12. a) Show the dissociation (ionization) of the following acids in water HCI HF syour one fasrite and one les avorite pa of the de points) b) Identify the Bronsted acid, Bronsted base, conjugate acid, and conjugate base in each reaction in part А. and ban gnibroooA (s omW (d

Q: Which would be a stronger Lewis acid, explain.   (a) BF3 or BCl3 (b) Fe2+ or Fe3+

A:

Q: The pH of an aqueous solution of NaC₂H3O2 is (Hint: Split the compound apart into separate ions,…

A: The given compound: NaC2H3O2  The compound is a salt . When we dissolve the salt into aqueous…

Q: The weak base, B O H, has a K b value of 3.9E-5. Calculate the pH of this solution if the…

A: Given: Kb of BOH = 3.9×10-5 Concentration of BOH = 0.706 M

Q: Question 6:- What salts (acidic. basie . neutral)z a, Na, GOu b, NaCHal00 (baric) 3 Nall Is the…

A: Hi, we are supposed to answer one question. To get the remaining questions solved please mention the…

Q: 25) Which one of the following is not a conjugate acid-base pair? a) NH, and NH, c) HS and H,S b)…

A: Two chemical species that differ by the presence of a proton (H+) are called as conjugate acid-base…

Q: Identify the acid on the left and its conjugate base on the right in the following equations: (a)…

A: Identify the acid which is present in left side and its conjugate base which is present on right…

Q: 16.88 Predict the stronger acid in each pair: (a) HCl or HF; (b) H3PO4 or H3ASO4; (c) HBr03 or HBRO2…

A: a) Acidic strength of acids depends on the stability of anion formed after removing the proton.…

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

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: Choose the phrase that best describes the relative acid strength of these acids. NH3 H,O. is more…

A: Acid is the compound which give hydronium ion . so, greater is the tendency to give hydronium ion…

Q: 6) a solution Boric Acid : %3D Calculate PH(? >eguilibri ?) um constant

A: H3BO3  + H2O  → H3O+  +  H2BO3- Given that,[H3BO3] = 0.200 M [H2BO3-] = [H3O+] = 1x10-5 M Calculate…

Q: The hydrogen-containing anions of many polyprotic acids are amphoteric. Write equations for HCO3 and…

A: Given HCO3- and H2PO4-  act as a base. HCl acts as strong acid and NaOH acts as a strong base.

Q: What is the pH and concentration of OH- of 0.0200 M CH3COONa?

A: The pH calculation from given concentration is as follows,The given compound is a salt in solid…

Q: a cetain juice sample has [H+] = 1.0*10-4(exponet)   a. what is the ph for this sample   b. what is…

A: Equations for pH, pOH calculation:

Q: A 0.25 aqueous solution of a weak acid has a pH=3.65 at 25 degrees C. What is the value od Ka?

A:

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: What are [H 3 O + ], [OH - ], and pOH in a solution with a pH of 8.59 at 25 o C? (5pts). Express…

A:

Q: 1 alBalance Mhe acid-base neutralicaton reaction: H3 PO4+ NaOH-7 Nag POq +H20 b) wrik the net…

A:

Q: You have at your disposal an ample quantity of a solutionof 0.0500 M NaOH and 500 mL of a solution…

A: When NaOH is added to formic acid (HCOOH), the net ionic reaction is:

Q: grai

A:

Q: 1. OH- concentration is 1.233x10(-7). Is the solution acidic or basic/ basic acdic 2. The hydronium…

A: Acidity and the basis city of the solution defined on the basis of pH and pOH. For a solution if pH…

Q: What ionic formes isare most prevalent at pH6 The pa values of phosphoric acid are 2.1,72, and 124…

A: Given: pKa of phosphoric acid are 2.1, 7.2 and 12.4. And pH of solution = 6.8.

Q: Water superheated under pressure to 200 "C and 750 utm hás Kw= 1.5 X10 Aut is (H,O And [OH) at 200…

A: The equilibrium reaction of water at constant temperature; 2H2O→H3O++OH- and equilibrium constant of…

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: Which of the following statements is/are TRUE? Choose all that apply. O Select all that apply A H,Se…

A:

Q: What is the pH of an aqueous solution of KNO₂? (Hint: Split the compound apart into separate ions,…

A: If pH is less than 7 than solution is acidic in nature.   If pH value is more than 7  than solution…

Q: 0.10M NaC2H3O2 solution ?

A: pH is the negative logarithm of hydronium ions. The acidic, basic and neural character of the…

Q: The weak acid, H A, has a K a value of 1.6E-5. Calculate the pH of the solution if the concentration…

A:

Q: 5. In the reaction: Bronsted would identify which of the following species as acids? H₂PO4 (aq) +…

A: According to Bronsted acids are the species which donates proton (H+) while bases are the species…

Q: Which of the following species can act as a Lewis acid? D A B OBF4 (A) None of these i (B) CH3 (C)…

A:

Q: What is the ph of a solutiong with a pOH of 4

A: pOH of the solution = 4  pH of the solution = ?

Q: Calculare the pH is a sirany. ocid of a5.2X10MH,SO Solution? HSO4

A:

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: b) conjugate acid pairs. i. ii. HCOOH + NH3 For the following reactions identify the acid-conjugate…

A:

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

A: The acid given is HClO.

Q: Understand:- 2. Explain how the following factors affect acidity. - Charge - The Role of the Atom…

A: Ans.2 i) Charge and acidity: When acidic compounds donate hydrogen ions or accepts electrons, they…

Q: ALL BEAICF 12 AN of 100 mL SOLUTION; HAve A QU EOUS 0.1M A: HN 03 B:HN O2 Ka = 7.2 X /0 CHNO;) = %3D

A: Since beaker A has acid HNO3 with concentration = 0.1 M  And beaker D has H2SO4 with concentration =…

Q: What is the pH of an aqueous solution at 25.0oC in which [OH-] is 0.0040M?

A: Given : [OH-] =0.0040M To Calculate the pH of an aqueous solution at 25.0oC

Q: The pH of a basic solution is 11.39. What is [OH-]?

A:

Q: D) H;O*/OH E) HCI/OCI" A) B) H2SO/SO,²- NH4*/NH3 none of these C) O A E D

A: Conjugate acid (C.A.) are those species which are formed from base by accepting a proton while…

Q: Oxonium ion is considered

A: The correct option has to be chosen regarding oxonium ion,

Q: Lemon has pH

A: Given options A. Acidic B. equal to 14 as it is neutral substance C. Basic D. More than 7

Q: Which of the following compounds are Lewis acids? Select all that apply OS O AIF, U (CHINH ONH₂ Fe…

A: The electron pair acceptor is a Lewis acid and electron pair donor is a Lewis base.

Q: Water superheated under pressure tọ 200,°C and 750 atm hás Kw= 1.5 X10h What is [H3O"]and [OH'] at…

A: Solution The constant of a chemical process (usually denoted by the image K) provides insight into…

Q: The pH of a solution of HCl in water is found to be 1.20. What volume of water would you add to 1.00…

A: When an acid is diluted from an initial volume V1 to final volume V2 by adding water  then its pH…

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.