neu as Question 8.07 Carbonic acid is a diprotic acid while formic acid is not. Why? (It may be useful to draw the structure for HCO2H.) What would have to happen for formic acid to be diprotic? How is that different from carbonic acid?

Q: The pH of a solution of a strong base is 10.51 at 25°C. What is its hydronium-ion concentration

A: Given that  The pH of a solution of a strong base is 10.51 at 25°C. The hydronium-ion concentration,…

Q: calculate the number of hydronium ions in 98.80 mL of an aqueous solution with a pH of 5.14

A: The objective of this question is to calculate the number of hydronium ions in a given volume of an…

Q: H3PO4 is another polyprotic acid with three acidic hydrogens.  Write a complete balanced equation…

A: Net Overall reaction:- 3NaOH + H3PO4 = Na3PO4 + 3H2O Phosphoric is a triprotic acid: it can “give…

Q: Calculate the pH of a 0.307 M NH3 solution. NH3 has a ?b=1.8×10−5.

A: First of all a balanced reaction should be written for the solution: Here, water concentration is…

Q: why an atom in the species must possess a lone pair of electrons for it to act as a Brønsted base

A: To find: Why an atom in the species must possess a lone pair of electrons for it to act as a…

Q: True or False: A substance that is acidic has very few hydronium ions present.

A: We know that  PH= -log[H+] We can observe from above formula As the no of mole of H+ increase PH…

Q: Complete the ?w expression for the autoionization of water. ?w=1.00×10−14=

A: The Kw expression for the auto-ionization of water is to be completed- Kw =1.00×10−14 =

Q: Polyproctic entities react with water multiple times and in each reaction a proton is transferred.…

A: The acids which  have more than  one acidic protons(H+) are known  as polyprotic acids. Carbonic…

Q: Summarize the important difference between strongacids and weak acids in terms of the battle of the…

A: ANSWER IS DISCUSSED BELOW :

Q: The products of the self - ionization of water are: H,0 and H,0 OH and H- HO- and OH OH and H*

A: The self-ionization of water or auto ionization of water is an ionization reaction in pure water or…

Q: Hydrogen selenide (H2Se) reacts with water according to the following equation. H2Se + H2O → SeH– +…

A:

Q: match the terms to the correct definition. (A choice that describes a property of an acid, but is…

A:

Q: What are the Four factors affect the acidity of HA ?

A:

Q: Pure water has a pH value of 7.0. How many times more acidic is apple juice, with a pH value of 6.6,…

A: Given-> pH of pure water = 7.0 pH of apple juice = 6.6

Q: Write an equation for the reaction that takes place when each acid is added to water. For a…

A: When acid is added into water then ionisation of acid take place.

Q: Ph for H3O+ = 2.19 × 10‐11

A: pH is negative logarithm of hydrogen ions

Q: What is the pH of a 6.7 × 10⁻⁴ M HClO₄ solution?

A: Consider the dissociation of HClO₄ in water is as follows;      It is given that one molecule of…

Q: HNO3(aq) - Ba(OH)₂ (s) H₂O HF (aq) H₂O H₂O

A: -> The species which behaves as acid that can produce Hydronium ion when dissolved in water .…

Q: Distinguish between Arrhenius’ theory and Bronsted-Lowry’s theories of acids and bases. Why was the…

A: The objective of the question is to understand the differences between Arrhenius’ theory and…

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.