Which of the following is a conjugate acid-base pair? A) OH-, H2O B) NH3, OH- C) OH¯, NH.* D) H:O, NH.

Q: [OH-] = 4.2 x 10-2 Express the concentration to two significant figures and include the appropriate…

A:

Q: In an acidic solution the H;O' concentration is concentration. (greater than/less than) the OH In a…

A: Concept: 1. The acid in aqueous solution give H3O+ ions. So as the concentration of H3O+ increases,…

Q: Which of the following can act as either a Bronsted acid or a Bronsted base? A. ) HCl B) PO4^-3…

A: Bronsted Acid-Base An species which is capable of donating a proton is called an acid whereas a…

Q: 1)Write balanced molecular equations for the neutralization of equal molar amounts of the following…

A: When acid an base reacts with each other, they produce water salt and heat. This reaction is also…

Q: A solution has a [H3O+] of 0.0015 M. Calculate the [OH-], the pH, and the pOH of the solution. Is…

A: In the question is given that concentration of [H3O]+  is 0.0015. i.e. [H]+ = 0.0015 [OH]- = ? pH =…

Q: 2) A) HClO4 B) HI C) HCl D) HF E) HNO3 Which one of the following is a weak acid?

A:

Q: In each of the chemical equation below, identify whether water is acting as an acid or a base.…

A: An acid can be defined as the substance which is capable of donating a proton H+ while a base is a…

Q: How do you find H3O+ from molarity, pH or pOH/OH-?

A: pH = - log [H3O+] pOH = - log [OH-] pH + pOH  = 14   [H3O+]  = 10-pH  [OH-] = 10-pOH    [H3O+] [OH-]…

Q: Calculate the H3O+ concentration from each pH: (a) 7.82;    (b) 13.96.

A: FORMULA  We can calculate HydroNium ion concentration  by using formula  [H3O]+ = 1 × 10-PH a) 7.82…

Q: Write down the equation for the reaction of the following acids with water and identify the…

A:

Q: Determine [H3O+] in each acid solution. If the acid is weak, indicate the value that [H3O+] is less…

A:

Q: Identify which of the following compounds CANNOT be classified as a Bronsted-Lowry base: H3C Na IV…

A: Bronsted–Lowry base is a proton acceptor. Bronsted-Lowry Acid is a proton donor.

Q: The pOH of a basic solution is 3.89. What is [OH-]?

A: Since, Negative logarithm of concentration of OH- ion is known as pOH of the solution. i.e. pOH =…

Q: 00 HO O more than one response is correct 19. Apply the Bronsted theory of acids and bases to the…

A: We have to predict acids and bases according to bronsted theory.

Q: CH3OH  is not a base. Why? A) because it's an acid B) because it's nonpolar C) because it's a…

A: Why is methanol not a base

Q: 19) Amphoteric substances can act as either an acid or a base. Which of the following is amphoteric?…

A: Amphoteric substances are those compounds which act as both an acid and a base.They can release a…

Q: 1) Which of the following compounds are amphoteric? -both HSO3^- and O^2- -HF -CO3^2- -O2 -BF3…

A: A solution is said to be acid if the solution contains amount of H+ higher than amount of OH- , then…

Q: Sulfuric acid is a strong acid because 0 has low astion disecites completely in water O Monices in…

A: (3) • Strong acids:-  An acid that completely dissociates into the water, is understood to be a…

Q: An aqueous solution of which of the following salts are basic? A) NANO3 B) K:SO: C) NH:CI D) NaBr E)…

A: A solution of any salt will be basic if it is formed by strong base and weak acid.

Q: What H 3O + concentration corresponds to each pH value: (a) 10.2; (b) 7.8; (c) 4.3?

A: Given data   pH value part(a) 10.2 part(b) 7.8 part(c) 4.3 Useful formula to calculate…

Q: cid. (CH)3 NH. Explanation is required

A: In this question it is mentioned that 2°amine (CH3)2NH is acid. But this is basic in nature because…

Q: If the pH of an acid solution at 25°C is 6.18what is the POH ; and the [H^ 1+ ],[OH^ 1-) in mol / L?

A: At 25°C, given that;   pH of the acidic solution = 6.18   pOH of the that solution = to be…

Q: Calculate the H3O+ concentration from each pH: (a) 2.42;    (b) 13.39.

A:

Q: The pressure of a gas in flask is 430.2 mmHg, what is the pressure in atmosphere (atm)? ( 1atm = 760…

A: Unit conversion involves the conversion of magnitude in one unit to the other unit. It may involve…

Q: 54 For each of the following solutions, calculate [OH ] from [H;O*], or [H30*] from [OH]. Classify…

A: Since, you have given multiple subparts, we will solve the first 3 subparts for you. For other parts…

Q: In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a…

A: Given, the chemical reaction is as follows,C6H5NH2(aq) +H2O(l)   → C6H5NH3+(aq)+ OH-(aq)we are asked…

Q: Write the formula of the conjugate base of each acid: HCI, HPO,?-, and CH3CH,OH. Be sure to answer…

A: Conjugate base is formed by lose of one proton from an acid.

Q: The following equation shows the equilibrium in an aqueous solution of ammonia: NH3 (aq) + H2O(l) ⇌…

A: Conjugate acid can be defined as the species which can donate a proton H+ and conjugate base is the…

Q: The conjugate base of HCIO is: (a) HCI (b) ClO- (c) H+ (d) none of these

A: The acid given is HClO.

Q: Part A Calculate (OH] in the following aqueous solution at 25 °C: [H3O*] = 1.6x10-8 mol - L Express…

A: Answer :-  A) [OH-] = 6.7 × 10-7 (mol.L-1)  B) The solution is Basic…

Q: Which of the following is the strongest acid? A. CH3CH₂OH B. CH3OCH3 С. D. E. CH3CH O CH3COCH3 || O…

A: The strength of an acid depends on the stability of its conjugate base.The stronger an acid, the…

Q: For the reaction H,0 + SO, ? «HSO, +0H¯, water behaves as a(n) O acid O base O both acid and base O…

A: Bronsted-Lowry acid-base theory: According to the Bronsted-Lowry acid-base theory, acid is a…

Q: Identify the weak acid from the list. - HF - H2CO3 - H2SO2 - all of these

A: The species that increase the concentration of hydrogen ions or hydronium in an aqueous solution act…

Q: 33. Which set represents a conjugate acid/base pair? (A) H₂PO. and HPO (C) H₂PO. and H₂PO 34. For…

A: The objective of this question is to show the given chemical equations contain species that,…

Q: Which of the following weak acids has the weakest conjugate base? Acid (a): H3PO4 Acid (b): H₂PO4…

A: The compounds containing more than one ionizable hydrogen (H) atom are identified as polyprotic…

Q: How would I the conjugate acid and the base including ions pair and electron

A: Conjugate acid is a species able to donate proton and formed by accepting a proton of a acid.…

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.