For the diprotic weak acid H2A, K = 3.3 × 10-6 and K2 = 6.1 x 10-9 %3D What is the pH of a 0.0800 M solution of H, A? pH = 1.09 %3D Incorrect What are the equilibrium concentrations of H, A and A²- in this solution? [H,A] = 0.08 %3! (A-] = 9.74 x10¬4

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Q: For the diprotic weak acid H2A, Kal = 3.8 × 10-6 and K2 = 7.8 x 10-9. What is the pH of a 0.0750 M…

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Q: For the diprotic weak acid H2A, Ka1 = 3.0 × 10-6 and Ka2 = 7.1 x 10-9. What is the pH of a 0.0700 M…

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Q: For the diprotic weak acid H2A, Kal = 3.7 x 10-6 and Ka2 = 6.9 x 10-9. What is the pH of a 0.0550 M…

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Q: For the diprotic weak acid H₂A, K₁1 = 2.3 x 10-6 and K₁2 = 6.5 x 10-⁹. What is the pH of a 0.0550 M…

A: Given that for diprotic weak acid,  Ka1 = 2.3 × 10-6 Ka2 = 6.5 × 10-9  Initial concentration of H2A…

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Q: For the diprotic weak acid H2A, Kal = 3.7 × 10-6 and K2 = 6.9 × 10-9. What is the pH of a 0.0550 M…

A:

Q: For the diprotic weak acid H₂A, K₁1 = 3.5 x 10-6 and K₁2 = 8.3 × 10-⁹. What is the pH of a 0.0500 M…

A:

Q: For the diprotic weak acid H₂A, Kal = 3.7 x 10-6 and Ka2 = 6.1 x 10-⁹. What is the pH of a 0.0800 M…

A:

Q: (1) [H*] %3D 1.59 x 10-7 м (II) [H+] = 1.04 x 10-8 M 4.0 (а) pHI = 49 %3D PHII 4.0 %3D (I) [H*] 5.69…

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Q: For the diprotic weak acid H,A, Kal = 3.2 x 10 and Ka2 = 6.3 x 10-9 What is the pH of a 0.0800 M…

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Q: For the diprotic weak acid H 2 A, K a1 = 3.7 x 10 5 & K a2 = 5.7 x 10 -7 What is the pH of a 0.0600…

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Q: For the diprotic weak acid H2A, Kaj = 3.1 x 10-6 and Ka2 = 8.9 x 10-9. What is the pH of a 0.0550 M…

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Q: For the diprotic weak acid H,A, Kal = 2.4 x 10-6 and K2 = 6.9 × 10-9. What is the pH of a 0.0500 M…

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A: HC3H5O2 (aq) <---> C3H5O2- (aq) + H+ (aq)  Ka = ([C3H5O2-] [H+] / [HC3H5O2]) Ka = 1.3 × 10-5…

Q: For the diprotic weak acid H2A, Kal = 3.1 x 10-6 and Ka2 = 5.6 x 10-9. What is the pH of a 0.0650 M…

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A:

Q: For the diprotic weak acid H2A, Kal = 2.3 x 10-6 and K2 = 6.9 × 10-9. What is the pH of a 0.0600 M…

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Q: For the diprotic weak acid H2A, Kal = 2.5 × 10-6 and K2 = 6.5 x 10-9. What is the pH of a 0.0400 M…

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Q: For the diprotic weak acid H₂A, Kal = 2.8 × 10-º and K₁2 = 7.5 × 10-⁹. What is the pH of a 0.0650 M…

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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.