on both sides of this complete ionic equation, you have the same ions that are disassociated in water. hydronium ion is one to one. Be sure to balance this equation. about the contribution of the ammonium cations. moles of our weak base and strong acid, the weak base and strong acid will completely neutralize each other and produce the ammonium ion NH4 plus. chloride anion, Cl minus. get dissolved in water, they're no longer going to Note that when variable-charge metals such as copper appear as part of a compound, we have to determine the charge on the cation by looking at the number of anions and their charge. It is still the same compound, but it is now dissolved. \\end{align}, Or is it, since phosphoric acid is a triprotic acid . The advantage of the second equation above over the first is that it is a better representation Ammonium chloride is a soluble salt, therefore, an aqueous solution, we show it as the ions. Is the dissolution of a water-soluble ionic compound a chemical reaction? Direct link to RogerP's post No, we can't call it deco, Posted 6 years ago. When an excess of an aqueous hydroxide salt is added to a solution containing ammonium ions, ammonia gas is formed: (8.5.4) 2 NH 4 Cl ( aq) + Ba ( OH) 2 ( aq) 2 NH 3 ( g) + BaCl 2 ( aq) + 2 H 2 O ( l) Write the full ionic and net ionic equations for this reaction. See also the discussion and the examples provided in the following pages: We can just treat this like a strong acid pH calculation problem. 0000018685 00000 n How to Write the Net Ionic Equation for NH3 + HCl = NH4Cl Wayne Breslyn 631K subscribers Subscribe 57K views 2 years ago There are three main steps for writing the net ionic equation for NH3 +. When a weak base and a strong acid are mixed, they react according to the following net-ionic equation: B (aq) + HO (aq) HB (aq) + HO (l). 0000004305 00000 n In the complete ionic equation, soluble ionic compounds and strong acids are rewritten as dissociated ions. Direct link to Richard's post With ammonia (the weak ba. Q4.99P In a combination reaction, 1.62 [FREE SOLUTION] | StudySmarter Always start with a balanced formula (molecular) equation. And once we take out our spectator ion, we're left with our net ionic equation, which is aqueous ammonia 4.5: Writing Net Ionic Equations - Chemistry LibreTexts Since the solid sodium chloride has undergone a change in appearance and form, we could simply be in that crystalline form, crystalline form. Chemical reaction - The Brnsted-Lowry theory | Britannica However we'll let But the silver chloride is in solid form. How to Write the Net Ionic Equation for NH3 + HNO3 = NH4NO3 0000005636 00000 n To get the net ionic equation, we cancel them from both sides of the equation: \[ \ce{ Cu^2+(aq) + Mg(s) \rightarrow Cu(s) + Mg^2+(aq)} \]. The strong acid (HClO 4) and strong base react to produce a salt (NaClO 4) and water (H 2 O). Creative Commons Attribution/Non-Commercial/Share-Alike. 0000002525 00000 n If we then take a small sample of the salt and Write a net ionic equation for the reaction that occurs when aqueous We need to think about the ammonium cation in aqueous solution. %%EOF aren't going to be necessarily together anymore. Direct link to Audrey Harmon-Montrull's post how do you know whether o, Posted 7 years ago. Net Ionic Eqns with Acids and Bases Dissociate all strong acids and bases. nitrate stays dissolved so we can write it like this Step 2: From the reactivity of inorganic compounds handout, we know that when carbonate or bicarbonate ions react with acids, carbon dioxide and water are the normal products. combine it with a larger amount of pure water, the salt (which we denote as the solute) Let me free up some space. Under normal circumstances, carbonic acid decomposes into CO2 and H2O. 0000019272 00000 n Write the dissolution equation for any given formula of a water-soluble ionic compound. The balanced equation for this reaction is: \[\ce{3Ca^2+ (aq) + 2PO4^{3-}(aq) \rightarrow Ca3(PO4)2(s)}\], Example \(\PageIndex{2}\): Writing Net Ionic Equations, Write a net ionic equation to describe the reaction that occurs when 0.1 M HC2H3O2 solution is mixed with 0.1 M KOH solution. write the net ionic equation is to show aqueous ammonia It is a neutralisation . . The chloride ions are spectator ions. Why do people say that forever is not altogether real in love and relationship. KNO3 is water-soluble, so it will not form. which of these is better? 6.5K views 2 years ago There are three main steps for writing the net ionic equation for NH3 + HF = NH4F (Ammonia + Hydrofluoric acid). Direct link to nik.phatslap's post How can we tell if someth, Posted 7 years ago. it to a net ionic equation in a second. We learn to represent these reactions using ionic equa- tions and net ionic equations. On the product side, the ammonia and water are both molecules that do not ionize. So when the reaction goes to completion, we'll have ammonium cations in solution, and we'll also have some leftover ammonia. Direct link to astunix's post Why is it that AgCl(s) is, Posted a year ago. indistinguishable in appearance from the initial pure water, that we call the solution. Wiki User 2010-12-01 14:24:36 Study now See answer (1) Best Answer Copy NH3 (aq) + HNO2 (aq) => HN4+. I have a question.I am really confused on how to do an ionic equation.Please Help! Direct link to Richard's post Mathematically it's compl, start text, A, g, N, O, end text, start subscript, 3, end subscript, start text, N, a, N, O, end text, start subscript, 3, end subscript, start text, A, g, N, O, end text, start subscript, 3, end subscript, left parenthesis, a, q, right parenthesis, plus, start text, N, a, C, l, end text, left parenthesis, a, q, right parenthesis, right arrow, start text, A, g, C, l, end text, left parenthesis, s, right parenthesis, plus, start text, N, a, N, O, end text, start subscript, 3, end subscript, left parenthesis, a, q, right parenthesis, start text, N, a, end text, start superscript, plus, end superscript, start text, C, l, end text, start superscript, minus, end superscript, start text, A, g, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start color #11accd, start text, N, O, end text, start subscript, 3, end subscript, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, end color #11accd, plus, start color #ca337c, start text, N, a, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, end color #ca337c, plus, start text, C, l, end text, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, right arrow, start text, A, g, C, l, end text, left parenthesis, s, right parenthesis, plus, start color #ca337c, start text, N, a, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, end color #ca337c, plus, start color #11accd, start text, N, O, end text, start subscript, 3, end subscript, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, end color #11accd, start text, A, g, C, l, end text, left parenthesis, s, right parenthesis, start color #11accd, start text, N, O, end text, start subscript, 3, end subscript, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, end color #11accd, start color #ca337c, start text, N, a, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, end color #ca337c, start text, A, g, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start cancel, start color #11accd, start text, N, O, end text, start subscript, 3, end subscript, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, end color #11accd, end cancel, plus, start cancel, start color #ca337c, start text, N, a, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, end color #ca337c, end cancel, plus, start text, C, l, end text, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, right arrow, start text, A, g, C, l, end text, left parenthesis, s, right parenthesis, plus, start cancel, start color #ca337c, start text, N, a, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, end color #ca337c, end cancel, plus, start cancel, start color #11accd, start text, N, O, end text, start subscript, 3, end subscript, start superscript, minus, end superscript, left parenthesis, a, q, right parenthesis, end color #11accd, end cancel, start text, A, g, end text, start superscript, plus, end superscript, left parenthesis, a, q, right parenthesis, plus, start text, C, l, end text, start superscript, , end superscript, left parenthesis, a, q, right parenthesis, right arrow, start text, A, g, C, l, end text, left parenthesis, s, right parenthesis, start text, A, g, end text, start superscript, plus, end superscript, start text, H, end text, start subscript, 2, end subscript, start text, S, O, end text, start subscript, 4, end subscript, left parenthesis, a, q, right parenthesis, start text, H, end text, start superscript, plus, end superscript, start text, S, O, end text, start subscript, 4, end subscript, start superscript, 2, minus, end superscript, start text, N, a, O, H, end text, left parenthesis, a, q, right parenthesis, start text, O, H, end text, start superscript, minus, end superscript, start text, N, a, end text, start subscript, 2, end subscript, start text, S, O, end text, start subscript, 4, end subscript, left parenthesis, a, q, right parenthesis. In writing the dissolution equation, it is assumed that the compound undergoing dissolution is indeed Since the mole ratio of xref Creative Commons Attribution/Non-Commercial/Share-Alike. the solid form of the compound. anion on the left side and on the right side, the chloride anion is the - HCl is a strong acid. Net Ionic Equation Definition (Chemistry) - ThoughtCo the silver chloride being the thing that's being So the sodium chloride an example of a weak base. The base and the salt are fully dissociated. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. So for example, on the left-hand How many 5 letter words can you make from Cat in the Hat? Step 1: Identify the species that are actually present, accounting for the dissociation of any strong electrolytes. water and you also have on the right-hand side sodium If no reaction occurs leave all boxes blank and click on "submit". You don't need to, for any practical reason since tables are provided on some Periodic Table of Elements anyway. both sides of this reaction and so you can view it as a This makes it a little Write the state (s, l, g, aq) for each substance.3. If you're seeing this message, it means we're having trouble loading external resources on our website. Direct link to Icedlatte's post You don't need to, for an. NaNO3 is very soluble in water so it isn't formed as a compound, Na^+ and NO3^- ions are instead, that is why they both are (aq). Write a net ionic equation to show that hydrocyanic acid behaves as a Brnsted-Lowry acid in water. <<0E3A66ABCCE85E48B6E7192D2C7FA130>]>> silver into the solution, these are the things that First, we balance the molecular equation. Step 1: The species that are actually present are: For the second situation, we have more of the weak solvated ionic species. The following is the strategy we suggest following for writing net ionic equations in Chem 101A. What is the net ionic equation of the reaction between ammonia and First, we balance the molecular equation. We're simply gonna write Only the aqueous ionic compounds (the two chloride salts) are written as ions: \[ \ce{ Cu^2+(aq) + 2Cl^- (aq) + Mg(s) \rightarrow Cu(s) + Mg^2+(aq) + 2Cl^- (aq)} \]. Now you might say, well Step 3: The reaction is the combination of bicarbonate ions and hydrogen ions that will first form carbonic acid (H2CO3). The balanced, net ionic equation for the reaction occurring in this titration is I2(aq) + 2 S2O32(aq)2 I(aq) + S4O62(aq) Suppose 50.00 mL of 0.0520 M I2 was added to the sample containing ascorbic acid. Symbolically, the condition or potential for dynamic equilibrium is represented by replacement of Y>k'I9brR/OI+ao? 0000018450 00000 n pH of the resulting solution by doing a strong acid The equation looks like this:HNO3 . or complete ionic equation. Who is Katy mixon body double eastbound and down season 1 finale? WRITING NET IONIC EQUATIONS FOR CHEM 101A. Direct link to Nafia Farzana's post So when compounds are aqu, Posted 5 years ago. Answered: Write the balanced formula, complete | bartleby Has a chemical reaction occurred or is dissolution of salt a merely physical process? In case of hydrates, we could show the waters of hydration So how should a chemical equation be written to represent this process? Direct link to Ryan W's post NaNO3 is very soluble in , Posted a year ago. Direct link to Hema Punyamoorty's post At 0:50, it is said that , Posted 6 years ago. The silver ion, once it's will be slightly acidic. Ammonia present in ammonium hydroxide | US EPA J. D. Cronk Finally, we cross out any spectator ions. the equation like this. Share sensitive information only on official, secure websites. And because the mole HCN (aq) + H2O CN- (aq) + H3O+ (aq) Write a net ionic equation to show that caffeine, C8H10N4O2, behaves as a Bronsted-Lowry base in water.-Bronsted-Lowry base accepts a proton (H+).-C8H10N4O2 accepts a proton from H2O to form HC8H10N4O2+ . What is the net ionic equation for the reaction between aqueous ammonia And remember, these are the Let's now consider a number of examples of chemical reactions involving ions. Strictly speaking, this equation would be considered unbalanced. The OH and H+ will form water. The reason they reacted in the first place, was to become more stable. What is the net ionic equation of the reaction between ammonia and bulk environment for solution formation. really deals with the things that aren't spectators, For the purposes of the risk management program regulations at 40 CFR Part 68, ammonium hydroxide must be treated as a solution of ammonia and water, regardless of the fact that ammonium hydroxide may be identified by a unique CAS number. reactions, introduction to chemical equations. So in this case H 2 SO 4 (aq) and Ba (OH) 2 (aq) must be . To do that, we first need to of ammonium chloride. 0000019076 00000 n When they dissolve, they become a solution of the compound. If you're seeing this message, it means we're having trouble loading external resources on our website. unbalanced "skeletal" chemical equation it is not wildly out of place. So, can we call this decompostiton reaction? Finally, we cross out any spectator ions. come from the strong acid. Now, what would a net ionic equation be? They're going to react The net ionic equation results from cancelling them from the full ionic equation: \[ \ce{ 2NH_4^+ (aq) + 2OH^- (aq) \rightarrow 2NH_3(g) + 2H_2O(l)} \]. startxref (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.152 M aqueous hydrocyanic acid and diethylamine are mixed. Remember to show the major species that exist in solution when you write your equation. Let's start with ammonia. Explanation: According to the details in the question, amonia is written N H 3 because it is a weak base, and does not ionize to a large extent in water. spectator, and that's actually what it's called. Q4.47 Que Complete the following acid- [FREE SOLUTION] | StudySmarter Both the compounds on the reactant side of the equation are soluble ionic compounds, so they will need to be separated into their respective ions. solution from our strong acid that we don't need to worry How would you recommend memorizing which ions are soluble? acid than the weak base, all of the weak base will be used up and we'll have some strong acid in excess. and we could calculate the pH using the The chemical equation is:HCN + NH3 + H2O = NH4CNH+ + (CN)- + (NH4)+ (OH)- = (NH4)+ (CN)- + H2O, NH3(aq) + CH3COOH (aq) ---> NH4+ (aq) + C2H3O2- (aq). If we wanted to calculate the actual pH, we would treat this like a In the molecular equation for a reaction, all of the reactants and products are represented as neutral molecules (even soluble ionic compounds and strong acids). It is not necessary to include states such as (aq) or (s). In the complete ionic equation, soluble ionic compounds and strong acids are rewritten as dissociated ions. Ammonia is making so many hydroxide ions that ammonium is more likely to react with those than neutral water. Direct link to RogerP's post Without specific details , Posted 2 years ago. Write the balanced molecular equation.2. Once we begin to consider aqueous solutions hydroxide ions in solution has increased at 25 degrees Celsius, the resulting solution will be basic and the pH will be greater than seven. This form up here, which daBL:nC[ -|7LDVp)J0s~t@Vg,0G' bm@S 0(xX,CF$ If you wanna think of it in human terms, it's kind of out there and This is the same process we followed when naming a compound with a variable-charge metal in chapter 4. 1 Answer anor277 Jan 17, 2016 #NH_3(aq) + H_3O^+ rarr NH_4^+ + H_2O(l)# . The molecular and net ionic equations for the reaction of hydrochloric acid and ammonia are shown below. The list of regulated toxic substances at 40 CFR Section 68.130 includes both "ammonia (anhydrous)" and "ammonia (conc 20% or greater)," but does not include a specific listing for "ammonium hydroxide." Please click here to see any active alerts. To write the ionic equation we must separate all aqueous species into their ions and leave any solid, liquid or gaseous substance in its molecular form. base than the strong acid, all of the strong acid will be used up. I'm assuming that you're talking about the last reactionH2SO4 (aq) + 2 NaOH (aq) Na2SO4 (aq) + 2 H2O (). In this case, Identify what species are really present in an aqueous solution. 8.5: Complete Ionic and Net Ionic Equations - More Examples Weak base-strong acid reactions (video) | Khan Academy TzW,%|$fFznOC!TehXp/y@=r By gaining a hydrogen (and a unit of charge) the hydroxide ion transforms into a water molecule. molecular equation. Well what we have leftover is we have some dissolved chloride, and Write balanced (a) molecular, (b) overall ionic, and (c) net ionic equations for the reaction between an aqueous solution of phosphoric acid, H3PO4(aq), and an aqueous solution of sodium hydroxide. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. You'll probably memorise some as you study further into the subject though. So for example, in the ), 6) 0.1 M HClO and 0.1 M Ba(OH)2 (no precipitate forms), 1) 0.1 M Na2HPO4 and 0.1 M HI (equal volumes), 4) 0.1 M K2CO3 and 0.1 M HNO3 (equal volumes), 5) 0.1 M H3PO4 and 0.1 M NH3 (equal volumes), 3) solid Cu(OH)2 and 1 M H2SO4 (equal numbers of moles), AnswerS TO NET IONIC EQUATIONS PRACTICE PROBLEMS, 3) 2 Fe3+(aq) + 3 CO32(aq) --> Fe2(CO3)3(s), 8) 2 PO43(aq) + 3 Cu2+(aq) --> Cu3(PO4)2(s), 1) HC2H3O2(aq) + OH(aq) --> C2H3O2(aq) + H2O(l), 3) 2 H+(aq) + Mn(OH)2(s) --> Mn2+(aq) + 2 H2O(l), 4) 3 H+(aq) + AlPO4(s) --> Al3+(aq) + H3PO4(aq), 5) 2 Ag+(aq) + 2 OH(aq) --> Ag2O(s) + H2O(l), 6) HClO(aq) + OH(aq) --> ClO(aq) + H2O(l), 2) Fe2+(aq) + 2 NH3(aq) + 2 H2O(l) --> Fe(OH)2(s) + 2 NH4+(aq), 3) HCO3(aq) + H+(aq) --> H2O(l) + CO2(g), 5) H3PO4(aq) + NH3(aq) --> H2PO4(aq) + NH4+(aq), 1) 2 Ag+(aq) + 2 NH3(aq) + H2O(l) --> Ag2O(s) + 2 NH4+(aq), 2) BaCO3(s) + 2 HC2H3O2(aq) --> Ba2+(aq) + 2 C2H3O2(aq) + H2O(l) + CO2(g), 3) Cu(OH)2(s) + H+(aq) + HSO4(aq) --> Cu2+(aq) + 2 H2O(l) + SO42(aq), 4) Ag2O(s) + 2 H+(aq) + 2 Cl(aq) --> 2 AgCl(s) + H2O(l). going to be attracted to the partially positive Direct link to Quinn Becker's post Why when you divide 2H+ b, Posted 7 years ago. One source is from ammonia with the individual ions disassociated. The net ionic equation for a precipitation reaction is formally the reverse of a dissolution. 0000003112 00000 n reaction is complete and all the H3O plus is used up, we'll have some leftover ammonia. Write a net ionic equation for the reaction that occurs when aqueous solutions of nitrous acid and ammonia are combined. Direct link to RogerP's post Yes, that's right. 61 0 obj <>stream I know this may sound silly, but can we subtract or add a reactant to both sides just like in mathematics? The H+ from the HC2H3O2 can combine with the OH to form H2O. Direct link to Dillon Mccarthy's post How do we know which of t, Posted 6 years ago. Direct link to Ernest Zinck's post Memorize the six common s, Posted 7 years ago. Because the concentration of is providing the chloride that eventually forms the silver chloride, but the sodium is just kind of watching. A net ionic equation shows only the chemical species that are involved in a reaction, while a complete ionic equation also includes the spectator ions. reacting with water to form NH4 plus, and the other source came from Therefore, the Ka value is less than one. Net ionic equation for hydrolysis of nh4cl - Write the net ionic equation for the hydrolysis reaction that occurs when ammonium chloride, NH.CI. plus H plus yields NH4 plus. 0000000016 00000 n Now, in order to appreciate Mathematically it's completely acceptable to do so, however we have to consider the actual chemical makeup of our reaction if we do so. Yup! Example \(\PageIndex{1}\): Writing Net Ionic Equations, Write a net ionic equation to describe the reaction that occurs when 0.100 M K3PO4 solution is mixed with 0.100 M Ca(NO3)2 solution. The chloride is gonna Official websites use .gov The balanced equation for this reaction is: \[\ce{Mg(OH)2(s) + 2H^+ (aq) \rightarrow 2H2O(l) + Mg^2+ (aq)}\], Example \(\PageIndex{4}\): Writing Net Ionic Equations, Write a net ionic equation to describe the reaction that occurs when 0.1 M KHCO3 solution is mixed with excess 0.1 M HNO3 solution. phosphoric acid and sodium hydroxide net ionic equation of some sodium chloride dissolved in water plus write the formula NaCl along with the label ("s") to specifically represent than one at equilibrium, there are mostly reactants 0000007425 00000 n hydrogen ends of the water molecules and the same 153 Reactions-in-Aqueous-Solutions Chemistry 10th Edition Raymond Chang Nitric acid and ammonium hydroxide balanced equation Step 2: Identify the products that will be formed when the reactants are combined. To be more specific,, Posted 7 years ago. The Agency has made it clear that the listing for "ammonia (conc 20% or greater)" applies to aqueous solutions of ammonia (List Rule Response to Comments document, page 50). For the following aqueous reactions, complete and balance the molecular equation and write a net ionic equation: (a) Manganese(II) sulfide + hydrobromic acid (b) Potassium carbonate + strontium nitrate (c) Potassium nitrite + hydrochloric acid (d) Calcium hydroxide + nitric acid (e) Barium acetate + iron(II) sulfate (f) Zinc carbonate . Only soluble ionic compounds dissociate into ions. There are three main steps for writing the net ionic equation for NH3 + HCl = NH4Cl (Ammonia and Hydrochloric Acid). base than the strong acid, therefore, we have the Second,. Direct link to skofljica's post it depends on how much is, Posted a year ago. we see more typically, this is just a standard Isn't NaNo also formed as part of the reaction, meaning that the Cl and Ag ions were the spectators? arrow going to the right, indicating the reaction The elemental metals (magnesium on the reactant side, copper on the product side) are neutral solids. Posted 2 months ago. (Insoluble ionic compounds do not ionize, but you must consider the possibility that the ions in an insoluble compound might still be involved in the reaction.). CHEM 101 - General Chemistry topic - Gonzaga University 0000006157 00000 n The term we'll use for this form of the equation representing this process is the 28 0 obj <> endobj What is the net ionic equation for ammonia plus hydrocyanic acid? For ionic equations like these it's possible for us to eliminate, essentially subtract out, spectator ions from an equation. If you're behind a web filter, please make sure that the domains *.kastatic.org and *.kasandbox.org are unblocked. Nitric Acid is a strong acid, therefore, its hydrogen atom dissociates completely. the pH of this solution is to realize that ammonium as a complete ionic equation. The sodium is going to Write net ionic equations for reactions that occur in aqueous solution. Molecular, complete ionic, and net ionic equations Both the barium ions and the chloride ions are spectator ions. represent this symbolically by replacing the appended "s" label with "aq". In acid/base reaction it's common for the H+, OH-, and H2O to be the only species left in a net ionic equation after all the other spectator ions have been eliminated. What is the net ionic equation of the reaction between ammonia and nitrous acid? plus solid silver chloride and if you were to look You get rid of that, and then thing is gonna be true of the silver nitrate. Hydrolysis of Salts NH4Cl is the salt of a strong acid (hydrochloric acid) and a weak base (ammonia) The NH4+ ions will react with water: NH4+(aq) + H2O(aq) partially negative oxygen end. Well it just depends what 0000012304 00000 n What type of electrical charge does a proton have? Using the familiar compound sodium chloride as an illustrative example, we can Other examples of dissolution equations for water-soluble ionic compounds, such as the one for lead(II) nitrate shown at left When ions are involved in a reaction, the equation for the reaction can be written with various levels of detail. identify these spectator ions. Write a partial net ionic equation: water, and that's what this aqueous form tells us, it 0000001926 00000 n You're not dividing the 2Na- to make it go away. some dissolved silver, plus some dissolved silver. and encounter the phenomenom of electrolytes,
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