For a system involving complexation, the [Ag+] can be replaced using the formation constant of the reaction, Ag+ + 2 S2O32- ⇌ Ag(S2O3)23-. Show the process of obtaining the formation constant.

Q: . Calculate the activity coefficients of Ca2 + and Cl- ions in the presence of 0.0036 M CaCl and…

A: The ratio of the chemical activity of a substance to its molar concentration is its molar activity.…

Q: 2. Calculate the solubility of AgBr at: a) zero ionic strength and b) in a solution containing…

A: If the solubility of AgBr is s mol/L, then AgBr will dissociate to s mol/L of Ag+ and s mol/L of Br-

Q: Which of these expressions correctly expresses the solubilityproductconstant for Ag3PO4 in water?(a)…

A: Solubility product can be defined as that equilibrium constant in which the salt dissociates into…

Q: A 3650-mg sample containing bromate and bromide was dissolved in sufficient water to give 250.0 mL.…

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Q: Given the following activity coefficient data: Ion Ion Size (pm) Ionic Strength (μ, M) 0.001…

A: The medium is mentioned to be 0.0213 M Mg(CN)2

Q: Calculate the activity of I03 in a saturated solution of La(IO3)3 with 0.01OM La(NO3)3. Ksp = 1.0 x…

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Q: Considering only the equilibrium HgBr21s2 Δ Hg21 1 2Br2, and includingactivity coefficients,…

A: The solubility product of HgBr2 is equal to 6.2 × 10-20. On dissolving this salt in a solution of…

Q: Calculate the molar solubility of Mn(OH)2 in a solution that contains 0.20 M NaOH Ksp for…

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Q: B. Determination of the Solubility-Product Constant UA T 0 Absorbance [Cro,?-] 2.8K10-4 3,9 x10-4…

A: solubility is defined as the maximum amount of solute that can be dissolve in a solvent or we can…

Q: 0.281 mol AgNO3 and 3.17 mol NH3 were added to enough water to give 1.00 L of solution at 25 °C.…

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Q: Calculate the solubility of silver chromate (Ag2Cr04) at 25 °C in 0.0050 mol L-1 K2Cr04 solution.…

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Q: A solution in part C initially contains (4.2100x10^-4) molar SCN¯ and (3.1700x10^-3) molar Fe3+.…

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Q: The cation M2+ reacts with NH3 to form a series of complex ions as follows: M2+ + NH3 = M(NH3)²+…

A: From first equation We can say that K1 = [(M(NH3))2+]/[M2+][NH3] From second- K2=…

Q: C. 8.12 d. 3.44 e. 5.28 3. Determine the solubility of the ions that is calculated from the Ksp for…

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Q: Describe the common-ion effect?

A: The common ion effect has to be described.

Q: Calculate the equilibrium Ni2+ concentration of a solution that has been prepared by mixing 50.0 ml…

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Q: Part C Given that 4,HP = -5.9 kJ mol1 and A,S° = -119.6 JK1 mor1, determine the standard Gibbs…

A: Gibbs free energy is given by. ∆rG° = ∆rH° - T∆rS°-S∆rT At constant Temperature ∆rT=0 So, ∆rG° =…

Q: Calculate the molar solubility in M for Mn(OH)2 in 0.1 M KI. Take activity into consideration. Hint:…

A: Formula used :-  Ksp = 4s3

Q: a) Impurity removal from leach solutions may be accomplished through neutralization as discussed in…

A: Precipitation reactions occur when cations and anions combine to form an insoluble solid product in…

Q: (6) 11. Calculate the molar solubility of silver thiocyanate (Ksp= 1.0 x 10-12), AgSCN, in a. pure…

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Q: Calculate the solubility (in mol/L) of silver oxalate, Ag2C204, in 0.15M Na2C204. = 1.0 x 10-11 Ksp…

A: Ksp is the product of concentration of each ions and each ions are raised by respective powers.

Q: Question: 1. Determine the lambda max used to read the solutions. How was this obtained? 2.…

A: λmax is the wavelength corresponding to maximum absorbsionAccording to Lambert-Beer's law…

Q: Titration of 25.0 mL of a 0.0500 M Zn2+ solution with 0.0550 M EDTA in a solution buffered at pH 8.…

A: Conditional formation Constant, Kf’ can be determined as follows: where Kf is the formation…

Q: Calculate molar conductance (L = 1000k/C ) of the complex [Co(NH3)4CO3]NO3, if the specific…

A: Reaction: [Co(NH3)4CO3]NO3  ⇌[Co(NH3)4CO3]+  +  NO3- Molar conductance is calculated as:…

Q: DG° = -53.6 kJ/molxn for the following reaction at 25°C. Zn2"(aq) + 4 NH3(aq) Zn(NH3),2"(aq) What is…

A: ∆G° = -2.303 RT log K  -53.6 x 103 = - 2.303 x 8.314 x 298 log K log K = 9.4 = log ( 2.5 x 109 ) K =…

Q: For the aqueous [Cd(CN)4]^2- complex =Kf×7.7x10^16 at 25°C.Suppose equal volumes of 0.0010M Cd(NO3)2…

A: The equation for the formation of complex can be given as

Q: [M(H2O)4(en)]²* [M(H2O)2(en)2]²* [M(en)3]3+ Cu 3 x 1010 1 x 109 0.1 Ni 1 x 1010 1 x 1010 1 x 1010…

A: Solution -

Q: Solid KSCN was added to a(2.20x10^0) M Co2+ solution so that it was also initially (2.20x10^0) M…

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Q: The Ksp of AgCl(s) at a specific temperature is 1.8 × 10^-10 M. The concentration of Cl-(aq) in…

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Q: Use the Debye-Hückel equation to calculate the activity cocfficient of each ion at the given ionic…

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Q: 9. Consider the equilibrium reaction: YZ2(s) = Y2*(aq) + 2Z°(aq). What is the molar solubility of…

A: Different salts dissolves to different extend in a solvent. Some are highly soluble while others are…

Q: [Ag(NH3)₂] complex K₁=1.12 × 10² at 25 °C. Suppose equal volumes of 0.0034 M AgNO3 solution and…

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Q: For the aqueous [HgCl4]2- complex Kf=5.0 x1015 at 25°C.Suppose equal volumes of 0.0074M Hg(NO3)2…

A: Given,Kf = 5.0 × 1015 at 25 oC0.0074M of Hg(NO3)2  solution and 0.84M of NaCl

Q: The formation constant for [Cu(CN)2]` is 1.0 × 1016, what is the value of the dissociation constant…

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Q: The Ksp Value of magnesium fluoride is 5.16 × 10 11 at 25 °C. MgF2(s) = Mg²+(aq) + 2 F¯(aq) a.…

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Q: (v) At what pH would the given concentrations of Ce3, Ce*, Mn2*, and MnO4 to be in Activ Go to…

A: Given as  The solution contains 0.100 M Ce3+; 1.00*10-1 M Ce4+; 1.00*10-4M Mn2+; 0.100 M MnO4- and…

Q: In which of the following aqueous solutions will the Mn(OH)2 be least soluble? Ksp = 2.0x10-13 A.…

A: Adding a common ion decreases the solubility of a component, also known as common ion affect.

Q: Titration of 25.0 mL of a 0.0500 M Zn2+ solution with 0.0550 M EDTA in a solution buffered at pH 8.…

A: Calculation of the concentration of Zn2+ before addition of the titrant: Calculation of no. of…

Q: For the aqueous [Hg(NH3)4]²* complex K, = 1.91 × 10¹⁹ at 25 °C. Suppose equal volumes of 0.0062 M…

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Q: The value of Ksp for Cd(OH)2 is 2.5 x 10-14. (a) Whatis the molar solubility of Cd1OH22? (b) The…

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Q: If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?…

A: Given,  a). If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this…

Q: The blue complex Cu(H, O);+ and the yellow complex CuCl exist in equilibrium. Cu(H,O)*(aq) + 4…

A: We have added LiCl to the equilibrium, we have to tell the effect of this.

Q: Calculate the molar solubility of AgSCN (Ksp = 1.1 x 10^-12) in a solution maintained at pH 9.00 and…

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Q: What are the new concentrations for the standard solutions?

A: Clearly, this is a case of half dilution. 25 mL of aliquote is reacted with Fe(NO3)3 to form the…

Q: B. Determination of the Solubility-Product Constant Absorbance [Ag*] of Ag, Cro, 0.217 1.0g 0.928 1.…

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Q: Find the conditional formation constant, Kr, for FeY² at pH 8.00 given: ay = 4.2 x 10³ and Kp=…

A: Formation constant ( Kf) The equilibrium constant for the reaction with metal with ligand is called…

Q: Develop two methods to quantify Ag+, firstly using acid-base equilibria and then redox equilibria.…

A: An acid is a substance that can enhance the hydrogen ion (H+) concentration when dissolved in an…

Q: Consider the equilibrium reaction: YZ2(s) ⇌ Y2+(aq) + 2Z-(aq). What is the molar solubility of YZ₂…

A: The molar solubility, which is directly related to the solubility product, is the amount of moles…

Q: ne formation constant for [Cu(CN)2] is 1.0 x 1016, what is the value of the dissociation constant…

A: Applying concept of chemical constants relationship between two chemical reaction.

Q: Assuming that no equilibria other than dissolution are involved, calculate the concentration of all…

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Potentiometric Titrations

Potentiometric titration is one of the important titration methods and is mainly carried out to characterize acid solutions. It follows a method similar to that of the normal titration technique, but the main difference is that there is no indicator used in the potentiometric titrations. Instead of using an indicator, electrodes are employed for monitoring the whole titration process. A scientist named Robert Behrend did the potentiometric titration for the first time, and it was done using the mercurous solution and potassium chloride.