18). The formulas and the structures of two acids are shown below. Which acid is a stronger acid? If the acid strength of the two acids is equal, say so. Cl2CHCOOH CH3COOH но но CI-C-C-OH н-с-с-он ČI Ką = 0.0324 Ką = 1.82 x 10-5 %3D a. Cl¿CHCOOH is a stronger acid than CH;COOH. b. CH;COOH is a stronger acid than CI½CHCOOH c. The two have equal acid strength. d. none of the above

Q: Periodic acid, HIO4, is an important oxidizing agent and a moderately strong acid. In a 0.10 M…

A:

Q: Consider a weak acid "HA". What is the pH of a 0.626 mol L¯' solution of HA? The KA of HA is 6.5 x…

A:

Q: Calculate the [H3O+] of a 0.280 M acid solution; Ka=3.10 x 10-9 Group of answer choices   5.92 x…

A: Given, Concentration of acid solution (C) = 0.280 M Ka value of acid = 3.10 × 10-9 [H3O+] = ? Note:…

Q: None

A: In order to calculate the Ka from pKa, the equation that will be used is: Ka​=10−pKa​ In order to…

Q: What are the major products of the foll

A: Dehydrohalogenation :  alkyl halide inpresence of strong base gives alkene as product by HX…

Q: 3. Calculate the pK, of hypochlorous acid from its K, value. (Refer to Appendix H.) HCO Ka 3.5x10-8²

A: Given that: Ka of HClO = 3.5×10-8

Q: What is the equilibrium constant expression, Ki, for the following weak acid? H3PO4(aq) + H*(aq) +…

A:

Q: What are the major and minor products of this reaction

A: The major product can be obtained by E2 pathway and the minor product can be obtained through SN2…

Q: In the following reaction, which best describes the role of water, H₂O? H₂O + HPO4² = H₂PO4 + OH…

A: Since, From the definition, Brønsted-Lowry acid are proton donar and Brønsted-Lowry base are proton…

Q: The value of Ka for phenol (a weak acid) , C,H5OH , is 1.00×10-10 . Write the equation for the…

A: Phenol acts as a weak base that means the hydrogen attached to -OH group in phenol is removed as a…

Q: Calculate the pH of a 0.40 M solution of benzoic acid, C6H5COOH? (Ka-6.3 x 10-5) What is the %…

A:

Q: Part C Consider the following polyprotic acid solution: 0.135 mol - L H2CO3. Kal = 4.3 x 10-7 Ka2 =…

A: Answer:- This question is answered by using the simple concept of ionisation of weak acid and then…

Q: 2. Answer the questions for the acid below: a) Write the acid dissociation constant, Ka, expression…

A: Given reaction:                          HA(aq) + H2O(l) ⇔H3O+(aq) + A-(aq) Acidic strength is…

Q: Calculate the pH and fraction of dissociation (a) for each of the acetic acid (CH,COOH, pK, = 4.756)…

A: We have to calculate PH and fraction of dissociation for acetic acid having PKa = 4.756 A) 0.00149M…

Q: 2a. Circle the most acidic compound. 2b. Box the least acidic compound. О F F ОН ОН F О ОН

A: All the given carboxylic acids have fluorine atoms attached to it at various positions. Since…

Q: What is the hydronium-ion concentration of a 5.58 x 104 M solution of p-bromobenzoic acid, BrCg H4…

A:

Q: What is the pH of a solution that is 0.15 M NH4Cl and 0.35 M NH3?   The Ka of NH4Cl is 5.01 x…

A: In this question , we have to calculate the correct pH of given problem by the help of…

Q: Which of the following salts may be obtained by the reaction of a weak acıd With a strong base?…

A: a) LiClO4  Made by strong base : Li(OH)  Made by strong acid: HClO4   b) NaCl Made by strong base :…

Q: equilibrium. You can leave out water tself Write the chemical formulas of the species that will act…

A: When pH> 7 ,then solution is basic if pH <7 then solution is acidic

Q: Rank the following acids in order of increasing acidity

A:

Q: Lowest base strength benzoate ion Ka = 6.46 x 10-5 acetate ion CH3COO K 1.76-105 carbonate ion co,…

A: According to Bronsted lowry theory greater is the value of Ka of any acid more is acidity of that…

Q: The Ka of a weak acid is 3.33 x 10-5, what is the pKb of it's conjugate base?

A: The objective of this question is to calculate the pKb of the conjugate base of a weak acid given…

Q: In the following reaction, HCO; (aq) + H20(E)=co;²(aq) + H;0*(aq) Select one: O a. H3O* is an acid…

A:

Q: NH3 is a weak base (Kp = 1.8 x 10³) and so the salt NHĄCI acts as a weak acid. What is the pH of a…

A: At Temperature 25°C Kb (NH3) = 1.8 × 10-5 [NH4Cl] = 0.028 M

Q: Consider the following compound for the next three questions. Ha Ha Hb Hb Which acids approximate…

A: To find out the acids that approximate to the given hydrogens

Q: What is the [OH–] in an aqueous solution with [H3O+] 1.30 mol L–1

A:

Q: Consider an acid HA dissolved in water at 25°C. HA(aq) + H2O(l) ⇌ H3O+(aq) + A-(aq)         Ka =…

A: An acid is a substance that gives H+ ions in its solution whereas a basic substance gives OH- ions…

Q: Based on the given Ka values, which is the weakest base? Acid Ka CH3COOH 1.8 x 10–5…

A: Equilibrium constant (K) is ratio of concentration of products and reactants. Addition or removal of…

Q: START ORDER benzoic acid: 6.3 x 10-5 E nitrous acid: 4.4 × 10¬4 : oxalic acid: 5.6 × 10¬2 : ethanoic…

A:

Q: What is the pH of an acetic acid, CH3COOH, solution that has an initial concentration of CH3COOH of…

A: Acetic acid is a weak monoprotic acid. In water it is dissociated as acetate ion and protons.

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.