Calculate the [OH-] of a strong acid solution that is 8.8 x 10-3 M HCl.

Q: Determine the pH of a solution with [OH] = 1.8  10-4 M and indicate if thesolution is acidic,…

A: The objective of this question is to determine the pH of a solution given the concentration of…

Q: In the following equation, identify the acids, bases, and conjugate pairs. NH4+ CN NH3 + HCN (a)…

A:

Q: Calculate the [H+] and pH of a 1.39×10-4 M butanoic acid solution. The Ka of butanoic acid is…

A: The objective of this question is to calculate the concentration of hydrogen ions [H+] and the pH of…

Q: 4- A solution is prepared by adding 50.0 mL of 0.050 M HBr to 150.0 mL of 0.10 M HI. Calculate [H*]…

A: [H+] and pH of the solution is to be calculated.

Q: If we used H2C4H4O5 as the weak diprotic acid, which of the four species, H2C4H4O5, HC4H4O5^-,…

A: Given that, H2C4H4O5 is a weak diprotic acid & the four species are H2C4H4O5, HC4H4O5-,…

Q: What is the pH of a solution in which 15 mL of 0.39 M NaOH is added to 25 mL of 0.39 M HCl?

A: Since NaOH and HCl are strong base and acid respectively Hence they will react as per the reaction…

Q: Chloroacetic acid, HC2H2ClO2, has a greater acid strength than acetic acid, because the…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Rank the solutions in order of decreasing H3O|.

A: Acids donate [H+] ions and increase H+ ions concentration in the solution  Strong acids…

Q: Rank the 0.06 m aqueous solutions of monoprotic acids from the weakest acid to the strongest acid.…

A: Solution and their Ka values0.06 m acetylsalicylic acid (HC9H7O4)      3.31×10-4 0.06 m hydroazoic…

Q: Calculate the pH for the following reaction: NaOH   +   HCO2H   --->   H2O   +   HCO2-   +   Na+…

A: The Balanced chemical equation for the reaction between HCO2H and NaOH is                      HCO2H…

Q: Calculate [OH⁻] in a solution obtained by adding 1.50 g solid KOH to 1.00 L of 10.0 M NH₃. (Kb of…

A: Given: mass of KOH = 1.5 g volume = 1.0 L Molarity = 10.0 M NH3 Kb of NH3 = 1.80×10-5  moles of NH3…

Q: The Kb of C6H5NH3+ is 3.98x10-10 1. What is its Ka? 2. What is the [H3O+] concentration in a…

A:

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.