Classify each cation as a weak acid or pH-neutral.(a) C5H5NH+ (b) Ca2 + (c) Cr3 +

Q: Identify the conjugate acids and bases in the substances mentioned in question 7(a) above.

A: Conjugate pairs are acids and bases that differ only by a proton (H+).

Q: (b) What are [H3O+], [OH -], and pH in a solution with a pOH of 4.19?

A: Since we know that pH + pOH = 14  => pH for the above case = 14 - pOH = 14 - 4.19 = 9.81

Q: The weak acid HZ has a Ka of 2.55 x 10-4.(a) Calculate the pH of 0.075 M HZ.(b) Calculate the pOH of…

A: Acid dissociation constant Ka is utilized to determine the acidic and basic nature of a solution. It…

Q: The equilibrium system not affected by the pressure change which results from a volume change at…

A:

Q: Give the formula of the conjugate acid:(a) NH₃(b) NH₂⁻(c) nicotine, C₁₀H₁₄N₂

A: The species which accepts a proton in the bronsted acid base theory. The species which accepts a…

Q: 2. Barbituric acid, HC,H,N,O, a weak organic acid used to manufacture hypnotic drugs and some…

A: Here the concentration of barbituric acid is 0.25M and Ka of barbituric acid is 9.8×10^-5. We have…

Q: Calculate the pH of each of the following strong acid solutions. (a) 0.00813 M HBrO4 pH = (b) 0.443…

A: pH of the given solutions

Q: The probe of the pH meter shown here is sitting in a beakerthat contains a clear liquid. (a) You are…

A: The probe of the pH meter shown here is sitting in a beakerthat contains a clear liquid.  (a) You…

Q: The pH of a solution is 4. Which of the following is correct? (A) The solution is basic with an [OH]…

A:

Q: Identify the Lewis acid and Lewis base in each equation:

A: a) Sodium ion accepts the electron pair from water therefore Sodium ion is the Lewis acid, water…

Q: (b) If the pH of water in a lake falls below a value of 5, fish often fail to reproduce. How much…

A: pH is a measure of acidity. pH = – log[H+] [H+]= 10–pH

Q: What is the pH of a solution that has an H+ concentration of                        (a) 1.75 × 10 –5…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: Calculate the pH of each solution and indicate whether the solution is acidic or basic.(a) [H3O+] =…

A: pH of the solution is calculated as, pH =-logH+

Q: (a) What is the pH of 0.75 M NaF?(b) What is the pH of 0.88 M pyridinium chloride, C₅H₅NHCl?

A: a) The pH of 0.75 M NaF is 8.52.

Q: 6.)Calculate the pH of a 0.400M solution of phosphoric acid, H3PO4.

A:

Q: Calculate the concentration of HNO3 in a solution at 25°C that has pH (a) 2.06, (b) 1.77, and (c)…

A:

Q: Calculate the molar H3O+ion concentration of a solution that has a pH of (A) 4.31 (B) 13.89 (C) 5.32…

A: The molar H3O+ concentration can be determined by raising 10 to the negative reciprocal of the pH.…

Q: a) What are [H₃O⁺], [OH⁻], and pOH in a solution with a pH of 3.47? (b) What are [H₃O⁺],…

A: pH is equal to the negative logarithm of hydronium while pOH is equal to the negative logarithm of…

Q: Calculate the pH of each of the following strong acid solutions: (a) 0.0167 M HNO3

A: pH is the measure of the acidity or basicity of the solutions. pH ranges from 0 to 14. If the pH…

Q: (a) What is the pH of 0.0333 M HNO₃? Is the solution neu-tral, acidic, or basic? (b) What is the pOH…

A: The pH of any compound can be calculated on the basis of the concentration of hydronium ions present…

Q: Define a Lewis acid and a Lewis base. (b) Define an Arrhenius acid and an Arrhenius base. (c)…

A: The question is based on the concept of acid and base. we have to identify and explain different…

Q: Classify each as a strong or weak acid or base:(a) RbOH(b) HBr(c) H₂Te(d) HClO

A: Strong bases are those that dissociate completely in the aqueous medium.

Q: Consider 1.3 M HNO2 solution. (a) Show the reaction of dissociation (ionization) of HNO2.  (b)…

A:

Q: Calculate the pH of solutions having the following [H+]: (a) 0.68 M (b) 1.42 M (c) 4.5 × 10-5 M

A: The pH is the negative logarithm of hydronium ion concentration. pH=-logH+

Q: Determine the OH− in a solution with a pH of 3.7.

A:

Q: if [H 3 O+}=0.1M, what is pH?

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.