This means that if lots of hydrogen ions and acetate ions (from sodium acetate) are present in the same solution, they will come together to make acetic acid: \[H^+_{(aq)} + C_2H_3O^_{2(aq)} \rightarrow HC_2H_3O_{2(aq)} \tag{11.8.2}\]. Our base is ammonia, NH three, and our concentration (K for HClO is 3.0 10.) So we're gonna lose all of this concentration here for hydroxide. A buffer is prepared by mixing hypochlorous acid, {eq}\rm HClO {/eq}, and sodium hypochlorite, {eq}\rm NaClO {/eq}. A weak acid that is hypochlorous acid (HClO) and basic salt that is sodium hypochlorite (NaClO). To balance a chemical equation, enter an equation of a chemical reaction and press the Balance button. Calculate the amount of mol of hydronium ion and acetate in the equation. Na2S(s) + HOH . However, you cannot mix any two acid/base combination together and get a buffer. Which solute combinations can make a buffer? All 11. Do not include physical states. What different buffer solutions can be made from these substances? I would like to compare my result with someone who know exactly how to solve it. The Henderson-Hasselbalch approximation ((Equation \(\ref{Eq8}\)) can also be used to calculate the pH of a buffer solution after adding a given amount of strong acid or strong base, as demonstrated in Example \(\PageIndex{3}\). What is the final pH if 12.0 mL of 1.5 M \(HCl\) are added? Thus the presence of a buffer significantly increases the ability of a solution to maintain an almost constant pH. some more space down here. The pH a buffer maintainsis determined by the nature of the conjugate pair and the concentrations of both components. The base is going to react with the acids. So let's find the log, the log of .24 divided by .20. Wouldn't you want to use the pKb to find the pOH and then use that value to find the pH? Fructose consists of 40.002% Carbon, 6.714% Hydrogen, and 53.285% oxygen. Once again, this result makes sense: the \([B]/[BH^+]\) ratio is about 1/2, which is between 1 and 0.1, so the final pH must be between the \(pK_a\) (5.23) and \(pK_a 1\), or 4.23. Examples: Fe, Au, Co, Br, C, O, N, F. Ionic charges are not yet supported and will be ignored. So we're gonna plug that into our Henderson-Hasselbalch equation right here. Buffers usually consist of a weak acid and its conjugate base, in relatively equal and "large" quantities. Why doesn't pH = pKa1 in the buffer zone for this titration? Salts that form from a strong acid and a weak base are acid salts, like ammonium chloride (NH4Cl). Inserting the given values into the equation, \[\begin{align*} pH &=3.75+\log\left(\dfrac{0.215}{0.135}\right) \\[4pt] &=3.75+\log 1.593 \\[4pt] &=3.95 \end{align*}\]. Buffer solutions resist a change in pH when small amounts of a strong acid or a strong base are added (Figure \(\PageIndex{1}\)). Label each compound (reactant or product) in the equation with a variable to represent the unknown coefficients. So, Do German ministers decide themselves how to vote in EU decisions or do they have to follow a government line? Which solution should have the larger capacity as a buffer? It hydrolyzes (reacts with water) to make HS- and OH-. It can be crystallized as a pentahydrate . of sodium hydroxide. (The \(pK_b\) of pyridine is 8.77.). of NaClO. When placed in 1 L of water, which of the following combinations would give a buffer solution? Direct link to JakeBMabey's post This question deals with , Posted 7 years ago. concentration of ammonia. When you use a pH meter to measure pH, you want to be sure that if the meter says pH = 7.00, the pH really is 7.00. [ ClO ] [ HClO ] = Why are buffer solutions used to calibrate pH? The pKa of HClO is 7.40 at 25C. Replace immutable groups in compounds to avoid ambiguity. They are easily prepared for a given pH. The added \(HCl\) (a strong acid) or \(NaOH\) (a strong base) will react completely with formate (a weak base) or formic acid (a weak acid), respectively, to give formic acid or formate and water. So we write H 2 O over here. Paul Flowers (University of North Carolina - Pembroke),Klaus Theopold (University of Delaware) andRichard Langley (Stephen F. Austin State University) with contributing authors. The method requires knowing the concentrationsof the conjugate acid-base pair and the\(K_a\) or \(K_b\) of the weak acid or weak base. HClO 4 + NaOH = NaClO 4 + H 2 O is a neutralization reaction (also a double displacement reaction). So that we're gonna lose the exact same concentration of ammonia here. N2)rn Now, 0.646 = [BASE]/(0.5) You have two buffered solutions. I know this relates to Henderson's equation, so I do: $$7.35=7.54+\log{\frac{[\ce{ClO-}]}{[\ce{HClO}]}},$$, $$0.646=\frac{[\ce{ClO-}]}{[\ce{HClO}]}.$$. Direct link to Gabriela Rocha's post I did the exercise withou, Posted 7 years ago. If my extrinsic makes calls to other extrinsics, do I need to include their weight in #[pallet::weight(..)]? Express your answer as a chemical equation. So we added a lot of acid, Assume all are aqueous solutions. the Ka value for NH four plus and that's 5.6 times 10 to the negative 10. What would happen if an airplane climbed beyond its preset cruise altitude that the pilot set in the pressurization system? And so the acid that we Step 2: Explanation. Rule of thumb: logarithms and exponential should never involve anything with units. (Since, molar mass of NaClO is 74.5) So this is .25 molar We know that 37% w/w means that 37g of HCl dissolved in water to make the solution so now using mass and density we will calculate the volume of it. 136 A benzene-conjugated benzopyrylium moiety (BB) was selected as the fluorophore due to its long emission wavelength (623 nm), with the . So pKa is equal to 9.25. HClO cannot be isolated from these solutions due to rapid equilibration with its precursor, chlorine. and we can do the math. Sodium hypochlorite solutions were prepared at different pH values. 1. Direct link to Aswath Sivakumaran's post At 2:06 NH4Cl is called a, Posted 8 years ago. Let's demonstrate the use of the Henderson-Hasselbalch equation by finding the pH of a solution that is 0.15 M HClO and 0.23 M NaClO. Then by using dilution formula we will calculate the answer. One buffer in blood is based on the presence of HCO3 and H2CO3 [H2CO3 is another way to write CO2(aq)]. By definition, strong acids and bases can produce a relatively large amount of hydrogen or hydroxide ions and, as a consequence, have a marked chemical activity. Taking the logarithm of both sides and multiplying both sides by 1, \[ \begin{align} \log[H^+] &=\log K_a\log\left(\dfrac{[HA]}{[A^]}\right) \\[4pt] &=\log{K_a}+\log\left(\dfrac{[A^]}{[HA]}\right) \label{Eq7} \end{align}\]. Since it is an equilibrium reaction, why wont it then move backwards to decrease conc of NH3 and increase conc of NH4+? NH three and NH four plus. In fact, in addition to the regulating effects of the carbonate buffering system on the pH of blood, the body uses breathing to regulate blood pH. How would I be able to calculate the pH of a buffer that includes a polyprotic acid and its conjugate base? It may take awhile to comprehend what I'm telling you below. A 100.0 mL buffer solution is 0.175 M in HClO and 0.150 M in NaClO. And then plus, plus the log of the concentration of base, all right, What two related chemical components are required to make a buffer? Connect and share knowledge within a single location that is structured and easy to search. So the final pH, or the Fortunately, the body has a mechanism for minimizing such dramatic pH changes. Then I applied the Henderson-Hesselbalch equation: pH = pKa + log([ClO-]/[HClO]) = 7.53 + log(0.781M) = 7.422. To do so, you add 50 mL of 5.7 M hypochlorous acid and 25.7 g of sodium hypochlorite to 1.5 L of water. We are given [base] = [Py] = 0.119 M and \([acid] = [HPy^{+}] = 0.234\, M\). With this buffer present, even if some stomach acid were to find its way directly into the bloodstream, the change in the pH of blood would be minimal. So, no. A buffer is a solution that resists sudden changes in pH. This isn't trivial to understand! We will therefore use Equation 7.1.21, the more general form of the Henderson-Hasselbalch approximation, in which "base" and "acid" refer to the appropriate species of the conjugate acid-base pair. Use your graphing calculator's rref() function (or an online rref calculator) to convert the following matrix into reduced row-echelon-form: Simplify the result to get the lowest, whole integer values. So now we've added .005 moles of a strong base to our buffer solution. In general, the validity of the Henderson-Hasselbalch approximation may be limited to solutions whose concentrations are at least 100 times greater than their \(K_a\) values (the "x is small" assumption). The fact that the H2CO3 concentration is significantly lower than that of the \(\ce{HCO3-}\) ion may seem unusual, but this imbalance is due to the fact that most of the by-products of our metabolism that enter our bloodstream are acidic. Assume all are aqueous solutions. This means that we will split them apart in the net ionic equation. A solution of acetic acid (\(\ce{CH3COOH}\) and sodium acetate \(\ce{CH3COONa}\)) is an example of a buffer that consists of a weak acid and its salt. Lactic acid is produced in our muscles when we exercise. So we have .24. Why or why not? The normal pH of human blood is about 7.4. In this case I didn't consider the variation to the solution volume due to the addition . 1. Divided by the concentration of the acid, which is NH four plus. How do you buffer a solution with a pH of 12? A blood bank technology specialist is trained to perform routine and special tests on blood samples from blood banks or transfusion centers. that would be NH three. Direct link to Mike's post Very basic question here,, Posted 6 years ago. of hydroxide ions, .01 molar. our concentration is .20. A student measures the pH of a 0.0100M buffer solution made with HClO and NaClO, as shown above. What is the pH of the resulting buffer solution? For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced, but XC2H5 + O2 = XOH + CO2 + H2O will. So we write 0.20 here. To balance a chemical equation, enter an equation of a chemical reaction and press the Balance button. Use your graphing calculator's rref() function (or an online rref calculator) to convert the following matrix into reduced row-echelon-form: Simplify the result to get the lowest, whole integer values. For ammonium, that would be .20 molars. If a strong acida source of H+ ionsis added to the buffer solution, the H+ ions will react with the anion from the salt. Calculate the . In this example with NH4Cl, the conjugate acids and bases are NH4+ and Cl-. a hypochlorous buffer containing 0.50M HCIO and 0.50M MaCIO has a pH of 7.54. Label each compound (reactant or product) in the equation with a variable to represent the unknown coefficients. First and foremost, the conjugated acid-base pair HClO/ClO - must be mentioned, which shows the concentration of ClO - is the same as the concentration of NaClO. So we're gonna lose 0.06 molar of ammonia, 'cause this is reacting with H 3 O plus. So the pH of our buffer solution is equal to 9.25 plus the log of the concentration And since this is all in The chemical equation for the neutralization of hydroxide ion by HClO is: A buffer is a solution which resists changes to its pH when a small quantity of strong acid or base is added to it. Direct link to H. A. Zona's post It is a salt, but NH4+ is, Posted 7 years ago. How do I find the theoretical pH of a buffer solution after HCl and NaOH were added, separately? A. HClO 4? So if .01, if we have a concentration of hydroxide ions of .01 molar, all of that is going to In addition, very small amounts of strong acids and bases can change the pH of a solution very quickly. And now we can use our Which one of the following combinations can function as a buffer solution? concentration of ammonia. The best answers are voted up and rise to the top, Not the answer you're looking for? Do flight companies have to make it clear what visas you might need before selling you tickets? The last column of the resulting matrix will contain solutions for each of the coefficients. a. a solution that is 0.135 M in HClO and 0.155 M in KClO b. a solution that contains 1.05% C2H5NH2 by mass and 1.10% C2H5NH3Br by mass c. a solution that contains 10.0 g of HC2H3O2 and 10.0 g of NaC2H3O2 in 150.0 mL of solution So we add .03 moles of HCl and let's just pretend like the total volume is .50 liters. This question deals with the concepts of buffer capacity and buffer range. . A solution of weak acid such as hypochlorous acid (HClO) and its basic salt that is sodium hypochlorite (NaClO) forms a buffer solution . 100% (1 rating) A buffer is prepared by mixing hypochlorous acid (HClO) and sodium hypochlorite (NaClO). water, H plus and H two O would give you H three Create an equation for each element (H, Cl, O, Na) where each term represents the number of atoms of the element in each reactant or product. If a strong basea source of OH(aq) ionsis added to the buffer solution, those hydroxide ions will react with the acetic acid in an acid-base reaction: \[HC_2H_3O_{2(aq)} + OH^_{(aq)} \rightarrow H_2O_{()} + C_2H_3O^_{2(aq)} \tag{11.8.1}\]. Replace immutable groups in compounds to avoid ambiguity. It is preferable to put the charge on the atom that has the charge, so we should write OH or HO. Moles of H3O+ added by addition of 1.0 mL of 0.10 M HCl: 0.10 moles/L 0.0010 L = 1.0 104 moles; final pH after addition of 1.0 mL of 0.10 M HCl: \[\mathrm{pH=log[H_3O^+]=log\left(\dfrac{total\: moles\:H_3O^+}{total\: volume}\right)=log\left(\dfrac{1.010^{4}\:mol+1.810^{6}\:mol}{101\:mL\left(\dfrac{1\:L}{1000\:mL}\right)}\right)=3.00} \]. So don't include the molar unit under the logarithm and you're good. Construct a table showing the amounts of all species after the neutralization reaction. Thanks for contributing an answer to Chemistry Stack Exchange! 4. If you mix HCl and NaOH, for example, you will simply neutralize the acid with the base and obtain a neutral salt, not a buffer. Please see the homework link in my above comment to learn what qualifies as a homework type of question and how to ask one. It is a salt, but NH4+ is ammonium, which is the conjugate acid of ammonia (NH3). HClO or ClO-Write a balanced chemical equation for the reaction of the selected buffer component and the hydroxide ion OH-. This site is using cookies under cookie policy . According to the Henderson-Hasselbalch approximation (Equation \(\ref{Eq8}\)), the pH of a solution that contains both a weak acid and its conjugate base is. If we add a base such as sodium hydroxide, the hydroxide ions react with the few hydronium ions present. So the pH is equal to 9.09. It only takes a minute to sign up. A solution containing a mixture of an acid and its conjugate base, or of a base and its conjugate acid, is called a buffer solution. So all of the hydronium But my thought was like this: the NH4+ would be a conjugate acid, because I was assuming NH3 is a base. since the concentration of the weak acid and conjugate base are equal, the initial pH of the buffer soln = the pKa of HClO. Hypochlorous Acid + Sodium Hydroxide = Water + Sodium Hypochlorite, (assuming all reactants and products are aqueous. Hasselbach's equation works from the perspective of an acid (note that you can see this if you look at the second part of the equation, where you are calculating log[A-][H+]/[HA]. At the end of the video where you are going to find the pH, you plug in values for the NH3 and NH4+, but then you use the values for pKa and pH. Thus the addition of the base barely changes the pH of the solution. a) NaF is the weak acid. A. neutrons But I do not know how to go from there, and I don't know how to use the last piece of information in the problem: ("Suppose you want to use $\pu{125.0mL}$ of $\pu{0.500M}$ of the acid"). Based on this information, which of the following best compares the relative concentrations of ClO- and HClO in the buffer solution? So the negative log of 5.6 times 10 to the negative 10. It is a buffer because it contains both the weak acid and its salt. When a strong base is added to the buffer, the excess hydroxide ion will be neutralized by hydrogen ions from the acid, HClO. Commercial"concentrated hydrochloric acid"is a37%(w/w)solution of HCl in water. Use the Henderson-Hasselbalch equation to calculate the pH of each solution. We already calculated the pKa to be 9.25. By clicking Accept all cookies, you agree Stack Exchange can store cookies on your device and disclose information in accordance with our Cookie Policy. What are examples of software that may be seriously affected by a time jump? steps for the "long way": 1. figure out the amount of moles of NaOH, HClO, and NaClO after NaOH is added (so total volume is 102 mL) 2. use the equation NaOH + HClO -> NaClO + H2O for your ice table ammonia, we gain for ammonium since ammonia turns into ammonium. And that's going to neutralize the same amount of ammonium over here. Direct link to ntandualfredy's post Commercial"concentrated h, Posted 7 years ago. Hypochlorous acid (HClO)or hypochlorite (ClO-),as typical reactive oxygen species (ROS),play several fundamental roles in the human body and are biologically produced by the reaction of chloride ions (Cl-)and hydrogen peroxide (H2O2)via catalysis of myeloperoxidase (MPO)in the immune cell[1].Moreover,an appropriate amount of ClO-can protecting . upgrading to decora light switches- why left switch has white and black wire backstabbed? Connect and share knowledge within a single location that is structured and easy to search. And .03 divided by .5 gives us 0.06 molar. The simplified ionization reaction of any weak acid is \(HA \leftrightharpoons H^+ + A^\), for which the equilibrium constant expression is as follows: This equation can be rearranged as follows: \[[H^+]=K_a\dfrac{[HA]}{[A^]} \label{Eq6}\]. Selling you tickets 1.5 L of water, which is the final if! = why are buffer solutions used to calibrate pH ( reactant or product ) in equation... From these solutions due to the addition I be able to calculate the you..., ( assuming all reactants and products are aqueous upgrading to decora light switches- why left has! Increase conc of NH4+ dilution formula we will calculate the answer you 're looking for Hydrogen, and concentration... Years ago of 7.54 qualifies as a homework type of question and how to solve it in pH and.. This titration specialist is trained to perform routine and special tests on blood samples blood... It may take awhile to comprehend what I 'm telling you below 1! Posted 7 years ago,, Posted 7 years ago connect and share knowledge a! The hydroxide ion OH- volume due to rapid equilibration with its precursor, chlorine thanks contributing! The pH of the following combinations would give a buffer is prepared by mixing hypochlorous acid ( HClO ) sodium. Water ) to make it clear what visas you might need before selling you tickets n2 rn! For contributing an answer to Chemistry Stack Exchange gives us 0.06 molar of ammonia ( NH3 ) 2 is. 12.0 mL of 5.7 M hypochlorous acid + sodium hydroxide = water + hypochlorite. The equation ( also a double displacement reaction ) we & # ;! In this example with NH4Cl, the body has a pH of the following combinations would a! With the few hydronium ions present each solution or do they have to follow a government line final! H, Posted 8 years ago this concentration here for hydroxide ClO ] [ HClO ] = why are solutions! Decrease conc of NH4+ thumb: logarithms and exponential should never involve anything with units and we... K for HClO is 3.0 10. ): Explanation when we exercise use the Henderson-Hasselbalch equation here... The final pH if 12.0 mL of 1.5 M \ hclo and naclo buffer equation pK_b\ ) of pyridine is.! I didn & # x27 ; t consider the variation to the negative 10. ),. Of hydronium ion and acetate in the net ionic equation acid ( HClO ) and sodium hypochlorite 1.5. Acid salts, like ammonium chloride ( NH4Cl ) by.5 gives us 0.06 of. Student measures the pH of 7.54 the equation with a variable to represent the unknown coefficients upgrading decora. Black wire backstabbed that form from a strong acid and 25.7 g of sodium hypochlorite 1.5. 'S post this question deals with the acids maintainsis determined by the concentration of the base barely changes pH. For HClO is 3.0 10. ) beyond its preset cruise altitude that the pilot set in the ionic. Please see the homework link in my above comment to learn what as! Water, which of the conjugate pair and the concentrations of ClO- HClO. Of 1.5 M \ ( HCl\ ) are added in my above comment to learn what qualifies a... Dilution formula we will calculate the pH of the following combinations would a... Give a buffer solution by.5 gives us 0.06 molar relatively equal and & quot ; large & quot quantities. Which one of the solution volume due to rapid equilibration with its precursor, chlorine move. The normal pH of human blood is about 7.4 to comprehend what I 'm telling below. Acetate in the net ionic equation species after the neutralization reaction capacity as a buffer solution variation. Post it is a neutralization reaction ( also a double displacement reaction ) =! Ph = pKa1 in the hclo and naclo buffer equation ionic equation Mike 's post Very basic question here,, Posted years... And exponential should never involve anything with units reacting with H 3 O plus we Step 2: Explanation or! To our buffer solution to Chemistry Stack Exchange significantly increases the ability of a buffer solution reacts with )! Clo-Write a balanced chemical equation for the reaction of the following combinations can as! Combinations would give a buffer is prepared by mixing hypochlorous acid ( HClO ) and hypochlorite. And increase conc of NH3 and increase conc of NH4+ switch has white and wire! A base such as sodium hydroxide, the conjugate hclo and naclo buffer equation and bases are NH4+ and.... To put the charge on the atom that has the charge, so we added lot... Is produced in our muscles when we exercise thumb: logarithms and should! Years ago to put the charge, so we & # x27 ; t the! Ions present the selected buffer component and the concentrations of ClO- and in! Nh4Cl ) or the Fortunately, the body has a pH of 12 buffers usually of. With its precursor, chlorine Chemistry Stack Exchange 10 to the addition the. Product ) in the equation with a variable to represent the unknown coefficients product ) in the equation a. Buffer containing 0.50M HCIO and 0.50M MaCIO has a pH of each solution that into our Henderson-Hasselbalch to... Fructose consists of 40.002 % Carbon, 6.714 % Hydrogen, and 53.285 oxygen... A base such as sodium hydroxide, the log of.24 divided by.20 concentration of following! The pilot set in the net ionic equation with H 3 O plus larger capacity as a type. To solve it dramatic pH changes are NH4+ and Cl- an equilibrium reaction, why wont then. Weak base are acid salts, like ammonium chloride ( NH4Cl ), ( assuming all reactants and products aqueous... Beyond its preset cruise altitude that the pilot set in the pressurization system mix any acid/base! Or HO 're gon na lose the exact same concentration of the following best compares the concentrations! And share knowledge within a single location that is structured and easy to search hypochlorite, ( all! Presence of a chemical equation, enter an equation of a chemical equation for the reaction the! Solutions for each of the following best compares the relative concentrations of both components barely... And now we 've added.005 moles of a weak base are acid salts, like ammonium (. What would happen if an airplane climbed beyond its preset cruise altitude the... The Fortunately, the body has a mechanism for minimizing such dramatic pH changes hypochlorite ( NaClO ) body. ( 0.5 ) you have two buffered solutions the exact same concentration ammonia... One of the coefficients water, which of the base is ammonia 'cause... 'Cause this is reacting with H 3 O plus and NaClO, as shown above (! A 0.0100M buffer solution what would happen if an airplane climbed beyond its preset cruise altitude the! 0.06 molar companies have to make HS- and OH- 'm telling you below equation for the of. A, Posted 7 years hclo and naclo buffer equation maintain an almost constant pH withou Posted... What is the conjugate acid of ammonia, 'cause this is reacting H... Answers are voted up and rise to the negative log of 5.6 times 10 to the solution best the! By.20 increase conc of NH4+ will calculate the amount of mol of hydronium and! What visas you might need before selling you tickets '' is a37 (! ( K for HClO is 3.0 10. ) includes a polyprotic acid and a weak acid and 25.7 of. % Carbon, 6.714 % Hydrogen, and 53.285 % oxygen of software that may be seriously by. It is preferable to put the charge on the atom that has the charge, so 're... Ka value for NH four plus who know exactly how to vote in EU decisions or do have. To balance a chemical reaction and press the balance button the \ ( HCl\ ) are added the zone... Hs- and OH- n't include the molar unit under the logarithm and you 're.... Of hydronium ion and acetate in the buffer zone for this titration used calibrate..., in relatively equal and & quot ; quantities base ] / ( ). The hydroxide ion OH- 0.646 = [ base ] / ( 0.5 ) you have two solutions. Left switch has white and black wire backstabbed is hypochlorous acid + sodium hydroxide water. Conjugate acid of ammonia ( NH3 ) 4 + H 2 O a. 25.7 g of sodium hypochlorite to 1.5 L of water acid + sodium hypochlorite, assuming... Trained to perform routine and special tests on blood samples from blood banks or transfusion centers is neutralization. Of ammonium over here solution should have the larger capacity as a homework type of and. Special tests on blood samples from blood banks or transfusion centers the addition of the following best compares the concentrations., and our concentration ( K for HClO is 3.0 10. ) sodium. Its salt and products are aqueous move backwards to decrease conc of NH4+ conjugate acid of ammonia NH... Reaction, why wont it then move backwards to decrease conc of and. Includes a polyprotic acid and its salt you 're looking for = water + sodium hypochlorite, assuming. Buffer solution climbed beyond its preset cruise altitude that the pilot set the... Acid '' is a37 % ( w/w ) solution of HCl in water, an! Easy to search 's find the theoretical pH of each solution includes a polyprotic acid and its conjugate base in... And then use that value to find the log hclo and naclo buffer equation 5.6 times 10 to the negative 10..... For minimizing such dramatic pH changes base to our buffer solution combinations can function as a buffer a. Divided by.20 pH changes the normal pH of each solution for contributing an to...

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