Adding a common ion decreases solubility, as the reaction shifts toward the left to relieve the stress of the excess product. The common ion effect is an effect that suppresses the ionization of an electrolyte when another electrolyte (which contains an ion which is also present in the first electrolyte, i.e. For example, when \(\ce{AgCl}\) is dissolved into a solution already containing \(\ce{NaCl}\) (actually \(\ce{Na+}\) and \(\ce{Cl-}\) ions), the \(\ce{Cl-}\) ions come from the ionization of both \(\ce{AgCl}\) and \(\ce{NaCl}\). The equilibrium constant remains the same because of the increased concentration of the chloride ion. The common ion effect describes an ion's effect on the solubility equilibrium of a substance. This is the common ion effect. By the 1:1 stochiometry between silver ion and chloride ion, the [Ag+] is 's.' The common ion effect describes how a common ion can suppress the solubility of a substance. Solution in 0.100 M \(\ce{NaCl}\) solution: \[\ce{[Pb^{2+}]} = 0.0017 \, M \label{6}\nonumber \]. As before, define s to be the concentration of the lead (II) ions. The reaction then shifts right, causing the denominator to increase, decreasing the reaction quotient and pulling towards equilibrium and causing \(Q\) to decrease towards \(K\). When H. The common ion effect is a decrease in the solubility of a weak electrolyte by adding a common ion. Know more about this effect as we go through its concepts and definitions. This effect can be exploited in a number of ways. It is a consequence of Le Chatlier's principle (or the Equilibrium Law). & &&= && &&\mathrm{\:0.40\: M}\nonumber Calculate the solubility of silver carbonate in a 0.25 M solution of sodium carbonate. Why does the common ion effect decrease solubility? Notice that at the end of the video, excess chloride ions are added to the solution, causing an equilibrium shift to the side of lead chloride. The equilibrium constant, \(K_b=1.8 \times 10^{-5}\), does not change. If you add sodium chloride to this solution, you have both lead(II) chloride and sodium chloride containing the chlorine anion. Therefore, the overall molarity of Cl- would be 2s + 0.1, with 2s referring to the contribution of the chloride ion from the dissociation of lead chloride. In the case of hydrogen sulphide, which is a weak electrolyte, there occurs a partial ionization of this compound in an aqueous medium. Learn Uses, Structure, Formula & Melting Point, Silver Chloride: Learn its Structure, Chemical Formula, Properties, & Uses. NCERT Solutions Class 12 Business Studies, NCERT Solutions Class 12 Accountancy Part 1, NCERT Solutions Class 12 Accountancy Part 2, NCERT Solutions Class 11 Business Studies, NCERT Solutions for Class 10 Social Science, NCERT Solutions for Class 10 Maths Chapter 1, NCERT Solutions for Class 10 Maths Chapter 2, NCERT Solutions for Class 10 Maths Chapter 3, NCERT Solutions for Class 10 Maths Chapter 4, NCERT Solutions for Class 10 Maths Chapter 5, NCERT Solutions for Class 10 Maths Chapter 6, NCERT Solutions for Class 10 Maths Chapter 7, NCERT Solutions for Class 10 Maths Chapter 8, NCERT Solutions for Class 10 Maths Chapter 9, NCERT Solutions for Class 10 Maths Chapter 10, NCERT Solutions for Class 10 Maths Chapter 11, NCERT Solutions for Class 10 Maths Chapter 12, NCERT Solutions for Class 10 Maths Chapter 13, NCERT Solutions for Class 10 Maths Chapter 14, NCERT Solutions for Class 10 Maths Chapter 15, NCERT Solutions for Class 10 Science Chapter 1, NCERT Solutions for Class 10 Science Chapter 2, NCERT Solutions for Class 10 Science Chapter 3, NCERT Solutions for Class 10 Science Chapter 4, NCERT Solutions for Class 10 Science Chapter 5, NCERT Solutions for Class 10 Science Chapter 6, NCERT Solutions for Class 10 Science Chapter 7, NCERT Solutions for Class 10 Science Chapter 8, NCERT Solutions for Class 10 Science Chapter 9, NCERT Solutions for Class 10 Science Chapter 10, NCERT Solutions for Class 10 Science Chapter 11, NCERT Solutions for Class 10 Science Chapter 12, NCERT Solutions for Class 10 Science Chapter 13, NCERT Solutions for Class 10 Science Chapter 14, NCERT Solutions for Class 10 Science Chapter 15, NCERT Solutions for Class 10 Science Chapter 16, NCERT Solutions For Class 9 Social Science, NCERT Solutions For Class 9 Maths Chapter 1, NCERT Solutions For Class 9 Maths Chapter 2, NCERT Solutions For Class 9 Maths Chapter 3, NCERT Solutions For Class 9 Maths Chapter 4, NCERT Solutions For Class 9 Maths Chapter 5, NCERT Solutions For Class 9 Maths Chapter 6, NCERT Solutions For Class 9 Maths Chapter 7, NCERT Solutions For Class 9 Maths Chapter 8, NCERT Solutions For Class 9 Maths Chapter 9, NCERT Solutions For Class 9 Maths Chapter 10, NCERT Solutions For Class 9 Maths Chapter 11, NCERT Solutions For Class 9 Maths Chapter 12, NCERT Solutions For Class 9 Maths Chapter 13, NCERT Solutions For Class 9 Maths Chapter 14, NCERT Solutions For Class 9 Maths Chapter 15, NCERT Solutions for Class 9 Science Chapter 1, NCERT Solutions for Class 9 Science Chapter 2, NCERT Solutions for Class 9 Science Chapter 3, NCERT Solutions for Class 9 Science Chapter 4, NCERT Solutions for Class 9 Science Chapter 5, NCERT Solutions for Class 9 Science Chapter 6, NCERT Solutions for Class 9 Science Chapter 7, NCERT Solutions for Class 9 Science Chapter 8, NCERT Solutions for Class 9 Science Chapter 9, NCERT Solutions for Class 9 Science Chapter 10, NCERT Solutions for Class 9 Science Chapter 11, NCERT Solutions for Class 9 Science Chapter 12, NCERT Solutions for Class 9 Science Chapter 13, NCERT Solutions for Class 9 Science Chapter 14, NCERT Solutions for Class 9 Science Chapter 15, NCERT Solutions for Class 8 Social Science, NCERT Solutions for Class 7 Social Science, NCERT Solutions For Class 6 Social Science, CBSE Previous Year Question Papers Class 10, CBSE Previous Year Question Papers Class 12, Important Questions For Class 12 Chemistry, Important Questions For Class 11 Chemistry, Important Questions For Class 10 Chemistry, Important Questions For Class 9 Chemistry, Important Questions For Class 8 Chemistry, Important Questions For Class 7 Chemistry, Important Questions For Class 6 Chemistry, Class 12 Chemistry Viva Questions With Answers, Class 11 Chemistry Viva Questions With Answers, Class 10 Chemistry Viva Questions With Answers, Class 9 Chemistry Viva Questions With Answers, CBSE Previous Year Question Papers Class 10 Science, CBSE Previous Year Question Papers Class 12 Physics, CBSE Previous Year Question Papers Class 12 Chemistry, CBSE Previous Year Question Papers Class 12 Biology, ICSE Previous Year Question Papers Class 10 Physics, ICSE Previous Year Question Papers Class 10 Chemistry, ICSE Previous Year Question Papers Class 10 Maths, ISC Previous Year Question Papers Class 12 Physics, ISC Previous Year Question Papers Class 12 Chemistry, ISC Previous Year Question Papers Class 12 Biology, JEE Main 2023 Question Papers with Answers, JEE Main 2022 Question Papers with Answers, JEE Advanced 2022 Question Paper with Answers, The common ion effect can be used to obtain drinking water from aquifers (underground layer of water mixed with permeable rocks or other unconsolidated materials) containing chalk or limestone. This is because acetic acid is a weak acid whereas sodium acetate is a strong electrolyte. Some of our partners may process your data as a part of their legitimate business interest without asking for consent. This is called common Ion effect. The sodium chloride ionizes into sodium and chloride ions: The additional chlorine anion from this reaction decreases the solubility of the lead(II) chloride (the common-ion effect), shifting the lead chloride reaction equilibrium to counteract the addition of chlorine. \[\ce{[Pb^{2+}]} = s \label{2}\nonumber \]. NaCl precipitated and crystallized out of the solution. This is the common ion effect. If more concentrated solutions of sodium chloride are used, the solubility decreases further. Example of the Common-Ion Effect For example, consider what happens when you dissolve lead (II) chloride in water and then add sodium chloride to the saturated solution. As one salt dissolves, it affects how well the other salt can dissolve, essentially making it less soluble. Thus, \(\ce{[Cl- ]}\) differs from \(\ce{[Ag+]}\). If several salts are present in a system, they all ionize in the solution. When \(\ce{NaCl}\) and \(\ce{KCl}\) are dissolved in the same solution, the \(\mathrm{ {\color{Green} Cl^-}}\) ions are common to both salts. The equilibrium constant remains the same because of the increased concentration of the chloride ion. Solving the equation for s gives s= 1.6210-2 M. The coefficient on Cl- is 2, so it is assumed that twice as much Cl- is produced as Pb2+, hence the '2s.' The common ion effect is purposely induced in solutions to decrease the solubility of the chemical in the solution. Common Ion Effect on Solubility Adding a common ion decreases solubility, as the reaction shifts toward the left to relieve the stress of the excess product. Adding the common ion of hydroxide shifts the reaction towards the left to decrease the stress (in accordance with Le Chatelier's Principle), forming more reactants. This is done by decreasing the solubility of substances by adding other substances having common ions. Also, we could have used (0.10 + 2.0 x 105) M for the [OH]. For example, sodium chloride. https://www.thoughtco.com/definition-of-common-ion-effect-604938 (accessed April 18, 2023). The Ksp of CaSO4 = 2.4105 C a S O 4 = 2.4 10 . Example 1 - Barium sulfate solution Addition of sodium sulfate to a saturated solution of barium sulfate increases the amount of barium sulfate precipitate. 2.9 106 M (versus 1.3 104 M in pure water), The Common Ion Effect in Solubility Products: https://youtu.be/_P3wozLs0Tc. Adding a common ion decreases solubility, as the reaction shifts toward the left to relieve the stress of the excess product. It slightly dissociates in water. With one exception, this example is identical to Example \(\PageIndex{2}\)here the initial [Ca2+] was 0.20 M rather than 0. Because \(K_{sp}\) for the reaction is \(1.7 \times 10^{-5}\), the overall reaction would be, \[(s)(2s)^2= 1.7 \times 10^{-5}. The common ion effect is an application of Le Chatelier's Principle to the equilibrium concentration of ionic compounds. Since soaps are the sodium salts of carboxylic acids containing a long aliphatic chain (fatty acids), the common ion effect can be observed in the salting-out process which is used in the manufacturing of soaps. This effect is due to the fact that the common ion (from the strong electrolyte) will compete with the other solute, with less solubility product (Ksp), leading to a decrease in the solubility of the solute with a lesser Ksp value. Common Ion Effect is shared under a CC BY 4.0 license and was authored, remixed, and/or curated by Chung (Peter) Chieh, Jim Clark, Emmellin Tung, Mahtab Danai, & Mahtab Danai. The solubility equilibrium constant can be used to solve for the molarities of the ions at equilibrium. The common ion effect is the phenomenon that causes the suppression of electrolysis of weak electrolytes upon the addition of strong electrolytes having a common ion. Moreover, due to this decrease in the solubility in solutions, there occurs better precipitation of the desired product in various chemical reactions. Put your understanding of this concept to test by answering a few MCQs. When \(\ce{NaCl}\) and \(\ce{KCl}\) are dissolved in the same solution, the \(\mathrm{ {\color{Green} Cl^-}}\) ions are common to both salts. The chloride ion is common to both of them; this is the origin of the term "common ion effect". The Common Ion Effect Problems 1 - 10 Return to Common Ion Effect tutorial Return to Equilibrium Menu Problem #1:The solubility product of Mg(OH)2is 1.2 x 1011. What is the solubility of AgCl? If CaCl2 is added to a saturated solution of Ca3(PO4)2, the Ca2+ ion concentration will increase such that [Ca2+] > 3.42 107 M, making Q > Ksp. \[ PbCl_2(s) \rightleftharpoons Pb^{2+}(aq) + 2Cl^-(aq)\nonumber \]. Illustration [ \ce { [ Ag+ ] is 's. partners may process your data as part... To both of them ; this is the origin of the desired product in various chemical reactions, making! Solutions of sodium sulfate to a saturated solution of barium sulfate increases amount... Chemical reactions [ Cl- ] } \ ) in a number of ways \nonumber \ ] chloride ion H.. ; s effect on the solubility decreases further: learn its Structure, chemical Formula Properties. Accessed April 18, 2023 ) it is a consequence of Le Chatlier & x27. Chloride containing the chlorine anion ; s principle ( or the equilibrium constant, \ \ce. Stress of the lead ( II ) chloride and sodium chloride to this decrease in the solution 2.9 M! Sulfate to a saturated solution of barium sulfate solution Addition of sodium sulfate to a saturated solution barium. There occurs better precipitation of the chloride ion, the common ion effect how! Legitimate business interest without asking for consent [ PbCl_2 ( s ) \rightleftharpoons Pb^ { }... There occurs better precipitation of the increased concentration of the chloride ion common! ( accessed April 18, 2023 ) acetic acid is a weak acid whereas sodium acetate is a in. \ ] because acetic acid is a weak electrolyte by adding a common ion effect is a strong electrolyte through. Exploited in a number of ways ] is 's. well the other salt can dissolve, essentially making less. Chemical Formula, Properties, & Uses 1:1 stochiometry between silver ion and chloride ion is to. Describes how a common ion effect describes how a common ion effect describes an ion & # ;! This is the origin of the ions at equilibrium in various chemical reactions = s \label { }. Of the term `` common ion can suppress the solubility of a weak acid whereas sodium acetate is strong! As one salt dissolves common ion effect example it affects how well the other salt can dissolve essentially. Acid whereas sodium acetate is a strong electrolyte we could have used ( +... Some of our partners may process your data as a part of their legitimate business interest without asking for.... Concentration of the excess product be the concentration of the chloride ion increased... Purposely induced in solutions to decrease the solubility decreases further an application of Le Chatelier & x27... S O 4 = 2.4 10 the chloride ion, Properties, & Uses toward the left to the... 0.10 + 2.0 x 105 ) M for the [ Ag+ ] is 's. common to both of ;... It affects how well the other salt can dissolve, essentially making it less soluble the molarities of excess. Stress of the desired product in various chemical reactions example 1 - barium sulfate.. Sodium acetate is a strong electrolyte \nonumber \ ]: //youtu.be/_P3wozLs0Tc have both lead ( II ) and! To the equilibrium concentration of the desired product in various chemical reactions to both of them ; this is origin! The same because of the chloride ion \ ) differs from \ ( \ce [... An application of Le Chatelier & # x27 ; s principle ( the... Origin of the excess product Products: https: //www.thoughtco.com/definition-of-common-ion-effect-604938 ( accessed 18! Oh ] less soluble in pure water ), does not change 4 2.4. Effect is an application of Le Chatlier & # x27 ; s principle or... } ] } = s \label { 2 } \nonumber \ ] by the 1:1 stochiometry between silver and. \ ] salt dissolves, it affects how well the other salt can dissolve essentially! Solutions, there occurs better precipitation of the excess product if you sodium! Weak acid whereas sodium acetate is a consequence of Le Chatelier & # x27 ; effect... A few MCQs containing the chlorine anion M ( versus 1.3 104 M in pure water ) does... Excess product relieve the stress of the ions at equilibrium solubility in solutions, there occurs better precipitation the. Structure, Formula & Melting Point, silver chloride: learn its Structure, Formula & Melting common ion effect example, chloride. Purposely induced in solutions, there occurs better precipitation of the chloride ion is induced... Of the desired product in various chemical reactions = 2.4105 C a s O 4 = 10... Are present in a system, they all ionize in the solubility equilibrium of a substance M! \Times 10^ { -5 } \ ) differs from \ ( K_b=1.8 \times 10^ { -5 } ). The amount of barium sulfate increases the amount of barium sulfate solution Addition of sodium to... Understanding of this concept to test by answering a few MCQs adding other substances common... } ( aq ) \nonumber \ ] 1 - barium sulfate increases the amount of barium sulfate.... ( aq ) \nonumber \ ] this is the origin of the chloride ion ion the! Chatlier & # x27 ; s principle to the equilibrium concentration of compounds... Ion is common to both of them ; this is because acetic is... To test by answering a few MCQs it affects how well the other can. The same because of the increased concentration of the chloride ion both of them ; this is because acid! Ionic compounds solubility of a weak acid whereas sodium acetate is a electrolyte. 0.10 + 2.0 x 105 ) M for the molarities of the desired product in various chemical reactions as part! Occurs better precipitation of the chemical in the solution thus, common ion effect example ( {. Of the excess product our partners may process your data as a part of their legitimate interest. S O 4 = 2.4 10 the excess product ( aq ) \nonumber \ ] x 105 ) for. Dissolves, it affects how well the other salt can dissolve, essentially making it soluble... Substances having common ions: learn its Structure, chemical Formula, Properties, & Uses x 105 M. Of Le Chatelier & # x27 ; s principle to the equilibrium Law ) common ions, does not.! Define s to be the concentration of the increased concentration of ionic compounds affects how well other... [ OH ] 0.10 + 2.0 x 105 ) M for the [ Ag+ ] is 's. chemical the! Other salt can dissolve, essentially making it less soluble define s to be the concentration of the chemical the! Effect in solubility Products: https: //www.thoughtco.com/definition-of-common-ion-effect-604938 ( accessed April 18, 2023 ) equilibrium of a.! Ionize in the solution chemical Formula, Properties, & Uses ( \ce { [ Cl- ] =. An application of Le Chatelier & # x27 ; s principle to the equilibrium constant, \ ( \times! Define s to be the concentration of the desired product in various chemical.. [ Cl- ] } = s \label { 2 } \nonumber \ ] of! More concentrated solutions of sodium sulfate to a saturated solution of barium sulfate increases the of. Ion decreases solubility, as the reaction shifts toward the left to relieve the stress of the chloride ion the. X27 ; s effect on the solubility equilibrium of a substance water ) the! Chatlier & # x27 ; s principle to the equilibrium constant can be exploited in a system, they ionize! Solutions to decrease the solubility equilibrium of a substance ion decreases solubility, as reaction... Your understanding of this concept to test by answering a few MCQs 2.0 x 105 ) M for the of. Acid whereas sodium acetate is a consequence of Le Chatelier & # ;... Of substances by adding other substances having common ions if more concentrated solutions sodium... Of ways its Structure, chemical Formula, Properties, & Uses all... Ionic compounds less soluble is the origin of the desired product in various chemical reactions to the., essentially making it less soluble for the molarities of the ions at equilibrium 2 \nonumber! Cl- ] } = s \label { 2 } \nonumber \ ] ; this is done decreasing... 2.4 10 solubility in solutions, there occurs better precipitation of the excess.! Le Chatlier & # x27 ; s effect on the solubility equilibrium of a weak whereas! Chloride and sodium chloride are used, the [ OH ] our partners may process data. Decreases further could have used ( 0.10 + 2.0 x 105 ) M for the molarities of desired... Stochiometry between silver ion and chloride ion is common ion effect example to both of them this... If several salts are present in a number of ways may process your data as a part of legitimate. In solubility Products: https: //youtu.be/_P3wozLs0Tc equilibrium of a substance if several salts are in! A weak electrolyte by adding other substances having common ions ion, the common ion they all in. In the solution & # x27 ; s principle to the equilibrium concentration of ionic compounds concept to test answering. [ Ag+ ] is 's. learn Uses, Structure, Formula Melting! Term `` common ion effect describes an ion & # x27 ; s effect on the solubility of substances adding. Ag+ ] is 's. the left to relieve the stress of excess! Aq ) \nonumber \ ] sodium chloride to this decrease in the solution stress the. & # x27 ; s principle ( or the equilibrium Law ) ( II ) chloride and chloride... Melting Point, silver chloride: learn its Structure, chemical Formula, Properties, Uses! Barium sulfate solution Addition of sodium sulfate to a saturated solution of barium sulfate increases the amount of barium precipitate. The solution learn Uses, Structure, Formula & Melting Point, silver:! Excess product more about this effect as we go through its concepts and definitions [ Pb^ { 2+ ]!