Calculating the Effect of a Common Ion on Solubility
Consider a saturated solution of the salt MX3, which M is a metal cation with a 3+ charge and X is an anion with a 1− charge, in water at 298 K. Which of the following will affect the Ksp of MX3 in water?
Consider a saturated solution of the salt , which is a metal cation with a charge and is an anion with a charge, in water at 298 . Which of the following will affect the of in water?
diluting the solution | |
the addition of more X− to the solution | |
raising the temperature of the solution | |
the addition of more M3+ to the solution | |
more than one of the above factors |
MX3 --> M+3 and 3X-
Ksp = [M+3][X-]^3
diluting solution ---> since concnetration are affected
adding X- decrease M+3 solubility
raising T changes Ksp value, tehrefore solubiltiy
addition of M3+ affects solubiliyt of X-
all factors affect
Calculating the Effect of a Common Ion on Solubility Consider a saturated solution of the salt...
The Effect of a Common Ion on Molar Solubility: pH and
OH- as a Common Ion
We have seen from our study of acid/base chemistry that the
presence of a weak base such as ammonia (Kb = 1.8 X
10-5) can affect the pH of an aqueous solution. This pH
can in turn affect the solubility of a metal hydroxide salt as a
result of the common ion effect. The Ksp for manganese (II)
hydroxide = 2.0 X 10-13. What...
Consider a hypothetical salt of low solubility, "MX", where M+ is a metal cation and X- is a non-metal anion. A voltaic cell was set up with a cathode containing metal "M" immersed in a solution containing M+ at a concentration of 1.00 mol L-1. The anode consisted of metal "M" immersed in a saturated solution of "MX". The measured cell voltage was 0.251 V. What is the Ksp of "MX" at 25°C ?
Consider a hypothetical salt of low solubility, "MX", where M+ is a metal cation and X- is a non-metal anion. A voltaic cell was set up with a cathode containing metal "M" immersed in a solution containing M+ at a concentration of 1.00 mol L-1. The anode consisted of metal "M" immersed in a saturated solution of "MX". The measured cell voltage was 0.186 V. What is the Ksp of "MX" at 25°C ?
Consider a hypothetical salt of low solubility, "MX", where M+ is a metal cation and X- is a non-metal anion. A voltaic cell was set up with a cathode containing metal "M" immersed in a solution containing M+ at a concentration of 1.00 mol L-1. The anode consisted of metal "M" immersed in a saturated solution of "MX". The measured cell voltage was 0.429 V. What is the Ksp of "MX" at 25°C ? Remember: if you want to express...
1. How is the molar solubility of a slightly soluble salt affected by the addition of an ion common to the salt equilibrium? 2. A 3.11 mL volume of a standardized 0.0025 M HCl solution titrated 25.0 mL of a saturated Mg(OH)2 solution to the methyl orange endpoint. Calculate the Ksp of Mg(OH)2. 3. If the endpoint in the titration of a saturated Ca(OH)2 solution with a standardized HCI solution is surpassed, will the reported Kap of Ca(OH)2 be reported...
Suppose we have a salt of low solubility, "MX", X- represents a non-metal anion M+ represents a metal cation. We then employ a voltaic cell with a cathode containing metal "M" immersed in a solution containing M+ at a concentration of 1.00 mol L-1. The anode consisted of metal "M" immersed in a saturated solution of "MX". The measured cell voltage was 0.355 V. Calculate Ksp of "MX" at 25°C
7.Calculate the molar solubility for the binary salt MX3 with Ksp=0.0000071. Enter your answer as a decimal number with two significant figures. 8.Calculate the molar solubility of the binary salt MX2 with Ksp=0.000016. Enter your answer as a decimal with two significant figures. 9. Calculate the molar solubility of MX2 (Ksp=0.0000011) in 0.085 M NaX. Enter your answer as a decimal with two significant figures. 10.Determine the molar solubility of MX (Ksp=4.2x10-8) in 0.083 M NaCN. The metal ion M+...
The molar solubility of a salt is 1.2 x 10-3M. What is its Ksp of this salt in pure water? If 0.005 of a common ion is added to the solution, what is the new solubility (Common ion effect in salts) The solubility of an unknown salt with a formula XY2 is 3.9 x 10-11 mol/L. What is the value of Ksp of this salt?
The common ion effect • The presence of a common ion will always decrease the solubility of an ionic solid. • e.g. what is the solubility of BaSO4 in 0.30 mol L aqueous Na2SO4 solution? Ksp (BaSO4) =1.1 x 10-10
± Solubility of Zinc Hydroxide in Basic Solution A solubility-product constant, Ksp, corresponds to a reaction with the following general format: salt(s)⇌cation(aq)+anion(aq) A formation constant, Kf, corresponds to a reaction with the following general format: metal ion(aq)+Lewis base(aq)⇌complex ion(aq) Part A When Zn(OH)2(s) was added to 1.00 L of a basic solution, 1.18×10−2 mol of the solid dissolved. What is the concentration of OH− in the final solution? Express your answer with the appropriate units [OH−] =???