If in solution containing `Cl^(-) & Bt^(-)` ions, `AgNO_(3)` is added then initial precipitate of which colour will be formed ?
If in solution containing `Cl^(-) & Bt^(-)` ions, `AgNO_(3)` is added then initial precipitate of which colour will be formed ?
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Yellow
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The process in which solution containing more than one typeof ions (either cation or anion) and in which one ion undergoes almst complete precipitation followed by the second ion and similarly second ion undergoes complete precipitation followed by the third ion is known as preferential precipitation. It is the solubility of the salt,not the solubility product of the salt, by means of which one can predict the preferential precipitation of the salt or ion among the lot of ions in the solution. For example , in a solution containing Cl^(-), Br^(-) and I^(-) ions, if Ag^(+) ions are added, then out of three , the less soluble salt is precipitated first . If the addition of Ag^(+) ions is continued, eventually , a stage is reached when the next lesser soluble salt starts precipitating along with the least soluble salt and so on. If the stiochiometry of the salt is same, then the salt with the minimum K_(sp) ( solubility product ) will have minimum solubility and will precipitate first, followed by the salt of next higher solubility product and so on. If the stiochiometry of teh salt is not same, then from the solubility product data alone, we cannot predict which ions will precipitate first. For example, a solution containing Cl^(-) and CrO_(4)^(2-) . In order to predict which ion will precipitate first, we have to calculate the amount of Ag^(+) ions needed to start precipitation through the solubility product data given. When AgNO_93) is added to the solution, the minimum of the two concentrations needed to start the precipitation will be reached and thus corresponding [Ag^(+)] to start the precipitation increases. Its concentration eventually becomes equal to the value required for CrO_(4)^(2-) . At this stage, practically almost the whole of Cl^(-) ions get precipitated . Addition of more AgNO_(3) causes simultaneous precipitation of both the ions together. Suppose a student of chemistry performs the following two sets of experiments in order to known the preferential precipitation of ions as well as its precipitated percentage amount. Experiment 1. He prepare a solution of anions composed of 0.1 M each of Cl^(-),Br^(-) and I^(-) . Further he adds gradually solid AgNO_(3) to this solution. He assumes that volume of the solution does not change after the addition of solid AgNO_(3)(K_(sp)AgCl=1.0 xx 10^(-9)M^(2),K_(sp) AgBr=10^(-10)M^(2) and K_(sp) AgI=10^(-12)M^(2)) Experiment -2. He prepares a solution of cations Cd^(2+)(0.2 M) and Bi^(3+) (0.3 m) . Now he adds S^(2-) ions into the solution of cations in order to separate them by selective precipitation Cd^(2+) forms yellow precipitate of CdS and Bi^(3+) forms black precipitate of Bi_(2)S_(3) with S^(2-) ions respectively. (K_(sp)Bi_(2)S_(3) = 9 xx 10^(-25) M^(5) and K_(sp)CdS =2 xx 10^(-20)M^(2)) .Answer the following questions ont he basis of the above write up. What % of the (ion) will get precipitate when the second ion start precipitating in experiment -1 ?
The process in which solution containing more than one typeof ions (either cation or anion) and in which one ion undergoes almst complete precipitation followed by the second ion and similarly second ion undergoes complete precipitation followed by the third ion is known as preferential precipitation. It is the solubility of the salt,not the solubility product of the salt, by means of which one can predict the preferential precipitation of the salt or ion among the lot of ions in the solution. For example , in a solution containing Cl^(-), Br^(-) and I^(-) ions, if Ag^(+) ions are added, then out of three , the less soluble salt is precipitated first . If the addition of Ag^(+) ions is continued, eventually , a stage is reached when the next lesser soluble salt starts precipitating along with the least soluble salt and so on. If the stiochiometry of the salt is same, then the salt with the minimum K_(sp) ( solubility product ) will have minimum solubility and will precipitate first, followed by the salt of next higher solubility product and so on. If the stiochiometry of teh salt is not same, then from the solubility product data alone, we cannot predict which ions will precipitate first. For example, a solution containing Cl^(-) and CrO_(4)^(2-) . In order to predict which ion will precipitate first, we have to calculate the amount of Ag^(+) ions needed to start precipitation through the solubility product data given. When AgNO_93) is added to the solution, the minimum of the two concentrations needed to start the precipitation will be reached and thus corresponding [Ag^(+)] to start the precipitation increases. Its concentration eventually becomes equal to the value required for CrO_(4)^(2-) . At this stage, practically almost the whole of Cl^(-) ions get precipitated . Addition of more AgNO_(3) causes simultaneous precipitation of both the ions together. Suppose a student of chemistry performs the following two sets of experiments in order to known the preferential precipitation of ions as well as its precipitated percentage amount. Experiment 1. He prepare a solution of anions composed of 0.1 M each of Cl^(-),Br^(-) and I^(-) . Further he adds gradually solid AgNO_(3) to this solution. He assumes that volume of the solution does not change after the addition of solid AgNO_(3)(K_(sp)AgCl=1.0 xx 10^(-9)M^(2),K_(sp) AgBr=10^(-10)M^(2) and K_(sp) AgI=10^(-12)M^(2)) Experiment -2. He prepares a solution of cations Cd^(2+)(0.2 M) and Bi^(3+) (0.3 m) . Now he adds S^(2-) ions into the solution of cations in order to separate them by selective precipitation Cd^(2+) forms yellow precipitate of CdS and Bi^(3+) forms black precipitate of Bi_(2)S_(3) with S^(2-) ions respectively. (K_(sp)Bi_(2)S_(3) = 9 xx 10^(-25) M^(5) and K_(sp)CdS =2 xx 10^(-20)M^(2)) .Answer the following questions ont he basis of the above write up. What percent of the anions Br^(-) and I^(-) get precipitated respectively when the third ion starts precipitating in experiment -1 ?
Knowledge Check
AgNO_(3) solution will not give white precipitate with
AgNO_(3) solution will not give white precipitate with
A
`[Co(NH_(3))_(3)Cl_(3)]`
B
`[Co(NH_(3))_(4)Cl_(2)]Cl`
C
`[Co(NH_(3))_(5)Cl]Cl_(2)`
D
`[Co(NH_(3))_(6)]Cl_(3)`
The process in which solution containing more than one typeof ions (either cation or anion) and in which one ion undergoes almst complete precipitation followed by the second ion and similarly second ion undergoes complete precipitation followed by the third ion is known as preferential precipitation. It is the solubility of the salt,not the solubility product of the salt, by means of which one can predict the preferential precipitation of the salt or ion among the lot of ions in the solution. For example , in a solution containing Cl^(-), Br^(-) and I^(-) ions, if Ag^(+) ions are added, then out of three , the less soluble salt is precipitated first . If the addition of Ag^(+) ions is continued, eventually , a stage is reached when the next lesser soluble salt starts precipitating along with the least soluble salt and so on. If the stiochiometry of the salt is same, then the salt with the minimum K_(sp) ( solubility product ) will have minimum solubility and will precipitate first, followed by the salt of next higher solubility product and so on. If the stiochiometry of teh salt is not same, then from the solubility product data alone, we cannot predict which ions will precipitate first. For example, a solution containing Cl^(-) and CrO_(4)^(2-) . In order to predict which ion will precipitate first, we have to calculate the amount of Ag^(+) ions needed to start precipitation through the solubility product data given. When AgNO_93) is added to the solution, the minimum of the two concentrations needed to start the precipitation will be reached and thus corresponding [Ag^(+)] to start the precipitation increases. Its concentration eventually becomes equal to the value required for CrO_(4)^(2-) . At this stage, practically almost the whole of Cl^(-) ions get precipitated . Addition of more AgNO_(3) causes simultaneous precipitation of both the ions together. Suppose a student of chemistry performs the following two sets of experiments in order to known the preferential precipitation of ions as well as its precipitated percentage amount. Experiment 1. He prepare a solution of anions composed of 0.1 M each of Cl^(-),Br^(-) and I^(-) . Further he adds gradually solid AgNO_(3) to this solution. He assumes that volume of the solution does not change after the addition of solid AgNO_(3)(K_(sp)AgCl=1.0 xx 10^(-9)M^(2),K_(sp) AgBr=10^(-10)M^(2) and K_(sp) AgI=10^(-12)M^(2)) Experiment -2. He prepares a solution of cations Cd^(2+)(0.2 M) and Bi^(3+) (0.3 m) . Now he adds S^(2-) ions into the solution of cations in order to separate them by selective precipitation Cd^(2+) forms yellow precipitate of CdS and Bi^(3+) forms black precipitate of Bi_(2)S_(3) with S^(2-) ions respectively. (K_(sp)Bi_(2)S_(3) = 9 xx 10^(-25) M^(5) and K_(sp)CdS =2 xx 10^(-20)M^(2)) .Answer the following questions ont he basis of the above write up. Which of the following will precipitate first in experiment -1 ?
The process in which solution containing more than one typeof ions (either cation or anion) and in which one ion undergoes almst complete precipitation followed by the second ion and similarly second ion undergoes complete precipitation followed by the third ion is known as preferential precipitation. It is the solubility of the salt,not the solubility product of the salt, by means of which one can predict the preferential precipitation of the salt or ion among the lot of ions in the solution. For example , in a solution containing Cl^(-), Br^(-) and I^(-) ions, if Ag^(+) ions are added, then out of three , the less soluble salt is precipitated first . If the addition of Ag^(+) ions is continued, eventually , a stage is reached when the next lesser soluble salt starts precipitating along with the least soluble salt and so on. If the stiochiometry of the salt is same, then the salt with the minimum K_(sp) ( solubility product ) will have minimum solubility and will precipitate first, followed by the salt of next higher solubility product and so on. If the stiochiometry of teh salt is not same, then from the solubility product data alone, we cannot predict which ions will precipitate first. For example, a solution containing Cl^(-) and CrO_(4)^(2-) . In order to predict which ion will precipitate first, we have to calculate the amount of Ag^(+) ions needed to start precipitation through the solubility product data given. When AgNO_93) is added to the solution, the minimum of the two concentrations needed to start the precipitation will be reached and thus corresponding [Ag^(+)] to start the precipitation increases. Its concentration eventually becomes equal to the value required for CrO_(4)^(2-) . At this stage, practically almost the whole of Cl^(-) ions get precipitated . Addition of more AgNO_(3) causes simultaneous precipitation of both the ions together. Suppose a student of chemistry performs the following two sets of experiments in order to known the preferential precipitation of ions as well as its precipitated percentage amount. Experiment 1. He prepare a solution of anions composed of 0.1 M each of Cl^(-),Br^(-) and I^(-) . Further he adds gradually solid AgNO_(3) to this solution. He assumes that volume of the solution does not change after the addition of solid AgNO_(3)(K_(sp)AgCl=1.0 xx 10^(-9)M^(2),K_(sp) AgBr=10^(-10)M^(2) and K_(sp) AgI=10^(-12)M^(2)) Experiment -2. He prepares a solution of cations Cd^(2+)(0.2 M) and Bi^(3+) (0.3 m) . Now he adds S^(2-) ions into the solution of cations in order to separate them by selective precipitation Cd^(2+) forms yellow precipitate of CdS and Bi^(3+) forms black precipitate of Bi_(2)S_(3) with S^(2-) ions respectively. (K_(sp)Bi_(2)S_(3) = 9 xx 10^(-25) M^(5) and K_(sp)CdS =2 xx 10^(-20)M^(2)) .Answer the following questions ont he basis of the above write up. Which of the following will precipitate first in experiment -1 ?
A
`I^(-)`ion
B
`Br^(-)` ion
C
`Cl^(-)` ion
D
cannot be predicted
The process in which solution containing more than one typeof ions (either cation or anion) and in which one ion undergoes almst complete precipitation followed by the second ion and similarly second ion undergoes complete precipitation followed by the third ion is known as preferential precipitation. It is the solubility of the salt,not the solubility product of the salt, by means of which one can predict the preferential precipitation of the salt or ion among the lot of ions in the solution. For example , in a solution containing Cl^(-), Br^(-) and I^(-) ions, if Ag^(+) ions are added, then out of three , the less soluble salt is precipitated first . If the addition of Ag^(+) ions is continued, eventually , a stage is reached when the next lesser soluble salt starts precipitating along with the least soluble salt and so on. If the stiochiometry of the salt is same, then the salt with the minimum K_(sp) ( solubility product ) will have minimum solubility and will precipitate first, followed by the salt of next higher solubility product and so on. If the stiochiometry of teh salt is not same, then from the solubility product data alone, we cannot predict which ions will precipitate first. For example, a solution containing Cl^(-) and CrO_(4)^(2-) . In order to predict which ion will precipitate first, we have to calculate the amount of Ag^(+) ions needed to start precipitation through the solubility product data given. When AgNO_93) is added to the solution, the minimum of the two concentrations needed to start the precipitation will be reached and thus corresponding [Ag^(+)] to start the precipitation increases. Its concentration eventually becomes equal to the value required for CrO_(4)^(2-) . At this stage, practically almost the whole of Cl^(-) ions get precipitated . Addition of more AgNO_(3) causes simultaneous precipitation of both the ions together. Suppose a student of chemistry performs the following two sets of experiments in order to known the preferential precipitation of ions as well as its precipitated percentage amount. Experiment 1. He prepare a solution of anions composed of 0.1 M each of Cl^(-),Br^(-) and I^(-) . Further he adds gradually solid AgNO_(3) to this solution. He assumes that volume of the solution does not change after the addition of solid AgNO_(3)(K_(sp)AgCl=1.0 xx 10^(-9)M^(2),K_(sp) AgBr=10^(-10)M^(2) and K_(sp) AgI=10^(-12)M^(2)) Experiment -2. He prepares a solution of cations Cd^(2+)(0.2 M) and Bi^(3+) (0.3 m) . Now he adds S^(2-) ions into the solution of cations in order to separate them by selective precipitation Cd^(2+) forms yellow precipitate of CdS and Bi^(3+) forms black precipitate of Bi_(2)S_(3) with S^(2-) ions respectively. (K_(sp)Bi_(2)S_(3) = 9 xx 10^(-25) M^(5) and K_(sp)CdS =2 xx 10^(-20)M^(2)) .Answer the following questions ont he basis of the above write up. Which of the following is the correct order of appearance of coloour of the precipitate in experiment ?
The process in which solution containing more than one typeof ions (either cation or anion) and in which one ion undergoes almst complete precipitation followed by the second ion and similarly second ion undergoes complete precipitation followed by the third ion is known as preferential precipitation. It is the solubility of the salt,not the solubility product of the salt, by means of which one can predict the preferential precipitation of the salt or ion among the lot of ions in the solution. For example , in a solution containing Cl^(-), Br^(-) and I^(-) ions, if Ag^(+) ions are added, then out of three , the less soluble salt is precipitated first . If the addition of Ag^(+) ions is continued, eventually , a stage is reached when the next lesser soluble salt starts precipitating along with the least soluble salt and so on. If the stiochiometry of the salt is same, then the salt with the minimum K_(sp) ( solubility product ) will have minimum solubility and will precipitate first, followed by the salt of next higher solubility product and so on. If the stiochiometry of teh salt is not same, then from the solubility product data alone, we cannot predict which ions will precipitate first. For example, a solution containing Cl^(-) and CrO_(4)^(2-) . In order to predict which ion will precipitate first, we have to calculate the amount of Ag^(+) ions needed to start precipitation through the solubility product data given. When AgNO_93) is added to the solution, the minimum of the two concentrations needed to start the precipitation will be reached and thus corresponding [Ag^(+)] to start the precipitation increases. Its concentration eventually becomes equal to the value required for CrO_(4)^(2-) . At this stage, practically almost the whole of Cl^(-) ions get precipitated . Addition of more AgNO_(3) causes simultaneous precipitation of both the ions together. Suppose a student of chemistry performs the following two sets of experiments in order to known the preferential precipitation of ions as well as its precipitated percentage amount. Experiment 1. He prepare a solution of anions composed of 0.1 M each of Cl^(-),Br^(-) and I^(-) . Further he adds gradually solid AgNO_(3) to this solution. He assumes that volume of the solution does not change after the addition of solid AgNO_(3)(K_(sp)AgCl=1.0 xx 10^(-9)M^(2),K_(sp) AgBr=10^(-10)M^(2) and K_(sp) AgI=10^(-12)M^(2)) Experiment -2. He prepares a solution of cations Cd^(2+)(0.2 M) and Bi^(3+) (0.3 m) . Now he adds S^(2-) ions into the solution of cations in order to separate them by selective precipitation Cd^(2+) forms yellow precipitate of CdS and Bi^(3+) forms black precipitate of Bi_(2)S_(3) with S^(2-) ions respectively. (K_(sp)Bi_(2)S_(3) = 9 xx 10^(-25) M^(5) and K_(sp)CdS =2 xx 10^(-20)M^(2)) .Answer the following questions ont he basis of the above write up. Which of the following is the correct order of appearance of coloour of the precipitate in experiment ?
A
yellow `gt` pale yellow `gt` curdy white
B
yellow `lt` pale yellow `lt` curdy white
C
pale yellow `gt` yellow `lt` curdy white
D
pale yellow `gt` yellow `gt` curdy white
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The process in which solution containing more than one typeof ions (either cation or anion) and in which one ion undergoes almst complete precipitation followed by the second ion and similarly second ion undergoes complete precipitation followed by the third ion is known as preferential precipitation. It is the solubility of the salt,not the solubility product of the salt, by means of which one can predict the preferential precipitation of the salt or ion among the lot of ions in the solution. For example , in a solution containing Cl^(-), Br^(-) and I^(-) ions, if Ag^(+) ions are added, then out of three , the less soluble salt is precipitated first . If the addition of Ag^(+) ions is continued, eventually , a stage is reached when the next lesser soluble salt starts precipitating along with the least soluble salt and so on. If the stiochiometry of the salt is same, then the salt with the minimum K_(sp) ( solubility product ) will have minimum solubility and will precipitate first, followed by the salt of next higher solubility product and so on. If the stiochiometry of teh salt is not same, then from the solubility product data alone, we cannot predict which ions will precipitate first. For example, a solution containing Cl^(-) and CrO_(4)^(2-) . In order to predict which ion will precipitate first, we have to calculate the amount of Ag^(+) ions needed to start precipitation through the solubility product data given. When AgNO_93) is added to the solution, the minimum of the two concentrations needed to start the precipitation will be reached and thus corresponding [Ag^(+)] to start the precipitation increases. Its concentration eventually becomes equal to the value required for CrO_(4)^(2-) . At this stage, practically almost the whole of Cl^(-) ions get precipitated . Addition of more AgNO_(3) causes simultaneous precipitation of both the ions together. Suppose a student of chemistry performs the following two sets of experiments in order to known the preferential precipitation of ions as well as its precipitated percentage amount. Experiment 1. He prepare a solution of anions composed of 0.1 M each of Cl^(-),Br^(-) and I^(-) . Further he adds gradually solid AgNO_(3) to this solution. He assumes that volume of the solution does not change after the addition of solid AgNO_(3)(K_(sp)AgCl=1.0 xx 10^(-9)M^(2),K_(sp) AgBr=10^(-10)M^(2) and K_(sp) AgI=10^(-12)M^(2)) Experiment -2. He prepares a solution of cations Cd^(2+)(0.2 M) and Bi^(3+) (0.3 m) . Now he adds S^(2-) ions into the solution of cations in order to separate them by selective precipitation Cd^(2+) forms yellow precipitate of CdS and Bi^(3+) forms black precipitate of Bi_(2)S_(3) with S^(2-) ions respectively. (K_(sp)Bi_(2)S_(3) = 9 xx 10^(-25) M^(5) and K_(sp)CdS =2 xx 10^(-20)M^(2)) .Answer the following questions ont he basis of the above write up. In experiment 02, what is the maximum concentration of S^(2-) ion at which one of the two metal ions gets maximum precipitation ?
The process in which solution containing more than one typeof ions (either cation or anion) and in which one ion undergoes almst complete precipitation followed by the second ion and similarly second ion undergoes complete precipitation followed by the third ion is known as preferential precipitation. It is the solubility of the salt,not the solubility product of the salt, by means of which one can predict the preferential precipitation of the salt or ion among the lot of ions in the solution. For example , in a solution containing Cl^(-), Br^(-) and I^(-) ions, if Ag^(+) ions are added, then out of three , the less soluble salt is precipitated first . If the addition of Ag^(+) ions is continued, eventually , a stage is reached when the next lesser soluble salt starts precipitating along with the least soluble salt and so on. If the stiochiometry of the salt is same, then the salt with the minimum K_(sp) ( solubility product ) will have minimum solubility and will precipitate first, followed by the salt of next higher solubility product and so on. If the stiochiometry of teh salt is not same, then from the solubility product data alone, we cannot predict which ions will precipitate first. For example, a solution containing Cl^(-) and CrO_(4)^(2-) . In order to predict which ion will precipitate first, we have to calculate the amount of Ag^(+) ions needed to start precipitation through the solubility product data given. When AgNO_93) is added to the solution, the minimum of the two concentrations needed to start the precipitation will be reached and thus corresponding [Ag^(+)] to start the precipitation increases. Its concentration eventually becomes equal to the value required for CrO_(4)^(2-) . At this stage, practically almost the whole of Cl^(-) ions get precipitated . Addition of more AgNO_(3) causes simultaneous precipitation of both the ions together. Suppose a student of chemistry performs the following two sets of experiments in order to known the preferential precipitation of ions as well as its precipitated percentage amount. Experiment 1. He prepare a solution of anions composed of 0.1 M each of Cl^(-),Br^(-) and I^(-) . Further he adds gradually solid AgNO_(3) to this solution. He assumes that volume of the solution does not change after the addition of solid AgNO_(3)(K_(sp)AgCl=1.0 xx 10^(-9)M^(2),K_(sp) AgBr=10^(-10)M^(2) and K_(sp) AgI=10^(-12)M^(2)) Experiment -2. He prepares a solution of cations Cd^(2+)(0.2 M) and Bi^(3+) (0.3 m) . Now he adds S^(2-) ions into the solution of cations in order to separate them by selective precipitation Cd^(2+) forms yellow precipitate of CdS and Bi^(3+) forms black precipitate of Bi_(2)S_(3) with S^(2-) ions respectively. (K_(sp)Bi_(2)S_(3) = 9 xx 10^(-25) M^(5) and K_(sp)CdS =2 xx 10^(-20)M^(2)) .Answer the following questions ont he basis of the above write up. In experiment -2 what % of the metal ions get precipitated at which S^(2-) get saturated with another ion ?
The process in which solution containing more than one typeof ions (either cation or anion) and in which one ion undergoes almst complete precipitation followed by the second ion and similarly second ion undergoes complete precipitation followed by the third ion is known as preferential precipitation. It is the solubility of the salt,not the solubility product of the salt, by means of which one can predict the preferential precipitation of the salt or ion among the lot of ions in the solution. For example , in a solution containing Cl^(-), Br^(-) and I^(-) ions, if Ag^(+) ions are added, then out of three , the less soluble salt is precipitated first . If the addition of Ag^(+) ions is continued, eventually , a stage is reached when the next lesser soluble salt starts precipitating along with the least soluble salt and so on. If the stiochiometry of the salt is same, then the salt with the minimum K_(sp) ( solubility product ) will have minimum solubility and will precipitate first, followed by the salt of next higher solubility product and so on. If the stiochiometry of teh salt is not same, then from the solubility product data alone, we cannot predict which ions will precipitate first. For example, a solution containing Cl^(-) and CrO_(4)^(2-) . In order to predict which ion will precipitate first, we have to calculate the amount of Ag^(+) ions needed to start precipitation through the solubility product data given. When AgNO_93) is added to the solution, the minimum of the two concentrations needed to start the precipitation will be reached and thus corresponding [Ag^(+)] to start the precipitation increases. Its concentration eventually becomes equal to the value required for CrO_(4)^(2-) . At this stage, practically almost the whole of Cl^(-) ions get precipitated . Addition of more AgNO_(3) causes simultaneous precipitation of both the ions together. Suppose a student of chemistry performs the following two sets of experiments in order to known the preferential precipitation of ions as well as its precipitated percentage amount. Experiment 1. He prepare a solution of anions composed of 0.1 M each of Cl^(-),Br^(-) and I^(-) . Further he adds gradually solid AgNO_(3) to this solution. He assumes that volume of the solution does not change after the addition of solid AgNO_(3)(K_(sp)AgCl=1.0 xx 10^(-9)M^(2),K_(sp) AgBr=10^(-10)M^(2) and K_(sp) AgI=10^(-12)M^(2)) Experiment -2. He prepares a solution of cations Cd^(2+)(0.2 M) and Bi^(3+) (0.3 m) . Now he adds S^(2-) ions into the solution of cations in order to separate them by selective precipitation Cd^(2+) forms yellow precipitate of CdS and Bi^(3+) forms black precipitate of Bi_(2)S_(3) with S^(2-) ions respectively. (K_(sp)Bi_(2)S_(3) = 9 xx 10^(-25) M^(5) and K_(sp)CdS =2 xx 10^(-20)M^(2)).Answer the following questions ont he basis of the above write up. Which one of the following statements is correct regarding the experiment ?
K_(sp) of AgCl, Ag_(2)CrO_(4) and AgBr are 10^(-10),10^(-13) and 10^(-12) respectively. If to a solution of 0.1 M each of Cl^(-), CrO_(4)^(2-) and Br^(-) ions, AgNO_(3) is added slowly, which will precipitate first :
A solution contains Cl^( - ) , I^( - ) and SO _ 4^( 3- ) ions in it. Which of the following ion is capable to precipitate all of the above when added in this solution ?