Which has the greater molar solubility:  AgCl with Ksp=1,8 × 10-10 Or  Ag2CrO4 th Ksp = 1,1 × 10 -12

Q: What concentration of SO3 is in equilibrium with Ag₂ SO₂ (s) and 9.40 × 10−³ M Ag+? The Ksp of…

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Q: What is the pH of a buffer that is 0.307 M HF and 0.417 M LiF? The Ka for HF is 3.5 x 10-4.

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Q: A 60.0-mL sample of 0.00200 M AgNO3 is added to 60.0 mL of 0.0100 M NalO3. What is the equilibrium…

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Q: What is the pH of a buffer that is 0.307 M HF and 0.417 M LiF? The Ka for HF is 3.5 x 10-4.

A:

Q: What is the molar solubility of Ag2CO3 in pure water, given that its Ksp= 8.10x10-12?   2.54x10^-3…

A:

Q: Calculate the molar solubility of Ag2 CrO4 in a solution that is 0.01 M in AgNO3. Ksp of Ag2 CrO4 =…

A: Given,  The solubility product of Ag2CrO4 = 1.2 × 10-12  The solubility of Ag2CrO4 in 0.01 M of…

Q: A buffer is prepared by dissolving 0.80 mol of sodium dihydrogenphosphate, NaH2PO4, and 0.60 mol of…

A: Moles of sodium dihydrogenphosphate, NaH2PO4 = 0.80 mol  Moles of sodium hydrogenphosphate, Na2HPO4…

Q: What is the molar solubility of a hypothetical compound AB in pure water given a Ksp = 4.5 x 10-2?…

A:

Q: Calculate the minimum concentration of each of these anions which would be required for…

A: Concentration of [Ag+] = 0.40 M               Given Ksp Find out the minimum concentration of each…

Q: = Ksp of lead(II) carbonate, PbCO3, is 7.40 x 10-¹4. Calculate the molar solubility, S, of this…

A: Solubility product constant (Ksp) is equilibrium constant of solid substance dissolve in aqueous…

Q: Phosphoric acid is a triprotic acid (K₁1 = 6.9 x 10³, K₁2 = 6.2 x 10%, and K3 = 4.8 × 10-1³). To…

A: Given,

Q: What is the molar solubility of strontium carbonate in a solution that contains 0.19-M SrCl2?…

A: Data given: Concentration of SrCl2 = 0.19 M Ksp (SrCO3) = 9.3 × 10–10

Q: The Ksp for Ag2CO3 at a certain temperature is equal to 8.59x10-12. What is the molar solubility of…

A: Sparingly soluble salt are dissolved is water partially.

Q: What pH is required to reduce a high concentration of a dissolved Mg2+ to 25 mg/L? The solubility…

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Q: The molar solubility of palladium (II) thiocyanate at 25°C is 2.22 x 10-8 M. What is its Ksp value?…

A: molar solubility=S=2.22×10-8M KSP=?

Q: What is the molar solubility of AgCl in 0.10 M NH3? Ksp for AgCl is 1.8 × 10-10 and the Kf for…

A: The solubility product constant (Ksp) represents the solubility of products at equilibrium for…

Q: How many moles of solid NaOH must be added to 1.0 litre of H2O  in order to dissolve 0.10 mole of…

A: The 0.20 moles of solid NaOH must be added to 1.0 litre of water to dissolve 0.10 mole of…

Q: Determine the molar solubility of BaF 2 in pure water. K sp for BaF 2 = 2.45 x 10 -6. 2.45 x 10 -6…

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Q: For which salt should the aqueous solubility be most sensitive to pH? O Ca(NO3)2 O Cal2 O CaF2 O…

A: The aqueous solubility of a salt can be influenced by pH when one of the ions in the salt undergoes…

Q: hat is 0.10M in AgNO3 and 0.075M in NaCl. What will happen once these solutions are mixed?…

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Q: Which of the following salts has the highest molar solubility in pure water? 1 2 3 4 5 O O O 1 3 4 5…

A:

Q: 19) What is the molar solubility of AgCl in 0. 30 M NH3? Ksp for AgCl is 1.8 x 10-10 and Kf for…

A: Answer: When AgCl is added in the ammonia solution then Ag+ ion reacts with NH3 to form a soluble…

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.