why is nahco3 used in extractionjenny lee bakery locations

In this way, blue Drierite can be used as a visual indicator for the presence of water.\(^8\). E>!E?h!I'Xyg6WqfB%t]` B;h_~m3wRq`ja4AM$@0?x/,P:a=93X=v4{g5:YAp[Lkcb-kPl`b. Pink (wet) Drierite can be dried by spreading it on a watch glass and drying in a \(110^\text{o} \text{C}\) oven overnight. When it is known, through experience, that some mixtures may form emulsions, vigorous shaking should be avoided. First of, when mixed together, benzoic acid and sodium bicarbonate (NaHCO3) react and produce sodium benzoate, water and carbon dioxide (Separation 2). Excessive washing will also lower the yield of the product, if the desired compound dissolves noticeably in the other phase. Create an account to follow your favorite communities and start taking part in conversations. Why was 5% sodium bicarbonate used in extraction? I'm just spitballing but that was my initial guess when I saw this. Any ECG signs of hyperkalemia warrant treatment with calcium chloride, beta agonist (albuterol), insulin/glucose and sodium bicarbonate. does not react with compounds that are sensitive to strong bases or nucleophiles (esters, ketones, aldehydes) because it is a weaker base and a weak nucleophile due to its. stream Strictly speaking, hardly ever all of the solute will be extracted since there is finite distribution coefficient for the compound (see also Extraction II). This strategy saves steps, resources and time, and most of all, greatly reduces waste. The task of getting a clean phase separation will be more difficult if the liquids are spread out over a large, flat or curved surface. A laser is used to destroy one of the four cells (this technique is called laser ablation). Ammonium salts from primary amines are much more soluble in water than salts from tertiary amines due the increased ability to form hydrogen bonds [(H3NEt)Cl: 280 g/100 g H2O, (H2NEt2)Cl: 232 g/100 g H2O, (HNEt3)Cl: 137 g/100 g H2O (all at 25 oC)]. The reason sodium carbonate is added to the tea is because the tannins are acidic and sodium carbonate is a base, so when sodium carbonate is added to the tea water mixture, the acids are . For instance, if the target compound was the base in the system, the extraction with HCl should be performed first. The organic layer now contains basic alkaloids, while the aq. Which of the two reagents should be used depends on the other compounds present in the mixture. 2. The most common wash in separatory funnels is probably water. Never dispose of any layer away until you are absolutely sure (=100 %) that you will never need it again. Cite advantages and disadvantages of using the following drying agents: a) sodium sulfate b) magnesium sulfate c) sodium carbonate d) potassium carbonate. Product Use. The conjugate base is a salt and is water soluble; therefore, it is removed from the organic solvent layer . What functional groups are present in carbohydrates? The CO2 is visible as bubbles; as the pressure from the CO2 builds up, gas and some of the liquid is pushed up and out. x]7r_n}Fqb'@EXq.FzFZ~O`c'_B 3lXgVr]\54uvt|S/xhe=M[~ijpa]OW-^mWwWW4Ww(Nw>~k)5cU8o?n]a@+O | :v}-Oy]-|%o$BY_@8P Why was the caution in question #3a not as important when adding the hydroxide base to the ether solution? This is the weird part. Why is sodium bicarbonate used resuscitation? Before using the separatory funnel, the user should check if the stopcock plug and the stopcock fit together well. The reason of using $\ce {NaHCO3}$ is the reaction: $$\ce {HCO3- + OH- <=> CO3^2- + H2O}$$ First, near all hydroxide is converted to carbonate, and then an excess of bicarbonate shifts $\mathrm {pH}$ below 10. You will use sulfuric acid to catalyze the reaction. Be sure to close the jar of drying agent when not in use, as the reagents are hygroscopic. the gross of the water from the organic layer. Become a Study.com member to unlock this answer! To test whether a base wash with \(\ce{NaHCO_3}\) or \(\ce{Na_2CO_3}\) was effective at removing all the acid from an organic layer, it is helpful to test the pH. - Solid Inorganic: excess anhydrous sodium sulfate. Epinephrine and sodium bicarbonate . Testing the pH After a Wash To test whether a base wash with NaHCO 3 or Na 2CO 3 was effective at removing all the acid from an organic layer, it is helpful to test the pH. because a pressure build-up will be observed in the extraction container. Multiple extractions with smaller quantities are preferred over one extraction with the same quantity of solution/solvent. If solutions with higher concentrations are used, extra caution is advised because neutralization reactions are exothermic. Summary. Why is sulphuric acid used in redox titration? The amount of material left behind after two or three extractions is usually very small (less than 5 % in most cases) and does not justify the effort and resources (solvent and time to perform the extractions and to remove the solvent later on). The work-up refers to methods aimed at purifying the material, and most commonly occur in a separatory funnel. Why is NaHCO3 used in extraction? Write the balanced chemical equation with the state symbols of the following reaction: Solutions of Barium chloride and Sodium sulphate in water react to give insoluble Barium sulphate and the solution of Sodium chloride. What should I start learning after learning the basics of alkanes, alkenes, and alkynes? What happens chemically when quick lime is added to water? e) Remove the solvent with a rotary evaporator. This constant depends on the solvent used, the solute itself, and temperature. This method estimates the relative bioavailability of inorganic ortho-phosphate (PO4-P) in soils with neutral to alkaline pH. The higher water solubility lowers the solubility of weakly polar or non-polar compounds in these solvents i.e., wet Jacobsen ligand in ethyl acetate. The solution of these dissolved compounds is referred to as the extract. Why is cobalt-60 used for food irradiation? Draw the reaction between acetylsalicylic acid and NaHCO 3 then draw the reaction between that product and HCl. With a finger placed atop a glass pipette, insert the pipette into the separatory funnel so the tip is positioned in the bottom aqueous layer (Figure 4.42a). Using as little as possible will maximize the yield. Why is acid alcohol used as a decolorizing agent? known as brine). Pressure builds up that pushes some of the gas and the liquid out. Early C. elegans embryos display mosaic determination, whereas early mouse embryos exhibit regulative determination. If the total percent recovery is unusually low or unusually high, briefly explain the possible sources of error that might've occurred. The dye has obviously partitioned toward the aqueous layer, which is consistent with its very polar structure (Figure 4.46). The purpose of washing the organic layer with saturated sodium chloride is to remove. This is because NaHCO3 will deprotonate only the benzoic acid , allowing it to go into the aqueous layer while the phenol is left behind in the organic layer. A procedural advantage to these drying agents is that their granules are not easily dispersed, allowing for the solutions to be easily decanted (poured). NaHCO3 (Sodium Bicarbonate) is mainly prepared by the Solvay Process, which is the reaction of sodium chloride, ammonia, and carbon dioxide in water. In addition, the salt could be used to neutralize your organic layer. Bicarbonate ion has the formula HCO 3 H C O. Background Extraction is a frequently used technique to selectively transfer a compound of interested from one solvent to another. Createyouraccount. This will allow to minimize the number of transfer steps required. removing impurities from compound of interest. Washing is also used as a step in the recrystallization procedure to remove the impurity containing mother liquor adhering to the crystal surface. More concentrated solutions are rarely used for extraction because of the increased evolution of heat during the extraction, and potential side reactions with the solvent. For example, acetic acid has a \(K\) of 0.5 when partitioning between diethyl ether and water, meaning acetic acid favors the aqueous layer only twice as much as the organic layer.\(^4\) The ability of acetic acid and other polar compounds to dissolve in the organic layer of a separatory funnel should not be ignored. the possible sources of error may have occurred when: one was emptying the solution in the clean beaker while filtering the acetanilide solution, some of the solution may have been wasted because it remained in the filtered flask. What is the average pressure on the soles of the feet of a standing 90.0 kg person due to the contact force with the floor? We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Synthesis or preparation of esters in the laboratory involves 3 steps: Step 1: Synthesis of the ester. WE|>t{_[g(qlLo? h~dBSF~x"xoHjN$z_&Sq?$5QyN~.uAoFCh,.1?a1ccEQKWk ~c1/?kqu-vG- pnO_XfhxgC@Nd&rKf\]Ep ^l [4##KCX Why is eriochrome black T used in complexometric titration? Many organic solvents dissolve a significant portion of water (Table 4.6) that must be removed before rotary evaporation, or else water will be found in the concentrated product. Additionally, ionic solutions have high dielectric constants, making them less compatible with organic compounds. What do I use when to extract? The purpose of this wash is to remove large amounts of water than may be dissolved in the organic layer. g. The separatory funnel leaks Before using the separatory funnel, the user should check if the stopcock plug and the stopcock fit together well. \(^7\)From: Fessenden, Fessenden, Feist, Organic Laboratory Techniques, 3\(^\text{th}\) ed., Brooks-Cole, 2001. These solvents dissolve large quantities of water in comparison to other solvents (Table 4.5). \" When the lighting light ratio, the absorbance is only related to the concentration.Why is the sodium extraction solution absorbing 10ml . NaHco3 allows us to just ionize the acid; any base would deprotonate the stronger acid, it's more about not also deprotonating the phenol. In cases, where the phases have similar polarity or density, the addition of more solvent can assist the separation. For most washing processes, 10-20 % of the volume of the solution to be washed will do an adequate job. However, if compounds were present that are sensitive towards strong bases or nucleophiles (i.e., esters, ketones, aldehydes, etc. If using a fine powder, the solution must be gravity filtered and drying agent rinsed. Let's consider two frequently encountered Drying agents (Figure 4.48) remove trace amounts of water from organic solutions by forming hydrates. In many cases, centrifugation or gravity filtration works as well. Removal of a carboxylic acid or mineral acid. % Because of this, sodium bicarbonate is often used to treat conditions caused by high acidity in the body, such as heartburn. If the litmus paper turns pink at all\(^5\), the base wash has not fully neutralized the organic layer, and subsequent base washes are needed. Commonly used solvents like ethyl acetate (8.1 %), diethyl ether (6.9 %), dichloromethane (1.3 %) and chloroform (0.8 %) dissolved up to 10 % in water. However, the solubility of the ammonium salts decreases as the number and size of R-groups increases. Hence, the solution becomes basic due to the presence of additional OH- ions produced by hydrolysis. This undesirable reaction is called. Absorbs water as well as methanol and ethanol. Many. samples of the OG mixture to use later. b. What is the goals / purpose of the gravimetric analysis of chloride salt lab? Extraction Techniques LAB extraction techniques in mixture of water and diethyl ether, which layer will contain an organic compound that has higher solubility Skip to document Ask an Expert \(\ce{CaCl_2}\) value is quoted for the formation of \(\ce{CaCl_2} \cdot 2 \ce{H_2O}\). Why is it that sodium iodide can be used as a catalyst for some SN2 reactions? All rights reserved. What is N-(2,2,2-Trichloroethyl)carbonyl] Bisnor-(cis)-tilidine's functional group? around the world. What is the purpose of salt in DNA extraction? It can be difficult to completely remove a water layer by pipette, so leaving a tiny bit is acceptable. this solvent will form two layers in contact with aqueous solutions if it is used in sufficient quantities; this is because the solvent is immiscible in water. The center is the most concentrated spot, and it's possible a color change may not be seen on the outside where the solution has spread and diluted. For an organic compound, it is relatively safe to assume that it will dissolve better in the organic layer than in most aqueous solutions unless it has been converted to an ionic specie, which makes it more water-soluble. In addition, it is preferable to manipulate neutral materials rather than acidic or basic ones, as spills are then less hazardous. A typical drying procedure is to add anhydrous \(\ce{MgSO_4}\) to an organic solution until it stops clumping and fine particles are seen, which indicate that there is no longer water available to form the clumpy hydrates. The presence of water with the product makes the yield inaccurate, and water also must be removed before GC-MS analysis, as water is incompatible with mass-spectrometer detectors. In order to effect the extraction, the two solvents must be immiscible, which means that neither dissolves in the other. In some procedures \(\ce{Na_2SO_4}\) or \(\ce{CaCl_2}\) are used if they seem to work just as well as \(\ce{MgSO_4}\), or if the solution is incompatible with \(\ce{MgSO_4}\) (see Table 4.8). Why use methyl orange instead of phenolphthalein as a pH indicator. A familiar example of the first case is making a cup of tea or . By easy I mean there are no caustic solutions and . Process of removing a compound of interest from a solution or solid mixture. Why was it important to be careful when adding the bicarbonate base to the ether solution when extracting the toluic acid? Water has a particular density and naphthalene, as well as benzoic acid, are insoluble in water. Water may be produced here; this will not lead to a build up of pressure. The container should be vented immediately before the pressure build-up can cause an explosion, an ejection of the stopper on the top or excessive spillage upon opening. Acid-Base Extraction. A drying agent is swirled with an organic solution to remove trace amounts of water. Sodium Bicarbonate Sodium bicarbonate is an ionic compound of sodium ion and bicarbonate ion. 75% (4 ratings) for this solution. Why are sulfide minerals economically important? Get access to this video and our entire Q&A library. For example, it is safely used in the food and medical industry for various applications. Anhydrous magnesium sulfate \(\left( \ce{MgSO_4} \right)\) is a fine, loose powder (Figure 4.49a), but its hydrate is clumpy and often clings to the glass (Figure 4.49b). This phenomenon will often be observed if sodium bicarbonate is used for the extraction in order to neutralize or remove acidic compounds. This highly depends on the quantity of a compound that has to be removed. anhydrous sodium sulfate, magnesium sulfate, or calcium chloride), these reagents at best remove only small amounts of water. so to. Why is sodium bicarbonate added to water? If a desired product can hydrogen bond with water and is relatively small, it may be difficult to keep it in the organic layer when partitioning with an aqueous phase (\(K\) will be <1). Why was NaHCO3 used in the beginning of the extraction, but not at the end? How can I draw the following amines: butan-1-amine, pentan-2-amine, propan-1,2-diamine? 4. : r/OrganicChemistry r/OrganicChemistry 10 mo. Additionally, solutes dissolved in an organic layer with polar functional groups (e.g. But Baking soda (NaHCO 3 ) can act as acid as well as a base, Because of its bicarbonate anion (HCO 3-) amphoteric activity. On a large scale, it is prepared by passing carbon dioxide gas through calcium hydroxide (slaked lime). Its high surface area means it will somewhat adsorb compound: be sure to rinse after filtering. #R'OH + HO(O=)CRstackrel(H_3O^+)rightleftharpoonsR'O(O=)CR+H_2O#. Figure 3. Why does sodium carbonate not decompose when heated? This is because the concentrated salt solution wants to become more dilute and because salts. 5Q. The conical shape of these pieces of equipment makes it easier to collect the solution on the bottom using a Pasteur pipette because of the smaller interface. Extraction. . Are most often used in desiccators and drying tubes, not with solutions. Use Baking soda (NaHCO3 ) Method 2 is the easiest. Give the purpose of washing the organic layer with saturated sodium chloride. The ether layer is then to the solubility.Extraction becomes a very useful tool if you choose a suitable extraction solvent. If the entire drying agent clumps into pieces that are much larger than the original size (Figure 4.52b+c), there is still water remaining in the flask. Why is the bicarbonate in blood an effective buffer when its pKa is 6.1, while the pH of the blood is 7.4? Why wash organic layer with sodium bicarbonate? Why is bicarbonate of soda used to bake a cake? Becoming familiar with its theory and correct use are essential to successful completion of many organic experiments. It helps to regulate and neutralise high acidity levels in the blood. This often leads to the formation of emulsions. 1. Add a small portion of drying agent to the flask,the size of one pea for macroscale work (Figure 4.51b), and swirl the solution (Figure 4.51c). In the aqeuous phase, I do not understand where the HCl comes from, shouldn't it be H2CO3 instead? Why is the removal of air bubbles necessary before starting titration? Step 2) DCM extraction NOTE: Chromic s method separates the water first to increase the yield. The density is determined by the major component of a layer which is usually the solvent. 20mL of 10% aqueous sodium bicarbonate following the same procedure as detailed above. The method is based on the extraction of phosphate from the soil by 0.5 N sodium bicarbonate solution adjusted to pH 8.5. It does not react with these compounds because it is a weaker base and a weak nucleophile (due to its resonance stabilization). Why is EDTA used in complexometric titration? If using \(\ce{MgSO_4}\), gravity filter the solution into an appropriately sized round-bottomed flask (Figure 4.53c). You will loose some yield, but not much. 5% sodium bicarbonate is used in extraction to remove the remaining acid present. sodium bicarbonate is used. \(\ce{CaSO_4} \cdot \frac{1}{2} \ce{H_2O}\). Describe how you will be able to use melting point to determine if the . Why is sodium bicarbonate used in extraction? Solutions are added to the funnel to either extract or wash the mixture, with the goal of isolating the product from excess reagents, catalysts, side products, solvents, or compounds formed from side reactions. Keep in mind that it is always easier to recover the product from a different layer in a beaker than from the waste container or the sink. Add another portion of drying agent and swirl. In the case of Caffeine extraction from tea Why potassium is more reactive than sodium. copyright 2003-2023 Homework.Study.com. Why is bicarbonate important for ocean acidification? The organic solution to be dried must be in an. Many liquid-liquid extractions are based on acid-base chemistry. Why is aqueous NaHCO3 used for separation of 'x' gm of a compound A3B2C5 contains 'y' gm of A atoms Using above information Match the following, WHAT IS THE VALUE OF THE elementary STATE OF AN ELEMENT. One has to keep this in mind as well when other compounds are removed. Aqueous solutions of saturated sodium bicarbonate \(\left( \ce{NaHCO_3} \right)\) and sodium carbonate \(\left( \ce{Na_2CO_3} \right)\) are basic, and the purpose of these washes is to neutralize an organic layer that may contain trace acidic components. G3LS0 no=P80Gv-\JGExFJy-T[61Z>2P IqQ.Xk+_a{vLw))efJ_%*S7VCrb_ +nAuV%YuVE&EIMX> JFj)z{iQ8s&"5,k@eU|+~@(C_dJFvhEG\2p:s/]AprC Discover how to use our sodium bicarbonate in a pancake recipe. What do you call this undesirable reaction? Note that many of these steps are interchangeable in simple separation problems. Figure 4.47d shows the brine layer containing the dye after shaking with a portion of ethyl acetate. The salt water works to pull the water from the organic layer to the water layer. Instead, gently rocking the separatory funnel back and forth for 2-3 minutes will accomplish sufficient degree of mixing while minimizing the formation of emulsions. Problem. The most common drying agents used to remove water from organic solutions are anhydrous sodium sulfate \(\left( \ce{Na_2SO_4} \right)\) and anhydrous magnesium sulfate \(\left( \ce{MgSO_4} \right)\). 11.30.2010. f. The centrifuge tube leaks In this example, even after filter and rinsing the drying agent with additional solvent, the drying agent remained pink (Figure 4.45c). Why use sodium bicarbonate in cardiac arrest? varieties are used, the small-leaved China plant (C. sinensis sinensis) and the large-leaved Assam plant (C. sinensis assamica). Any pink seen on blue litmus paper means the solution is acidic. What is the purpose of a . How much solvent/solution is used for the extraction? %PDF-1.3 Which sequence is the most efficient highly depends on the target molecule. Water can potentially remove water-soluble impurities from an organic layer, as long as they are present in quantities that do not exceed their water solubility. layer contains quarternary ammonium ions. Acid-Base Extraction. Why does sodium chloride have brittle crystals? Quickly removes water, but needs large quantities as it holds little water per gram. They should be vented directly after inversion, and more frequently than usual. A similar observation will be made if a low boiling solvent is used for extraction. Subsequently, an emulsion is formed instead of two distinct layers. EXPERIMENT 1_ Preparation of Artificial Flavors and Fragrances.pdf, toaz.info-chem-33-postlabs-expt-10-13-pr_105e1de6982cfe165053482d3243ef17.pdf, of consequences then the crime is to most likely be committed but if the, ACTIVITY REPORT for covid Sensitization.docx, 444 Differentiate Variant BOM from Multiple BOM 173 445 Is it Possible to, Betelhem Esyas st marry university Marketing Managment.pdf, it hence the term enzyme conjugated that reacts with the substrate added in the, Which line on graph A best describes the relationship between vessel radius on, The Platinum Rule can be summarized as a Do unto others as you would have them, The dose response relationship which reflects the fact that toxicity is a, Companies engaged in a single line of business utilize an organizational, of the clients death The duty of candor also required disclosure to opposing, Exercise 022 Find the values of t for which t 0 1 0 0 T is a solution of the, Problem 47 Let W denote max window size Let S denote the buffer size For, DA991D3D-92E0-4826-A8B6-5C837418CDD3.jpeg. With a finger placed atop the glass pipette again, remove the pipette from the separatory funnel. Why does sodium bicarbonate raise blood pH? Beets in poor conditions start to 'juice', creating a large amount of high organic content liquid. Using sodium bicarbonate ensures that only one acidic compound forms a salt. The only time that you can really be sure about it is if you isolated the final product in a reasonable yield, and it has been identified as the correct compound by melting point, infrared spectrum, etc. This means that solutions of carbonate ion also often bubble during neutralizations. Extraction involves dissolving a compound or compounds either (1) from a solid into a solvent or (2) from a solution into another solvent. Why should KMnO4 be added slowly in a titration? However, they do react with a strong base like NaOH. A vigorous stream of bubbles is seen originating from a small portion of organic layer trapped on the bottom of the funnel. Liquid-liquid extraction also known as solvent extraction is a common method in separating liquids inn virtue of their relative solubility in different solvents (polar and non-polar solvents).. Register Yourself for a FREE Demo Class by Top IITians & Medical Experts Today ! Thus, the density of a solid i.e., sodium hydroxide (2.1 g/cm3 in the solid) does not provide the information sought. 1. transfer ether solution to clean labeled 125 mL Erlenmeyer flask; add anhydrous sodium sulfate until it stops clumping. Why is back titration used to determine calcium carbonate? At 2 h after CPR, the brain, heart, and lung were collected and mRNA extraction, followed by cDNA synthesis and real-time PCR were performed. This technique selectively dissolves one or more compounds into an appropriate solvent. What is the purpose of using washing buffer during RNA extraction? 8.4.1.7 Sodium bicarbonate Sodium bicarbonate (NaHCO3) does not have any direct antibacterial effect but it has a cleansing action by loosening debris and dissolving mucus. The . Because this process requires the second solvent to separate from water when . g. The separatory funnel leaks Removal of a phenol. alcohols, carboxylic acids) can hydrogen-bond with water and increase the likelihood of water dissolving in the organic layer. Extraction is one of the more common procedures in organic chemistry, and it's often performed to remove an organic solvent from water. For instance, epoxides hydrolyze to form diols catalyzed by acids and bases. The bottom layer is always removed first independently if this is the one of interest or not because it is much easier to do. Why is an indicator not used in redox titration? Cannot dry diethyl ether well unless a brine wash was used. The \(\ce{^1H}\) NMR spectrum of the final product (Figure 4.39b) showed the washes were effective as the acetic acid signal at \(2.097 \: \text{ppm}\) is absent. Figure 4.47b shows the water layer containing the dye after shaking with a portion of ethyl acetate. Ca (OH)2 + CO2 CaCO3 + H2O Therefore a uncharged acidic compound dissolved in diethyl ether can be converted to a salt and . Why does sodium iodide solution conduct electricity? After solvent removal using a rotary evaporator, it occasionally happens that so much water is present that droplets or a second layer is seen amongst the oily liquid in a round-bottomed flask. Explain why sodium chloride, which is a nasal spray ingredient, can decongest a stuffed nose. Why would you use an insoluble salt to soften water? Use of two different bases with two different strengths allows for selective reaction of the stronger acid versus the weaker acid. In chemistry, the main safety issues are when using sodium bicarbonate to neutralize acids. Why is bicarbonate buffer system important? ago Posted by WackyGlory A normal part of many work-ups includes neutralization. Use ACS format. Experiment 8 - Extraction pg. After a short period of time, inspect the mixture closely. Sodium hydroxide is usually easier to handle because it does not evolve carbon dioxide as a byproduct. The formation of CO 2 results in belching and gastric distention. 5. such as sodium hydroxide or sodium bicarbonate to produce the conjugate base of the acid. Quickly removes water well, although larger quantities are needed than other drying agents (holds \(0.30 \: \text{g}\) water per \(\text{g}\) desiccant). The leaves may be fermented or left unfermented. Sodium bicarbonate is a salt that breaks down to form sodium and bicarbonate in water. ~85F?$_2hc?jv>9 XO}.. Since no phenolic compound is present in this mixture, two extractions with base solution are not required; thus, the benzoic acid could be separated from the neutral compound by extraction with either aqueous sodium bicarbonate or aqueous sodium hydroxide solution. From this point of view, a solvent with higher density than water would be preferential, especially when very small quantities are used. Most reactions of organic compounds require extraction at some stage of product purification. Touch the aliquot to blue litmus paper and observe the color (Figure 4.42d).

Erin Mckenna Bakery Nutrition, Articles W