(b) Hydrazine, N2H4, is a Brønsted-Lowry base used as a rocket fuel. Write the formula for the conjugate acid of hydrazine.   (c) Phenol, HOC6H5, is a Brønsted-Lowry acid used to make plastics, nylon, and slimicides. Write the formula for its conjugate base.   (d) Aniline, C6H5NH2, is a Brønsted-Lowry base used to make polyurethane. Write the formula for its conjugate acid

Q: What is the pH of a .100M CH3COOH(aq) solution?

A: Acetic acid is a weak acid, it does not dissociate completely but exists in equilibrium with acetate…

Q: Calculate the pH of a solution prepared by dissolving 2.05 g of sodium acetate, CH3COONa, in 71.0 mL…

A:

Q: If a 10 L sample of sulfuric acid contains 0.843 mol of hydronium ions, what is the pH of the…

A: Given ,Volume of sulfuric acid = 10LHydromium ion = 0.843 molwe have to find pHpH = - log [ H3O+]

Q: Complete the equation for the dissociation of NH4NO3(aq). Omit water from the equation because it is…

A:

Q: cation acts as an acid.

A:

Q: The acid dissociation constant Ka of hypobromous acid HBrO is 2.3 x 10^−9. Calculate the pH of a…

A:

Q: The equilibrium expression for any weak acid can be written as HA (aq) + H2O (1) = A- (aq) + H3O+…

A: The equilibrium constant of a chemical reaction  at equilibrium is defined as the ratio of the…

Q: Write the formula of the conjugate base of CH₃CO₂H.

A: Given  Acid =  CH3COOH  formula of Conjugate base = ?

Q: pH

A:

Q: The pH of an aqueous solution of 0.1690 M hydrosulfuric acid, H₂S (aq), is

A: The question is based on the concept of pH of the solution.  it is defined as a negative logarithm…

Q: The substance trimethylamine is a weak nitrogenous base like ammonia. Write a net ionic equation to…

A:

Q: The pH of an aqueous solution of 0.0916 M ascorbic acid, H2C,H,06 (aq), is

A: pH = −log [H+] Where, [H+] is molar concentration of the H+ ion.

Q: For the following acid-base reaction, (1) predict the products, showing both reactants and products…

A:

Q: Calculate the concentration of HS in an aqueous solution of 6.29x10-2 M hydrosulfuric acid, H₂S…

A:

Q: Write the formula of the conjugate base of C₆H₅SH.

A: According to Bronsted and Lowry theory, when an acid releases a proton, the remaining part must be a…

Q: The pH of an aqueous solution of 0.532 M hydrofluoric acid, ( K₂ (HF) = 7.20 × 10¯4) is

A: Concentration of HF solution (C) = 0.532 MKa for HF = 7.20 × 10-4 pH of the solution = ?

Q: Determine the pH of 0.231 M Ca(OH)2 (aq

A: Given:Concentration of Ca(OH)2 = 0.231 MWe have to determine the pH of the solution

Q: The pH of an aqueous solution of 0.259 M hydrosulfuric acid, H2S (aq), is .

A: Given Concentration of H2S = 0.259 M

Q: In a solution of 0.015 mol L-1 HBr(aq) at 25 °C (a) What are the concentrations of the hydronium,…

A: pH stands for the potential of hydrogen ion concentration or power of hydrogen. The pH of an aqueous…

Q: Estimate the pH of 0.010 M NaCH3CO2(aq).

A:

Q: What is the pH and the pOH of a 0.0125 M KOH solution at 100.0 °C? The value for Kw for water is…

A: Concentration of KOH solution as 0.0125 M at 100 °C

Q: The pH of an aqueous solution of 0.021 M hydrosulfuric acid, H2S (aq), is .

A: H2S is a weak diprotic acid. Since the Ka2 of H2S is << Ka1 of H2S  Hence we can assume only…

Q: 7. Identify the Brønsted-Lowry acid, the Brønsted-Lowry base, the conjugate acid, and the conjugate…

A:

Q: What is the pH of 5.35 x 103 M H2CO3 (aq)? O 4.3 O 8.6 O 2.3 O 4.9 O 9.1

A: Concentration of H2CO3 = 5.35 × 10-3 M  pH of the H2CO3 = ?

Q: The pH is measured to be 2.58 for a solution of 0.035 M cyanic acid, HOCN (aq). Write the hydrolysis…

A: HOCN is a weak acid. Weak acid are those acid which does not dissociates completely in equilibrium.…

Q: 5. A solution is initially 0.050 M in ammonia, NH3 (Kp = 1.8 x 10°). (a) Write the equilibrium…

A:

Q: For C6H5NH3, enter an equation that shows how the cation acts as an acid. Express your answer as a…

A: Bronsted Lowry acid: It donates proton (H+ ion) to other compounds and form conjugate base.

Q: Explain how ammonia can function both as a Brønsted base and as a Lewis base.

A: According to Bronsted-Lowry concept, the acidic and basic character of a compound can be interpreted…

Q: What is the pH of a 0.138 M solution of H2SO4 (sulfuric acid)?

A: We will use formula of pH

Q: The substance morphine is a weak nitrogenous base like ammonia. Write a net ionic equation to show…

A: The compound which accept H+ is known as base.  Here morphine is base.

Q: A solution of 1.7×10−6 M HNO3(aq) (10.0 mL) is diluted to 10.0 L with pure deionized water at 25 °C…

A:

Q: 1. Solid NH4NO3 dissolves in water and then reacts with KOH (aq). The container releases a smell as…

A: When aqueous solution of NH4NO3 treated with KOH, acid - base reaction occurs.Here we have to give…

Q: Determine the pH of each of the following solutions (Ka and Kb values can be found in the appendices…

A: (a) 0.045M hypochlorous acid  pKa  value = 7.53 Now, pH = (1/2)(pKa   - log[HOCl]                  =…

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.