lewis base vs bronsted base

Lewis Acid Definition: The H+ on Hydronium accepts the attacking electron pair to form a bond. The conjugate acid of a Brnsted-Lowry base is the species formed after a base accepts a proton. And so, when we're accepting a pair of electrons. Because of its ability to both accept and donate protons, water is known as an. synonymous with electrophiles. Strong acids and bases ionize completely in aqueous solution, while weak acids and bases ionize only partially in aqueous solution. Whether you need help solving quadratic equations, inspiration for the upcoming science fair or the latest update on a major storm, Sciencing is here to help. Now that we have an understanding of Brnsted-Lowry acids and bases, we can discuss the final concept covered in this article: conjugate acid-base pairs. Lewis from UC Berkeley proposed an alternate . And then we also had some Direct link to Amit Mukherjee's post I have a very basic quest, Posted 7 years ago. Let's go ahead and She has an interest in astrobiology and manned spaceflight. with that proton. In 1923 G. N. Lewis suggested another way of looking at the reaction between H + and OH-ions. And so, let's go ahead At what point would you balance the equation you write to show the reaction of acids or bases in water? Some of the ammonia molecules accept a proton from water to form ammonium ions and hydroxide ions. 1 Answer Owen Bell Mar 30, 2016 Nitrogen trifluoride, or NF3, is a base. And that makes it very reactive. Want to save this article for later? Acid strength, anion size, and bond energy. A Brnsted-Lowry acid is any species that donates a proton to another molecule. A Brnsted-Lowry acid is any species that donates a proton to another molecule. The Bronsted-Lowry theory talks about removal or transfer of hydrogen ions (H+) ie. If you having trouble remembering the difference between the theories of acids, try coming up with your own mnemonic device. If water is electronically neutral before this extraction then the addition of another positive proton will give the resulting product an overall positive charge. So if HCl is our H$^{+}$ has no electrons by itself. Arrhenius acids and bases (article) | Khan Academy Is there a video on here where this is explained? acted as a proton acceptor. Weak acid-base equilibria. The two species in a conjugate acid-base pair have the same molecular formula except the acid has an extra. { Arrhenius_Concept_of_Acids_and_Bases : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Bronsted_Concept_of_Acids_and_Bases : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Dissociation_Fraction : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Exact_pH_Calculations : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Graphical_Treatment_of_Acid-Base_Systems" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Indicators : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Lewis_Concept_of_Acids_and_Bases : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Overview_of_Acids_and_Bases : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { Acid : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Acids_and_Bases_in_Aqueous_Solutions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Acid_and_Base_Indicators : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Acid_Base_Reactions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Acid_Base_Titrations : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Buffers : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Buffers_II : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Ionization_Constants : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Monoprotic_Versus_Polyprotic_Acids_And_Bases : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "Lewis Acid", "Lewis base", "showtoc:no", "license:ccbyncsa", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FPhysical_and_Theoretical_Chemistry_Textbook_Maps%2FSupplemental_Modules_(Physical_and_Theoretical_Chemistry)%2FAcids_and_Bases%2FAcid%2FLewis_Concept_of_Acids_and_Bases, $ \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}$ $ \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} $$\newcommand{\id}{\mathrm{id}}$ $ \newcommand{\Span}{\mathrm{span}}$ $ \newcommand{\kernel}{\mathrm{null}\,}$ $ \newcommand{\range}{\mathrm{range}\,}$ $ \newcommand{\RealPart}{\mathrm{Re}}$ $ \newcommand{\ImaginaryPart}{\mathrm{Im}}$ $ \newcommand{\Argument}{\mathrm{Arg}}$ $ \newcommand{\norm}[1]{\| #1 \|}$ $ \newcommand{\inner}[2]{\langle #1, #2 \rangle}$ $ \newcommand{\Span}{\mathrm{span}}$ $\newcommand{\id}{\mathrm{id}}$ $ \newcommand{\Span}{\mathrm{span}}$ $ \newcommand{\kernel}{\mathrm{null}\,}$ $ \newcommand{\range}{\mathrm{range}\,}$ $ \newcommand{\RealPart}{\mathrm{Re}}$ $ \newcommand{\ImaginaryPart}{\mathrm{Im}}$ $ \newcommand{\Argument}{\mathrm{Arg}}$ $ \newcommand{\norm}[1]{\| #1 \|}$ $ \newcommand{\inner}[2]{\langle #1, #2 \rangle}$ $ \newcommand{\Span}{\mathrm{span}}$$\newcommand{\AA}{\unicode[.8,0]{x212B}}$, Various species can act as Lewis acids. Question: iPr k) Allylic cation vs Allylic anion. to make that electron green. little bit more broad. Direct link to saadia peerzada's post Chemical species are atom, Posted 7 years ago. So these electrons in red on The Bronsted-Lowry definition of an acid is: Anything that donates H+ to anything else Lewis Acids: Most University Students use This Lewis Acids are electron pair acceptors Lewis Bases are electron pair donors. Note, when this happens, the number of positive charged hydronium ions equals the number of negatively charged hydroxide ions, and so even though there are charged particles, the water is still neutral. Direct link to Matthew Main's post At 5:36, how is Boron sp2, Posted 9 years ago. and mark those electrons. Because sulfurous acid is a weak acid you have an equilibrium with all three species existing, H2SO3, HSO3- and SO3-2. Neutral water does not consist of pure H2O, as sometimes when two water molecules collide a proton is transferred from one molecule to another. \[H_2O + NH_3 \rightarrow NH_4^+ + OH^- \label{3}\], \[H_2O + HCl \rightarrow Cl^- + H_3O^+ \label{4}\]. In the following acid-base reactions, 1. draw Lewis structures of the reactants and the products. Direct link to awemond's post Neither definition is "mo, Posted 9 years ago. \[ \underset{both\: Arrhenius\: and \\ \: Bronsted\: base}{NH_3 (g)} + {H_2 O(l)} \rightleftharpoons {NH_4^+ (aq)} + {OH^- (aq)} \], \[\underset{only\: a\: Bronsted\: base} {NH_3 (g)} + {HCl(aq)} \rightleftharpoons {NH_4^+ (aq)} + {Cl^- (aq)} \]. Top Jamie Park 2F Posts: 59 Joined: Wed Nov 25, 2020 8:19 am talking about a proton, we're talking about the Are nucleophiles Lewis bases? Why? | Socratic Since ammonia is a weak base, the ammonium ion can donate a proton back to hydroxide to reform ammonia and water. Since hydrogen phosphate is acting as a Brnsted-Lowry base, water must be acting as a Brnsted-Lowry acid. Direct link to Christopher Knudtson's post Sulfur is a larger atom t, Posted 10 years ago. Since hydrogen phosphate is acting as a weak base in this particular example, we will need to use equilibrium arrows. (CH 3 CH 2) 2 And then we have HCl Their Equilibrium constant is so high, and the equilibrium is shifted so far right that all of a strong acid dissociates and does't want to be put back together. Our other product, 3.2: Brnsted and Lewis Acids and Bases - Chemistry LibreTexts and the boron. Direct link to sanzoo123456's post Does ammonia act both as , Posted 7 years ago. A fish market where a variety of fresh and packaged fish are displayed on ice. proton to water. It's able to accept The definition of Lewis acids includes the proton since the proton can accept electron pairs. Lewis' theory used electrons instead of proton transfer and specifically stated that an acid is a species that accepts an electron pair while a base donates an electron pair. However, water can also act as a base by accepting a proton from an acid to become its conjugate base, H3O+. And we have this cyclic to donate a pair of electrons. And then just flipping it Riti Gupta holds a Honors Bachelors degree in Biochemistry from the University of Oregon and a PhD in biology from Johns Hopkins University. One is able to expand the definition of an acid and a base via the Lewis Acid and Base Theory. Bronsted and Lewis are just different ways of naming acids and bases, there is actually no difference between them! Using the Brnsted-Lowry definition, an acid-base reaction is any reaction in which a proton is transferred from an acid to a base. Consider the reactions of ammonia with water and HCl. definitions for Bronsted-Lowry and, also, Lewis. here on that oxygen. And nucleophile, PDF INTRODUCTION TO LEWIS ACID-BASE CHEMISTRY - University of Texas at Dallas Acids and bases are an important part of chemistry. Direct link to Ernest Zinck's post You must balance an equat, Posted 7 years ago. (a) Draw the products for the given Bronsted/Lowry acid-base reactions. Finally, the Lewis definition is the broadest, stating that any electron pair acceptor is a Lewis acid, and an electron pair donor is a Lewis base. It dissociates completely in water to form hydronium. Video$\PageIndex{2}$ (https://youtu.be/iqINYjHyimY): 10 Youtube uploaded by akumich showing the formation of hydronium ions and hydroxide ions as protons are transferred between water molecules. Because B (boron) has 3 valence electrons (you can easily look that up in the periodic table), and the formal charge is calculated as follows: amount of valence electrons of the atom - actual amount of electrons surrounding it (see also the previous video, Oxidation States II, between. with Bronsted-Lowry. Thus Bronsted acids are a subset of Lewis acids since all Bronsted acids yield a proton. acid-base reaction here. The above animation and the longer video it links to does a good job of showing the transient nature of the actual hydronium or hydroxide ions in neutral water. Common weak bases include neutral nitrogen-containing compounds such as ammonia, trimethylamine, and pyridine. Lewis Bases donate an electron pair. and draw those in. Direct link to Mujtaba Hussain's post How is a reaction such as, Posted 6 years ago. Each of the following anions can "give up" their electrons to an acid, e.g., $OH^-$, $CN^-$, $CH_3COO^-$, $:NH_3$, $H_2O:$, $CO:$. magenta formed this bond between the oxygen So let's look at Why does the arrow go from the electron in water to the hydrogen in HCl instead of the other way around? The one in green that Note that according to the Arrhenius theory, the above reaction would. You may have noticed that the degree to which a molecule acts depends on the medium in which the molecule has been placed in. conjugate acid-base pairs, you're looking for Direct link to Gavin Peng's post I was wondering as well, , Posted 7 years ago. You may have noticed this with water, which can act as both an acid or a base. A Brnsted-Lowry base is any species that accepts a proton from another molecule. A Lewis acid after having accepted an electron pair, involved in Bronsted-acidic activity, just wants to give up a proton and is thermodynamic behavior. An acid that can donate more than one proton is a polyprotic acid, and a base that can accept more than one proton is a polyprotic base. A Lewis base is an electron pair donor. 2023 Leaf Group Ltd. / Leaf Group Media, All Rights Reserved. The differences between the definitions. be accepting a proton. Direct link to Ryan W's post Kinda depends on the theo, Posted 2 years ago. So let's go ahead and identify represent the empty p orbital like this. The acidity or basicity depends on the strength of the equilibrium constants and will be covered later in this chapter. In contrast, Arrhenius says that an acid is a substance that increases the concentration of hydronium ions (H +) when added to the water. with the proton here. And if we look at what we What is the difference between a reaction of Lewis acids with Lewis The lack of $H^+$ or $OH^-$ ions in many complex ions can make it harder to identify which species is an acid and which is a base. However, if an oxygen that already has two covalent bonds shares one of its lone pairs of electrons in a third covalent bond (for example, with an H+), it will still have an octet. Note how Brnsted Theory of Acids and Bases will not be able to explain how this reaction occurs because there are no $H^+$ or $OH^-$ ions involved. Direct link to Matt B's post Each covalent bond needs , start text, H, end text, start superscript, plus, end superscript, start text, O, H, end text, start superscript, minus, end superscript, start text, N, H, end text, start subscript, 3, end subscript, left parenthesis, g, right parenthesis, start text, H, end text, start text, C, l, end text, left parenthesis, g, right parenthesis, start text, N, H, end text, start subscript, 4, end subscript, start text, C, l, end text, left parenthesis, s, right parenthesis, start text, N, H, end text, start subscript, 3, end subscript, left parenthesis, g, right parenthesis, plus, start color #11accd, start text, H, end text, end color #11accd, start text, C, l, end text, left parenthesis, g, right parenthesis, right arrow, start text, N, end text, start color #11accd, start text, H, end text, end color #11accd, start subscript, 4, end subscript, start text, C, l, end text, left parenthesis, s, right parenthesis, start color #11accd, start text, H, end text, end color #11accd, start text, C, l, end text, start text, N, H, end text, start subscript, 3, end subscript, start text, N, H, end text, start subscript, 4, end subscript, start text, C, l, end text, start text, H, N, O, end text, start subscript, 3, end subscript, start color #11accd, start text, H, end text, end color #11accd, start text, N, O, end text, start subscript, 3, end subscript, left parenthesis, a, q, right parenthesis, plus, start text, H, end text, start subscript, 2, end subscript, start text, O, end text, left parenthesis, l, right parenthesis, right arrow, start color #11accd, start text, H, end text, end color #11accd, start subscript, 3, end subscript, start text, O, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start text, N, O, end text, start subscript, 3, end subscript, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, start color #11accd, start text, H, end text, end color #11accd, start subscript, 3, end subscript, start text, O, end text, start superscript, plus, end superscript, start text, N, H, end text, start subscript, 3, end subscript, left parenthesis, a, q, right parenthesis, plus, start color #11accd, start text, H, end text, end color #11accd, start subscript, 2, end subscript, start text, O, end text, left parenthesis, l, right parenthesis, \rightleftharpoons, start text, N, end text, start color #11accd, start text, H, end text, end color #11accd, start subscript, 4, end subscript, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start text, O, H, end text, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, start text, N, H, end text, start subscript, 4, end subscript, start superscript, plus, end superscript, start text, H, end text, start subscript, 3, end subscript, start text, O, end text, start superscript, plus, end superscript, start text, N, O, end text, start subscript, 3, end subscript, start superscript, minus, end superscript, start text, C, H, end text, start subscript, 3, end subscript, start text, C, O, O, H, end text, start text, C, H, end text, start subscript, 3, end subscript, start text, C, O, O, end text, start superscript, minus, end superscript, start text, C, H, end text, start subscript, 3, end subscript, start text, C, O, O, H, end text, left parenthesis, a, q, right parenthesis, plus, start text, H, end text, start subscript, 2, end subscript, start text, O, end text, left parenthesis, l, right parenthesis, \rightleftharpoons, start text, H, end text, start subscript, 3, end subscript, start text, O, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start text, C, H, end text, start subscript, 3, end subscript, start text, C, O, O, end text, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, start text, H, end text, start subscript, 2, end subscript, start text, S, O, end text, start subscript, 4, end subscript, start text, H, C, l, O, end text, start subscript, 4, end subscript, start text, N, a, O, H, end text, left parenthesis, a, q, right parenthesis, right arrow, start text, N, a, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start text, O, H, end text, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, start text, N, a, end text, start superscript, plus, end superscript, start text, N, H, end text, start subscript, 3, end subscript, left parenthesis, a, q, right parenthesis, plus, start text, H, end text, start subscript, 2, end subscript, start text, O, end text, left parenthesis, l, right parenthesis, \rightleftharpoons, start text, N, H, end text, start subscript, 4, end subscript, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start text, O, H, end text, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, start text, H, P, O, end text, start subscript, 4, end subscript, start superscript, 2, minus, end superscript, start text, H, end text, start subscript, 2, end subscript, start text, P, O, end text, start subscript, 4, end subscript, start superscript, minus, end superscript, start text, H, P, O, end text, start subscript, 4, end subscript, start superscript, 2, minus, end superscript, left parenthesis, a, q, right parenthesis, plus, start text, H, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, right arrow, start text, H, end text, start subscript, 2, end subscript, start text, P, O, end text, start subscript, 4, end subscript, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, start text, H, P, O, end text, start subscript, 4, end subscript, start superscript, 2, minus, end superscript, left parenthesis, a, q, right parenthesis, plus, start text, H, end text, start subscript, 2, end subscript, start text, O, end text, left parenthesis, l, right parenthesis, \rightleftharpoons, start text, H, end text, start subscript, 2, end subscript, start text, P, O, end text, start subscript, 4, end subscript, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, plus, start text, O, H, end text, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, start text, H, C, l, end text, left parenthesis, a, q, right parenthesis, plus, start text, H, end text, start subscript, 2, end subscript, start text, O, end text, left parenthesis, l, right parenthesis, right arrow, start text, H, end text, start subscript, 3, end subscript, start text, O, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start text, C, l, end text, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, space, space, space, space, space, space, space, space, space, space, start color #1fab54, start text, a, c, i, d, end text, end color #1fab54, space, space, space, space, space, space, space, space, space, space, space, space, start color #aa87ff, start text, b, a, s, e, end text, end color #aa87ff, space, space, space, space, space, space, space, space, space, space, space, space, space, space, start color #aa87ff, start text, a, c, i, d, end text, end color #aa87ff, space, space, space, space, space, space, space, space, space, space, space, start color #1fab54, start text, b, a, s, e, end text, end color #1fab54, start text, C, l, end text, start superscript, minus, end superscript, start color #1fab54, start text, C, o, n, j, u, g, a, t, e, space, p, a, i, r, space, 1, end text, end color #1fab54, equals, start text, H, C, l, end text, start text, space, a, n, d, space, end text, start text, C, l, end text, start superscript, minus, end superscript, start text, H, end text, start subscript, 2, end subscript, start text, O, end text, start color #aa87ff, start text, C, o, n, j, u, g, a, t, e, space, p, a, i, r, space, 2, end text, end color #aa87ff, equals, start text, H, end text, start subscript, 2, end subscript, start text, O, end text, start text, space, a, n, d, space, end text, start text, H, end text, start subscript, 3, end subscript, start text, O, end text, start superscript, plus, end superscript, space, space, space, space, space, space, space, space, space, space, start color #1fab54, start text, b, a, s, e, end text, end color #1fab54, space, space, space, space, space, space, space, space, space, space, space, space, start color #aa87ff, start text, a, c, i, d, end text, end color #aa87ff, space, space, space, space, space, space, space, space, space, space, space, space, start color #1fab54, start text, a, c, i, d, end text, end color #1fab54, space, space, space, space, space, space, space, space, space, space, space, space, space, start color #aa87ff, start text, b, a, s, e, end text, end color #aa87ff, start color #1fab54, start text, C, o, n, j, u, g, a, t, e, space, p, a, i, r, space, 1, end text, end color #1fab54, equals, start text, N, H, end text, start subscript, 3, end subscript, start text, space, a, n, d, space, end text, start text, N, H, end text, start subscript, 4, end subscript, start superscript, plus, end superscript, start color #aa87ff, start text, C, o, n, j, u, g, a, t, e, space, p, a, i, r, space, 2, end text, end color #aa87ff, equals, start text, H, end text, start subscript, 2, end subscript, start text, O, end text, start text, space, a, n, d, space, end text, start text, O, H, end text, start superscript, minus, end superscript, start text, L, i, O, H, end text, left parenthesis, a, q, right parenthesis, plus, start text, H, B, r, end text, left parenthesis, a, q, right parenthesis, right arrow, start text, H, end text, start subscript, 2, end subscript, start text, O, end text, left parenthesis, l, right parenthesis, plus, start text, L, i, B, r, end text, left parenthesis, a, q, right parenthesis, 2, start text, C, r, end text, left parenthesis, s, right parenthesis, plus, 3, start text, C, l, end text, start subscript, 2, end subscript, left parenthesis, g, right parenthesis, right arrow, 2, start text, C, r, C, l, end text, start subscript, 3, end subscript, left parenthesis, s, right parenthesis, start text, Z, n, end text, left parenthesis, s, right parenthesis, plus, 2, start text, H, C, l, end text, left parenthesis, a, q, right parenthesis, right arrow, start text, H, end text, start subscript, 2, end subscript, left parenthesis, g, right parenthesis, plus, start text, Z, n, C, l, end text, start subscript, 2, end subscript, left parenthesis, a, q, right parenthesis, start text, N, H, end text, start subscript, 3, end subscript, plus, start text, N, H, end text, start subscript, 3, end subscript, \rightleftharpoons, start text, N, H, end text, start subscript, 4, end subscript, start superscript, plus, end superscript, plus, start text, N, H, end text, start subscript, 2, end subscript, start superscript, minus, end superscript, start text, H, F, end text, left parenthesis, a, q, right parenthesis, plus, start text, H, end text, start subscript, 2, end subscript, start text, O, end text, left parenthesis, l, right parenthesis, \rightleftharpoons, start text, H, end text, start subscript, 3, end subscript, start text, O, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start text, F, end text, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, start text, F, end text, start subscript, 2, end subscript, left parenthesis, g, right parenthesis, start text, H, end text, start subscript, 3, end subscript, start text, O, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, start text, F, end text, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, start text, H, end text, start subscript, 2, end subscript, start text, O, end text, left parenthesis, l, right parenthesis, How is a reaction such as LiOH(aq)+HBr(aq)H2.
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