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. Mass of \(\ce{HC2H3O2}\) in vinegar sample, Mass of vinegar sample (assume density = 1.00 g/mL), Mass Percent of \(\ce{HC2H3O2}\) in vinegar, \[\ce{Ba(OH)2 (aq) + 2 HC2H3O2 (aq) -> Ba(C2H3O2)2 (aq) + 2 H2O (l)}\]. The titration betweenacetic acid and sodium hydroxide is a 1:1 stoichiometry. When finished, dispose of your chemical waste as instructed. 3. 2. An equilibrium expression can be written for the reactions of weak bases with water. A: All the class of molecules are organic molecules. What type of solution forms when a metal oxide dissolves in water? startxref Volume of HNO2 = 2.50 mL = 0.0025 L A: Since you have asked multiparts, we will solve the first three subparts for you. If your standardised sodium hydroxide solution was determined to be 0.060 M, and it required an average titre (titration volume) of 20.3 mL, what is the concentration (in M) of the undiluted vinegar sample (the initial vinegar sample)? PDF ap07 chemistry q1 - College Board The ionization constant for acetic acid is 1.8 x 10-5. Kw at 35.0C is 2.1 1014. Hence the \(pK_b\) of \(SO_4^{2}\) is 14.00 1.99 = 12.01. What is the Similarly, the equilibrium constant for the reaction of a weak base with water is the base ionization constant (\(K_b\)). endstream endobj 127 0 obj<. Consider 50.0 mL of a solution of weak acid HA (Ka = 1.00 106), which has a pH of 4.000. Notice the inverse relationship between the strength of the parent acid and the strength of the conjugate base. 0000007180 00000 n What will be the pH of a 0.10 M HC2H3O2 solution which is 0.10 M in NaC2H3O2 2. Calculate the pH of this buffer. A: 2.303 comes from the conversion of the "ln" function into the "log" function. If we are given any one of these four quantities for an acid or a base (\(K_a\), \(pK_a\), \(K_b\), or \(pK_b\)), we can calculate the other three. (a) Calculate the pH and pOH in the final solution. The \(\ce{NaOH}\) will be added to the vinegar sample until all the acetic acid in the vinegar has been exactly consumed (reacted away). What would happen if 0.1 mole of HCI is added to the original solution? 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. 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. Now use the volumetric pipette to transfer 5.00-mL of vinegar into a clean 250-mL Erlenmeyer flask (see instructions on page 4). Carbonated water is a solution of carbonic acid (H2CO3). Why is the use of high-precision volumetric material essential for titration? A weak base is a base that ionizes only slightly in an aqueous solution. Which of these compounds would be the best buffer at pH 5.0: formic acid (pKa = 3.8), acetic acid (pKa = 4.76), or ethylamine (pKa = 9.0)? = + [H O ][F . A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. This page titled 21.13: Strong and Weak Bases and Base Ionization Constant is shared under a CK-12 license and was authored, remixed, and/or curated by CK-12 Foundation via source content that was edited to the style and standards of the LibreTexts platform; a detailed edit history is available upon request. Volume of 0.100 M HCl = 7.0 mL = 0.007 L We write the equation as an equilibrium because both the forward and reverse processes are occurring at the same time. For any conjugate acidbase pair, \(K_aK_b = K_w\). Write the acidic equilibrium equation for HPO c. Write the acidic ionization equation for HSO. (b) Why would we wait for it to return to room temperature? pH = -log[H3O+], A: The two molecules are structural isomers of each other i.e. ln(Keq) = 2.303 *. Consider, for example, the \(HSO_4^/ SO_4^{2}\) conjugate acidbase pair. The values of \(K_b\) for a number of common weak bases are given in Table \(\PageIndex{2}\). How do I determine the molecular shape of a molecule? What type of solution forms when a nonmetal oxide dissolves in water? In an acidbase reaction, the proton always reacts with the stronger base. b. When HCl is added then NaA will react with it and, A: Make an ICE table,Ka =[CH3COO-][H3O+][CH3COOH]= (0.10+X)(X)(0.050-X)=1.80x10-5, A: A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate, A: Moles = Concentration X volume of solution in L, A: Buffer solution: A buffer solutions is an aqueous solution consisting of a mixture of a weak base, A: The solution of 0.25 M HCOOH and 0.3 M HCOONa is n acidic buffer. Solved Write the ionization reaction equation and the proper - Chegg A student wants to prepare a buffer with a pH of 4.76 by combining 25.00mL of 0.30MHC2H3O2 with 75.00mL of 0.10MNaC2H3O2. 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 equilibrium constant for this dissociation is as follows: \[K=\dfrac{[H_3O^+][A^]}{[H_2O][HA]} \label{16.5.2} \]. 0000003482 00000 n 0000011905 00000 n The larger the concentration of ions, the better the solutions conducts. A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. For example, nitrous acid (\(HNO_2\)), with a \(pK_a\) of 3.25, is about a million times stronger acid than hydrocyanic acid (HCN), with a \(pK_a\) of 9.21. But,, A: Molecular formula = C4H8SOx The most common strong bases are soluble metal hydroxide compounds such as potassium hydroxide. The table below is a listing of base ionization constants for several weak bases. In this case, we are given \(K_b\) for a base (dimethylamine) and asked to calculate \(K_a\) and \(pK_a\) for its conjugate acid, the dimethylammonium ion. (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.) A: The purpose of adding sodium azide is explain which is given below. Write the remaining substances as the net ionic equation.Writing and balancing net ionic equations is an important skill in chemistry and is essential for understanding solubility, electrochemistry, and focusing on the substances and ions involved in the chemical reaction and ignoring those that dont (the spectator ions).More chemistry help at http://www.Breslyn.org A: The "solubility product (Ksp)" is a constant which remains proportional to the salts solubility., A: The question is based on the concept of titrations. Give an example of such an oxide. a. What was the purpose of the phenolphthalein indicator in this experiment? Solved 1. The ionization constant, K | Chegg.com DrnBSmq;@R25oso+H&x2x+#W5! kK>fQy)3(NH`VErAt#>w O0'#38KayO]"?#Px^OOy%#T/B#4iv!>>1VWnIc#4>=J`i 0000003615 00000 n 0000020215 00000 n Begin the titration by slowly adding \(\ce{NaOH}\) (, As the equivalence point is approached, the pink color will become more pervasive and will take longer to disappear. Polyprotic acids (and bases) lose (and gain) protons in a stepwise manner, with the fully protonated species being the strongest acid and the fully deprotonated species the strongest base. The ionization constant, Ka, for acetic acid, HC2H3O2, is 1.76 10-5. Papaverine hydrochloride (abbreviated papH+Cl; molar mass = 378.85 g/mol) is a drug that belongs to a group of medicines called vasodilators, which cause blood vessels to expand, thereby increasing blood flow. John C. Kotz, Paul M. Treichel, John Townsend, David Treichel, David W. Oxtoby, H. Pat Gillis, Laurie J. Butler. 0000011316 00000 n A base ionization constant \(\left( K_\text{b} \right)\) is the equilibrium constant for the ionization of a base. Show all work for each step in the spaces provided. HC2H3O2(aq) + K+(aq) +OH-(aq) K+(aq) +C2H3O- 2(aq)+ H2O (l) This gives the net ionic equation With your left hand, squeeze the pipette bulb. How does Charle's law relate to breathing? A: Given: 0000036750 00000 n Then determine the total mass of the vinegar sample from the vinegar volume and the vinegar density. Note: Assume that the ionization of the acid is small enough in comparison to its starting concentration that the concentration First, we balance the molecular equation. Be especially careful when handling the sodium hydroxide base (\(\ce{NaOH}\)), as it is corrosive and can cause chemical burns to the skin. Phenolphthalein is a pH sensitive organic dye. NaOH +, A: Calculate the total number of moles of HCl and sodium acetate. 8.3x10^-7, basic b.) Use your two best sets of results along with calculated values in the previous table to determine the mass percent of acetic acid in vinegar. The pH of the buffer solution = 5.0 126 0 obj <> endobj What possible reasons could there be fornot simply weighing the solid NaOH, dissolving to a known volume and calculating itsmolarity? (a) What is the pH of the buffer? Sodium hydroxide dissociates in water as follows: 0000002736 00000 n First, convert the moles of \(\ce{HC2H3O2}\) in the vinegar sample (previously calculated) to a mass of \(\ce{HC2H3O2}\), via its molar mass. Acidbase reactions always proceed in the direction that produces the weaker acidbase pair. What are the molecular, ionic, and net ionic equations for the reaction Accessibility StatementFor more information contact us atinfo@libretexts.org. If any NaOH spills on you, rinse immediately under running water for up to 15 minutes and report the accident to your instructor. The \(pK_a\) and \(pK_b\) for an acid and its conjugate base are related as shown in Equations \(\ref{16.5.15}\) and \(\ref{16.5.16}\). A strong base is a base thationizes completely in an aqueous solution. Write the ionization equation for this weak acid. One of the components of this system is a series of coils filled with ammonia that are located on the outside of the shuttle. 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, \(H_3O^+\). 0000022399 00000 n Solved Acetic acid, HC2H3O2, is a weak acid. The following - Chegg HC2H3O2 + H2O H3O+ + C2H3O2 arrow_forward Acids You make a solution by dissolving 0.0010 mol of HCl in enough water to make 1.0 L of solution. HC2H3O2 to maintain a hydrogen ion Show all work for each step in the spaces provided. A titration involves performing a controlled reaction between a solution of known concentration (the titrant) and a solution of unknown concentration (the analyte). 1.2x10^-10, acidic c.) 2.9x10^-13, acidic Calculate the pH and pOH of each solution. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. The other hydrogen atoms are not acidic. \[HA_{(aq)} \rightleftharpoons H^+_{(aq)}+A^_{(aq)} \label{16.5.3} \]. For ammonia, the expression is: \[K_\text{b} = \frac{\left[ \ce{NH_4^+} \right] \left[ \ce{OH^-} \right]}{\left[ \ce{NH_3} \right]}\nonumber \]. Please resubmit the, A: First calculate molarity of HCl In this experiment, a technique known as a titration will be used to determine the concentration of acetic acid in vinegar. Then add about 20-mL of distilled water and 5 drops of phenolphthalein to this Erlenmeyer flask. pH is expressed in terms of the PKa and the ratio of the base to acid concentrations using the Henderson-Hasselbalch equation. 16.6: Finding the [H3O+] and pH of Strong and Weak Acid Solutions is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. Calculate \(K_a\) and \(pK_a\) of the dimethylammonium ion (\((CH_3)_2NH_2^+\)). 0000015832 00000 n Concentration of HCH3CO2 = 0.6100 M An example of an Arrhenius base is the highly soluble sodium hydroxide, \text {NaOH} NaOH. \[\ce{NH_3} \left( aq \right) + \ce{H_2O} \left( l \right) \rightleftharpoons \ce{NH_4^+} \left( aq \right) + \ce{OH^-} \left( aq \right)\nonumber \]. A Video Calculating pH in Strong Acid or Strong Base Solutions: Calculating pH in Strong Acid or Strong Base Solutions [youtu.be]. David W. Oxtoby, H. Pat Gillis, Laurie J. Butler, Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer, Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste. The relative order of acid strengths and approximate \(K_a\) and \(pK_a\) values for the strong acids at the top of Table \(\PageIndex{1}\) were determined using measurements like this and different nonaqueous solvents. Slowly roll your finger to one side and allow the liquid to drain until the bottom of the meniscus is aligned with the volume mark. At what pH does the equivalence point occur? Calculate \(K_a\) for lactic acid and \(pK_b\) and \(K_b\) for the lactate ion. Ionic equilibri. This approach is both inexpensive and effective. Again, for simplicity, \(H_3O^+\) can be written as \(H^+\) in Equation \(\ref{16.5.3}\). A weak base is a base that ionizes only slightly in an aqueous solution. Volume of NaOH =V1=10.5ml (a) Write the equilibrium-constant expression for the dissociation of HF(aq) in water. Then allow the liquid to drain from the pipette. We write the equation as an equilibrium because both the forward and reverse processes are occurring at the same time. Specialized equipment is needed to perform a titration. (credit: modification of work by Sahar Atwa) This image shows two bottles containing clear colorless solutions. Calculate the pH of this buffer. Note that three titrations must be performed. The ionization constant of acetic acid 50-mL burette*, 5-mL volumetric pipette*, pipette bulb*, ~ 0.1 M \(\ce{NaOH}\) (aq), vinegar, phenolphthalein, burette stand, two 250-mL (or 125 mL) Erlenmeyer flasks, wash bottle with distilled water, funnel. 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. Molarity of C3H7NH2 = 0.2500 M The sodium hydroxide will be gradually added to the vinegar in small amounts from a burette. The relative strengths of some common acids and their conjugate bases are shown graphically in Figure \(\PageIndex{1}\). Rinse the inside of the burette with distilled water. Volume of formic acid = 225 ml 0000000016 00000 n 0.100 M propanoic acid (HC3H5O2, Ka = 1.3 105) b. Stephen Lower, Professor Emeritus (Simon Fraser U.) 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) + H2O ( l) H3O + ( aq) + A ( aq) The equilibrium constant for this dissociation is as follows: K = [H3O +][A ] [H2O][HA] A: Draw the structural formula of 2-nitropropanoic acid ? An acidic buffer is formed by mixing an aqueous, A: Use acidic buffer equation to get the answer . First, convert the moles of HC 2 H 3 O 2 in the vinegar sample (previously calculated) to a mass of HC 2 H 3 O 2, via its molar mass. How to Write the Net Ionic Equation for HC2H3O2 - YouTube The conjugate base of a strong acid is a weak base and vice versa. Acid rain has a devastating effect on marble statuary left outdoors. weight of sample = 12.64 mg 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. trailer Similarly, in the reaction of ammonia with water, the hydroxide ion is a strong base, and ammonia is a weak base, whereas the ammonium ion is a stronger acid than water. You will then take a 25.00 mL aliquot from this diluted vinegar solution and titrate it against the standardised sodium hydroxide. Calculate the pH of a solution prepared by mixing 250. mL of 0.174 m aqueous HF (density = 1.10 g/mL) with 38.7 g of an aqueous solution that is 1.50% NaOH by mass (density = 1.02 g/mL). Solved Acetic acid, HC2H3O2, is a weak acid. The following - Chegg 0000005035 00000 n Cu2+ + e- ---> Cu+ E=, A: From solubility product constant values and the concentration of S2-will give the concentration of, A: Express your answer in condensed form in order of increasing orbital energy--, A: Which one of the following is correct answer, A: Plasma is a very good electrical conductor. At 25C, \(pK_a + pK_b = 14.00\). Why was benzoic acid used as a solvent when making up the glucose stock standard solution? Acetic acid, HC2H3O2 (aq), was used to make the buffers in this experiment. 0000002052 00000 n In one part : given a structure of a amine Molecule. Note: Assume that the ionization of the acid is small enough in comparison to its starting concentration that the concentration of unionized acid is almost as large at equilibrium as it was originally. Since at equilibrium [H 3O +] = 1.0 10 7M, it must also be true that [OH ] = 1.0 10 7M. 0000010984 00000 n All, A: We will use buffer equation in all parts, A: Ammonia is a weak base and HNO3 is a strong acid. Thus nitric acid should properly be written as \(HONO_2\). Like all equilibrium constants, acidbase ionization constants are actually measured in terms of the activities of \(H^+\) or \(OH^\), thus making them unitless. 0000019399 00000 n In a situation like this, the best approach is to look for a similar compound whose acidbase properties are listed. Why did the color of the solution in the conical flask change at the end of the titration? When mixed, a neutralization reaction occurs between sodium hydroxide and the acetic acid in vinegar: \[\ce{NaOH (aq) + HC2H3O2 (aq) NaC2H3O2 (aq) + H2O (l)}\]. 16.6: Weak Acids - Chemistry LibreTexts Assume that the vinegar density is 1.000 g/mL (= to the density of water). There are 0.2 mole of HC2H3O2 and 0.2 mole Finally, calculate the mass percent of acetic acid in vinegar from the mass of \(\ce{HC2H3O2}\) and the mass of vinegar. The base ionization constant \(K_b\) of dimethylamine (\((CH_3)_2NH\)) is \(5.4 \times 10^{4}\) at 25C. Hence, A: H5,H6,H7 are aromatic protons which are in 6.5 to 7 ppm and H1, H2, H3,H4 and H8/H9 are non-,, A: Given Because of the use of negative logarithms, smaller values of \(pK_a\) correspond to larger acid ionization constants and hence stronger acids. Reaction between the standard and analyte must be known. Unfortunately, however, the formulas of oxoacids are almost always written with hydrogen on the left and oxygen on the right, giving \(HNO_3\) instead. When the bottom of the meniscus is even with the volume mark, press your index finger firmly on the top of the pipette so no liquid leaks out. The following is the equilibrium equation for its reaction with water: HC2H3O2 (aq) + H2O (l) <----------> H3O+ (aq) + C2H3O2- (aq) Ka = 1.8 x 10-5 What is the pOH of a 4.27 M HC2H3O2 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. When a weak base such as ammonia is dissolved in water, it accepts an \(\ce{H^+}\) ion from water, forming the hydroxide ion and the conjugate acid of the base, the ammonium ion. Concentration of NaOH, A: To gain a general understanding of Gibbs energy and its applications in chemistry. Second, we write the states and break the soluble ionic compounds into their ions (these are the strong electrolytes with an (aq) after them). One method is to use a solvent such as anhydrous acetic acid. Equilibrium always favors the formation of the weaker acidbase pair. If the base (NaOH) is standardized to 0.12 M in Part A of this experiment, calculate the amount of oxalic acid dihydrate (H2C2O42H2O, MW = 126.06 g/mol) required to neutralize 35 mL of this NaOH solution. (Write equations to show your answer.) = + [H O ][F ] 3 a [HF] K One point is earned for the correct expression. For HCHO (acetic acid), the acidic equilibrium equation is: HCHO (aq) H (aq) + CHO (aq) b. 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]. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. The acid that has lost the #"H"^"+"# (the conjugate base) then gets a negative charge. 0000021736 00000 n Accessibility StatementFor more information contact us atinfo@libretexts.org. Marble is almost pure CaCO3. The numerical value of \(K_\text{b}\) is a reflection of the strength of the base. Write the ionization reaction equation and the proper Ka expression for the ionization of acetic acid, HC2H3O2 The ionization reaction equation: Ka expression = This problem has been solved! An indicator solution is used to indicate when all the acetic acid has been consumed and that the reaction in complete. The neutralization of HC2H3O2 (aq) by NaOH (aq) can be considered to be the sum of the neutralization of H+ (aq) by OH- and ionization of HC2H3O2 (HC2H3O2<==> H+ + C2H3O2). What specialized device is used to obtain this precise volume? Conversely, smaller values of \(pK_b\) correspond to larger base ionization constants and hence stronger bases. (b) the molar solubility of CaCO3 in pure water. having same molecular formula but. %PDF-1.6 % What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)? This page titled 11: Titration of Vinegar (Experiment) is shared under a CC BY-NC license and was authored, remixed, and/or curated by Santa Monica College. Predict whether the equilibrium for each reaction lies to the left or the right as written. What is the buffer capacity of the buffers in Problem 10? What type of flask is the acetic acid placed in? NaOH to the original solution? We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. new pH? A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. Legal. From this mole value (of \(\ce{NaOH}\)), obtain the moles of \(\ce{HC2H3O2}\) in the vinegar sample, using the mole-to-mole ratio in the balanced equation. Acid-base reaction - Dissociation of molecular acids in water Is the acetic acid the analyte or the titrant? This is a buffer solution, A: Glacial acetic acid is purest form of acetic acid in which anhydrous form or undiluted form of, A: According to the question we have the reaction for the piperidine (C5H10NH) and iodic acid (HIO3):-, A: Since the exact question is not mentioned we only answer the first question. Smaller values of \(pK_a\) correspond to larger acid ionization constants and hence stronger acids. 0000005547 00000 n 0000007403 00000 n The equilibrium for the acid ionization of HC2H3O2 is represented by the equation above. The buffer capacity indicates how much OH- or H+ ions a buffer can react with. Then remove the pipette tip from the beaker of solution. Volume of HNO3 = 15.4, A: Amount of acid added can be calculated using Henderson-Hasselbalch equation for buffer solution: 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: \[pK_b = \log_{10}K_b \label{16.5.13} \]. Touch the tip once to the side of the beaker to remove any hanging drops. A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. Using the pipette bulb, draw the water into the pipette up above the 5-mL mark, then allow it to drain out through the tip. The magnitude of the equilibrium constant for an ionization reaction can be used to determine the relative strengths of acids and bases. While balancing a redox. Obtain a 50-mL burette, 5-mL volumetric pipette and a pipette bulb from the stockroom. Be sure not to press the tip against the bottom of the container. How do you calculate the ideal gas law constant? A: The given experiments are for organic reactions. 0000017781 00000 n Acetic acid, HC2H3O2 (aq), was used to make the buffers in this experiment. What is the new pH? We could also have converted \(K_b\) to \(pK_b\) to obtain the same answer: \[pK_b=\log(5.4 \times 10^{4})=3.27 \nonumber \], \[K_a=10^{pK_a}=10^{10.73}=1.9 \times 10^{11} \nonumber \].