Which of the following species is amphoteric? O co,? O HF O NHA O HPO42 None of the above are amphoteric.

Q: Zno is Amphotoric Fa O TbO

A: ZnO is amphoteric or not

Q: Which of the following is the stronger Brønsted–Lowry acid, HBrO or HBr?

A: Brønsted -Lowry acids or proton donors are the species, that can transfer the proton to another…

Q: What are the [H3Oʻ] and pH of 0.085M weak base C2HSNH2?

A:

Q: A solution turns red litmus blue, its pH is likely to be(a) 1(b) 4(c) 5 (d) 10

A: An important concept of pH can be given as: Acids have a pH level below 7 Bases have a pH level…

Q: In the Bllowing ns tn the Bllowing reactio s - lowry base? a Brønsted

A: Bronsted-Lowery theory ,also called proton theory of acids and bases.According to Bronsted-Lowery…

Q: What is the pH of abaffer which has been prepurel y miking 250 my AM,el ane! 200 ml , oi M viz…

A:

Q: Electron pair acceptors are bases. This is stated by... O a. Lewis-Arrehnius O b. Lewis O C.…

A: Electron pair are those electron that are present in non bonding molecular orbital of molecule.

Q: A solution with a pOH of 5.55 has an [OH–] of __________

A: We know,                            pOH = - log[OH-]                    Or, log[OH-] = - pOH…

Q: The pOH of an aqueous solution of 0.528 M hypochlorous acid is

A: Given :-  concentration of hypochlorous acid = 0.528 M  To calculate :-  pOH of solution    pH + pOH…

Q: Which one of the following aqueous solutions has the highest [OH-]?? A .a 1x10-3 M solution of…

A:

Q: Which of the following statements is/are correct? O A. All of the choices are correct. O B. In a…

A: An acid is a substance or compound that releases hydrogen ions (H+) when in solution. In a strong…

Q: 2) Calculate the PH of the solution if Ece = 0.10 when [Co*] = 0.45 M, [H:] = 0.30 M, and PH = -log…

A:

Q: Which of the following is not amphoteric? O H3 PO4 OHCO, OHSO OH2O

A: Given,  H3PO4 HCO3-  HSO4-  H2O

Q: A solution has [H+]=4.0x10-8M. Determine the POH of the solution.

A: Given: [H+]  = 4.0x10-8 M

Q: Given a 21.50mL of 0.0500M HBr solution at 25C What is the H3O ion concentration What is the pH of…

A:

Q: The pOH of 0.050 M HCl is

A:

Q: The pH of a lime is 1.90. What is the [H3O+]? What is the [-OH]?

A: Since the relationship between pH and  [H3O+] is  pH = -log[H3O+] and the relationship between pH…

Q: Acidic solution such as 10-8 M acetic acid and 10-8 M HCI contains H* that is supplied mostly by a.…

A: Solution: ⇒We are given with the acidic solution of 10-8 M acetic acid and 10-8 HCl. Since its a…

Q: 0.1 M NaHCO3 solution, using the given pH data, calculate value of (Ka or Kb)

A:

Q: The pOH of an aqueous solution of 0.453 M acetic acid is

A: Dissociation of weak polyprotic acid and pH  calculation:

Q: A solution NaOH has 0,04%w/v. Find the pH of the solution, when it is given that the solution NaOH…

A: pH is defined as the negative logarithm of Hydrogen ion concentration. In Chemistry, pH denotes as…

Q: Using data from Appendix D, calculate 3OH-4 and pH for each of the following solution 0.035 M Na2S

A: 0.035 M Na2S hydrolyze in water to produce OH- ions. The ICE table is as follows:

Q: given équatión? НРО /hich of the following statements is FALSE for the 2- HSO elect one: OSH•…

A: Bronsted Lowry acid : A substance which donates a proton. Bronsted Lowry base : A substance which…

Q: Given a 21.50mL of 0.0500M KOH solution at 25C what is the H3o+ ion concetration? What is the pH of…

A:

Q: What mass of HNO, is present in 211.0 mL of a nitric acid solution having a pH = 5.70? 5.96e-5

A: Given data :  pH of solution = 5.70  Volume of Solution = 211.0 ml = 0.211 L

Q: Which of are neutral salts? 口 KF O KNO3 OSrBr, O Sr(OH), O HF O NH,Br

A:

Q: THe pOH of 0.5 M solution of weak base is 4.72. What is its pKa?

A: Given-> pOH = 4.72  Molarity =0.5 M

Q: Which of the following is the strongest acid: н, с. ОА Ов C OD A 'OH H, C FH В OH HC C OH F ж Н D…

A:

Q: Give a clear handwritten answer...

A: Acidic strength of molecules can be compared by resonance stabilization of their conjugate bases.…

Q: Chronium 1) hydroxide is amphiprotic. Write Wite o belamaed demiel eguedion shoming hom an aguacous…

A: Amphoteric nature means that the compound equally reacts with both strong base and acid . And…

Q: The pH of a 0.0231 M HNO3 solution is: 4 sig figs if possible please

A: PH=-logH+

Q: Which of the following could not be amphoteric? Oa) so Ob) HCO3 OO H20 O d) HPO,

A: Need to tell which are not amphoteric.

Q: Vhat is the pOH of a solution with [H,O)=1x10-5M 9. 4 10

A: This is ionic equilibrium chemistry

Q: Calculate the pOH of a solution that is 0.04M in HCI 3.0 1.4 .b O 0.04 .c O 12.6

A: Given that : Molarity of HCl = 0.04 M pOH = ?

Q: The most basic solution from the following is: * Pb(CH3C00)2 O CH3COONA O FECL3 O Al(CN)3

A: The acid-base nature of the salt solution depends on the nature of the acid and base from which the…

Q: Calculate [H+]. [CIO,], and [OH ] in an aqueous solution that is 0.105 M in HCIO, (aq) at 25 °C.…

A: HClO4 is strong acid. So this is completely dissociated.

Q: The pOH of an aqueous solution of 0.528 M acetic acid is

A: The solution is as follows:

Q: Which of the following is a Lewis acid but not a Brønsted-Lowry acid? А) CH:ОН В) H-О С) СH3COОH D)…

A: (40)  Lewis acid can be defined as the species which can accept pair of electrons while…

Q: Which of the following statements is/are correct? O A. All of the choices are correct. O B. In a…

A: An acidic solution is that which contains more H+ ions than OH- A basic solution is that which…

Q: A solution with a pOH of 11.70 has an [H3O+] of

A:

Q: In the Brønsted-Lowry definition of acids and bases, an acid O A. is a proton donor. O B. is a…

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: The most basic solution from the following is: Pb(CH3CO0)2 FECL3 CH3COONA Al(CN)3

A: Basic solution are those which are good proton acceptor or hydroxide donors.

Q: 20. The following reaction may undergo under CH3 OH CH OCH o Basic condition. o Acidic condition.…

A: Epoxides are strained moieties. They can undergo ring opening by the nucleophilic attack, which is…

Q: The pOH of an aqueous solution of 0.377 M acetic acid is

A:

Q: Which of the following is/are NOT true for a solution at 25°C that has a hydroxide concentration of…

A:

Q: What is the pH of a 0.200 M NaHCO, solution? The K, for HCO, is 5.6 x 1011

A:

Q: 165 Determine the pH of (a) a 0.40 M CH,COOH solu- tion, (b) a solution that is 0.40 M CH,COOH and…

A: CH3COOH is a weak acid. To calculate the pH, degree of dissociation is calculated first (α) using…

Q: For a 0.15 M H3PO4(aq) solution, determine pH [H3PO4], [H2PO4-], [HPO42-], and [PO43-]

A: Given: Concentration of H3PO4 = 0.15 M Ka1 = 7.1×10-3 Ka2 = 6.3×10-8 Ka3 = 4.5×10-13

Q: Calculate the theoretical pH of the solution please 0.100 M aluminum nitrate Hydrated aluminum ion…

A: Al^3+ solution is slightly acidic in nature. This is because Al^3+ has very high ionic potential.…

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.