Estimate the equilibrium constant for the system indicated at 25oC.     3 Mg2+ + 2 Al --> 3 Mg + 2 Al3+     A.   ~10-36   B.   ~1069   C. ~1023 D.   ~10-24   E.   ~10-72

Q: Calculate the molar concentration of Agtao) kons in a 2.12 M solution of AgCl 2 with no excess…

A:

Q: Determine the molar solubility of Al(OH)3 in a solution containing 0.0500 M AlCl3. Ksp (Al(OH)3) =…

A: Given : Concentration of AlCl3 = 0.0500 M And Ksp of Al(OH)3 = 1.3 X 10-33

Q: Consider an amphoteric hydroxide, M(OH), (s), where M is a generic metal. Kp = 6 x 10-16 K¢ = 0.08…

A: To determine the solubility of M(OH)2 at PH 7. Ksp =6 x 10-16. The concentration of OH- . pH =7.…

Q: A 50.0 mL sample of 0.0543 M AgNO3(aq) is added to 50.0 mL of 0.100 M NaIO3(aq). Calculate the [Ag+]…

A:

Q: Calculate the molar solubility of CuS in a medium containing H;S at pH=1 and pH=4. KspCus =…

A: Part A -log H+ = 1 H+ = 10-1 = 0.1 HH2S ⇌ H++HS-  , Ka1 = 5.7 x 10-8Ka1 = H+HS- H2S5.7 x 10-8 =…

Q: In the presence of I-, Hg2+ forms the complex ion Hgl4²-. The equilibrium concentrations of Hg2+ and…

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Q: What is the molar solubility of Ag2SO4 in 1.1 M Na2SO4? Ksp(Ag2SO4) = 1.5 × 10-5?

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Q: Determine the molar solubility of Al(OH)3 in a solution containing 0.0500 M AICI3. For Al(OH)3, Kp =…

A: Given : Concentration of AlCl3 = 0.0500 M And Ksp of Al(OH)3 = 1.3 X 10-33  Since AlCl3 is…

Q: The solubility product of AgCl at 25°C is 1.44 x 10-10. Calculate the solubility of AgCl in 1.0…

A: Common ion effect : AgCl is a weak electrolyte. It has very less solubility . When KCl ( strong…

Q: f 27.5 mL of 1.63x10-9M of FeCl3 is added to 98.6mL of 2.58x10-9 M NaOH, will a precipitate of…

A: The question is based on the concept of solubility product principle. it  states that a weak…

Q: A 1.00-L solution contains 2.50×10-4 M  Cu(NO3)2 and 1.00×10-3 M  ethylenediamine (en). The Kf for…

A:

Q: A solution (total volume = 1L) of 0.4 M NH3 contains 12.78 g of NH4CI (MW = 53.491 g/mol). Kb = 1.8…

A: First we would Calculate initial pH of solution before adding HCl.  Then pH after adding HCl is…

Q: mmonia solution, NH3. ) Calculate the pH value of the mixture. i) Calculate the concentrations of OH…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: Calculate the concentration of dissolved sulfate ion in solution if 75.0 mL of a 0.0250 M Ba(NO3)2…

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Q: To 20,00 ml of 0,0500 mol/l solution of potassium bromide – 19,90 ml of solution of silver nitrate…

A:

Q: Calculate the molar solubility of Ag2SO4. Ksp = 1.5 × 10-5 O 0.016 M O 0.0027 M O 0.0039 M O There…

A: Ag2SO4 dissociates as :  Ag2SO4  ----> 2Ag2+ + SO42-  Solubility product, ksp given= 1.5 × 10-5

Q: Determine the molar solubility of CuCl in a solution containing 0.050 M KCl. Ksp (CuCl) = 1.0 ×…

A:

Q: The solubility product constant of silver arsenate is 1.0x10-23 (ksp) the molar slubiility of…

A: The solubility reaction of Ag3AsO4 can be written as, => Ag3AsO4 (s) ------> 3 Ag+ (aq) +…

Q: 9- Hydrolysis constant of ammonium chloride is ----- (when Kw & Kb are 1x10-14 & 1.8 x10-5…

A: There is following relationship between acid Dissociation constant, Ka , base Dissociation constant…

Q: For the aqueous [Ni(NH3 )6]2+ complex Kf=5.50 x 108 at 25C . Suppose equal volumes of 0.0024 M…

A: Given :  Kf = 5.50 x 108   Concentration of Ni(NO3)2 = 0.0024 M  Concentration of NH3 = 0.94 M

Q: Percent variance for Kc for Fe3+ + SCN- Fe(SCN)2+ = 110%, the average value for kc = 186 Percent…

A:

Q: What is the molar solubility of AgCI (Ksp = 1.8 x 10-10)? %3D A 7.31 x 10-5 M B 5.13 x 10-6 M 3.84 x…

A: The explanation is given below-

Q: What is the molar solubility of a hypothetical compound AB in a solution containing 19.92 M B- given…

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Q: Calculate the pOH of a 0.0267 M aqueous sodium cyanide (NaCN) solution at 25.0 °C. Kb for CN- is 4.9…

A: Answer is explained below.

Q: The solubility product constant for La(IO3)3 is 1.00×10-11 at 25 oC. How many grams of La(IO3)3 can…

A: Given, solubility product constant for La(IO3)3 is 1.00×10-11 0.100 M KIO3

Q: : For PBC12 (Ksp = 2.4 x 10-4), will a precipitate of PbCl2 form when 0.10 L of 3.0 x 10 2M Pb(NO3)2…

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Q: Calculate the molar solubility of zinc carbonate in ZnCO3(s)  Zn2+(aq) + CO32-(aq)…

A:

Q: If 10.0mL of 2.0x10^-3 M Cr(NO3)3 is added to 10.0mL of a pH = 10.0 NaOH solution, will a…

A: The number of moles of a substance is given as the mass of a substance upon its molar mass. The pH…

Q: mass of NaCH3COO must be dissolved in 400 mL of 0.46 M CH3COOH in order to prepare a solution with…

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Q: 5.00 mL of 5.00 x 103 M Fe(NO3)3 (5.00 times 10 to the minus 3rd power M Fe (NO3)3) is added to 7.00…

A: Given: Concentration of Fe(NO3)3 taken = 5.00 × 10-3 M Volume of Fe(NO3)3 solution taken = 5.00 mL…

Q: Calculate the solubility of AgCl(s) in 2.0 M NH3(aq). Ksp = 1.6 × 10-10 for AgCl Kf = 1.7 × 107 for…

A: Given: Ksp = 1.6 × 10-10 for AgClKf = 1.7 × 107 for Ag(NH3)2+(aq) We have to calculate the…

Q: What is the molar solubility of Ag2SO4 in a solution that is 0.0522 M AgNO3? Ksp= 1.40x10^-5

A:

Q: What is the molar solubility of a hypothetical compound AB in a solution containing 19.92 M B- given…

A: We have to predict the molar solubility.

Q: Consider an amphoteric hydroxide, M(OH), (s), where M is a generic metal. M(OH), (s) = M²+(aq) + 2…

A: The reaction is as follows: M(OH)2(s)⇌M2+(aq)+2OH-(aq) 1) Calculation of concentration of OH- at pH…

Q: 50.0 ml of 0.01 M Cd(NO3)2 is added to 50.0 ml of 0.1 M H2S. Will a precipitate form? (the Ksp of…

A: All known compounds can be dissolve in certain solvents whereas they remain insoluble in other…

Q: What is the molar solubility of Ag2SO4 in the presence of 1.52 M aqueous solution of AgNO3?…

A: Given : [AgNO3] = 1.52M  Ksp = 1.5 x 10-5

Q: 13.0 mL of 0.19 M MgCl2 are mixed with 21.9 mL of 0.54 M NaOH, what will be the final concentration…

A:

Q: Calculate the molar solubility of Ag2S in a solution maintained at pH 11.00 and where the…

A: The overall chemical equation of the given system and Koverall is calculated as shown below.

Q: Calculate the concentration of dissolved sulfate ion in solution if 75.0 mL of a 0.0250 M Ba(NO3)2…

A:

Q: Calculate the pH of a solution saturated in calcite and in equilibrium with atmospheric CO2. The…

A: In the mentioned system, the following equilibria persists: CaCO3(s)→Ca2+(aq)+CO32-(aq)…

Q: Consider the equilibrium shown. SrF, (s) = Sr² +(aq) + 2 F¯(aq) Ksp = 2.60 × 10-9 Determine the…

A: The equation is as follows: SrF2(s)-->Sr2+(ag) + 2F-(ag)The Ksp expression for this reaction is…

Q: Determine the molar solubility of MF2 in a solution containing 0.0952 M KF. Ksp MF2  =  1.71 × 10–6…

A: The common ion effect is all about the effect on ​equilibrium that happens when a common ion is…

Q: A 0.5 L aqueous solution of 0.05 M Ca(NO3)2 is mixed with 2.0 L aqueous solution of 0.01 M NaF.…

A:

Q: Calculate the molar solubility of Mg(OH) 2 in a solution with pH = 12.20. (K sp (Mg(OH)₂ = 1.2 x…

A:

Q: Solid potassium hydroxide is slowly added to 175 mL of a 0.318 M nickel(II) acetate solution until…

A: Soluble compounds which are also known as strong electrolytes possess large solubility product (Ksp)…

Q: A solution in part C initially contains (4.06x10^-4) molar SCN and (2.960x10^-3) molar Fe3+. This…

A: Given the initial concentration values of the reactants: [SCN-(aq)]i = 4.06*10-4 M [Fe3+(aq)]i =…

Q: Determine the molar solubility (moles/L) of Ni(OH)2. Ksp = 2.0 x 10-15 Express the answer to 3 sig.…

A: Using equilibrium concept and using Ksp value we can find molar solubility. Given Ksp = 2 * 10-15

Q: A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the value of Ka for the weak…

A:

Q: Ksp for Agl = 1.2 x 10-17. Calculate the molar solubility of Agl in 1 x 10-4 molar AGNO3 solution. O…

A: The given data contains, Ksp for AgI=1.2×10-17Ag+=1×10-4 M.

Q: Sn(OH), 48 = 5.45 x 10-27 CUCN K,= S =3.47 x 10- MgF; = 45- 5.16 x 10-1 NICO, K„ = s² = 1.42 × 10-7…

A: Given Substance        KspSn(OH)2         Ksp = 4S3 = 5.45×10-27CuCN             Ksp  = S2 = 3.47…

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.