Write the formula for the conjugate base of each acid. (a) H2SO4 (b) H3BO3 (c) Hl (d) H3O+ (e) NH4+ (f) HPO42-

Q: The hydronium ion concentration of an aqueous solution of 0.591 M aniline (a weak base with the…

A: Given values -> Concentration of aniline = 0.591M Kb (aniline) = 4.3 × 10^-10

Q: Calculate the pH of the following acid or base: 1. 3.6x10 M HNO,

A: pH stands for hydrogen potential in a solution. Low pH (less than 7.0) - Acidic pH  pH = 7.0 -…

Q: Carbon dioxide in the atmosphere dissolves in raindrops toproduce carbonic acid (H2CO3), causing the…

A: To find the range of [H+] and [OH-] in the raindrops can be given by- Since, Product of the both…

Q: 6. 7 6. 10 11 12 13 Fill in the missing chemical formulae in the tables below. acid conjugate base…

A: According to Bronsted Lowry concept, acid is substance which donate hydrogen and  base is substance…

Q: 1. The formula for the conjugate base of H2S is 2. The formula for the conjugate acid of H2PO4" is

A: Determine conjugate base and acid of the given substance----

Q: Picric acid, used in the manufacture of explosives, has a K₂ = 0.160. What is the K, of its…

A:

Q: Write the formula of the conjugate base of C.H.SH.

A: When an Acid donates H+ , it forms conjugate base. When base accepts H+ , it forms conjugate acid.

Q: The pH of a 0.0068 M solution of Ca(OH)₂ is?

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

Q: A solution has a pOH of 6.50 at 50∘C. What is the pH of the solution given that Kw=6.22×10−15 at…

A: To determine pH of solution: First we have to calculate pKw,

Q: What is the pH of a 0.750 M solution of C,H,NHB (Kb of C,H̟N is 1.7 10°)?

A:

Q: 3) Define conjugate, with respect to acid-base conjugate pairs.

A: 3)  In Bronsted-Lowry definition of acids and bases, a conjugate acid–base pair consists of two…

Q: What is the pH of a 0.0556 M NH, (aq) solution at room temperature? The base ionization constant of…

A:

Q: If in a solution [H,01-10 [OH ], what is the pH of the solution?

A: Given that :  [H3O+] = 10 [OH-]  We need to determine pH of this solution.

Q: The hydronium ion concentration of an aqueous solution of 0.428 M aniline (a weak base with the…

A: PH is  defined as the power of Hydrogen.it measure acidity, basicity or neutrality of aqueous…

Q: write disocierion re action for rhe waole culesand label conj ugate acid base pairs . HA,HCIO,

A:

Q: How do I diffrentiate bewtween strong and weak acids and bases?

A:

Q: For the stepwise dissociation of aqueous HaPO, which of the follawing is a conjugate acid-base pair?…

A: conjugate acid–base pair It consists of two substances that differ only by the presence of a proton…

Q: The pH of a 0.550 M of weak base, A-,  is 9.93 at 25. What is the Kb of the base?

A: Since the base given is a weak base. Hence it will undergo partial ionisation as per the below…

Q: The pH of a solution with pOH = 8.5 Is this an acid, base, or neutral?

A: Given :- pOH of solution = 8.5  To be calculated :- pH and nature of the solution

Q: 1. The formula for the conjugate base of H2S is 2. The formula for the conjugate acid of HCO3 is

A:

Q: Write the formula of the conjugate base of each acid: HF, HCO, , and CH3OH. Be sure to answer all…

A: Write the conjugate base of the given-

Q: A. Write the formula of the conjugate acid or base of the following substances: 1. Acids a. HC1O b.…

A:

Q: The pH of an aqueous solution of 0.353 M aniline (a weak base with the formula C¿H2NH,) is

A: pH - pH is defined as negative logarithm to the base 10 of H+ ion concentration. Mathematically, pH…

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: If the pH of seawater is 8.50, what is the [H3O+]?

A: pH = 8.50  We also know that ., pH = - log[H3O+]

Q: If the pH is 13.2 what is the molarity?

A: The pH of a solution is mathematically expressed as: pH=-log[H+] where [H+] is the molarity of H+…

Q: An aqueous solution of 0.40M Mg(C6H5COO)2 has a pH of__________.

A: Given: The concentration of Mg(C6H5COO)2 0.40 M To find: pH Formula:

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: Which two species act as the acids in the following reaction? HF CH3CO0 2F+CH3COOH OA CH3COO, F¯ O…

A:

Q: The hydroxide ion concentration, [OH], of an aqueous solution of 0.453 M pyridine (a weak base with…

A:

Q: n acid or base in

A:

Q: Give the conjugate base of the following Brønsted-Lowry acids: (2pts)  (i) H2O  (ii) H3O+

A: For conjugate base , just remove H+ from given acid.

Q: HF a strong acid, justify your answer.

A: HF is a weak acid, because its ability to dissociate to donate proton is low. It is not strong…

Q: Identify the conjugate acid for each base. conjugate acid of HSO,: H,SO, conjugate acid of PO :…

A: To get conjugate acid add one proton to the given base. The conjugate acid of given base HSO4- is…

Q: The pH of a O.0086 M solution of Ca(OH)2 is

A: The negative logarithmic concentration of hydrogen ion concentration in as solution is called pH. It…

Q: Identify the conjugate acid for each base. conjugate acid of HS¯: H,S conjugate acid of HPO; -:…

A: Since conjugate acid of any given base is formed by adding 1 H+ ion on the compound  hence the…

Q: What is the differnce between bronsed and lowery acids and bases?

A: According to the Bronsted-Lowry concept, acid is a substance that donates a proton while a base…

Q: Calculate the pH of each of the following strong acid solutions: (a) 8.5 * 10-3M HBr,

A: pH is a measure of how acidic/basic water is. The range goes from 0 to 14, with 7 being neutral. pHs…

Q: Why conjugate pairs are composed of weak acids and strong bases, and vise versa.

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

Q: The pH of a 0.0077 M solution of Ca(OH)₂ is?

A:

Q: Write a net ionic equation to show that ascorbic acid, H2C6H6O6, behaves as an acid in water.…

A:

Q: siven a solution with a hydroxide ion (OH") concentration of 4.30x108 M, what is the pH? s the…

A: pH + pOH = 14 pOH =  -log [OH −]          = -log[4.30 X 10-8]          = 7.37 pH = 14 - pOH       =…

Q: The pH of a solution is the negative logarithm of the molar concentration of hydronium ion, that is,…

A: The detailed solution of the given question is typed below.  Here it is important to note that the…

Q: Give the formula of the conjugate base:(a) HPO₄²⁻(b) NH₄⁺(c) HS⁻

A: Conjugate base of an acid is produced by loosing a proton from acid.          HA        ⇔      H+…

Q: 15D.5. What is the difference between (a) monoprotic acid and a diprotic acid, (b) a weak acid and a…

A: Since you have posted a question with multiple subparts, we can only first three subparts. To get…

Q: Are these solutions acidic, basic, or neutral? Then on the section below, categorize HCI and HC2H3O2…

A: We have to categorize HCI and HC2H3O2 as either weak or strong acids as follows in step 2:

Q: Give the conjugate base of the following Brønsted-Lowry acids: (a) HIO3, (b) NH4+, (c) H2PO4- (d)…

A:

Q: (a) Give the conjugate base of the following Brønsted– Lowry acids: (i) HCOOH, (ii) HPO4 2-.

A: The conjugate base of given Bronsted-Lowry acids has to be given.

Q: The "leftover" from when an acid gives up a proton is called O protonic ampoteric conjugate acids…

A: we need to select the term which describes leftover from an acid after giving up a proton

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.