of calcium fluoride that dissolves. is 1.1 x 10-10. AlPO_{4}, K_{sp} = 9.8*10^{-21}. We can calculate the molar solubility using Ksp, but we have to know the ions produced by the dissociation during the dissolution of the substance in the solution. 10-5? For dilute solutions, the density of the solution is nearly the same as that of water, so dissolving the salt in 1.00 L of water gives essentially 1.00 L of solution. The more soluble a substance is, the higher the K s p value it has. This cookie is set by GDPR Cookie Consent plugin. $K_s_p$ represents how much of the solute will dissolve in solution. We have a new and improved read on this topic. Calculate the solubility product for PbCl2. For what it's worth, my "Handbook of Chemistry and Physics" gives the Ksp as 9.86 x 1025. Determine the solubility of barium fluoride in a solution containing 5.0 mg/mL KF. The solubility product of calcium fluoride (CaF2) is 3.45 1011. Divide the mass of the compound by the mass of the solvent and then multiply by 100 g to calculate the solubility in g/100g . Solubility Constant Ksp: Solubility constant, Ksp, is the same as equilibrium constant. This would mean the $K_s_p$ unit would be different for every problem and would be difficult to solve, so in order to make it simpler, chemists generally drop $K_s_p$ units altogether. The equation for the precipitation of BaSO4 is as follows: \[BaSO_{4(s)} \rightleftharpoons Ba^{2+}_{(aq)} + SO^{2}_{4(aq)}\]. solution is common to the chloride in lead(II) chloride. Transcribed image text: Temperature of solution: 31.6 C Trial 1 Trial 1 Trial 2 Trial 3 1.0 mL Original volume of KHP solution: 10 mL 1.0mL .08953 Concentration of NaOH solution: 5.1ml 5.3 ml 5.Oml Volume of NaOH solution added: Concentration of KHP solution: Ksp calculated from solution: H2O] is a sparingly soluble salt that is the other major component of kidney stones [along with Ca3(PO4)2]. Calculating
Educ. solid doesn't change. Necessary cookies are absolutely essential for the website to function properly. All rights reserved. IT IS NOT!!! Direct link to Shariq Khan's post What would you do if you , Posted 7 years ago. These cookies will be stored in your browser only with your consent. fluoride anions raised to the second power. To use this website, please enable javascript in your browser. in terms of molarity, or moles per liter, or the means to obtain these
The concentration of Mg2+ ion in the solution was found to be 2.34 x 10-4 M. Calculate the Ksp for MgF2. We use cookies on our website to give you the most relevant experience by remembering your preferences and repeat visits. So, solid calcium fluoride As a reminder, a solute (what is being dissolved) is considered soluble if more than 1 gram of it can be completely dissolved in 100 ml of water. The concentration of Cl^-(aq) in seawater is 0.54 M. i. Calcul, Calculate the molar solubility of FeF2 in: (a) pure water (b) 0.150 M solution of NaF. copyright 2003-2023 Homework.Study.com. You need to ask yourself questions and then do problems to answer those questions. write the Ksp expression from the balanced equation. Jay misspoke, he should have said x times 2x squared which results in 4x cubed. Convert the solubility of the salt to moles per liter. If 2.0 mL of a 0.10 M solution of NaF is added to 128 mL of a 2.0 105M solution of Ca(NO3)2, will CaF2 precipitate? Finding Ksp from Ion Concentrations Finding Ksp from Ion Concentrations: Finding Ksp from Ion Concentrations (opens in new window) [youtu.be] Solving K sp Problems I: Calculating Molar Solubility Given the K sp. Thus, the Ksp K s p value for CaCl2 C a C l 2 is 21. The solubility product constant, Ksp , is the equilibrium constant for a solid substance dissolving in an aqueous solution. 1998, 75, 1179-1181 and J. Chem. Our goal was to calculate the molar solubility of calcium fluoride. What is the concentration of OH- ions in 0.125M Ba(OH)2 solution? Calculate the concentration of NH_3 required to just dissolve 0.022 mol of NiC_2O_4 (K_sp = 4.0 x 10^-10) in 1.00 L of solution. Therefore, 2.1 times 10 to First, we need to write out the two equations. Therefore: Ksp= (1.071 x 105)3(7.14 x 106)2 Ksp= 6.26 x 1026 barium sulfate. That gives us X is equal to 2.1 times 10 to the negative fourth. concentration of fluoride anions. Transcript A compound's molar solubility in water can be calculated from its K value at 25C. This short video is an example of calculating the concentration of one ion given the concentration of the other ion and the Ksp for a particular insoluble salt. Direct link to Matthew Belliveau's post It is explained in this v, Posted 7 years ago. 100 mL of 0.50 M K2SO4 is mixed with 75.0 mL of 0.25 M Al(NO3)3. What is the concentration of hydrogen ions commonly expressed as? How to Calculate Mass Percent Concentration of a Solution . The solubility product constant, K s p , is the equilibrium constant for a solid substance dissolving in an aqueous solution. molar concentrations of the reactants and products are different for each equation. it will not improve the significance of your answer.). In his writing, Alexander covers a wide range of topics, from cutting-edge medical research and technology to environmental science and space exploration. Substitute these values into the solubility product expression to calculate Ksp. Assume that the volume of the solution is the same as the volume of the solvent. As summarized in Figure \(\PageIndex{1}\) "The Relationship between ", there are three possible conditions for an aqueous solution of an ionic solid: The process of calculating the value of the ion product and comparing it with the magnitude of the solubility product is a straightforward way to determine whether a solution is unsaturated, saturated, or supersaturated. 1998, 75, 1182-1185).". What does molarity measure the concentration of? After completing his doctoral studies, he decided to start "ScienceOxygen" as a way to share his passion for science with others and to provide an accessible and engaging resource for those interested in learning about the latest scientific discoveries. For example, if we took some solid lead two fluoride, which is a white solid, and we put it in some distilled water, the solid is going to reach an equilibrium with the ions in solution. When you have a solid grasp of $K_s_p$, those questions become much easier to answer! One important factor to remember is there
Performance cookies are used to understand and analyze the key performance indexes of the website which helps in delivering a better user experience for the visitors. So to solve for X, we need Q exceeds the Ksp value. (Ksp = 9.8 x 10^9). Some of the calcium $K_s_p$ represents how much of the solute will dissolve in solution, and the more soluble a substance is, the higher the chemistry $K_s_p$ value. Consider this equilibrium: I2(s) + H2O(l) H+(aq) + I-(aq) + HOI(aq). Next, we plug in the $K_s_p$ value to create an algebraic expression. Calculate the molar solubility (in mol/L) of BiI3. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. Calculate the concentration of 6.73 g of Na2CO3 dissolved in 250 mL of H2O. If they asked for the concentration of the chloride anion during equilibrium would you just multiply the molar solubility by two? And since it's a one-to-two mole ratio for calcium two plus 2) divide the grams per liter value by the molar mass of the substance. Calculate the solubility of Au(OH)3 in water (Ksp=5.5x10^46). This is shown below: Note that the reactant, aA, is not included in the \(K_{sp}\) equation. Step 1: Determine the dissociation equation of the ionic compound. How do you calculate pH from hydrogen ion concentration? a. AgIO 3 (S= 7 x 10-4 mol/L) b. Pb(IO 3 ) 2 (S=4 x 10-5 mol/L) c. SrF 2 (S=8 x 10-4 mol/L) d. Ag 3 PO 4 (S=4 x 10-6 mol/L) 5. Direct link to tyersome's post Concentration is what we . of calcium two plus ions is zero plus X, or just X, and the equilibrium concentration Example: Calculate the solubility product constant for
Calculate the molar solubility of PbCl2 in pure water at 25c. Ini, Posted 7 years ago. Check out Tutorbase! make the assumption that since x is going to be very small (the solubility
So Ksp is equal to the concentration of M sodium sulfate solution. For each compound, the molar solubility is given. MITs Alan , In 2020, as a response to the disruption caused by COVID-19, the College Board modified the AP exams so they were shorter, administered online, covered less material, and had a different format than previous tests. So we're going to leave calcium fluoride out of the Ksp expression. Analytical cookies are used to understand how visitors interact with the website. and calcium two plus ions. You aren't multiplying, you're squaring. The value of K_sp for AgCl(s) is 1.8 x 10^-10. What is the formula for calculating solubility? For the reaction $A_aB_b$(s) $aA^b^{+}$(aq) + $bB^a^{-}$ (aq), The solubility expression is $K_s_p$= $[A^b^{+}]^a$ $[B^a^{-}]^b$. When Hg2Br2 dissolves, it dissociates like this: Important note: it is NOT 2Hg+. Solubility product constants can be
A saturated solution
What is the molar concentration of scandium ions in a 0.260 mol/L solution of scandium sulfate? Example: Calculate the solubility product constant for We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. For very soluble substances (like sodium nitrate, NaNO3), this value can be quite high, exceeding 10.0 moles per liter of solution in some cases. of ionic compounds of relatively low solubility. of the ions in solution. Also, the key thing to be aware of with these equations is that each concentration (represented by square brackets) is raised to the power of its coefficient in the balanced $K_s_p$ expression. Technically at a constant Euler, William B.; Kirschenbaum, Louis J.; Ruekberg, Ben. In a saturated solution the solid is in equilibrium with its ions e.g : CaCO3(s) Ca2+ (aq) + CO2 3(aq) The expression for Ksp is: Ksp = [Ca2+ (aq)][CO2 3(aq)] We don't include the concentration of the solid as this is assumed constant. Inconsolable that you finished learning about the solubility constant? Calculate the value for K sp of Ca(OH) 2 from this data. concentration of calcium two plus and 2X for the equilibrium temperature of 25 degrees, the concentration of a liter. 3 years ago GGHS Chemistry. Step 2: Determine the Ksp equation from the dissociation equation. SAT is a registered trademark of the College Entrance Examination BoardTM. This indicates how strong in your memory this concept is. Direct link to Richard's post Jay misspoke, he should h, Posted 7 years ago. For the fluoride anions, the equilibrium concentration is 2X. Whereas Ksp describes equilibrium concentrations, the ion product describes concentrations that are not necessarily equilibrium concentrations. that occurs when the two soltutions are mixed. What is the equilibrium constant for the weak acid KHP? with 75.0 mL of 0.000125 M lead(II) nitrate. Yes! In contrast, the ion product (Q) describes concentrations that are not necessarily equilibrium concentrations. [6] In our example, C = (10 g)/ (1,210 g) = 0.00826. Video transcript. When you open the can, the pressure decreases, and, if you leave the soda sitting out long enough, the bubbles will eventually disappear because solubility has decreased and they are no longer dissolved in the liquid (theyve bubbled out of the drink). A crystal of calcite (CaCO3), illustrating the phenomenon of double refraction. in our Ksp expression are equilibrium concentrations. 2.3 \cdot 10^{-6} b. 1) Write the chemical equation for the dissolving of barium phosphate in water: 2) Write the Ksp expression for barium phosphate: 4) Put values into and then solve the Ksp expression: 5) Note that the formula weight of Ba3(PO4)2 is not involved at any point. Find the Ksp. Ca_{3}(PO_{4})_{2}, K_{sp} = 2.1 * 10^{-33} 2. concentration of each ion using mole ratios (record them on top of the equation). Next we need to solve for X. Compound AX2 will have the smallest Ksp value. 18.1: Solubility Product Constant, Ksp is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. Simply use a scale to measure the mass of the solute and the final solution and express the ratio as a percentage. Do NOT follow this link or you will be banned from the site! A crystal of calcite (CaCO3), illustrating the phenomenon of double refraction. Here is a skeleton outline of the process: Example #1: Determine the Ksp of silver bromide, given that its molar solubility is 5.71 x 107 moles per liter. For calcium oxalate monohydrate, the balanced dissolution equilibrium and the solubility product expression (abbreviating oxalate as ox2) are as follows: \(\mathrm{Ca(O_2CCO_2)}\cdot\mathrm{H_2O(s)}\rightleftharpoons \mathrm{Ca^{2+}(aq)}+\mathrm{^-O_2CCO_2^-(aq)}+\mathrm{H_2O(l)}\hspace{5mm}K_{\textrm{sp}}=[\mathrm{Ca^{2+}}][\mathrm{ox^{2-}}]\). More important, the ion product tells chemists whether a precipitate will form when solutions of two soluble salts are mixed. Calcium carbonate, CaCO3 has a Ksp value of 1.4 10^-8 . Wittenberg is a nationally ranked liberal arts institution with a particular strength in the sciences. The solubility product of barium fluoride (BaF2) is 2 x 10-6 at 25 C. All Modalities Calculating Ksp from Solubility Loading. lead(II) chromate form. Pressure can also affect solubility, but only for gases that are in liquids. How do you calculate the molar concentration of an enzyme? in pure water from its K, Calculating the solubility of an ionic compound
value for calcium fluoride. Relating Solubilities to Solubility Constants. Learn about solubility product constant. (You can leave x in the term and use the quadratic
You do this because of the coefficient 2 in the dissociation equation. negative fourth molar is the equilibrium concentration The solubility of NiCO_{3} ( K_{sp} = 1.3 \cdot 10^{-7}) increases with adding which of the following? root of the left side and the cube root of X cubed. Direct link to Jerry J. Francais II's post How do you know what valu, Posted 7 years ago. Determining Whether a Precipitate will, or will not Form When Two Solutions
The cookies is used to store the user consent for the cookies in the category "Necessary". Formulate Solubility Reaction Write the balanced solubility reaction equation for the substance you're interested in. 4) Putting the values into the Ksp expression, we obtain: Example #2: Determine the Ksp of calcium fluoride (CaF2), given that its molar solubility is 2.14 x 104 moles per liter. If the concentration of fluoride in fluoridated drinking water is 1 \times 10^{-5} M and the calcium iron concentration in b. Whereas solubility is usually expressed in terms of mass of solute per 100 mL of solvent, Ksp is defined in terms of the molar concentrations of the component ions. Fourth, substitute the equilibrium concentrations into the equilibrium
a common ion must be taken into account when determining the solubility
Then calculate the Ksp based on 2 mol/L Ag^+ and 1.5 mol/L CO3^2-. calcium two plus ions, and since there's a coefficient of one in the balanced equation, that's the concentration this case does refer to the molar solubility. The concentrations of lead two plus and sulfate in the KSP expression, are equilibrium concentrations. In order to calculate a value for $K_s_p$, you need to have molar solubility values or be able to find them. Solubility product constants are used to describe saturated solutions
The solubility constant can be affected by temperature, pressure, and molecular size, and its important for determining solubility, predicting if a precipitate will form, and understand the common ion effect. The $K_s_p$ value does not have any units because the molar concentrations of the reactants and products are different for each equation. Calculate the value of Ksp . 9.0 x 10-10 M b. First, determine the overall and the net-ionic equations for the reaction
Ksp for sodium chloride is 36 mol^2/litre^2 . It is given by the formula Ksp = [A+]m[B+]n Where Ksp = Solubility Constant [A+] and [B+] = Concentration of the products n and m = stoichiometric coefficients Answer link the equation for the dissolving process so the equilibrium expression can
What is the weight per volume method to calculate concentration? Write the solubility product expression (Ksp) for the decomposition of Ag2CO3. Get Free Guides to Boost Your SAT/ACT Score, our complete guide to the 11 solubility rules, Learn how to balance chemical equations here, read through these six examples of physical and chemical change, (aq) and (s) indicate which state the product is in (aqueous or solid, respectively). The Ksp for CaCO3 is 6.0 x10-9. Understand the definition of Ksp, the Ksp formula, how to calculate Ksp, and how to find molar solubility from Ksp. Calculate the molar solubility of calcium fluoride. How do you calculate Ksp from concentration? It represents the level at which a solute dissolves in solution. Calculate the standard molar concentration of the NaOH using the given below. And looking at our ICE table, X represents the equilibrium concentration The solubility product of silver carbonate (Ag2CO3) is 8.46 1012 at 25C. The value of $K_s_p$ varies depending on the solute. Will barium sulfate precipitate if 10.0 mL of 0.0020 M Na2SO4 is added to 100 mL of 3.2 104 M BaCl2? For example, the chloride ion in a sodium chloride
So that would give us 3.9 times 10 to the Get the latest articles and test prep tips! What SAT Target Score Should You Be Aiming For? values. textbooks not to put in -X on the ICE table. Tell us Notes/Highlights Image Attributions Show Details Show Resources Was this helpful? (For Mn(OH)2, Ksp = 1.95 x 10^ -6) A) 9.20 B) 2.10 C) 7.00 D) 5.10 E) 11.89, What is the solubility of Fe(OH)2 in 828 mL of NaOH with a pH of 8.08? See how other students and parents are navigating high school, college, and the college admissions process. equation for calcium fluoride. Determine the molar solubility. When we know the $K_s_p$ value of a solute, we can figure out if a precipitate will occur if a solution of its ions is mixed. Using the initial concentrations, calculate the reaction quotient Q, and
As , EL NORTE is a melodrama divided into three acts. Researchers have discovered that the teeth are shaped like needles and plates and contain magnesium. it's a one-to-one mole ratio between calcium fluoride Drown your sorrows in our complete guide to the 11 solubility rules. A neutral solution is one that has equal concentrations of OH ions and H3O + ions. The concentration of magnesium increases toward the tip, which contributes to the hardness. The next step is to set up an ICE table, where I stands for initial concentration, C stands for the change in concentration, and E stands for What is the concentration of Ca^{2+}_{(aq)} in a saturated solution of CaCO_{3}? How to calculate the equilibrium constant given initial concentration? What is the solubility of AgCl in water if Ksp 1.6 10 10? How nice of them! (A solute is insoluble if nothing or nearly nothing of it dissolves in solution.) A) If 0.0067g CaCO3 soluble in 1.0L of water, calculate the molar solubility and the Ksp. of calcium two plus ions. One reason that our program is so strong is that our . What is the concentration of lead(II) ions (Pb2+) in a sample of polluted water given the following information? Calculate Ksp using one ion concentration BCchemistry 375 subscribers Subscribe 104 Share 19K views 9 years ago This video shows you how to calculate Ksp when only one ion concentration in. our salt that dissolved to form a saturated It is given by the formula #-> K_sp = [A^+]^m [B^+]^n#, #color(white)(xxxx) [A^+] and [B^+] = "Concentration of the products"#, #color(white)(xxxx) n and m = "stoichiometric coefficients"#, 10560 views Calculate the molar solubility of calcium hydroxide (Ks,-6.0% 106) in pure water and in a solution with a pH of 13.3. What is $K_s_p$ in chemistry? Solubility constant, Ksp, is the same as equilibrium constant. The 5 Strategies You Must Be Using to Improve 160+ SAT Points, How to Get a Perfect 1600, by a Perfect Scorer, Free Complete Official SAT Practice Tests. The values given for the Ksp answers are from a reference source. The next step is to Educ. Calculate the mass of solute in 100 mL of solution from the molar solubility of the salt. The solubility of CaC2O4 is 0.00081 g/100 mL at 25 degrees Celsius. In our calculation, we have ignored the reaction of the weakly basic anion with water, which tends to make the actual solubility of many salts greater than the calculated value. Calculate the molar solubility of BaSO_{4} in: a) Water b) A solution containing 1.0 M SO_{4}^{2-} ions c) Explain the difference in solubilities. Select one: a) 2.3 \times 10^{-6} b) 3.4 \times 10^{-9} c) 1.4 \times 10^{-8} d) 1.5 \times 10^{-3}, The molar solubility of PbI_{2} is 1.5 \cdot 10^{-3} mol/L. $PbBr_2$(s) $Pb^2^{+}$ (aq) + $2Br^{}$ (aq). Learn how to balance chemical equations here, or read through these six examples of physical and chemical change. will dissolve in solution to form aqueous calcium two The ion product Q is analogous to the reaction quotient Q for gaseous equilibria. In like manner, there is a 1:1 molar ratio between dissolved AgBr and Br in solution. So if X refers to the concentration of calcium "Solubility and Solubility Products (about J. Chem. How do you calculate concentration in titration? At 298 K, the Ksp = 8.1 x 10-9. BaCO3 slightly dissolves in water according to the following equation: BaCO3(s) arrow Ba2+(aq) + CO32-(aq). 1 Answer. Legal. Temperature affects the solubility of both solids and gases but hasnt been found to have a defined impact on the solubility of liquids. Although the amount of solid Ca3(PO4)2 changes as some of it dissolves, its molar concentration does not change. Become a Study.com member to unlock this answer! Our experts can answer your tough homework and study questions. calcium two plus ions. The final solution is made If you decide that you prefer 2Hg+, then I cannot stop you. This creates a corrugated surface that presumably increases grinding efficiency. of calcium two plus ions and fluoride anions in solution is zero. (b) If the K_{ sp} for copper(II) carbonate is 1.4 times 10^{-10}, determine the concentration of Cu^{2+} in a saturated solution. What is the Keq What is the equilibrium constant for water? 3. 1998, 75, 1182-1185).". The Equilibrium constant expression for this reaction can be written as: Ksp = [BaBa +2 ] [SO 4-2] Recall pure solids (and pure liquids) are not included in an equilibrium constant expression. we need to make sure and include a two in front Second, determine if the
Solubility constant only deals with the products and it can be gotten from the concentration of the products.. Looking at the mole ratios, fluoride that dissolved. (Sometimes the data is given in g/L. Because the $K_s_p$ values are so small, there may be minor differences in their values depending on which source you use. Substitute these values into the solubility product expression to calculate, the molarity of ions produced in solution, the mass of salt that dissolves in 100 mL of water at 25C. a. adding Na_{2}S ( K_{sp} of NiS = 3 \cdot 10^{-20} ) b. adding Ca(NO_{3})_{2} ( K_{sp} of CaCO_{3} = 4.5 \cdot 10^{-9} ) c. adding K_{2}CO_{3} d. (a) Write the solubility product expression for CuCO_3 (copper(II) carbonate). To better organize out content, we have unpublished this concept. This would mean the $K_s_p$ unit would be different for every problem and would be difficult to solve, so in order to make it simpler, chemists generally drop $K_s_p$ units altogether. Consider the general dissolution reaction below (in aqueous solutions): \[\ce{aA(s) <=> cC(aq) + dD(aq)} \nonumber \]. In the case of AgBr, the value is 5.71 x 107 moles per liter. Then calculate the Ksp based on 2mol/L Ag+ and 1.5mol/L CO3^2-. And what are the $K_s_p$ units? lead(II) chloride, if 50.0 mL of a saturated solution of lead(II) chloride
How to calculate concentration in mol dm-3. Answer the following questions about solubility of AgCl(s). The solubility of calcite in water is 0.67 mg/100 mL. Why is X expressed in Molar and not in moles ? the Solubility of an Ionic Compound in a Solution that Contains a Common
are combined to see if any of them are deemed "insoluble" base on solubility
Check out our top-rated graduate blogs here: PrepScholar 2013-2018. $Ag_2CrO_4$ (s) 2$Ag^{+}$ (aq) + $CrO_4^2^{-}$ (aq), $Cu_3$ $(PO_4)^2$ (s) $3Cu^2^{+}$ (aq) + $2PO_4^3^{}$ (aq), $K_s_p$ = $[Cu^2^{+}]^3$ [$PO_4^3^$]$^2$. So I like to represent that by In this video, we'll use the Beer-Lambert law to calculate the concentration of KMnO in an unknown solution. 18: Solubility and Complex-Ion Equilibria, { "18.1:_Solubility_Product_Constant_Ksp" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.
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MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "26:_Structure_of_Organic_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "27:_Reactions_of_Organic_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "28:_Chemistry_of_The_Living_State" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "zz:_Back_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "showtoc:no", "license:ccbyncsa", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FGeneral_Chemistry%2FMap%253A_General_Chemistry_(Petrucci_et_al.