For the gas, see, Except where otherwise noted, data are given for materials in their, William Hyde Wollaston (1814) "A synoptic scale of chemical equivalents,", Last edited on 23 November 2022, at 05:56, "Clinical correlates of pH levels: bicarbonate as a buffer", "The chemistry of ocean acidification: OCB-OA", https://en.wikipedia.org/w/index.php?title=Bicarbonate&oldid=1123337121, This page was last edited on 23 November 2022, at 05:56. The dividing line is close to the pH 8.6 you mentioned in your question. Identify the general Ka and Kb expressions, Recall how to use Ka and Kb expressions to solve for an unknown. By clicking Post Your Answer, you agree to our terms of service, privacy policy and cookie policy. The Ka of NH4is 5.6x10- 10 and the Kb of HCO3 is 2.3x10-8. An acid's conjugate base gets deprotonated {eq}[A^-] {/eq}, and a base's conjugate acid gets protonated {eq}[B^+] {/eq} upon dissociation. What if the temperature is lower than or higher than room temperature? rev2023.3.3.43278. Correction occurs when the values for both components of the buffer pair (HCO 3 / H 2 CO 3) return to normal. Some of the $\mathrm{pH}$ values are above 8.3. The full treatment I gave to this problem was indeed overkill. I would like to evaluate carbonate and bicarbonate concentration from groundwater samples, but I only have values of total alkalinity as $\ce{CaCO3}$, $\mathrm{pH}$, and temperature. The higher the Kb, the the stronger the base. These constants have no units. $$K1 = \frac{\ce{[H3O+][HCO3-]}}{\ce{[H2CO3]}} \approx 4.47*10^-7 $$, Second stage: Titration Curves Graph & Function | How to Read a Titration Curve, R.I.C.E. For help asking a good homework question, see: How do I ask homework questions on Chemistry Stack Exchange? Question thumb_up 100% How can I check before my flight that the cloud separation requirements in VFR flight rules are met? It is an equilibrium constant that is called acid dissociation/ionization constant. \[pK_a + pK_b = 14.00 \; \text{at 25C} \], Stephen Lower, Professor Emeritus (Simon Fraser U.) In fact, the hydrogen ions have attached themselves to water to form hydronium ions (H3O+). All rights reserved. Substituting the values of \(K_b\) and \(K_w\) at 25C and solving for \(K_a\), \[K_a(5.4 \times 10^{4})=1.01 \times 10^{14}\]. The flow of bicarbonate ions from rocks weathered by the carbonic acid in rainwater is an important part of the carbon cycle. [10], "Hydrogen carbonate" redirects here. Bicarbonate also acts to regulate pH in the small intestine. At the bottom left of Figure 16.5.2 are the common strong acids; at the top right are the most common strong bases. The equation then becomes Kb = (x)(x) / [NH3]. The equation is NH3 + H2O <==> NH4+ + OH-. Like all equilibrium constants, acidbase ionization constants are actually measured in terms of the activities of \(H^+\) or \(OH^\), thus making them unitless. At 25C, \(pK_a + pK_b = 14.00\). HCO3 H CO3 2 (9.20a) and 2 H c b 3 2 ' 3 2 K [HCO ] . The renal electrogenic Na/HCO3 cotransporter moves HCO3- out of the cell and is thought to have a Na+:HCO3- stoichiometry of 1:3. Strong acids dissociate completely, and weak acids dissociate partially. 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 freshwater ecology, strong photosynthetic activity by freshwater plants in daylight releases gaseous oxygen into the water and at the same time produces bicarbonate ions. How do/should administrators estimate the cost of producing an online introductory mathematics class? There are no HCl molecules to be found because 100% of the HCl molecules have broken apart into hydrogen ions and chloride ions. From the equilibrium, we have: The Ka value is the dissociation constant of acids. My problem is that according to my book, HCO3- + H2O produces an acidic solution, thus giving acidic rain. The dissociation constant can be sought if information about the solution's pH was given. Its like a teacher waved a magic wand and did the work for me. What video game is Charlie playing in Poker Face S01E07? Subsequently, we have cloned several other . It is about twice as effective in fire suppression as sodium bicarbonate. If I have three species, but only two show up together at any given time, I can "forget" I'm dealing with a diprotic acid. Styling contours by colour and by line thickness in QGIS. Solving for {eq}[H^+] = 9.61*10^-3 M {/eq}. 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 \(H^3O^+\). 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. The Ka value is very small. When the calcium carbonate dissolves, a equilibrium is established between its three forms, expressed by the respective equilibrium equations: First stage: She has a PhD in Chemistry and is an author of peer reviewed publications in chemistry. John Wiley & Sons, 1998. \(K_a = 1.4 \times 10^{4}\) for lactic acid; \(pK_b\) = 10.14 and \(K_b = 7.2 \times 10^{11}\) for the lactate ion. TABLE OF CONJUGATE ACID-BASE PAIRS Acid Base K a (25 oC) HClO 4 ClO 4 - H 2 SO 4 HSO 4 - HCl Cl- HNO 3 NO 3 - H 3 O + H 2 O H 2 CrO 4 HCrO 4 - 1.8 x 10-1 H 2 C 2 O 4 (oxalic acid) HC 2 O 4 - 5.90 x 10-2 [H 2 SO 3] = SO 2 (aq) + H2 O HSO We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. A solution of this salt is acidic. For any conjugate acidbase pair, \(K_aK_b = K_w\). Find the pH. The magnitude of the equilibrium constant for an ionization reaction can be used to determine the relative strengths of acids and bases. It is a measure of the proton's concentration in a solution. vegan) just to try it, does this inconvenience the caterers and staff? Hydrochloric acid, on the other hand, dissociates completely to chloride ions and protons: {eq}HCl_(aq) \rightarrow H^+_(aq) + Cl^-_(aq) {/eq}. The reaction equations along with their Ka values are given below: H2CO3 (aq) <=====> HCO3- + H+ Ka1 = 4.3 X 107 mol/L; pKa1 = 6.36 at 25C What are practical examples of simultaneous measuring of quantities? All other trademarks and copyrights are the property of their respective owners. We have an acetic acid (HC2H3O2) solution that is 0.9 M. Its hydronium ion concentration is 4 * 10^-3 M. What is the Ka for acetic acid? O c. HCO3- (aq) + OH- (aq)-CO32- (aq) + H20 (/) O d. H2C03 (aq) + H2O (/)-HCO3Taq) + H3O+ (aq) O e. Kenneth S. Johnson, Carbon dioxide hydration and dehydration kinetics in seawater, Limnol. Oceanogr., 27 (5), 1982, 849-855 p.851 table 1. [4][5] The name lives on as a trivial name. So we are left with three unknown variables, $\ce{[H2CO3]}$, $\ce{[HCO3-]}$ and $\ce{[CO3^2+]}$. Ocean Biomes, Working Scholars Bringing Tuition-Free College to the Community. What ratio of bicarb to vinegar do I need in order for the result to be pH neutral? We know that the Kb of NH3 is 1.8 * 10^-5. Thus the proton is bound to the stronger base. So: {eq}K_a = \frac{[x^2]}{[0.6]}=1.3*10^-8 \rightarrow x^2 = 0.6*1.3*10^-4 \rightarrow x = \sqrt{0.6*1.3*10^-8} = 8.83*10^-5 M {/eq}, {eq}[H^+] = 8.83*10^-5 M \rightarrow pH = -log[H^+] \rightarrow pH = -log 8.83*10^-5 = 4.05 {/eq}. $[\mathrm{alk}_{tot}]=[\ce{HCO3-}]+2[\ce{CO3^2-}]+[\ce{OH-}]-[\ce{H+}]$, $[\mathrm{alk}_{tot}]=[\ce{HCO3-}]+[\ce{OH-}]-[\ce{H+}]$. As an inexpensive, nontoxic base, it is widely used in diverse application to regulate pH or as a reagent. For acids, these values are represented by Ka; for bases, Kb. The respective proportions in comparison with the total concentration of calcium carbonate dissolved are $\alpha0$, $\alpha1$ and $\alpha2$. Bicarbonate serves a crucial biochemical role in the physiological pH buffering system.[3]. Once again, the concentration does not appear in the equilibrium constant expression.. The Ka equation and its relation to kPa can be used to assess the strength of acids. In darkness, when no photosynthesis occurs, respiration processes release carbon dioxide, and no new bicarbonate ions are produced, resulting in a rapid fall in pH. What is the pKa of a solution whose Ka is equal to {eq}2*10^-5 mol/L {/eq}? Thanks for contributing an answer to Chemistry Stack Exchange! Ka for HC2H3O2: 1.8 x 10 -5Ka for HCO3-: 4.3 x 10 -7Using the Ka's for HC2H3O2 and HCO3, calculate the Kb's for the C2H3O2- and CO32- ions. Their equation is the concentration of the ions divided by the concentration of the acid/base. We use the equilibrium constant, Kc, for a reaction to demonstrate whether or not the reaction favors products (the forward reaction is dominant) or reactants (the reverse reaction is dominant). B is the parent base, BH+ is the conjugate acid, and OH- is the conjugate base. I asked specifically for HCO3-: "Kb of bicarbonate is greater than Ka?". If we add Equations \(\ref{16.5.6}\) and \(\ref{16.5.7}\), we obtain the following (recall that the equilibrium constant for the sum of two reactions is the product of the equilibrium constants for the individual reactions): \[\cancel{HCN_{(aq)}} \rightleftharpoons H^+_{(aq)}+\cancel{CN^_{(aq)}} \;\;\; K_a=[H^+]\cancel{[CN^]}/\cancel{[HCN]}\], \[\cancel{CN^_{(aq)}}+H_2O_{(l)} \rightleftharpoons OH^_{(aq)}+\cancel{HCN_{(aq)}} \;\;\; K_b=[OH^]\cancel{[HCN]}/\cancel{[CN^]}\], \[H_2O_{(l)} \rightleftharpoons H^+_{(aq)}+OH^_{(aq)} \;\;\; K=K_a \times K_b=[H^+][OH^]\]. Does Magnesium metal react with carbonic acid? A bit over 6 bicarbonate ion takes over, and reigns up to pH a bit over 10, from where fully ionized carbonate ion takes over. Consider the salt ammonium bicarbonate, NH 4 HCO 3. B) Due to oxides of sulfur and nitrogen from industrial pollution. It makes the problem easier to calculate. 1. Why does Mister Mxyzptlk need to have a weakness in the comics? Sodium hydroxide is a strong base that dissociates completely in water. 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 Kb value is high, which indicates that CO_3^2- is a strong base. EDIT: I see that you have updated your numbers. Two species that differ by only a proton constitute a conjugate acidbase pair. What is the point of Thrower's Bandolier? So bicarb ion is. To subscribe to this RSS feed, copy and paste this URL into your RSS reader. It is measured, along with carbon dioxide, chloride, potassium, and sodium, to assess electrolyte levels in an electrolyte panel test (which has Current Procedural Terminology, CPT, code 80051). Calculate the Kb values for the CO32- and C2H3O2- ions using the Ka values for HCO3- (4.7 x 10-11) and HC2H3O2 (1.8 x 10-5), respectively. With the expressions for all species, it's helpful to use a spreadsheet to automate the calculations for a entire range of pH values, to grasp in a visual way what happens with carbonates as pH changes. Write the acid dissociation formula for the equation: Ka = [H_3O^+] [CH_3CO2^-] / [CH_3CO_2H]. As such it is an important sink in the carbon cycle. 133 lessons Enthalpy vs Entropy | What is Delta H and Delta S? 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. For acids, this relationship is shown by the expression: Ka = [H3O+][A-] / [HA]. Recently it has been also demonstrated that cellular bicarbonate metabolism can be regulated by mTORC1 signaling. * Compiled from Appendix 5 Chem 1A, B, C Lab Manual and Zumdahl 6th Ed. Because \(pK_a\) = log \(K_a\), we have \(pK_a = \log(1.9 \times 10^{11}) = 10.72\). Remember that Henderson-Hasselbalch provides the equilibrium ratio of concentrations at a given pH. Did any DOS compatibility layers exist for any UNIX-like systems before DOS started to become outmoded? The distribution of carbonate species as a fraction of total dissolved carbonate in relation to . The Ka of a 0.6M solution is equal to {eq}1.54*10^-4 mol/L {/eq}. However, we would still write the dissociation the same: HF + H2O --> H3O+ + F-. The plot that looks like a "XX" also allows us to see a interesting property of carbonates. $$K1 = \frac{\ce{[H3O+][HCO3-]}}{\ce{[H2CO3]}} \approx 4.47*10^-7 $$, $$K2 = \frac{\ce{[H3O+][CO3^2-]}}{\ce{[HCO3-]}} \approx 4.69*10^-11 $$, $$K1K2 = \frac{\ce{[H3O+]^2[CO3^2-]}}{\ce{[H2CO3]}}$$, $$Cs = \ce{[CaCO3]} = \ce{[H2CO3] + [HCO3-] + [CO3^2-]}$$, $$Cs = \ce{[H2CO3] + [HCO3-] + [CO3^2-]}$$, $$Cs = \ce{\frac{[HCO3-][H3O+]}{K1} + [HCO3-] + \frac{K2[HCO3-]}{[H3O+]}}$$, $$Cs = \ce{\frac{[HCO3-][H3O+]^2 + K1[HCO3-][H3O+] + K1K2[HCO3-]}{K1[H3O+]}}$$, $$\frac{\ce{[HCO3-]}}{Cs} = \ce{\frac{K1[H3O+]}{[H3O+]^2 + K1[H3O+] + K1K2}} = \alpha1$$, $$\alpha0 = \frac{\ce{[H2CO3]}}{Cs} = \ce{\frac{[H3O+]^2}{[H3O+]^2 + K1[H3O+] + K1K2}}$$, $$\alpha2 = \frac{\ce{[CO3^2-]}}{Cs} = \ce{\frac{K1K2}{[H3O+]^2 + K1[H3O+] + K1K2}}$$, $$\ce{[H3O+]} = \frac{\ce{K2[HCO3-]}}{\ce{[CO3^2-]}}$$, $$pH = pK2 + log(\frac{\ce{[HCO3-]}}{[CO3^2-]})$$, $$\ce{[H3O+]} = \frac{\ce{K1[H2CO3]}}{\ce{[HCO3-]}}$$, $$pH = pK1 + log(\frac{\ce{[H2CO3]}}{[HCO3-]})$$. HCl is the parent acid, H3O+ is the conjugate acid, and Cl- is the conjugate base. 1. The larger the Ka, the stronger the acid and the higher the H + concentration at equilibrium. These shift the pH upward until in certain circumstances the degree of alkalinity can become toxic to some organisms or can make other chemical constituents such as ammonia toxic. Substituting the \(pK_a\) and solving for the \(pK_b\). The conjugate acidbase pairs are listed in order (from top to bottom) of increasing acid strength, which corresponds to decreasing values of \(pK_a\). Conversely, smaller values of \(pK_b\) correspond to larger base ionization constants and hence stronger bases. Diprotic Acid Overview & Examples | What Is a Diprotic Acid? then: +2 2 3 T [ HCO ][ ]H = CZ (13) - + 3 1 T [ HCO][ ] HK = CZ (14) 2312 [] T HCOKK CZ = (15) Figure 5.1. Notice the inverse relationship between the strength of the parent acid and the strength of the conjugate base. Calculate \(K_a\) and \(pK_a\) of the dimethylammonium ion (\((CH_3)_2NH_2^+\)). It is a white solid. Sort by: $K_a = 4.8 \times 10^{-11}\ (mol/L)$. What is the significance of charge balancing when analysing system speciation (carbonate system given as an example)? In order to learn when a chemical behaves like an acid or like a base, dissociation constants must be introduced, starting with Ka. The \(pK_a\) and \(pK_b\) for an acid and its conjugate base are related as shown in Equation 16.5.15 and Equation 16.5.16. $$\alpha2 = \frac{\ce{[CO3^2-]}}{Cs} = \ce{\frac{K1K2}{[H3O+]^2 + K1[H3O+] + K1K2}}$$. Bicarbonate is the dominant form of dissolved inorganic carbon in sea water,[9] and in most fresh waters. The higher the Kb, the the stronger the base. For example, let's see what will happen if we add a strong acid such as HCl to this buffer. Does it change the "K" values? For example normal sea water has around 8.2 pH and HCO3 is . Potassium bicarbonate is used as a fire suppression agent ("BC dry chemical") in some dry chemical fire extinguishers, as the principal component of the Purple-K dry chemical, and in some applications of condensed aerosol fire suppression. Again, for simplicity, \(H_3O^+\) can be written as \(H^+\) in Equation \(\ref{16.5.3}\). In fact, for all acids we can use a general expression for dissociation using the generic acid HA: HA + H2O --> H3O+ + A-. copyright 2003-2023 Study.com. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. To solve this problem, we will need a few things: the equation for acid dissociation, the Ka expression, and our algebra skills. If we were to zoom into our sample of hydrofluoric acid, a weak acid, we would find that very few of our HF molecules have dissociated. From the equilibrium, we have: By clicking Accept all cookies, you agree Stack Exchange can store cookies on your device and disclose information in accordance with our Cookie Policy. Bronsted-Lowry defines acids as chemical substances that have the ability to donate protons to other substances. Ka = (4.0 * 10^-3 M) (4.0 * 10^-3 M) / 0.90 M. This Ka value is very small, so this is a weak acid. Why does it seem like I am losing IP addresses after subnetting with the subnet mask of 255.255.255.192/26? {eq}[A^-] {/eq} is the molar concentration of the acid's conjugate base. Hence the ionization equilibrium lies virtually all the way to the right, as represented by a single arrow: \[HCl_{(aq)} + H_2O_{(l)} \rightarrow \rightarrow H_3O^+_{(aq)}+Cl^_{(aq)} \label{16.5.17}\]. I would definitely recommend Study.com to my colleagues. Plug in the equilibrium values into the Ka equation. A conjugate base is the negatively charged particle that remains after a proton has dissociated from an acid. Electrochemistry: Cell Potential & Free Energy | What is Cell Potential? Use the relationships pK = log K and K = 10pK (Equation 16.5.11 and Equation 16.5.13) to convert between \(K_a\) and \(pK_a\) or \(K_b\) and \(pK_b\). Ka is the dissociation constant for acids. The base ionization constant \(K_b\) of dimethylamine (\((CH_3)_2NH\)) is \(5.4 \times 10^{4}\) at 25C. Its formula is {eq}pH = - log [H^+] {/eq}. $$Cs = \ce{[CaCO3]} = \ce{[H2CO3] + [HCO3-] + [CO3^2-]}$$, Where Cs here stands for the known concentration of the salt, calcium carbonate. But at the same time it states that HCO3- will react as a base, because it's Kb >> Ka, True, $HCO_3^-$ will react as both an acid and a base. (Kb > 1, pKb < 1). The larger the Ka value, the stronger the acid. This explains why the Kb equation and the Ka equation look similar. Potassium bicarbonate ( IUPAC name: potassium hydrogencarbonate, also known as potassium acid carbonate) is the inorganic compound with the chemical formula KHCO 3. potassium hydrogencarbonate, potassium acid carbonate, InChI=1S/CH2O3.K/c2-1(3)4;/h(H2,2,3,4);/q;+1/p-1, InChI=1/CH2O3.K/c2-1(3)4;/h(H2,2,3,4);/q;+1/p-1, Except where otherwise noted, data are given for materials in their, "You Have the (Baking) Power with Low-Sodium Baking Powders", "Why Your Bottled Water Contains Four Different Ingredients", "Powdery Mildew - Sustainable Gardening Australia", "Efficacy of Armicarb (potassium bicarbonate) against scab and sooty blotch on apples", Safety Data sheet - potassium bicarbonate, https://en.wikipedia.org/w/index.php?title=Potassium_bicarbonate&oldid=1107665193, Pages using collapsible list with both background and text-align in titlestyle, Articles containing unverified chemical infoboxes, Wikipedia articles incorporating a citation from the New International Encyclopedia, Creative Commons Attribution-ShareAlike License 3.0, This page was last edited on 31 August 2022, at 05:54. First, write the balanced chemical equation. What is the value of Ka? Given: pKa and Kb Asked for: corresponding Kb and pKb, Ka and pKa Strategy: The constants Ka and Kb are related as shown in Equation 16.5.10. {eq}[OH^-] {/eq} is the molar concentration of the hydroxide ion. The equilibrium constant expression for the ionization of HCN is as follows: \[K_a=\dfrac{[H^+][CN^]}{[HCN]} \label{16.5.8}\]. We need a weak acid for a chemical reaction. Stack Exchange network consists of 181 Q&A communities including Stack Overflow, the largest, most trusted online community for developers to learn, share their knowledge, and build their careers. They must sum to 1(100%), as in chemical reactions matter is neither created or destroyed, only changing between forms. The pH measures the acidity of a solution by measuring the concentration of hydronium ions. The same procedure can be repeated to find the expressions for the alphas of the other dissolved species. Yes, they do. The following example shows how to find Ka from pH: The pH of a weak acid is equal to 2.12. Acids are substances that donate protons or accept electrons. Potassium bicarbonate (IUPAC name: potassium hydrogencarbonate, also known as potassium acid carbonate) is the inorganic compound with the chemical formula KHCO3. What is the Ka of a solution whose known values are given in the table: {eq}pH = -log[H^+]=-logx \rightarrow x = 10^-1.7 = 0.0199 {/eq}, {eq}K_a = (0.0199)^2/0.048 = 8.25*10^-3 {/eq}. Alte Begriffe/Zusammenhnge: Das chemische Gleichgewicht: Massenwirkungsgesetz und Formulierung des MWG aus einer Reaktionsgleichung. How do I ask homework questions on Chemistry Stack Exchange? Potassium bicarbonate is a contact killer for Spanish moss when mixed 1/4 cup per gallon. Learn how to use the Ka equation and Kb equation. Full text of the 'Sri Mahalakshmi Dhyanam & Stotram', As a groundwater sample, any solids dissolved are very diluted, so we don't need to worry about. The term "bicarbonate" was coined in 1814 by the English chemist William Hyde Wollaston. The pH measures the concentration of hydronium at equilibrium: {eq}[H^+] = 10^-2.12 = 7.58*10^-3 M {/eq}. A solution of this salt is acidic . This compound is a source of carbon dioxide for leavening in baking. The pKa and pKb for an acid and its conjugate base are related as shown in Equation 16.5.15 and Equation 16.5.16. Browse other questions tagged, Start here for a quick overview of the site, Detailed answers to any questions you might have, Discuss the workings and policies of this site. How to calculate the pH value of a Carbonate solution? There is a simple relationship between the magnitude of \(K_a\) for an acid and \(K_b\) for its conjugate base. To learn more, see our tips on writing great answers. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. 2018ApHpHHCO3-NaHCO3. Acid with values less than one are considered weak. Conversely, smaller values of \(pK_b\) correspond to larger base ionization constants and hence stronger bases. It's a scale ranging from 0 to 14. Now we can start replacing values taken from the equilibrium expressions into the material balance, isolating each unknow. From your question, I can make some assumptions: Carbonic acid, $\ce{H2CO3}$, has two ionizable hydrogens, so it may assume three forms: The free acid itself, bicarbonate ion, $\ce{HCO3-}$(first-stage ionized form) and carbonate ion $\ce{CO3^2+}$(second-stage ionized form). Conjugate acids (cations) of strong bases are ineffective bases. TRUE OR FALSE Expert Answer 100% (6 ratings) Answer False Explanation Ammonium bicarbonate (NH4HCO3) is the salt made by the reaction between weak ba View the full answer However, that sad situation has a upside. The constants \(K_a\) and \(K_b\) are related as shown in Equation 16.5.10.
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