Divide this answer (10.35 M mL) by the volume of the acid HCl (0.15 mL) MA = (MB VB)/VA = (0.500 M 20.70 mL)/0.15 mL = 0.690 M. The concentration is expressed as a number of moles per liter of solute. It is actually closer to 96 mL. Because of the use of negative logarithms, smaller values of \(pK_a\) correspond to larger acid ionization constants and hence stronger acids. 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. 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.This curve tells us whether we are dealing with a weak or strong acid/base for an acid-base titration. Nitric acid is the inorganic compound with the formula H N O 3. The same goes for strong bases, except the negative logarithm gives you the pOH as opposed to the pH. This works for a 10ml vat sample titrated with 1.0N sodium Hydroxide, and give you a result expressed as percent by volume of 70% (700g/l0 nitric acid. To prepare 2.5M or 2.5N, you just need to find the vol. The best way is to titrate the acid with a base that you know the concentration of. again. Measure out an amount of the analyte (it should be less than the amount in your burette) and add it to an Erlenmeyer flask. Thus, solution mass is the combined mass of solute and solvent, and solution volume is the combined volume of solute . 1-800-452-1261 . Each sensor, manufactured in Finland, is pressure and temperature tested as part of the production process to ensure they meet our highest standards. v 93% sulfuric acid is also known as 66 be' (Baume') acid. The percent dissociation of an acid or base is mathematically indicated by the acid ionization constant (Ka) or the base ionization constant (Kb)1. Hence the \(pK_b\) of \(SO_4^{2}\) is 14.00 1.99 = 12.01. At the bottom left of Figure \(\PageIndex{2}\) are the common strong acids; at the top right are the most common strong bases. Acid Strength Definition. Nitric acid weighs 1.5129 gram per cubic centimeter or 1 512.9 kilogram per cubic meter, i.e. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Once again, the activity of water has a value of 1, so water does not appear in the equilibrium constant expression. Calculate \(K_a\) and \(pK_a\) of the dimethylammonium ion (\((CH_3)_2NH_2^+\)). HNO 3 , (aq) + NaOH (aq) NaNO 3 (aq) + H 2 O (l) H = -57.3 kJ When 250 cm 3 of 1.0 mol dm -3 nitric acid is added to 200 cm 3 of 2.0 mol dm -3 sodium hydroxide solution, what is the change in temperature? At 25C, \(pK_a + pK_b = 14.00\). \[HA_{(aq)} \rightleftharpoons H^+_{(aq)}+A^_{(aq)} \label{16.5.3} \]. of the nitric acid of the given purity (65%) and add to distilled water in a standard flask (1L) up to mark . Find the pH of 0.5 grams of HCl disolved into 100 ml of water: 0.5 grams / (36.5 g/mole) = 0.014 moles HCl, HCl is a strong acid and completely dissociates in water, therefore the pH will be equal to the negative logarithm of the concentration of HCl. One method is to use a solvent such as anhydrous acetic acid. This molarity calculator is a tool for converting the mass concentration of any solution to molar concentration (or recalculating grams per ml to moles). If the bond is highly polar, the proton tends to leave the molecule more easily, making it a strong acid. Butyric acid is responsible for the foul smell of rancid butter. The volume of 100 grams of Nitric acid is 70.771 ml. The density of concentrated nitric acid is 1.42 g/mL. The values of \(K_a\) for a number of common acids are given in Table \(\PageIndex{1}\). The values of \(K_b\) for a number of common weak bases are given in Table \(\PageIndex{2}\). A similar concept applies to bases, except the reaction is different. Hence the ionization equilibrium lies virtually all the way to the right, as represented by a single arrow: \[HCl_{(aq)} + H_2O_{(l)} \rightarrow H_3O^+_{(aq)}+Cl^_{(aq)} \label{16.5.17} \]. All acidbase equilibria favor the side with the weaker acid and base. Conversely, smaller values of \(pK_b\) correspond to larger base ionization constants and hence stronger bases. An acid or base which strongly conducts electricity contains a large number of ions and is called a strong acid or base and an acid or base which conducts electricity only weakly contains only a few ions and is called a weak acid or base. 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 \(NO_3^\). Hydronium ion H3O+ H2O 1 0.0 In contrast, acetic acid is a weak acid, and water is a weak base. Multiply the molarity of the strong base NaOH by the volume of the NaOH (MB VB = 0.500 M 20.70 mL). HSO 4-Hydrogen sulfate ion. For example, commercial aqueous reagents, such as concentrated acids and bases, are typically expressed as weight/weight % solutions. Upon distillation, nitric acid in its pure form begins to boil at 78.2C and becomes solid when it is well cooled. 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 . 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 They are also highly resistant to temperature changes. Two species that differ by only a proton constitute a conjugate acidbase pair. In a weak acid like hydrofluoric acid (HF), not all of the HF molecules split up, and although there will be some H+ and F- ions released, there will still be HF molecules in solution1. C6H5COOH\text{C}_6\text{H}_5\text{COOH}C6H5COOH. Input a temperature and density within the range of the table to calculate for concentration or input concentration . The stronger an acid is, the lower the pH it will produce in solution. Acid and Base Strength is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. Water . Similarly, the equilibrium constant for the reaction of a weak base with water is the base ionization constant (\(K_b\)). 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. Strong acids have mostly ions in solution, therefore the bonds holding H and A together must be weak. This result clearly tells us that HI is a stronger acid than \(HNO_3\). For weak acids and bases, the higher the Ka or Kb, the more acidic or basic the solution. pH is calculated by taking the negative logarithm of the concentration of hydronium ions. 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 word titration comes from the French word tiltre, originally meaning the "proportion of gold or silver in coins," later meaning the "concentration of a substance in a given sample." Thus propionic acid should be a significantly stronger acid than \(HCN\). (@37.5%) = 12.2 moles (range 11.85 - 12.34) Boiling Point 110C (230F) Nitric Acid. 16.4: Acid Strength and the Acid Dissociation Constant (Ka) is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. The selection of the indicator used depends on the initial concentration of the Nitric Acid and the strength of the alkali used. Enter both the weight and total volume of your application above if the chemical is a solid. This would be a simple mass particle and let me go get my mona math of nitric, acid, nitric acid, which will be 484959 plus 63. Let's consider the concentrated HNO3 found generally in labs (70%, normality- 15.8) In order to make 1L of 0.5(N) acid,. University of Maiduguri. A 50.0 mL sample of 0.200 M sodium hydroxide is titrated with 0.200 M nitric acid. Thus the proton is bound to the stronger base. The equilibrium constant for this dissociation is as follows: \[K=\dfrac{[H_3O^+][A^]}{[H_2O][HA]} \label{16.5.2} \]. [3] White fuming nitric acid, also called 100% nitric acid or WFNA, is very close to anhydrous nitric acid. The table below gives the density (kg/L) and the . Thus nitric acid should properly be written as \(HONO_2\). Nitric acid is the most commonly used wash for scale removal and pH stabilization after a caustic wash. At a typical concentration of 0.5%, it can be used effectively at lower temperatures than caustic solutions, requiring less heating. The blue line is the curve, while the red line is its derivative. * A base that has a very high pH (10-14) are known as . 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https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FGeneral_Chemistry%2FMap%253A_A_Molecular_Approach_(Tro)%2F16%253A_Acids_and_Bases%2F16.04%253A_Acid_Strength_and_the_Acid_Dissociation_Constant_(Ka), \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), Example \(\PageIndex{1}\): Butyrate and Dimethylammonium Ions, Solutions of Strong Acids and Bases: The Leveling Effect, Calculating pH in Strong Acid or Strong Base Solutions, status page at https://status.libretexts.org, \(\cancel{HCN_{(aq)}} \rightleftharpoons H^+_{(aq)}+\cancel{CN^_{(aq)}} \), \(K_a=[H^+]\cancel{[CN^]}/\cancel{[HCN]}\), \(\cancel{CN^_{(aq)}}+H_2O_{(l)} \rightleftharpoons OH^_{(aq)}+\cancel{HCN_{(aq)}}\), \(K_b=[OH^]\cancel{[HCN]}/\cancel{[CN^]}\), \(H_2O_{(l)} \rightleftharpoons H^+_{(aq)}+OH^_{(aq)}\). The Brnsted-Lowry theory describes acid-base interactions in terms of proton transfer between chemical species. The equilibrium will therefore lie to the right, favoring the formation of the weaker acidbase pair: \[ \underset{\text{stronger acid}}{CH_3CH_2CO_2H_{(aq)}} + \underset{\text{stronger base}}{CN^-_{(aq)}} \ce{<=>>} \underset{\text{weaker base}}{CH_3CH_2CO^-_{2(aq)}} +\underset{\text{weaker acid}} {HCN_{(aq)}} \nonumber \], A Video Discussing Polyprotic Acids: Polyprotic Acids [youtu.be]. 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. 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. Relevant comments and/or instructions will appear here after a calculation is performed. The experiment has possibilities for use as an assessed practical. Perchloric acid. In Imperial or US customary measurement system, the density is equal to 94.44726 pound per cubic foot [lb/ft], or 0. . Like any other conjugate acidbase pair, the strengths of the conjugate acids and bases are related by \(pK_a\) + \(pK_b\) = pKw. For example, propionic acid and acetic acid are identical except for the groups attached to the carbon atom of the carboxylic acid (\(\ce{CH_2CH_3}\) versus \(\ce{CH_3}\)), so we might expect the two compounds to have similar acidbase properties. Because it is 100% ionized or completely dissociates ions in an aqueous solution. The leveling effect applies to solutions of strong bases as well: In aqueous solution, any base stronger than OH is leveled to the strength of OH because OH is the strongest base that can exist in equilibrium with water. Acids or bases with strong bonds exist predominately as molecules in solutions and are called "weak" acids or bases. 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: . According to Tables \(\PageIndex{1}\) and \(\PageIndex{2}\), \(NH_4^+\) is a stronger acid (\(pK_a = 9.25\)) than \(HPO_4^{2}\) (pKa = 12.32), and \(PO_4^{3}\) is a stronger base (\(pK_b = 1.68\)) than \(NH_3\) (\(pK_b = 4.75\)). At the equivalence point, the number of moles of titrant added equals the number of moles of an analyte according to the reaction stoichiometry. For example, commercially available concentrated hydrochloric acid (HCl) is 37% by weight (w/w %). Weak acids exist mostly as molecules with only a few ions in solution, therefore the bonds holding H and A together must be strong. Its \(pK_a\) is 3.86 at 25C. As you may know, when an acid or a base dissolves in water, their H+\small\text{H}^+H+ and OH\small\text{OH}^-OH ions respectively dissociate, shifting the natural self-ionization equilibrium of water (2H2OH3O++OH\small2\text{H}_2\text{O}\rightleftharpoons\text{H}_3\text{O}^+ + \text{OH}^-2H2OH3O++OH), making the solution more acidic or more basic. The hydrogen ion concentration decreases by a factor of 10, so the pH increases by 1 . 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 ). The corresponding expression for the reaction of cyanide with water is as follows: \[K_b=\dfrac{[OH^][HCN]}{[CN^]} \label{16.5.9} \]. For example, the general equation for the ionization of a weak acid in water, where HA is the parent acid and A is its conjugate base, is as follows: \[HA_{(aq)}+H_2O_{(l)} \rightleftharpoons H_3O^+_{(aq)}+A^_{(aq)} \label{16.5.1} \]. where each bracketed term represents the concentration of that substance in solution. The difference between this and the starting point gives you the volume, and from this, you can calculate the molarity of the analyte using the equation above. Conversely, smaller values of \(pK_b\) correspond to larger base ionization constants and hence stronger bases. Question 2 (10 points) A concentrated aqueous solution of nitric acid (HNO3) has a density of 1.42 g/mL and contains 79.0% nitric acid by mass. Check out 19 similar mixtures and solutions calculators , Table of common acids and bases and their strengths. Because these molecules do not fully dissociate, the pH shifts less near the equivalence point. Other factors may also be important when deciding on the type of percent solution to prepare. 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. 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. In aqueous solutions, \(H_3O^+\) is the strongest acid and \(OH^\) is the strongest base that can exist in equilibrium with \(H_2O\). The larger the Ka, the stronger the acid and the higher the H + concentration at equilibrium. It depends on the strength of the H-A bond. Scope 1.1 This test method covers determination of the assay of nitric acid by total acidity. For this reason, you must select the correct indicator for the right combination of solutions, as the range of color changes needs to have the equivalence point in it. Is there a correlation of acidity with the formal charge on the central atom, E? Because the stronger acid forms the weaker conjugate base, we predict that cyanide will be a stronger base than propionate. 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). The titration curve can also determine whether the solution is a strong or weak acid/base. National Institutes of Health. Hydrofluoric acid is particularly dangerous because it is capable of eating through glass, as seen in the video in the links sectionV1. However, if you have two unknowns (the starting nitric acid concentration and the amount of sodium bicarbonate addition) you would need to first determine the concentration of the nitric acid with a standard acid-base titration. There are some exceptions, such as carbon monoxide, CO, nitrous oxide, N2O, and nitric oxide, NO. Acid & Base Molarity & Normality Calculator . About Nitric acid. We can use the relative strengths of acids and bases to predict the direction of an acidbase reaction by following a single rule: an acidbase equilibrium always favors the side with the weaker acid and base, as indicated by these arrows: \[\text{stronger acid + stronger base} \ce{ <=>>} \text{weaker acid + weaker base} \nonumber \]. 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 . To calculate sulfuric acid solution concentration use EBAS - stoichiometry calculator. Other examples that you may encounter are potassium hydride (\(KH\)) and organometallic compounds such as methyl lithium (\(CH_3Li\)). Therefore the solution of benzoic acid will have a lower pH. For example, to find the % w/v of a solution the calculation is: (Mass of Solute (g) / Volume of Solution (ml)) x 100. CALCULATOR OPTIONS Acid & Base Molarity & Normality Calculator. 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. The larger the \(K_b\), the stronger the base and the higher the \(OH^\) concentration at equilibrium. Because the initial quantity given is \(K_b\) rather than \(pK_b\), we can use Equation \(\ref{16.5.10}\): \(K_aK_b = K_w\). 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. The conjugate acidbase pairs are \(CH_3CH_2CO_2H/CH_3CH_2CO_2^\) and \(HCN/CN^\). Because the \(pK_a\) value cited is for a temperature of 25C, we can use Equation \(\ref{16.5.16}\): \(pK_a\) + \(pK_b\) = pKw = 14.00. The Complete Aqueous Hydrochloric Acid Solutions Density-Concentration Calculator. (In fact, the \(pK_a\) of propionic acid is 4.87, compared to 4.76 for acetic acid, which makes propionic acid a slightly weaker acid than acetic acid.) The constants \(K_a\) and \(K_b\) are related as shown in Equation \(\ref{16.5.10}\). When different volumes of an identical solution are added together, the final volume will always be exactly the sum of the individual portions added. Volume/volume % solutes are also common, and are used when pure solutes in liquid form are used. According to Table \(\PageIndex{1}\), HCN is a weak acid (pKa = 9.21) and \(CN^\) is a moderately weak base (pKb = 4.79). Predict its pH when it is diluted to 0.1 g/dm 3 . Nitric acid (HNO) is a colorless liquid with yellow or red fumes with an acrid odor. Our chemical concentration sensors can handle the most difficult acids, including hydrofluoric acid and oleum. 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. Name. The curve around the equivalence point will be relatively steep and smooth when working with a strong acid and a strong base. Initial Data. 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. * An acid that has a very low pH (0-4) are known as Strong acids. According to the reaction equation. It should take approximately 25 minutes. When dealing with a strong acid and a weak base, or vice versa, the titration curve becomes more irregular. For example, hydrochloric acid (HCl) is a strong acid. As we noted earlier, because water is the solvent, it has an activity equal to 1, so the \([H_2O]\) term in Equation \(\ref{16.5.2}\) is actually the \(\textit{a}_{H_2O}\), which is equal to 1. From the volume of titrant used, the composition of the analyte can be calculated knowing the stoichiometry of the chemical reaction. 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: \[HCN_{(aq)} \rightleftharpoons H^+_{(aq)}+CN^_{(aq)} \label{16.5.6} \], \[CN^_{(aq)}+H_2O_{(l)} \rightleftharpoons OH^_{(aq)}+HCN_{(aq)} \label{16.5.7} \]. Rounded to nearest 0.5ml. Titrations have many applications in the modern world, although a lot of the original uses have been made redundant by more modern techniques: To help determine an unknown solution, e.g., one collected from the field. Identify the conjugate acidbase pairs in each reaction. Your Safer Source for Science. This test method is suitable for concentrations between approximately 50 and 70 %, calculated as nitric acid. The weaker the bond, the lesser the energy required to break it. Instead, a pH meter is often used. Concentration Before Dilution (C1) %. 8.84 Lb/Gal. If you're getting enough nitrates in your diet, you can boost nitric oxide in other ways, as well. An important note is in order. For an acid, the reaction will be HA + H2O --> A- + H3O+ . Acids and bases behave differently in solution based on their strength. are hidden by default. 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. The \(pK_a\) of butyric acid at 25C is 4.83. The equilibrium will therefore lie to the right, favoring the formation of the weaker acidbase pair: \[ \underset{\text{stronger acid}}{NH^+_{4(aq)}} + \underset{\text{stronger base}}{PO^{3-}_{4(aq)}} \ce{<=>>} \underset{\text{weaker base}}{NH_{3(aq)}} +\underset{\text{weaker acid}} {HPO^{2-}_{4(aq)}} \nonumber \]. Nitric acid reacts with calcium compounds, forming calcium nitrate, which has a solubility of 56%. An older density scale is occasionally seen, with concentrated nitric acid specied as 42 Baum. The table was taken from "Perry's Chemical Engineers' Handbook" by Robert H. Perry, Don Green, Sixth Edition. 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Support under grant numbers 1246120, 1525057, and solution volume is combined! Thus the proton is bound to the stronger the acid and the higher the \ ( SO_4^ { 2 \. Is titrated with 0.200 M sodium hydroxide is titrated with 0.200 M hydroxide... } _6\text { H } _5\text { COOH } C6H5COOH be weak below the! Pure form begins to boil at 78.2C and becomes solid when it is diluted to 0.1 3... Ions in solution volume/volume % solutes are also common, and nitric oxide, N2O, and nitric oxide NO... 100 grams of nitric acid by total acidity around the equivalence point will be HA + H2O -- > +. And their strengths by the volume of titrant used, the density is equal to: 50.00 10-3 0.100... Very close to anhydrous nitric acid should be a stronger base than propionate 12.2 moles ( range 11.85 - )... Where each bracketed term represents the concentration of the dimethylammonium ion ( \ ( HCN\ ) of 56 % typically! Grams of nitric acid by total acidity HA + H2O -- > +... 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