Protic acid is one which furnishes [H*] ions. Therefore H2SO4 is O Not protic O Diprotic O Triprotic O Monoprotic

Q: -HO + HOODHƆ ← 02 +0³H

A: Acids are proton donors and bases are proton-acceptors. An acid has a conjugate base which is formed…

Q: When water acts as both Bronsted-Lowry acid or base it is called O a. amphiprotic O b. amphiphilic O…

A: Amphiprotic molecule can either donate or accept proton and hence act as both Bronsted -Lowery acid…

Q: Write formula for the conjugate acid of the foll F O H2F O HF O H+ O 2HF

A: Conjugate acid of F-  ?

Q: The pH of a 0.15-M solution of HSO4− is 1.43. Determine Ka for HSO4− from these data.

A: Given, initial concentration of HSO4− = 0.15 M            pH = 1.43 We know that, pH is the negative…

Q: All of the following are weak acids except O HCNO O HBr O HF O HNO, O HCN

A: An acid which dissociates completely or almost completely in water are strong acids.An acid that…

Q: In the reaction: H,BO, + H,o = H,BO, + H,0*, which of the following compounds are correctly lists…

A: The question is based on conjugate acid base principle. a strong acid has a weak conjugate base and…

Q: 1. Identify acid or base, give its conjugate form. A) HCO, в) он C) H;SO. D) H:PO.

A:

Q: In the reaction: H* + F → HF The Lewis acid is: HF H20 H* OH F

A:

Q: In the reaction: BCI3 + NH3 The Lewis acid is: (c) B-NH3 1. O cr O H,O O H O NH3 BCly

A: A Lewis acid is a chemical species which has an empty orbital in which it is able to accept…

Q: If the Kb of a weak base is 5.7 × 10-6, what is the pH of a 0.16 M solution of this base?

A: From the relation, pOH is calculated as,

Q: Which of the following species is not a Brønsted-Lowry base? Multinle Cho ice

A: According to Bronsted-Lowry acid is a substance which can give up a proton (H+) while base is a…

Q: Consider HCIO4(aq). Select all descriptions that apply to this compound. O It is an acid. O It is a…

A: Perchloric acid is a mineral acid . usually found as an aqueous solution , this compound is a…

Q: 3. Normal rainwater has a pH near 6. In rainwater that falls close to a coal-burning power plant,…

A: Hydronium ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.54. What is the Kb of this base?

A: pH = -log[H3O+] Where [H3O+] is the concentration of hydronium ion…

Q: The pH of a 0.55 M aqueous solution of hypobromous acid, HB1O, at 25.0 °C is 4.48. What is the…

A: The percentage of ionization of HBrO can be calculated as follows

Q: A sample of fruit juice is found to have à hydrogen concentration of 2.87 x 104. What would the pH…

A: Given hydrogen ion concentration of fruit juice is 2.87*10-4. We have to determine PH of fruit…

Q: What is the pH of a 0.250 M HOCI solution? K, of HOCI at 25°C is 3.5 x 10-8. O 7.46 O 4.03 O 3.57 O…

A: ​Given - - - >   Ka = 3.5*10-8   pH = 0.25

Q: 5. Write equations to illustrate the amphoteric nature of H2PO (aq) and label the conjugate acid-…

A: Write equations to illustrate the amphoteric nature of H2PO- (aq) and label the conjugate acid-base…

Q: Calculate the pH of a solution that is 0.0736 M KC2H3O2  at 25°C.

A:

Q: Find the [CO32 - ] of the 0.050 M carbonic acid (H2CO3)

A: Given  concentration of carbonic acid [H2CO3]= 0.050 M Carbonic acid is a diprotic acid having ka1 =…

Q: A solution at 25 °C has 3OH-4 = 6.7 * 10-3. What is the pH of the solution?

A: The pOH of a solution is given by, pOH = -log[OH-] The relation between pH and pOH is given by, pH +…

Q: 2) The PH of asolution of aweak ronoprotic ucid (HA) is 2.85 what is the Ka of the acid ? Ans.: 2*10

A: Given ,  Concentration of weak mono protic acid ( C ) = 0.1 M pH of the weak acid = 2.85 Acid…

Q: When the conjugate base of a weak acid (in the form of a salt) is dissolved in water, one can…

A: As we know that water is neither acidic nor basic and it is neutral in nature. We also know that…

Q: For HNO2, Ka = 4.6 x 10-4 and for HSO4-, Ka = 1.2 x 10-2. Which is the stronger acid?

A:

Q: A. i)Identify the conjugate acid and base pairs for the following reactions NH + H,O, - NH, (n+ OH)…

A: An acid is a substance which donates a proton (H+) and base is a substance which accepts a proton.…

Q: Calculate the percent ionization of a 0.125-M solution of nitrous acid (a weak acid), with a pH of…

A: pH of a solution is equal to negative logarithm of the concentration of the hydrogen ion. Write the…

Q: Arrange the substances based on their relative acid strength. CIO C,H,0, strongest acid C,H,CO0…

A: Strong acids are those which dissociate rapidly in water to gibe H+ ions. The dissociation of these…

Q: What is the pH of a solution that has [OH–] of 5.15×10-3 M ?

A: Given, Concentration of hydroxide ion = 5.15×10-3 M

Q: 1. Calculate the pH of a 0.045M sulfurous acid solution. H,SO, → H* + HSO, Ка, = 1.7 x 102 HSO3- H +…

A:

Q: Which of the following statements about acids is true? O All of the other statements are false O For…

A: The question is based on the concept of equilibrium.    it involves calculation of hydronium ion…

Q: What of the following options describes the term "pH and pOH"? O a. The negative logarithm (base 10)…

A: •pH=> it is a scale to determine the concentration of H+ ion. •pOH=>It is a scale which…

Q: Determine the [H*]. JOH-], and pOH of a solution with a pH of 11.62 at 25 °C. [H*] = M [OH] = %3D…

A:

Q: 5. Which of the following is Lewis acid BF3 FeC12 AICI3 All of the above

A: According to the definition of lewis acid is that, Element,atom or ion having incomplete octet or…

Q: Find the a0 and a1 values ​​of hypochlorous acid in a solution with a pH of 7.0. (Ka = 3x10^-8 for…

A:

Q: What

A: Hinderson equation is used for calculating the pH of the buffer solution.  pH = pKa + log( [salt] /…

Q: What is the pH strength of the following structure? CH3-OH O A. Weak acid O B. Strong acid O C.…

A: Acidic nature depend upon easily giving up the proton.

Q: The organic acid RCOOH has a Ka = 4.1e-5. What is the pH of a 0.50M aqueous solution of this acid?

A: given, Ka = 4.1e-5 [RCOOH]= 0.50M

Q: write out the stepwise ka reaction for the diprotic acid H2SO3

A: For a dissociation of acid (HA) in aqueous solution,

Q: The conjugate base of HPO,2 is OA H,PO42 O B. H2PO4 В.

A: Conjugate base  of acid formed by accepting H+

Q: Brønsted-Lowry acids?

A: A Brønsted-Lowry acid is defined as any species that can donate a proton [H+].

Q: Which of the following species is amphoteric? O CO3²- HCO3- HF None of the above are amphoteric.

A:

Q: pK, for the phenolate ion, C¿H;O¯, a weak base, is 4.204. Calculate the pH of a 0.339 M solution of…

A:

Q: I dentity the tollaming salts as Acidic, Basic or neutiral : HCook Naclos ,kCloy i CoH 5. CH; Nity…

A: Salt is substance produced via reaction between acid and base.  If salt produced via strong acid and…

Q: OH он CI. A B но HO. E D

A:

Q: In the reaction, Co32- + H20 → HCO3¯ + OH" the hydroxide ion (OH" ) is acting as a(n)...…

A: •According to Bronsted-Lowry concept of acids and bases, acids are those substances which can…

Q: If the hydrogen ion concentration of a solution is [H*] = 1 x 10 M, is the solution acidic,…

A: The hydrogen ion concentration of the given solution is = 1.0 x 10^-7 M The nature of the solution…

Q: What is the pH of a solution containing 0.055 mol L-1 HCOOH and 0.141 mol L-1 HCOO- ?

A:

Q: . .as the species (molecule or ion) that donates a proton (H+) O a. The Arrhenius acid O b. The…

A: Acid and base: Several kind of theory in chemistry which are described the acidity and basicity of…

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.