in logarithmic form as follows: The values of \(pK_a\) and \(pK_b\) are given for several common acids and bases in Tables \(\PageIndex{1}\) and \(\PageIndex{2}\), respectively, and a more extensive set of data is provided in Tables E1 and E2. Make sure not to pour the solution above your head and to remove the funnel after you have finished pouring. If the acid or base conducts electricity weakly, it is a weak acid or base. HClO 4. Weak acids do not readily break apart as ions but remain bonded together as molecules. pH Calculator. The conjugate base of a strong acid is a weak base and vice versa. One specication for white fuming nitric acid is that it has a maximum of 2% . The bond strengths of acids and bases are implied by the relative amounts of molecules and ions present in solution. 1.2 The values stated in SI units are to be regarded as standard. So, in 20 ml of acidic solution 1.80 x 10-3 equivalent of acids. Total volume of solution including acid/base (liters): Calculate . Nitric acid is the inorganic compound with the formula H N O 3. Calculated pH values of common acids and bases for 1, 10, and 100 mmol/L (valid for standard conditions at 25, 1 atm; acidity constants are taken from here ): other reactions: Free software ( Example) Demo: Online pH-Calculator. Nitric Acid is a strong acid in terms of chemical ionization and solutions of it can be assayed using a strong base, such as Sodium Hydroxide. By adding either an acid or a base with a known molarity (the titrant) and measuring how much is needed to cause this change, we can work out the molarity of the unknown using the equation below: Here is the method for an acid-base titration: Fill a burette with the solution of the titrant. The values of \(K_a\) for a number of common acids are given in Table \(\PageIndex{1}\). Calculate the pH in the titration after the addition of 60.0 mL of 0.200 MHNO3. 1. Usually, we are ultimately interested in the number of moles of acid used. Solution Dilution Calculator. Table of Acid and Base Strength . There are two different nitric acid production methods: weak nitric acid and high-strength nitric acid. The values of \(K_b\) for a number of common weak bases are given in Table \(\PageIndex{2}\). It was not until Mohr developed the modern burette in 1855 that the technique would become recognizable to us today and has since become a popular method of performing analytical chemistry. home; aqion; about; Add 1, 2 or 3 reactants to water: . Conversely, smaller values of \(pK_b\) correspond to larger base ionization constants and hence stronger bases. An acid is a solution that has an excess of hydrogen (H+) ions. The magnitude of the equilibrium constant for an ionization reaction can be used to determine the relative strengths of acids and bases. When placed in water, virtually every HCl molecule splits into a H + ion and a Cl - ion in the reaction. It is actually closer to 96 mL. Once the color change is permanent, stop adding the solution. You may notice on the titration curve that the pH will rise sharply around the equivalence point. National Institutes of Health. Note the endpoint on the burette. pH is calculated by taking the negative logarithm of the concentration of hydronium ions. The most accurate way to determine pH is through use of a calibrated pH meter and electrode. HO 2 C . You should multiply your titre by 0.65. Your Safer Source for Science. Hydrofluoric acid is particularly dangerous because it is capable of eating through glass, as seen in the video in the links sectionV1. Weak acids and bases are molecules that do not fully dissociate when in solution; that is, they are not salts. for suppose, 100ml of 0.5% Nitric acid need to be prepared, and 'q' is the quantity (in ml) of 69% Nitric acid required, we calculate the 'q' from above equation. An older density scale is occasionally seen, with concentrated nitric acid specied as 42 Baum. The blue line is the curve, while the red line is its derivative. Introduction Again. For example, commercially available concentrated hydrochloric acid (HCl) is 37% by weight (w/w %). Keep in mind, though, that free \(H^+\) does not exist in aqueous solutions and that a proton is transferred to \(H_2O\) in all acid ionization reactions to form hydronium ions, \(H_3O^+\). The thermochemical equation for the reaction between nitric acid and sodium hydroxide solution is as shown below. Oxtboy, Gillis, Campion, David W., H.P., Alan. The best way is to titrate the acid with a base that you know the concentration of. The Brnsted-Lowry theory describes acid-base interactions in terms of proton transfer between chemical species. Check out 19 similar mixtures and solutions calculators , Table of common acids and bases and their strengths. Lactic acid (\(CH_3CH(OH)CO_2H\)) is responsible for the pungent taste and smell of sour milk; it is also thought to produce soreness in fatigued muscles. Substituting the \(pK_a\) and solving for the \(pK_b\). 5.4 * 10-2. 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. Hydrochloric acid. The stronger an acid is, the lower the pH it will produce in solution. Here's the titration curve of NaOH\small\text{NaOH}NaOH neutralising HCl\small\text{HCl}HCl. M. 03. The Complete Aqueous Hydrochloric Acid Solutions Density-Concentration Calculator. result calculation. Then it remains 5.00 10-3 - (4.90 10-3) = 1.0 10-4 moles H+. The strength of an oxyacid is defined by the extent to which it dissociates in water (i.e . A standard acid-base titration uses a titrant of known concentration to titrate a tank of unknown concentration. When placed in water, virtually every HCl molecule splits into a H+ ion and a Cl- ion in the reaction.1, \[\ce{HCl(aq) + H2O(l) <=> H3O^{+}(aq) + Cl^{-}(aq)} \nonumber\], For a strong acid like HCl, if you place 1 mole of HCl in a liter of water, you will get roughly 1 mole of H30+ ions and 1 mole of Cl- ions. Place on a white tile under the burette to better observe the color. The equivalence point will occur at a pH within the pH range of the stronger solution, i.e., for a strong acid and a weak base, the pH will be <7. Legal. Answer (1 of 3): If you have a solution of nitric acid of unknown concentration, there are a few ways to determine that. Cl-Chloride. This calculator calculates for concentration or density values that are between those given in the table below by a Input a temperature and density within the range of the table to calculate for concentration or input concentration to calculate for density. In presence of strong acids like sulfuric acid, HNO 3 acts as the base because it has to accept the proton from the stronger acid. So 1 US gallon = 3.78 litres, Then 130 x 3.78 = 491 litres of liquid volume. Acid and Base Strength is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. Name. This order corresponds to decreasing strength of the conjugate base or increasing values of \(pK_b\). A similar concept applies to bases, except the reaction is different. All the other mixtures show a weight loss not exceeding 2% even after 56 days immersion. It is a highly corrosive mineral acid. Nitric acid reacts with calcium compounds, forming calcium nitrate, which has a solubility of 56%. Therefore, when preparing volume/volume percent solutions, it is always better to dissolve the solute in solvent and then add additional solvent to bring the total. Initial Data. About Nitric acid. The number of moles of H+ ions from HCl is equal to: 50.00 10-3 L 0.100 M HCl = 5.00 10-3 moles. \(K_a = 1.4 \times 10^{4}\) for lactic acid; \(K_b = 7.2 \times 10^{11}\) for the lactate ion, \(NH^+_{4(aq)}+PO^{3}_{4(aq)} \rightleftharpoons NH_{3(aq)}+HPO^{2}_{4(aq)}\), \(CH_3CH_2CO_2H_{(aq)}+CN^_{(aq)} \rightleftharpoons CH_3CH_2CO^_{2(aq)}+HCN_{(aq)}\), \(H_2O_{(l)}+HS^_{(aq)} \rightleftharpoons OH^_{(aq)}+H_2S_{(aq)}\), \(HCO^_{2(aq)}+HSO^_{4(aq)} \rightleftharpoons HCO_2H_{(aq)}+SO^{2}_{4(aq)}\), Acid ionization constant: \[K_a=\dfrac{[H_3O^+][A^]}{[HA]} \nonumber \], Base ionization constant: \[K_b= \dfrac{[BH^+][OH^]}{[B]} \nonumber \], Relationship between \(K_a\) and \(K_b\) of a conjugate acidbase pair: \[K_aK_b = K_w \nonumber \], Definition of \(pK_a\): \[pKa = \log_{10}K_a \nonumber \] \[K_a=10^{pK_a} \nonumber \], Definition of \(pK_b\): \[pK_b = \log_{10}K_b \nonumber \] \[K_b=10^{pK_b} \nonumber \], Relationship between \(pK_a\) and \(pK_b\) of a conjugate acidbase pair: \[pK_a + pK_b = pK_w \nonumber \] \[pK_a + pK_b = 14.00 \; \text{at 25C} \nonumber \]. Each acid and each base has an associated ionization constant that corresponds to its acid or base strength. To solve this problem, you need to know the formula for sodium carbonate. Measure out an amount of the analyte (it should be less than the amount in your burette) and add it to an Erlenmeyer flask. concentration (% weight) of Nitric Acid (HNO3) solutions in water at different temperatures in degrees centigrade (C). Because \(pK_b = \log K_b\), \(K_b\) is \(10^{9.17} = 6.8 \times 10^{10}\). That means number of moles of sulfuric acid is half that of number of moles of sodium hydroxide used. The experiment has possibilities for use as an assessed practical. Although \(K_a\) for \(HI\) is about 108 greater than \(K_a\) for \(HNO_3\), the reaction of either \(HI\) or \(HNO_3\) with water gives an essentially stoichiometric solution of \(H_3O^+\) and I or \(NO_3^\). b) How many moles of sulfuric acid (H 2SO 4) are required to produce 2.0 moles of iodine (I 2) Conversion factor: Mole ratio between the unknown substance (sulfuric acid) and the known substance (iodine): 7 mol H 2SO 4 3 mol l 2 7 mol H 2SO 4 3 mol l 2 2.0 mol l 2 = 4.7 mol H 2SO 4 7 Mole - mass calculations A balanced chemical equation Formula. The conjugate base of HNO 3 is NO 3- and conjugate acid is NO 2+. For more tools about acids and bases, have a look at our neutralization calculator or learn how to calculate pH of buffer solution as well! Here, we have used, As noted above, weight refers to mass (i.e., measured on a balance). The \(HSO_4^\) ion is also a very weak base (\(pK_a\) of \(H_2SO_4\) = 2.0, \(pK_b\) of \(HSO_4^ = 14 (2.0) = 16\)), which is consistent with what we expect for the conjugate base of a strong acid. If waste vegetable oil is being used to produce biodiesel, it is necessary to neutralize the batch before processing it. Asked for: corresponding \(K_b\) and \(pK_b\), \(K_a\) and \(pK_a\). The volume of 100 grams of Nitric acid is 70.771 ml. Enter appropriate values in all cells except the one you wish to calculate. The first method utilizes oxidation, condensation, and absorption to produce nitric acid at concentrations between 30 and 70 percent nitric acid. The strength of an acid or base can be either strong or weak. Hydronium ion H3O+ H2O 1 0.0 The Ka value of ammonium (NH4+) is 5.6*10-10, the Kb value of ammonia (NH3) 1.8*10-5, is ammonium more strongly acidic than ammonia is basic? National Center for Biotechnology Information. Thus nitric acid should properly be written as \(HONO_2\). The constants \(K_a\) and \(K_b\) are related as shown in Equation \(\ref{16.5.10}\). Equivalence point means the point during titration at which the titrant added has completely neutralized the analyte solution. Step 1: Calculate the volume of 100 grams of Nitric acid. High-strength acid (90 percent or greater nitric acid) can be produced from dehydrating . Acid or base "strength" is a measure of how readily the molecule ionizes in water. Nitric Acid | HNO3 | CID 944 - structure, chemical names, physical and chemical properties, classification, patents, literature, biological activities, safety/hazards/toxicity information, supplier lists, and more. A titration curve is a plot of the concentration of the analyte at a given point in the experiment (usually pH in an acid-base titration) vs. the volume of the titrant added. Perchloric acid. From the volume of titrant used, the composition of the analyte can be calculated knowing the stoichiometry of the chemical reaction. Example: Sodium chloride (1 + 19) Dissolved in 19 weight of water with respect to 1 of NaCl. For example, hydrofluoric acid is a weak acid1, but it is extremely dangerous and should be handled with great care. Equivalent to 28.0% w/w NH 3 . Meant to be used in both the teaching and research laboratory, this calculator (see below) can be utilized to perform a number of different calculations for preparing. For an aqueous solution of a weak acid, the dissociation constant is called the acid ionization constant (\(K_a\)). Like any other conjugate acidbase pair, the strengths of the conjugate acids and bases are related by \(pK_a\) + \(pK_b\) = pKw. 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. 0.5 X 100 = 69 X q. q= 50/69 = 0.7246 ml. Similarly, the higher the Kb, the stronger the substance is as a base, and the more weakly acidic its conjugate acid is.1, For an acid that reacts with water in the reaction, \[HA_{(aq)} + H_2O_{(l)} \rightleftharpoons H_3O^+_{(aq)} + A^-_{(aq)}\]. Weak bases react with water to produce the hydroxide ion, as shown in the following general equation, where B is the parent base and BH+ is its conjugate acid: \[B_{(aq)}+H_2O_{(l)} \rightleftharpoons BH^+_{(aq)}+OH^_{(aq)} \label{16.5.4} \]. PH is based on the concentration of the hydronium ion (H3O+) which is a product of the reaction of acid and water. Just like water, HSO4 can therefore act as either an acid or a base, depending on whether the other reactant is a stronger acid or a stronger base. In fact, all six of the common strong acids that we first encountered in Chapter 4 have \(pK_a\) values less than zero, which means that they have a greater tendency to lose a proton than does the \(H_3O^+\) ion. Keep in mind, concentrated HCl is about 35%, while concentrated HNO 3 is about 65%, so the volume ratio is usually 4 parts concentrated hydrochloric acid to 1 part concentrated nitric acid. A higher Ka value means a higher ratio of reactants to products, and so the acid with the higher Ka value will be producing more hydronium, and therefore have a lower pH. Acid HA A-Ka pKa Acid Strength Conjugate Base Strength Hydroiodic HI I-Hydrobromic HBr Br-Perchloric HClO4 ClO4-Hydrochloric HCl Cl-Chloric HClO3 ClO3-Sulfuric (1) H2SO4 HSO4-Nitric HNO3 NO3-Strong acids completely dissociate in aq solution (Ka > 1, pKa < 1). In this experiment, students determine the copper content in brass (an alloy of copper and zinc) by dissolving brass turnings in nitric acid and comparing the colour of the solution with that of solutions of various concentrations of copper. For any conjugate acidbase pair, \(K_aK_b = K_w\). At pH 7, the concentration of H3O+\small\text{H}_3\text{O}^+H3O+ ions to OH\small\text{OH}^-OH ions is a ratio of 1:1\small1:11:1 (the equivalence point). Hydrochloric Acid. Other factors may also be important when deciding on the type of percent solution to prepare. The base ionization constant \(K_b\) of dimethylamine (\((CH_3)_2NH\)) is \(5.4 \times 10^{4}\) at 25C. A Video Calculating pH in Strong Acid or Strong Base Solutions: Calculating pH in Strong Acid or Strong Base Solutions [youtu.be]. Rationalize trends in acid-base strength in relation to molecular structure; . To see them, click the 'Advanced mode' button at the bottom of the calculator. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. A base is a solution that has an excess of hydroxide (OH-) ions. Scope 1.1 This test method covers determination of the assay of nitric acid by total acidity. Instead, a pH meter is often used. 2. C6H5COOH\text{C}_6\text{H}_5\text{COOH}C6H5COOH. The pH is, in fact, a way to calculate concentration: learn about it at our pH calculator. Most commercially available nitric acid has a concentration of 68% in water. You will notice in Table \(\PageIndex{1}\) that acids like \(H_2SO_4\) and \(HNO_3\) lie above the hydronium ion, meaning that they have \(pK_a\) values less than zero and are stronger acids than the \(H_3O^+\) ion. To work out an unknown concentration of 0.15 mL HCl: Use the 1:1 ratio formula because one mole of HCl reacts with one mole of NaOH HCl + NaOH NaCl + H2O. Use the relationships pK = log K and K = 10pK (Equations \(\ref{16.5.11}\) and \(\ref{16.5.13}\)) to convert between \(K_a\) and \(pK_a\) or \(K_b\) and \(pK_b\). Other examples that you may encounter are potassium hydride (\(KH\)) and organometallic compounds such as methyl lithium (\(CH_3Li\)). Butyric acid is responsible for the foul smell of rancid butter. By using a solution with a known molarity and a color indicator, we measure how much of the solution is required to neutralize the unknown solution, indicated by a change in the indicator, which we can use to work out information about the unknown solution. In aqueous solutions, \(H_3O^+\) is the strongest acid and \(OH^\) is the strongest base that can exist in equilibrium with \(H_2O\). All acids and bases do not ionize or dissociate to the same extent. Alcohols and Carboxylic Acids - Physical Data - Molweight, melting and boiling point, density, pKa-values, as well as number of carbon and hydrogen atoms in molecules are given for 150 different alcohols and . Propionic acid (\(CH_3CH_2CO_2H\)) is not listed in Table \(\PageIndex{1}\), however. Like all equilibrium constants, acid-base ionization constants are actually measured in terms of the activities of H + or OH , thus making them unitless. Multiply the molarity of the strong base NaOH by the volume of the NaOH (MB VB = 0.500 M 20.70 mL). Representative value, w/w %. For example, if the percent solution under consideration is to be used at widely different temperatures, then it is better to prepare the solution as a weight/weight % solution because its concentration would be independent of variations in ambient temperature. Nitric Acid (HNO 3) is a clear, colorless to slightly yellow inorganic acid. Principles of Modern Chemistry. No acid stronger than \(H_3O^+\) and no base stronger than \(OH^\) can exist in aqueous solution, leading to the phenomenon known as the leveling effect. University of Maiduguri. If the acid or base conducts electricity strongly, it is a strong acid or base. Input a temperature and density within the range of the table to calculate for concentration or input concentration . When doing a titration, we usually have a solution with a known volume but unknown molarity (the analyte), to which a color indicator (e.g., phenolphthalein) is added. w Phosphoric acid comes in many strengths, but 75% is most common. Belmont: Thomson Higher Education, 2008. From Table \(\PageIndex{1}\), we see that the \(pK_a\) of \(HSO_4^\) is 1.99. Acids and bases behave differently in solution based on their strength. Nitric acid is highly corrosive. The Ka value is a measure of the ratio between reactants and products at equilibrium. Nitric acid is colorless when pure but has a yellowish appearance when it is old due to the collection of nitrogen oxides. It is a strong acid, completely ionized into hydronium (H 3 O +) and nitrate (NO 3) ions in aqueous solution, and a powerful oxidizing agent (one that acts as electron acceptor in oxidation-reduction reactions ). One method is to use a solvent such as anhydrous acetic acid. The fertilizer industry uses weak nitric acid in the range of 50 to 65% strength and thus the high concentration (above 70% weight) nitric acid production process is not included. pH is 3.00. N o 3 point: let's do it 1.49 grams of h, n o 3. Just as with \(pH\), \(pOH\), and pKw, we can use negative logarithms to avoid exponential notation in writing acid and base ionization constants, by defining \(pK_a\) as follows: \[pK_b = \log_{10}K_b \label{16.5.13} \]. More Thus, solution mass is the combined mass of solute and solvent, and solution volume is the combined volume of solute . So, the number of base equivalents = 12 15 = 1.8 10-3 equivalent. For example, adding 50 mL of water to 50 mL of water will result in a total volume of 100 mL, and adding 75 mL of 100% ethanol to 75 mL of 100% ethanol will result in a total volume of 150 mL. Molarity Calculate the molality of nitric acid solution a) 29.0 b) 11.0 c) 43.2 d) 16.0 Question 8 (10 points) A concentrated aqueous solution of nitric acid (HNO3) has a density . The corresponding expression for the reaction of cyanide with water is as follows: \[K_b=\dfrac{[OH^][HCN]}{[CN^]} \label{16.5.9} \]. 491 x 30 g/l = 14730 g or 14.7 kg of dichromate. Factors Affecting Acid Strength. This curve tells us whether we are dealing with a weak or strong acid/base for an acid-base titration. The light bulb circuit is incomplete. Base. Conjugate bases of strong acids are ineffective bases. You can also calculate the mass of a substance needed to achieve a desired molarity. All acidbase equilibria favor the side with the weaker acid and base. Acidbase reactions always contain two conjugate acidbase pairs. Consequently, the proton-transfer equilibria for these strong acids lie far to the right, and adding any of the common strong acids to water results in an essentially stoichiometric reaction of the acid with water to form a solution of the \(H_3O^+\) ion and the conjugate base of the acid. + + Examples of strong acids are hydrochloric acid (), perchloric acid (), nitric acid and sulfuric acid ().. A weak acid is only partially dissociated, with . For example, hydrochloric acid (HCl) is a strong acid. "Acid-Base Equilibria." Salts such as \(K_2O\), \(NaOCH_3\) (sodium methoxide), and \(NaNH_2\) (sodamide, or sodium amide), whose anions are the conjugate bases of species that would lie below water in Table \(\PageIndex{2}\), are all strong bases that react essentially completely (and often violently) with water, accepting a proton to give a solution of \(OH^\) and the corresponding cation: \[K_2O_{(s)}+H_2O_{(l)} \rightarrow 2OH^_{(aq)}+2K^+_{(aq)} \label{16.5.18} \], \[NaOCH_{3(s)}+H_2O_{(l)} \rightarrow OH^_{(aq)}+Na^+_{(aq)}+CH_3OH_{(aq)} \label{16.5.19} \], \[NaNH_{2(s)}+H_2O_{(l)} \rightarrow OH^_{(aq)}+Na^+_{(aq)}+NH_{3(aq)} \label{16.5.20} \]. HNO 3, 70% - 15.8 Molar Strength = 69-70%, Density = 1.42, Molecular Weight = 63.01 1 liter = 1420 gm = 994 gm HNO 3 (@70%) = 15.8 moles = 15.8 Molar Measurements of the conductivity of 0.1 M solutions of both HI and \(HNO_3\) in acetic acid show that HI is completely dissociated, but \(HNO_3\) is only partially dissociated and behaves like a weak acid in this solvent. Hence the ionization equilibrium lies virtually all the way to the right, as represented by a single arrow: \[HCl_{(aq)} + H_2O_{(l)} \rightarrow H_3O^+_{(aq)}+Cl^_{(aq)} \label{16.5.17} \]. Secondly, you could measure the density of the acid either by using a hydrometer or weighi. If we add Equations \(\ref{16.5.6}\) and \(\ref{16.5.7}\), we obtain the following: In this case, the sum of the reactions described by \(K_a\) and \(K_b\) is the equation for the autoionization of water, and the product of the two equilibrium constants is \(K_w\): Thus if we know either \(K_a\) for an acid or \(K_b\) for its conjugate base, we can calculate the other equilibrium constant for any conjugate acidbase pair. Once you realize there are two sodium ions per carbonate ion, the problem is simple: N = 0.321 g Na 2 CO 3 x (1 mol/105.99 g) x (2 eq/1 mol) N = 0.1886 eq/0.2500 L. N = 0.0755 N. Nitric acid weighs 1.5129 gram per cubic centimeter or 1 512.9 kilogram per cubic meter, i.e. HNO 3. Thus the conjugate base of a strong acid is a very weak base, and the conjugate base of a very weak acid is a strong base. 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