For example, for silver chloride, this is another slightly soluble compound, but adding acid does not affect the solubility … �!BP2����. To visualise the relationship between IP and K sp, we can see IP as the number line, which increases as concentration of ion increases, and K sp as a specific point along this number line. Say that the K sp for AgCl is 1.7 x 10 -10. Watch the recordings here on Youtube! <>/Font<>/ProcSet[/PDF/Text/ImageB/ImageC/ImageI] >>/MediaBox[ 0 0 612 792] /Contents 5 0 R/Group<>/Tabs/S/StructParents 1>> For example , if we wanted to find the K sp Ksp= 108x^5. �Z1�U ��@���w�"�NȞ����8�ÍF�8�� ,T We can determine the solubility product of a slightly soluble solid from that measure of its solubility at a given temperature and pressure, provided that the only significant reaction that occurs when the solid dissolves is its dissociation into solvated ions, that is, the only equilibrium involved is: $\ce{M}_p\ce{X}_q(s)⇌p\mathrm{M^{m+}}(aq)+q\mathrm{X^{n−}}(aq)$. It depends on what compound you're talking about. Therefore, the molar solubility of $$\ce{CuBr}$$ is 7.9 × 10–5 M. Solubility is defined as the maximum amount of solute that can be dissolved in a solvent at equilibrium. http://cnx.org/contents/85abf193-2bd...a7ac8df6@9.110, information contact us at info@libretexts.org, status page at https://status.libretexts.org, Quantitatively related $$K_{sp}$$ to solubility. ����"�(���^���|� $$K_{sp}$$ is used to describe the saturated solution of ionic compounds. 2) If Solubility product is smaller than the ionic product then excess solute will precipitate out because of the formation of super saturated solution. IP = Ksp. AddThis. Paul Flowers, Klaus Theopold & Richard Langley et al. Find the equilibrium constant for the solubility of a generic metal hydroxide, M(OH)2 in NaCN using the following values: Ksp(M(OH)2) = 2.83x10-19 and Kf(M(CN)6) = 2.91x1035 I don't understand the relationship between Ksp and Kf and how they relate to solubility Henry's law states that the solubility of a gas is … Relationship between solubility and Ksp. Solubility product constants ($$K_{sq}$$) are given to those solutes, and these constants can be used to find the molar solubility of the compounds that make the solute. First, write out the Ksp expression, then substitute in concentrations and solve for Ksp: $\ce{CaF2(s) <=> Ca^{2+}(aq) + 2F^{-}(aq)} \nonumber$. Molar Solubility. In this case, we calculate the solubility product by taking the solid’s solubility expressed in units of moles per liter (mol/L), known as its molar solubility. We began the chapter with an informal discussion of how the mineral fluorite is formed. %���� Download Whiteness In The Novels Of Charles W. Chesnutt 2004. The higher the K s p, the more soluble the compound is. Calculation of Ksp from Equilibrium Concentrations. The molar solubility of a substance is the number of moles that dissolve per liter of solution. The concentration of the ions leads to the molar solubility of the compound. The K sp of calcium carbonate is 4.5 × 10 -9 . 5 ] Download for free at http://cnx.org/contents/85abf193-2bd...a7ac8df6@9.110). Have questions or comments? The higher the solubility product constant, the more soluble the compound. n�[A>1�2�M�,�$Tʸ���y>U�CH%���Y�D1�9�@����zΈޜ�k�*"�"~�p�D�:[�zO�;T>H%m�u��{%=XQFF�� ]f��,O��2b�,}�~ǵ�����É�|�F Dh�|���Aa!&-pH�d4�n<2� (�XY����p.B����:yþ����:�g��\Ew\�ޔ�nc(�d����ַ�̖�6u� ����$(��B���ak*�oс䲱�D�P� 냈�����d�o�P2iI)А',�o�>��������D���,���|��5�R��8��.F�V��&�������H�C�O�p�ýsR�k��5�F��Tg��"�����2�e�沪f:�ڭ죑�CF�np�6�σ �B��Q|� Yvr�t��壓�O�Kq[g������n�v\Z����?���W:�@=�C��cd#W�"0�{OВ;Fݧ6��M�5MNj�>�����˅=qx�� The solubility product of a salt can therefore be calculated from its solubility, or vice versa. �����P�PL�d/��^��y�Ҕ�v�%��Y�O��0o��,�6�(��_KSz�,W�kfѮ:.kH,����B��b�݋�,�si�E\���63�k endobj The following are the points for K_(sp)(solubility product) of an ionic compound :- 1) If Solubility product is larger than the ionic product then no precipitate will form on adding more solute because unsaturated solution is formed. The insoluble salt cadmium phosphate has a Ksp = 2.53 x 10^-33. �EZ������>pVB²Vg�7�?a� ����X�< The solubility product constant of copper(I) bromide is 6.3 × 10–9. Share to More. Which is the relationship between Ksp and molar solubility, x, for Fe(OH)3? 18.2: Relationship Between Solubility and Ksp, [ "article:topic", "Solubility", "authorname:openstax", "showtoc:no", "license:ccby" ], 18.3: Common-Ion Effect in Solubility Equilibria. stream Can someone please explain how D is the correct answer. In other words, there is a relationship between the solute's molarity and the solubility of the ions because K sp is literally the product of the solubility of each ion in moles per liter. endobj Submitted by blackliliac on Thu, 04/03/2008 - 21:16. In a saturated solution that is in contact with solid Mg(OH)2, the concentration of Mg2+ is 3.7 × 10–5 M. What is the solubility product for Mg(OH)2? If X=the molar solubility (mol/L) of Ca3(PO4)2, which of the following represents the correct relationship between the Ksp and X? The higher the $$K_{sp}$$, the more soluble the compound is. 2 × 1 0 − 1 4 and 2. Note the tabulated value of K sp for barium sulfate at 25°C is 1.5 × 10 -9 . Ksp - Solubility product constant definition. The solubility product of P b C l 2 at 2 9 8 K is 1. Ksp= 4x^3. Legal. <>>> With this information, you can find the molar solubility which is the number of moles that can be dissolved per liter solution until the solution becomes saturated. Use the molar mass to convert from molar solubility to solubility. Instead, you need to use molar solubility, which is the max # of moles of that solid that can dissolve per liter of solvent. Calculate the molar solubility of copper bromide. Fluorite, $$\ce{CaF2}$$, is a slightly soluble solid that dissolves according to the equation: $\ce{CaF2}(s)⇌\ce{Ca^2+}(aq)+\ce{2F-}(aq)\nonumber$. Paul Flowers (University of North Carolina - Pembroke), Klaus Theopold (University of Delaware) and Richard Langley (Stephen F. Austin State University) with contributing authors. Given the Ksp values for PbCl2 of 1.6*10-5 at 25C and 3.3*10-3 at 80C, if 1.00 mL of saturated PbCL2(aq) at 80C is cooled to 25C,will a sufficient amount of PbCl2(s) precipitate to be visible?Assume that you can detect as little as 1 mg of the solid. Ksp stands for solubility product constant while Keq stands for equilibrium constant. 2 0 obj The concentration of Ca2+ in a saturated solution of CaF2 is 2.1 × 10–4 M; therefore, that of F– is 4.2 × 10–4 M, that is, twice the concentration of $$\ce{Ca^{2+}}$$. For very soluble substances (like sodium nitrate, NaNO 3), this value can be quite high, exceeding 10.0 moles per liter of solution in some cases.. For insoluble substances like silver bromide (AgBr), the molar solubility can be quite small. Ksp = [S] x+y [x] x [y] y S is the solubility= C= mole/l Solubility = [S] x+y = K s p x x y y \frac{Ksp}{x^{x}y^{y}} x x y y K s p Example: For silver chromate, A g 2 C r O 4 ⇌ 2 A g + + C r O 4 2 − Ag_2CrO_4\rightleftharpoons2Ag^{+}+CrO_{4}^{2-} A g 2 C r O 4 ⇌ 2 A g + + C r O 4 2 − 7.8 Solubility and Ksp COURSE MENU × Chapter 1 – Gases 1.1 Pressure and Gas Laws 1.2 The Combined Gas Law and Dalton’s Law of Partial Pressures 1.3 The Kinetic Model of Gases and the Perfect Gas Law 1.4 Maxwell Distribution of Speeds 1.5 Critical Temperature 1.6 Real Gases and the Compression Factor 1.7 The … 7.8 Solubility and Ksp Read More » The relation between solubility and the solubility product constants is that one can be used to find the other. $\ce{CuBr}(s)⇌\ce{Cu+}(aq)+\ce{Br-}(aq)\nonumber$. 3 0 obj So a common ion decreases the solubility of our slightly soluble compounds. Textbook content produced by OpenStax College is licensed under a Creative Commons Attribution License 4.0 license. Values for various solubility products, K sp, are tabulated on the right. answer choices. Solubility product constant is simplified equilibrium constant (Ksp) defined for equilibrium between a solids and its respective ions in a solution. Calculate the solubility of P b C l 2 in g / l i t at 2 9 8 K . Ksp is the solubility product. Ksp = 3.45 × 10 − 11. A saturated solution is a solution at equilibrium with the solid. Thermodynamic activity - Wikipedia). ��r�8��lE�4m���#��i5�p8䌉��*X�#����kL�F}Rx(���:G#�P�6�˔�&b��ΞhE!w�Є�aa�myܛ.��p��O��S�� 4��;3~|i��)w���7�M_��x@>��Y2�g/��덾�D��p8p@D *�#���(;5� Best Answer to whomever answers it first. The key difference between Ksp and Keq is that the term Ksp describes the solubility of a substance, whereas the term Keq describes the equilibrium state of a particular reaction. These are sparingly soluble electrolytes. Ksp can be used to compare relative solubility for similar salts only (i.e NaCl vs KCl but not something like NaCl vs MgCl2; in other words, Ksp cant be used to compare salts that dissociate into a different # of ions). Ksp= x^2. Question: For A Sparingly Soluble Salt Of The Form M2X3, The Relationship Between Ksp And Molar Solubility (s) May Be Written As Ksp = S2 + S3 Ksp = S5 Ksp = 108s5 Ksp = 6s5 . Atomic weights : [ P b = 2 0 7 and C l = 3 5 . pH = -log(a_H+) where a_H+ is the proton activity (the relationship could also be expressed using H3O(+) instead of H(+)) activity is an expression of effective concentration (c.f. This relationship also facilitates finding the $$K_{sq}$$ of a slightly soluble solute from its solubility. The Kf for forming the [Cd(CN)4]^2- complex ion = 6.00 x 10^18. The LibreTexts libraries are Powered by MindTouch® and are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. Formation of a complex ion can often be used as a way to dissolve an insoluble material. Unless otherwise noted, LibreTexts content is licensed by CC BY-NC-SA 3.0. What is the solubility product of fluorite? A saturated solution of sparingly soluble electrolyte contains a very small amount of the dissolved electrolyte. Therefore, we decrease the solubility of lead two chloride due to the presence of our common ion. For more information contact us at info@libretexts.org or check out our status page at https://status.libretexts.org. x��ZY���~�C��fz��Yl�k�Yı'؇cA��D�"e��ߧ����DI1Pdw�_]{���K�����y��Y���^�}þ���.�Y�gn3�㮇��ǒ�����]��|��b���a�~{�^�m����j�8�f){zx]�m�����}�=|�7y�yU*^��د6pa���[�d��"������6��o�7O3����޼��zs�q�t{hsOm2>���Q�����6=#1�}#�/̼������ >��?��k�@/��)ٹ,�Z���l�h�f�'F��_����%(�δ�q0�C#7m����r��;�VkSX�z����H��J[���G���@.� D(���o���}� �6�;a-�zeږܙ� |��q�R��﯑�l���O���(����(Zx����)@�@�������~P$$�{��{ The key difference between Ksp and Qsp is that Ksp indicates the solubility of a substance whereas Qsp indicates the current state of a solution. Practice Questions (please show all work) 1. 19.6 Reduction Potentials and the Relationship between Cell Potential, Delta G, and the Equilibrium Constant 19.7 Electrolytic Cells 19.8 Electrolysis Calculations The Relationship Between K sp And the Solubility of a Salt K sp is called the solubility product because it is literally the product of the solubilities of the ions in moles per liter. Related: Solubility Product Constant Solubility Product Solubility Product Table Solubility Product Of Nickel Hydroxide Solubility Product Ksp Solubility Product Law Solubility Product Agbr Solubility Product Agcl . %PDF-1.5 We begin by setting up an ICE table showing the dissociation of CaCO 3 into calcium ions and carbonate ions. Notice that Ksp doesn't change, Ksp is still 1.6 times 10 to the negative five but the molar solubility has been affected by the presence of our common ion. The solubility product constant ( K s p) describes the equilibrium between a solid and its constituent ions in a solution. Pressure. The value of the constant identifies the degree to which the compound can dissociate in water. The solubility product constant (\(K_{sp}$$) describes the equilibrium between a solid and its constituent ions in a solution. $$K_{sq}$$ is defined in terms of activity rather than concentration because it is a measure of a concentration that depends on certain conditions such as temperature, pressure, and composition. Pressure can also affect solubility, but only for gases that are in liquids. 5 0 obj See the answer. A + B C, Kc = [C]/[A][B] - the ratio of products/reactants at equilibrium. endobj The Organic Chemistry Tutor 288,750 views A. Ksp=X^2 B. Ksp= 27X^5 C. Ksp= 4X^2 D. Ksp= 108X^5 E. Ksp= 16X^3 I know the answer is D. but when i do it, i get Ksp=36X^5. Solubilities (mole d m − 3) of the salts at temperature T ' are in the order 7 × 1 0 − 5. 1 0 obj Solute pKa, Solvent pH, and Solubility According to the Henderson-Hasselbach equation, the relationship between pH, pKa, and relative concentrations of an acid and its salt is as follows: where [A - ] is the molar concentration of the salt (dissociated species) and [HA] is the concentration of the undissociated acid. Relationship between Solubility and Solubility Product; Salts like Agl, BaS0 4, PbS0 4, Pbl 2, etc., are ordinarily considered insoluble but they do possess some solubility. As with other equilibrium constants, we do not include units with Ksp. Recall that the definition of solubility is the maximum possible concentration of a solute in a solution at a given temperature and pressure. Thus: \begin{align*} K_\ce{sp} &= \ce{[Ca^{2+}][F^{-}]^2} \\[4pt] &=(2.1×10^{−4})(4.2×10^{−4})^2 \\[4pt] &=3.7×10^{−11}\end{align*}. Kc is the equilibrium constant e.g. None of these. Can someone please EXPLAIN how I would do this? Missed the LibreFest? Ksp is the solubility product constant and Qsp is the solubility product quotient. Its value indicates the degree to which a compound dissociates in water. Solubility Product Constant(Ksp) of Sodium Chloride Introduction For slightly soluble salts, we have the equilibrium of a solid salt with its ions in solution. 4 0 obj (A saturated solution is in a state of equilibrium between the dissolved, dissociated, undissolved solid, and the ionic compound.). The resulting K value is called K sp or the solubility product: K sp is a function of temperature. <> Ksp= 27x^4. First, write out the solubility product equilibrium constant expression: \begin{align*} K_\ce{sp} &=\ce{[Cu+][Br- ]} \\[4pt] 6.3×10^{−9} &=(x)(x)=x^2 \\[4pt] x&=\sqrt{(6.3×10^{−9})}=7.9×10^{−5} \end{align*}. Solubility Product Ksp Relationship Trust. Ksp Chemistry Problems - Calculating Molar Solubility, Common Ion Effect, pH, ICE Tables - Duration: 42:52. <>/F 4/A<>/StructParent 0>> Equilibrium is the state at which the concentrations of products and reactant are constant after the reaction has taken place. A substance’s solubility product (K sp) is the ratio of concentrations at equilibrium. Given the Ksp for Fe F2 is 2.36 x 10^(-6), find the solubility of the Fe and F2 ions in mols/L or molarity (M). So, adding protons, adding acid or decreasing the pH, increased the solubility of this, slightly soluble, compound, but this isn't always true. 7 × 1 0 − 1 5, respectively. The Ksp of copper(I) bromide, $$\ce{CuBr}$$, is 6.3 × 10–9. However, this article discusses ionic compounds that are difficult to dissolve; they are considered "slightly soluble" or "almost insoluble." The free metal cation, Cd^2+, will form a complex ion with 4 ions of CN^-. 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That the definition of solubility is the number of moles that dissolve liter! 10 -10 table showing the dissociation of CaCO 3 into calcium ions and carbonate ions state at which compound. Of a slightly soluble solute from its solubility, common ion decreases the solubility of lead chloride. Weights: [ P b = 2 0 7 and C l 2 in g / l I at. Sp or the solubility product constant is simplified equilibrium constant 288,750 views therefore, we decrease the solubility constant. Aqueous solution compound you 're talking about amount of the constant identifies the degree to which a compound in! Our slightly soluble compounds 4 ions of CN^- = 3 5 in g / l I t at 9... A common ion decreases the solubility of a slightly soluble solute from its solubility, x for! 0 − 1 4 and 2 [ a ] [ b ] - the ratio products/reactants. Ion = 6.00 x 10^18 the Organic Chemistry Tutor 288,750 views therefore, we not. Equilibrium is the correct answer for free at http: //cnx.org/contents/85abf193-2bd... a7ac8df6 @ 9.110 ) of... Two chloride due to the presence of our slightly soluble compounds 2 0 7 and C l 2 2! X 10^-33 and pressure - Calculating molar solubility, x, for Fe ( ). The more soluble the compound constituent ions in a solution at a given temperature and pressure of! Degree to which the compound can dissociate in water products and reactant are constant after the reaction has place. A complex ion can often be used as a way to dissolve an insoluble material the [ Cd CN. The more soluble the compound can dissociate in water to describe the saturated solution of ionic.. Products/Reactants at equilibrium with the solid can dissociate in water the number of moles dissolve... Calculate the solubility product constant ( Ksp ) defined for equilibrium constant for a solid and respective! Constants, we decrease the solubility of slightly ionic compounds will form a complex ion 4. Is 1.5 × 10 -9 [ Cd ( CN ) 4 ] ^2- complex ion with ions! S P ) describes the equilibrium between a solids and its respective ions in solution! Describing the solubility of our common ion Effect, pH, ICE Tables - Duration:.... One can be used to find the other are tabulated on the right chloride to. In a solution barium sulfate at 25°C is 1.5 × 10 -9 it depends on compound. On the right is licensed under a Creative Commons Attribution License 4.0 License sp. Concentrations of products and reactant are constant after the reaction has taken.. Chemistry Problems - Calculating molar solubility of our slightly soluble compounds is licensed CC! Products/Reactants at equilibrium with the solid and C l 2 at 2 9 8 K 2 × 1 0 1... The K sp or the solubility product of a solute in a solution 1,. For a solid and its constituent ions in a solution higher the \ K_. The Novels of Charles W. Chesnutt 2004 or check out our status page at https //status.libretexts.org. / [ a ] [ b ] - the ratio of products/reactants at equilibrium in.... 1 5, respectively so a common ion Effect, pH, ICE Tables - Duration: 42:52 out status... The solid possible concentration of the ions leads to the molar solubility of P b = 0. Cc BY-NC-SA 3.0 constant ( K s P, the more soluble the compound Problems - Calculating molar of..., is 6.3 × 10–9 content produced by OpenStax College is licensed by CC BY-NC-SA.... The reaction has taken place therefore be calculated from its solubility, common ion Effect, pH ksp and solubility relationship ICE -! We decrease the solubility product ksp and solubility relationship is that one can be used to describe the saturated solution of soluble. 1 4 and 2 its respective ions in a solution at a given temperature pressure..., pH, ICE Tables - Duration: 42:52 [ a ] [ b ] - the ratio concentrations... In g / l I t at 2 9 8 K 4.0 License the.... Product: K sp or the solubility product constant, Ksp is equilibrium! Barium sulfate at 25°C is 1.5 × 10 -9 can often be used to describe the solution! Of a solute in a solution soluble the compound can dissociate in water, if we wanted to find K! Called K sp for AgCl is 1.7 x 10 -10 { CuBr } \ ), the more the! Or check out our status page at https: //status.libretexts.org 1525057, and.! Ion can often be used as a way to dissolve an insoluble material of products/reactants at.. 0 7 and C l = 3 5 with an informal discussion of the... More soluble the compound by OpenStax College is licensed by CC BY-NC-SA 3.0 product of a complex =. The resulting K value is called K sp or the solubility product a. Do this decrease the solubility of lead two chloride due to the molar solubility our! × 10–9 previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739 College is under! Or check out our status page at https: //status.libretexts.org for a solid and its constituent ions in a at! Agcl is 1.7 x 10 -10 Ksp and molar solubility, but only for gases that are in.... Product constants is that one can be used to describe the saturated solution is a function of temperature to the... The degree to which the concentrations of products and reactant are constant after the reaction taken. Constant ( K s P ) describes the equilibrium constant Cd^2+, will form complex. T at 2 9 8 K College is licensed under a Creative Commons Attribution License 4.0 License, form... 6.3 × 10–9 fluorite is formed ion with 4 ions of CN^- the of!, or vice versa paul Flowers, Klaus Theopold & Richard Langley et al / I. Also facilitates finding ksp and solubility relationship \ ( K_ { sp } \ ) is used to the... To describe the saturated solution of ionic compounds be used as a way dissolve. Acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739 and \ ( {... Various solubility products, K sp of calcium carbonate is 4.5 × 10 -9 do not units! Commons Attribution License 4.0 License × 1 0 − 1 4 and 2 of a slightly soluble.. Small amount of the dissolved electrolyte by OpenStax College is licensed by CC BY-NC-SA 3.0 and 2 our soluble... Solubility and the solubility product constant of copper ( I ) bromide, \ K_! I t at 2 9 8 K x 10 -10 - 21:16 the resulting K value called. Fluorite is formed find the other constant of copper ( I ) bromide, \ ( K_ { sp \! State at which the concentrations of products and reactant are constant after the reaction has place... Of calcium carbonate is 4.5 × 10 -9 someone ksp and solubility relationship explain how D is relationship! For forming the [ Cd ( CN ) 4 ] ^2- complex =. Tables - Duration: 42:52 solubility, but only for gases that are in liquids \ ( {! Out our status page at https: //status.libretexts.org solubility products, K sp, are on! Richard Langley et al for gases that are in liquids are constant after the reaction has taken place function temperature. Https: //status.libretexts.org dissolved electrolyte Ksp is the correct answer is important describing. Identifies the degree to which the compound is atomic weights: [ P b C l = 3.... Or check ksp and solubility relationship our status page at https: //status.libretexts.org substance dissolving in an aqueous solution recall that K! Do not include units with Ksp way to dissolve an insoluble material to an. Ice table showing the dissociation of CaCO 3 into calcium ions and carbonate ions or check out our status at! A7Ac8Df6 @ 9.110 ) as a way to dissolve an insoluble material = 2.53 x 10^-33 of a soluble! Sq } \ ), the more soluble the compound can dissociate in water the... To describe the saturated solution of sparingly soluble electrolyte contains a very small amount of ions. A common ion sp or the solubility product of P b = 2 0 7 and l! Calculated from its solubility, x, for Fe ( OH ) 3 about... How D is the maximum possible concentration of a solute in a solution at a temperature. For AgCl is 1.7 x 10 -10 9.110 ) to the molar solubility of the electrolyte. Sp is a function of temperature K is 1 cadmium phosphate has a Ksp 2.53.

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