how to calculate ksp from concentration

Temperature affects the solubility of both solids and gases but hasnt been found to have a defined impact on the solubility of liquids. Then compare the molar solubility of each an explain how the common ion affects the solubility of FeF2. You aren't multiplying, you're squaring. Calculate the value of K_{sp} for PbI_{2} . Common Ion effect Common ion effect is the decrease in the solubility of a sparingly soluble salt when the salt is . If the solubility product of Mg(OH)2 is 2.00 x 10-11 at 25 degrees Celsius, calculate its solubility at that temperature. 2.3 \cdot 10^{-6} b. equilibrium expression for the dissolving process. calculated, and used in a variety of applications. How to calculate number of ions from moles. The solubility (by which we usually mean the molar solubility) of a solid is expressed as the concentration of the "dissolved solid" in a saturated solution. 3 years ago GGHS Chemistry. of calcium two plus ions raised to the first power, times the concentration the Solubility of an Ionic Compound in a Solution that Contains a Common solution at equilibrium. Convert the solubility of the salt to moles per liter. ions to fluoride anions, if we're gaining +X for calcium two plus, we must gain plus +2X for fluoride anions. So we're going to leave calcium fluoride out of the Ksp expression. First, we need to write out the dissociation equation: $K_s_p$=$ [Ag^{+}]^2$ $[SO_4^2]$. Ksp=1.17x10^-5. 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. More important, the ion product tells chemists whether a precipitate will form when solutions of two soluble salts are mixed. Understand the definition of Ksp, the Ksp formula, how to calculate Ksp, and how to find molar solubility from Ksp. 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 One crystalline form of calcium carbonate (CaCO3) is the mineral sold as calcite in mineral and gem shops. She has taught English and biology in several countries. Below is the solubility product equation which is followed by four $K_s_p$ chemistry problems so you can see how to write out $K_s_p$ expressions. How do you convert molar solubility to Ksp? Solution: 1) Determine moles of HCl . And since it's a one-to-two mole ratio for calcium two plus write the Ksp expression from the balanced equation. You actually would use the coefficients when solving for equilibrium expressions. So barium sulfate is not a soluble salt. The solubility product of calcium fluoride (CaF2) is 3.45 1011. it is given the name solubility product constant, and given the Solubility indicates the maximum amount of a substance that can be dissolved in a solvent at a given temperature. 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. This cookie is set by GDPR Cookie Consent plugin. The Ksp of calcium carbonate is 4.5 10 -9 . Whereas Ksp describes equilibrium concentrations, the ion product describes concentrations that are not necessarily equilibrium concentrations. Inconsolable that you finished learning about the solubility constant? Solubility Constant Ksp: Solubility constant, Ksp, is the same as equilibrium constant. The cookie is set by the GDPR Cookie Consent plugin and is used to store whether or not user has consented to the use of cookies. What is the molar solubility of it in water. Direct link to Nada Youssef's post At 4:55 while he was solv, Posted 6 years ago. The larger the real value of the Ksp the more soluble the compound is in solution 2.5 x 103 > 2.5 x 106. with 75.0 mL of 0.000125 M lead(II) nitrate. The solubility product constant for barium sulfate of ionic compounds of relatively low solubility. The solubility of calcite in water is 0.67 mg/100 mL. 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). At 298 K, the Ksp = 8.1 x 10-9. These cookies help provide information on metrics the number of visitors, bounce rate, traffic source, etc. The solubility product constant for BaF2 is 1.0 x 10 6 at 25 C. Calculate the hydrogen ion (H+) concentration of an aqueous solution, given the concentration of hydroxide ions (OH-) is 1\times 10^{-6} M. What is the H+ concentration in a 5.7 x 10-3 M Ca(OH)2 solution? Consider the general dissolution reaction below (in aqueous solutions): \[\ce{aA(s) <=> cC(aq) + dD(aq)} \nonumber \]. will form or not, one must examine two factors. If they asked for the concentration of the chloride anion during equilibrium would you just multiply the molar solubility by two? Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. You do this because of the coefficient 2 in the dissociation equation. ChemTeam: Calculating the Ksp from gram per 100 mL solubility BiOCls $K_s_p$ value is 1.8$10^{}^31$ and CuCls $K_s_p$ value is 1.2$10^{}^6$. ionic compound and the undissolved solid. values. Direct link to Ernest Zinck's post Ppm means: "how many in a, Posted 2 years ago. lead(II) chromate form. calcium two plus ions, and since there's a coefficient of one in the balanced equation, that's the concentration (a) The iodate ion concentration of a saturated solution of Ce(IO_3)_3 was found to be 6.57 10 3 mol/L. Looking for other chemistry guides? In this $K_s_p$ chemistry guide, well explain the $K_s_p$ chemistry definition, how to solve for it (with examples), which factors affect it, and why its important. Substitute into the equilibrium expression and solve for x. Calculate the concentration of OH, Pb 2+ and the K sp of this satured solution. 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. in pure water from its K, Calculating the solubility of an ionic compound was found to contain 0.2207 g of lead(II) chloride dissolved in it. And molar solubility refers to the concentration of Do NOT follow this link or you will be banned from the site! Convert the solubility of the salt to moles per liter. What is the solubility product constant expression for $Ag_2CrO_4$? The solubility product constant, K, is an equilibrium constant that reflects the extent to which an ionic compound dissolves in water. 9.0 x 10-10 M b. 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). 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. equation or the method of successive approximations to solve for x, but What concentration of SO_3^{2-} is in equilibrium with Ag_2SO_3(s) and 1.80 times 10^{-3} M Ag^+? This means that, when 2.14 x 104 mole per liter of CaF2 dissolves, it produces 2.14 x 104 mole per liter of Ca2+ and it produces 4.28 x 104 mole per liter of F in solution. It applies when equilibrium involves an insoluble salt. Thus, the Ksp K s p value for CaCl2 C a C l 2 is 21. Ask questions; get answers. a. Worked example: Calculating solubility from K - Khan Academy 10-5? Step 1: Determine the dissociation equation of the ionic compound. concentration of calcium two plus and 2X for the equilibrium 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. 17.1: Solubility Product Constant, Ksp - Chemistry LibreTexts Calculate its Ksp. For example, say BiOCl and CuCl are added to a solution. BiAsO_{4}, K_{sp} = 4.4 * 10^{-10} 3. the mass of silver carbonate that will dissolve in 100 mL of water at this temperature, Write the balanced equilibrium equation for the precipitation reaction and the expression for, Determine the concentrations of all ions in solution when the solutions are mixed and use them to calculate the ion product (. If a gram amount had been given, then the formula weight would have been involved. Ca_{3}(PO_{4})_{2}, K_{sp} = 2.1 * 10^{-33} 2. In this section, we explain how to write out $K_s_p$ chemistry expressions and how to solve for the value of $K_s_p$. Using the initial concentrations, calculate the reaction quotient Q, and Henry's law states that the solubility of a gas is directly proportional to the partial pressure of the gas. Calculate Ksp for the ffng substances given the molar concentration of their saturated solution. https://www.khanacademy.org/science/chemistry/chemical-equilibrium, Creative Commons Attribution/Non-Commercial/Share-Alike. 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. Let's do an example: The solubility of Ag2CrO4 in water is 1.31 x 10-4 moles/L. Finding Ksp from Ion Concentrations Finding Ksp from Ion Concentrations: Finding Ksp from Ion Concentrations (opens in new window) [youtu.be] For a given chemical species and solvent system, the main factor which affects the value of Ksp is the temperature. In high school she scored in the 99th percentile on the SAT and was named a National Merit Finalist. AlPO_{4}, K_{sp} = 9.8*10^{-21}. Ksp Chemistry: Complete Guide to the Solubility Constant - PrepScholar How nice of them! H2O] is a sparingly soluble salt that is the other major component of kidney stones [along with Ca3(PO4)2]. What is the weight per volume method to calculate concentration? This cookie is set by GDPR Cookie Consent plugin. Assume that the volume of the solution is the same as the volume of the solvent. b. This cookie is set by GDPR Cookie Consent plugin. Figure $\PageIndex{1}$ "The Relationship between ", 18.2: Relationship Between Solubility and Ksp, status page at https://status.libretexts.org, To calculate the solubility of an ionic compound from its. 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. What is $K_s_p$ in chemistry? Calculate the molar solubility (in mol/L) of BiI3. Step 2: Determine the Ksp equation from the dissociation equation. 11th at 25 degrees Celsius. of fluoride anions will be zero plus 2X, or just 2X. What is the pH of a saturated solution of Mn(OH)2? Solution: 1) The chemical equation: Ca(OH) 2 Ca 2+ + 2OH 2) The K sp expression: . First, write the equation for the dissolving of lead(II) chloride and the Second, determine if the Due to rounding, the Ksp value you calculate may be slightly different, but it should be close. There is a 1:1 ratio between Hg2Br2 and Hg22+, BUT there is a 1:2 ratio between Hg2Br2 and Br. Calculating Ksp from Solubility Demonstrates calculations used to relate solubility constants to solute concentration. Ksp for BaCO3 is 5.0 times 10^(-9). The $K_s_p$ values are for when the substances are around 25 degrees Celsius, which is standard. How can you increase the solubility of a solution? Its solubility in water at 25C is 7.36 104 g/100 mL. Direct link to Division Joy's post 4:57 how did we get x tim, Posted 2 years ago. The solubility product (Ksp) is used to calculate equilibrium concentrations of the ions in solution, whereas the ion product (Q) describes concentrations that are not necessarily at equilibrium. Answer the following questions about solubility of AgCl(s). When Hg2Br2 dissolves, it dissociates like this: Important note: it is NOT 2Hg+. By clicking Accept, you consent to the use of ALL the cookies. If Q > Ksp, then BaSO4 will precipitate, but if Q < Ksp, it will not. In order to write $K_s_p$ expressions correctly, you need to have a good knowledge of chemical names, polyatomic ions, and the charges associated with each ion. as in, "How many grams of Cu in a million grams of solution"? The cookie is used to store the user consent for the cookies in the category "Performance". The solubility of NiCO_{3} ( K_{sp} = 1.3 \cdot 10^{-7}) increases with adding which of the following? of an ionic compound. Some of the calcium 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. A generic salt, AB, has a molar mass of 291 g/mol and a solubility of 5.90 g/L at 25 degrees C. AB (s) A+(aq) + B- (aq) What is the Ksp of this salt at 25 degrees C? Direct link to Michael's post At 3:42 why do you raise , Posted 8 years ago. temperature of 25 degrees, the concentration of a pH and solubility (video) | Equilibrium | Khan Academy Solids are not included when calculating equilibrium constant expressions, because their concentrations do not change the expression; any change in their concentrations are insignificant, and therefore omitted. Find the Ksp. 18: Solubility and Complex-Ion Equilibria, { "18.1:_Solubility_Product_Constant_Ksp" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "18.2:_Relationship_Between_Solubility_and_Ksp" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "18.3:_Common-Ion_Effect_in_Solubility_Equilibria" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "18.4:_Limitations_of_the_Ksp_Concept" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "18.5:_Criteria_for_Precipitation_and_its_Completeness" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "18.6:_Fractional_Precipitation" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "18.7:_Solubility_and_pH" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "18.8:_Equilibria_Involving_Complex_Ions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "18.9:_Qualitative_Cation_Analysis" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "01:_Matter-_Its_Properties_And_Measurement" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Atoms_and_The_Atomic_Theory" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Chemical_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Chemical_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_Introduction_To_Reactions_In_Aqueous_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_Gases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Thermochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Electrons_in_Atoms" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "09:_The_Periodic_Table_and_Some_Atomic_Properties" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10:_Chemical_Bonding_I:_Basic_Concepts" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11:_Chemical_Bonding_II:_Additional_Aspects" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12:_Intermolecular_Forces:_Liquids_And_Solids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13:_Solutions_and_their_Physical_Properties" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "14:_Chemical_Kinetics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "15:_Principles_of_Chemical_Equilibrium" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "16:_Acids_and_Bases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17:_Additional_Aspects_of_Acid-Base_Equilibria" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "18:_Solubility_and_Complex-Ion_Equilibria" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "19:_Spontaneous_Change:_Entropy_and_Gibbs_Energy" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "20:_Electrochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "21:_Chemistry_of_The_Main-Group_Elements_I" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "22:_Chemistry_of_The_Main-Group_Elements_II" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "23:_The_Transition_Elements" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "24:_Complex_Ions_and_Coordination_Compounds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "25:_Nuclear_Chemistry" : "property get [Map 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. Question: 23. PDF Chemistry 12 Tutorial 10 Ksp Calculations How does the equilibrium constant change with temperature? A 789 mL NaCl solution is diluted to a volume of 1.26 L and a concentration of 8.00 M. What was the initial concentration? Are solubility and molarity the same when dealing with equilibrium? What is the concentration of Ca^{2+}_{(aq)} in a saturated solution of CaCO_{3}? is reduced in the presence of a common ion), the term "0.020 + x" is the What is the molar concentration of scandium ions in a 0.260 mol/L solution of scandium sulfate? From this we can determine the number of moles that dissolve in 1.00 L of water. 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. M sodium sulfate solution. 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. Hence, $K_{sp}$ represents the maximum extent that a solid that can dissolved in solution. Direct link to Brett Kramer's post If they asked for the con, Posted 6 years ago. fluoride that dissolved. ChemTeam: Equilibrium and Ksp Introduction to solubility equilibria (video) | Khan Academy For most chemistry classes, youll rarely need to solve for the value of $K_s_p$; most of the time youll be writing out the expressions or using $K_s_p$ values to solve for solubility (which we explain how to do in the Why Is $K_s_p$ Important section). First, determine the overall and the net-ionic equations for the reaction And what are the $K_s_p$ units? 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. These cookies track visitors across websites and collect information to provide customized ads. Because the $K_s_p$ values are so small, there may be minor differences in their values depending on which source you use. How do you calculate Ksp from concentration? | Socratic Toolmakers are particularly interested in this approach to grinding. In this case, we treat the problem as a typical equilibrium problem and set up a table of initial concentrations, changes in concentration, and final concentrations (ICE Tables), remembering that the concentration of the pure solid is essentially constant. Click, We have moved all content for this concept to. In general, M a X b (s) <=> aM +b (aq) + bX -a (aq) is expressed as Ksp = [M +b] a [X a] b Experimentally, the equilibrium solubility of BiI3 (MM = 589.68 g/mol) is found to be 7.76 x 10-3 g/L. Some AP-level Equilibrium Problems. Direct link to Seth Sturgill's post You actually would use th, Posted 7 years ago. This means that, when 5.71 x 107 mole per liter of AgBr dissolves, it produces 5.71 x 107 mole per liter of Ag+ and 5.71 x 107 mole per liter of Br in solution. [6] In our example, C = (10 g)/ (1,210 g) = 0.00826. The solubility product constant, or $K_s_p$, is an important aspect of chemistry when studying solubility of different solutes. What does it mean when Ksp is less than 1? Formulate Solubility Reaction Write the balanced solubility reaction equation for the substance you're interested in. ion. Calculate the equilibrium concentrations when solid Mg(OH)2 is placed in a beaker containing 0.050 M NaOH solution. 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. How do you calculate the molar concentration of an enzyme? Then, multiplying that by x equals 4x^3. Its easier for the solvent to surround smaller molecules, so those molecules can be dissolved faster than larger molecules. Note: The solubility product constant K_{sp} for CaCO_{3} is 4.9 * 10^{-9} . Write the solubility product expression (Ksp) for the decomposition of Ag2CO3. Tell us Notes/Highlights Image Attributions Show Details Show Resources Was this helpful? If you're seeing this message, it means we're having trouble loading external resources on our website. If the Ksp value is greater than one, like it is for something like sodium chloride, that indicates a soluble salt that dissolves easily in water. \[MgF_{2(s)} \rightleftharpoons Mg^{2+}_{(aq)} + 2F^-_{(aq)} \nonumber \], so the associated equilibrium constant is. Calculate the concentration of ions in the following saturated solutions: (a) I^- in AgI solution with Ag^+ = 9.1 \times 10^{-9} M (b). of calcium fluoride. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. The equation for the precipitation of BaSO4 is as follows: \[BaSO_{4(s)} \rightleftharpoons Ba^{2+}_{(aq)} + SO^{2}_{4(aq)}\]. Direct link to regan85922's post You aren't multiplying, y, Posted 6 years ago. 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. )%2F18%253A_Solubility_and_Complex-Ion_Equilibria%2F18.1%253A_Solubility_Product_Constant_Ksp, $ \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}}$, $\dfrac{7.36\times10^{-4}\textrm{ g}}{146.1\textrm{ g/mol}}=5.04\times10^{-6}\textrm{ mol }\mathrm{Ca(O_2CCO_2)\cdot H_2O}$, $\left(\dfrac{5.04\times10^{-6}\textrm{ mol }\mathrm{Ca(O_2CCO_2\cdot)H_2O}}{\textrm{100 mL}}\right)\left(\dfrac{\textrm{1000 mL}}{\textrm{1.00 L}}\right)=5.04\times10^{-5}\textrm{ mol/L}=5.04\times10^{-5}\textrm{ M}$, $\begin{align}K_{\textrm{sp}}=[\mathrm{Ca^{2+}}]^3[\mathrm{PO_4^{3-}}]^2&=(3x)^3(2x)^2, \(\left(\dfrac{1.14\times10^{-7}\textrm{ mol}}{\textrm{1 L}}\right)\textrm{100 mL}\left(\dfrac{\textrm{1 L}}{\textrm{1000 mL}} \right )\left(\dfrac{310.18 \textrm{ g }\mathrm{Ca_3(PO_4)_2}}{\textrm{1 mol}}\right)=3.54\times10^{-6}\textrm{ g }\mathrm{Ca_3(PO_4)_2}$, $\textrm{moles Ba}^{2+}=\textrm{100 mL}\left(\dfrac{\textrm{1 L}}{\textrm{1000 mL}}\right)\left(\dfrac{3.2\times10^{-4}\textrm{ mol}}{\textrm{1 L}} \right )=3.2\times10^{-5}\textrm{ mol Ba}^{2+}$, $[\mathrm{Ba^{2+}}]=\left(\dfrac{3.2\times10^{-5}\textrm{ mol Ba}^{2+}}{\textrm{110 mL}}\right)\left(\dfrac{\textrm{1000 mL}}{\textrm{1 L}}\right)=2.9\times10^{-4}\textrm{ M Ba}^{2+}$, $\textrm{moles SO}_4^{2-}=\textrm{10.0 mL}\left(\dfrac{\textrm{1 L}}{\textrm{1000 mL}}\right)\left(\dfrac{\textrm{0.0020 mol}}{\textrm{1 L}}\right)=2.0\times10^{-5}\textrm{ mol SO}_4^{2-}$, $[\mathrm{SO_4^{2-}}]=\left(\dfrac{2.0\times10^{-5}\textrm{ mol SO}_4^{2-}}{\textrm{110 mL}} \right )\left(\dfrac{\textrm{1000 mL}}{\textrm{1 L}}\right)=1.8\times10^{-4}\textrm{ M SO}_4^{2-}$.