Given that Agl would precipitate first than AgCl in a solution containing equimolar concentrations of I and CI, it can be concluded that: A. Ksp.Agi Ksp.AgCI B. Ksp.Agl< Ksp.AgCl C. Ksp.Agl Ksp.AgCI D. Cannot be determined

Q: Write solubility product constant expression and calculate numerical value (Ksp) of each ionic…

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Q: A chemist does a reaction in which H and I react to form J The chemist used solutions that were…

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Q: Consider the following equilibria: Equilibrium I: H,Og + C - Equilibrium II: Cr2O4 (aq) + 2H“(aq)…

A: The Le Chatelier's principles deal with the equilibrium of a reaction. It mainly predicts the…

Q: PART 1- Determination of solubility product (Kp) of different salts Table 1 - Solubility of Ag:SO4…

A: The balanced chemical equation for the solubility of Ag2SO4 is Ag2SO4(s)+H2O(s)…

Q: 4. a. b. C. d. e. Consider the following reaction: CO (g) + H₂O (g) CO₂ (g) + H₂ (g) Kc = 9 The…

A: Answer:- This question is answered by using the simple concept of calculation of equilibrium…

Q: Phosphorus pentachloride decomposes according to the chemical equation PCI,(g) = PCI,(g) + Cl,(g) K…

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Q: solution a. Calculate the number of moles of Fe and SCN added. b. Calculate the number of moles of…

A: (a) Volume of Fe3+ added = 5.0 mL [Fe(NO3)3] = 0.002 M Total volume = 10 mL Moles of Fe3+ added =…

Q: Consider a saturated solution of lead sulfide, PbS, in water. PbS(s) ⇌ Pb2+(aq) + S2-(aq) What is…

A: When a reaction is at equilibrium and then more reactants are added to it then according to Le…

Q: At a certain temperature, 0.307 mol CH, and 0.954 mol H,S are placed in a 3.50 L container. CH,(g)…

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Q: Write the equilibrium constant for the following reactions: a. 3NOg+ N2Og + NO2 b. Ni(CO)4lg +→…

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Q: 6. What is the equilibrium concentration of silver ions at 25°C in a 1.0L saturated solution of…

A: Solubility product is the product of concentration term of each ions present in dissolution reaction…

Q: How many grams of precipitate will form if 25 g of NH4CI is added to 50 mL of water at 55 degrees C?

A: By using the reference of solubility graph. At 55°C, The mass of NH4Cl soluble in 100 grams of water…

Q: 7. Ammonia can be synthesized according to the equation: 1/2 N₂(g) + 3/2 H₂(g) → NH3(g). The…

A: 7. Recall the given equation,                                12 N2 g + 32 H2 g → NH3 g…

Q: The Solubility Product Constant for silver iodide is 1.5 × 10-16. The molar solubility of silver…

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Q: Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of…

A: Given,volume of the tank = 75. LInitial moles of nitrogen dioxide = 27. molmoles of nitrogen dioxide…

Q: C. Iron(III) Chloride plus Potassium Thiocyanate 1. What is the evidence for a shift in equilibrium…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: The molar solubility of cobalt(II) carbonate in a 0.187 M sodium carbonate solution is _____ M.

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Q: The Solubility Product Constant for calcium carbonate is 3.8X10^-9 The molar solubility of calcium…

A: Write the dissociation reaction for calcium carbonate and on the basis of that, find out the…

Q: 4. Explain how temperature of a reaction can affect equilibrium. Be specific.

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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.