At 25°C, what is true about ka and kb for a weak acid and its conjugate base? O a. Ka x Kb = 1.0 × 10-14 O b. Kax Kb = 14 О с. Кa / Kb = 1.0 × 10-14 O d. Ka x Kb = 1.0 O e. Ka/Kb = 1.0

Q: The pH of a 0.244 M solution of sodium methanoate, HCOO-Na+, is 8.57. Calculate Kb for the…

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Q: Calculate the pH of 9.3×10−2  M propionic acid (C2H5COOH). Ka= 1.3x10-5

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Q: What is the pH of a solution that is 0.150 M NH3 and 0.200 M NH4CI? Kb of NH3 = 1.8 x 10-5 O9.26…

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Q: 10. How does this equation help you to understand acids and bases: H + OH) + H,O (ag)? It shows you…

A: According to Arrhenius concept of acid and base, acids are the substance that gives H+ ions in an…

Q: Construct the expression for Ka for the weak acid, HCN. HCN(aq) + H:O(I) = H.O(aq) + CN (aq Based on…

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Q: What is the conjugate base in the following reaction: HCI (aq) + H₂O (1) CI (aq) + H3O+ (aq)? O a)…

A: Given -> HCl(aq)  + H2O(l) <-----> Cl-(aq) + H3O+(aq)  -> Conjugate acid is formed when…

Q: Ka for phenol (a weak acid), C6H5OH, is 1.00 × 10-¹⁰. Ka for acetylsalicylic acid (aspirin),…

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Q: What is the correct relationship between Ka and Kb for a weak acid and its conjugate base…

A: We know, Ka × Kb  = Kw Kw is the ionisation constant of water.

Q: The acid dissociation constant K of carbonic acid (H₂CO₂) is 4.5 × 107. Calculate the pH of a 1.3M…

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Q: Equilibrium Concentration (mol/L) 10° 10-1 102 10-3 10-1 105 10-6 10-7 10-8 9.97 x 10-3 55.6 102 101…

A: The answer is-Explanation:Step 1: Step 2: Step 3: Step 4:

Q: 5. a. Determine the hydrogen ion concentration, [H*] for a solution with a pH of 3.42. Is this…

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Q: Acid strength decreases in the series HI>HSO4->HF>HCN. Which of the following anions is the…

A: To solve this problem we have to know about an acid and it's conjugate base .    An acid when…

Q: For each of the following aqueous reactions, identify the acid, the base, the conjugate base, and…

A: According to the Brønsted–Lowry acid base theory, a conjugate acid–base pair consists of two…

Q: Which of the following bases is the weakest? The base is followed by its K, value. O CH,N, 1.7 x 109…

A: The given bases along with their Kb are :

Q: (CH3)2NH is a weak base with a pKa of 11.0 a. Calculate the pH of a solution of dimethylamine at…

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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.