2. At 25°C , find the pH of (a) an ideal, 3.7 x 10³ M HCl solution; (b) an ideal, 1.00 x 10° M HCl solution?

Q: Write the formula of the conjugate base of CH3CO2H

A: Conjugate base of an acid contains one less proton.

Q: The pH of black tea is 5.5, while the pH of Coke is 2.5. Which of the following correctly describes…

A: To know the concentration of H+ ion , pH scale is introduced  Negative logaritham of H+ ion…

Q: What is the pH of [H30+]= 2.4 * 10 3 M?

A: Given :- [H3O+] = 2.4 x 10-3 M  To calculate :- pH of solution   pH = -log[H3O+]

Q: Suppose that, instead of using NaOH, a base such as Ba(OH)2 had been used. What changes in the…

A:

Q: 1) Calculate the pH of a solution prepared by dissolving 2.20 g of sodium acetate, CHCOONA, in 78.0…

A: Given: mass of sodium acetate=2.20 gvolume of acetic acid=78.0 mLmolarity=0.10 MKa=1.75×10-5 To…

Q: Write the formula of the conjugate base of CH₃CO₂H.

A: Given  Acid =  CH3COOH  formula of Conjugate base = ?

Q: What is the pH of a 0.680 M solution of Ca(NO2)2 (Ka of HNO, is 4.5 x 104)?

A:

Q: 2.00 L of sulfuric acid, H2 SO4 (ag), contains 0.70 mol of acid. Calculate the pH and the pOH of the…

A: Given, moles of H2SO4 = 0.70 mol Volume of the solution = 2.00 L pH of the solution = ? pOH of the…

Q: The pH of an aqueous solution of 0.0916 M ascorbic acid, H2C,H,06 (aq), is

A: pH = −log [H+] Where, [H+] is molar concentration of the H+ ion.

Q: Below is the reaction for the formation of acid rain due to high concentration of atmospheric…

A:

Q: Calculate the pH of the following solutions in which the [H+] is a) 0.01, b) 1.0 x 10 –8 , and c)…

A: Given that -  Hydrogen ion concentration , [H+] are -  a) 0.01 b)1.0 x 10 –8  c) 4.67 x 10 –4  Then,…

Q: Alcohols can act either as weak acids or as weak bases, just as water can. Show the reaction of…

A: We have to predict the reaction of methanol with acid and base.

Q: 4. If the molarity of hydrogen ions is 1.32(+0.02)x103 M, find the pH.

A: The molarity of hydrogen ion is given by 1.32 ±0.02 × 10-3 M.We have to calculate the pH of the…

Q: In the laboratory, a general chemistry student measured the pH of a 0.353 M aqueous solution of…

A: In order to find the Kb of the given compound we first write down the given data: pH= 12.146.…

Q: . Alcohols can act either as weak acids or as weak bases, just as water can. Show the reaction of…

A:

Q: The value of K, for acetylsalicylic acid (aspirin) is 3.00x104. What is the value of Kp, for its…

A: Given: Ka value of acetylsalicylic acid = 3.00×10-4

Q: Calculate the pH and pOH of the following solutions (see Appendix 11 of your textbook for pKa…

A: "Since you have asked multiple questions and not mentioned the question number to be solved, we will…

Q: What is the pH of a solution of 0.400 M CH,NH, containing 0.100 M CH,NH,1? (Kb of CH,NH, is 4.4 x…

A:

Q: At the freezing point of water, Kw = 1.2 x 1015, What is the pH of ice water?

A:

Q: pH of a 0.223 M solution of sodium hydrogen chromate (K, 3.0 X 107)

A: Given data are as follows

Q: The hydroxide ion concentration, [OH], of an aqueous solution of 0.393 M caffeine (a weak base with…

A: Caffeine is a weak base with formula C8H10N4O2. Hence it will dissociate partially as per the…

Q: The pH of an aqueous solution of acetic acid (CH3COOH) is 2.0. What is the initial molar…

A:

Q: What is the pH of a 0.10 M N(CH3)3(aq)? The base ionization constant  of trimethylamine is Kb=…

A:

Q: The pH of an aqueous solution of sulfurous acid, H2SO3, that has a concentration of 0.60 mol/L and…

A:

Q: The pH of an aqueous solution of 0.0327 M ascorbic acid, H,C,H,O6 (aq), is

A: The solution is as follows:

Q: Identify the reactant acid and base in each of the following reactions by letters. H BH, CN. 1. BH,…

A:

Q: The pH of an aqueous solution of 0.175 M ammonium iodide, NH¼I (aq), is This solution is

A: Given : Concentration of NH4I = 0.175 M Since NH4I is made up of weak base NH3 and strong acid HI.…

Q: Calculate the pH of a solution prepared by dissolving 1.15g of sodium acetate, CH3COONa, in 95.5 mL…

A: Buffer solution is a aqueous solution consisting mixture of  weak acid and its conjugate base or a…

Q: Determine the base ionization constant (in x 10^5) of a 0.0925 g sample of week base (molar mass =…

A:

Q: Calculate the pH of an aqueous solution of 6.45×10-2 M sodium sulfite.   pH = ?

A: Sodium sulfite is salt of mixture of strong base sodium hydroxide(NaOH) and weak acid sulfurous…

Q: Calculate the pH and pOH of a solution resulting from dissolving 0.75 grams of perchloric acid in…

A: Given: Mass of perchloric acid i.e HClO4 = 0.75 g And volume of solution = 1500 mL = 1.500 L…

Q: The pH of an aqueous solution of 0.223 M sodium hypochlorite, NaC1O (aq), is This solution is…

A: pH of salt produced from reaction of weak acid and strong base would be basic and pH of salt…

Q: Given that methylamine, CH3NH2, has a Kb of 4.4 x 10-4, what is the pH of a 0.20 M aqueous solution…

A: For weak base CH3NH2 : [OH-] = Kb×C          = 4.4×10-4×0.20           = 9.38 x 10-3 M pOH = - log…

Q: The base protonation constant K, of allantoin (C,H,N;0;NH,) is 9.12 x 10-°. Calculate the pH of a…

A:

Q: In the following reaction in aqueous solution, identify (a) which of the reactants is the acid and…

A: Applying conjugate acid base concept.

Q: The ionization constant, Ka, for dichloroacetic acid, HC2HO2Cl2 , is 5.0 × 10‑2.  What is the pH of…

A: The ionisation reaction for the  dichloroacetic acid will be  HC2HO2Cl2 ------> H+ + C2HO2Cl2-…

Q: Find the pH of a 0.0015 M morphine solution (weak base), Kb = 1.6 x 10−6.

A:

Q: Calculate the pH of 1.00M acetic acid, HC2H3O2(aq). (Ka = 1.8 x 10-5)

A: Dissociation constant, Ka = 1.8 x 10-5 Concentration of acid = 1 M

Q: The pH of an aqueous solution of 0.136 M sodium nitrite, NaNO2 (aq), is This solution is

A: NaNO2 is a salt of a weak acid (HNO2) and a strong base NaOH pH = 7 + (pKa + log C)/2

Q: Calculate the pOH value of a 0.0150 M solution of pyridine, C5H5N.

A:

Q: Calculate the pH of 0.400 M solution of ascorbic acid, HC6H;O6. (Ka of ascorbic acid = 6.80 x 105)

A: In this question, we want to determine the pH of this solution. How we can determine, you can see…

Q: ph of 0.10 M NaNO2 (Ka of HNO2 is 4.5 x 10-4 ?

A: Given information: 0.10 M NaNO2 Ka of HNO2 is 4.5 x 10-4

Q: Determine the pH of a 0.15 M solution of Ca(BrO2)2 at 25 °C. At the same temperature, Ka for HBRO, =…

A:

Q: The pH of orange juice is about 3.5. What would be the pOH of orange juice?

A: Given: pH= 3.5 pOH=? It is calculated as

Q: The value of K, for acetylsalicylic acid (aspirin) is 3.00x104. What is the value of Kp, for its…

A: Ans. 3.33*10-11

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.