10) What is the pH of a 0.100 M NH3 solution that has Kb = 1.8 × 10-5? The equation for the dissociation of NH3 is NH3(aq) + H20(1) =N H4+(aq) + O H - (aq). B) 12.13 A) 11.13 C) 1.87 D) 2.87

Q: 1.4 x 10 4M .

A: Concentration

Q: If you add NaHCO3 to this solution, which of the following will occur? A) The reaction quotient will…

A: When we add NaHCO3 in the solution HCO3- concentration increases because according to le chatlier's…

Q: A solution is made by dissolving 0.0015 mole Ba(OH)2 in enough water to make 1.50 liter of solution.…

A: dExplanation:

Q: Arrange the aqueous solutions from the most acidic to the most basic, at 25 ∘C Acidic 1) 2) 3) 4)…

A: First, determine the pH of the solution having [H+] = 1 × 10-2 M by using equation (1),

Q: 48. What is the pH of a solution that has a hydroxide ion con- centration of 1.0 X 10-10 M?

A: Given :- [OH-] = 1.0 × 10-10 M  To calculate :- pH of solution

Q: Determine [H3O+] in each acid solution. If the acid is weak, indicate the value that [H3O+] is less…

A:

Q: What is the pH of 3.78 *10^-2 M nitric acid in aqueous solution ?

A: Concentration of hydronium ion H3O+ present in the solution is known as the pH of the solution.

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: In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a…

A: The objective of the question is to identify the species in the reaction given for Bronsted Lowry…

Q: What is the pH of a 0.223 M LINO2 solution at 25 °C (Ka for HNO2 = 4.0 x 104)? (the answer should be…

A: Given, [LiNO2] = [Salt]=0.223 M Ka of HNO2= 4.0×10-4 pH = ?

Q: What type of ion is Na+?

A:

Q: 00 HO O more than one response is correct 19. Apply the Bronsted theory of acids and bases to the…

A: We have to predict acids and bases according to bronsted theory.

Q: 1) Which of the following compounds are amphoteric? -both HSO3^- and O^2- -HF -CO3^2- -O2 -BF3…

A: A solution is said to be acid if the solution contains amount of H+ higher than amount of OH- , then…

Q: strong base

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: 5. The dissociation reactions for several acids and their equilibrium constants are given below:…

A: The acid dissociation constant (Ka) of an acid is used to distinguish between strong acid and weak…

Q: 16. What is the pH of a 0.481 M solution of NH4Br? For NH3, Kb = 1.8 × 10–5

A: The solution is as follows :

Q: In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a…

A: Given, the chemical reaction is as follows,C6H5NH2(aq) +H2O(l)   → C6H5NH3+(aq)+ OH-(aq)we are asked…

Q: 13.3) Determine [OH–], pOH and pH of a 0.18 M  aqueous solution of LiC3H5O3 (K b = 7.1×10-11).

A:

Q: Which of the following is a Lewis acid? A) Fe3* B) CN C) NH3 D) SCN

A: In this question we have to tell that which is act as lewis acid.

Q: Determine the pH of a 0.62 M NH4NO3 solution. The Kp for NH3 is 1.76 × 10-5. A) 7.27 B) 9.45 С) 4.73…

A: Ammonia is a weak base that undergoes partial dissociation to form hydroxide ion (OH-) and ammonium…

Q: In a 1.00 M  aqueous solution of sulfuric acid, H2SO4, three processes producing the hydronium ion…

A: In this question, we will select the correct Reaction which give the pH of the solution.  You can…

Q: What is the pOH of a 0.1563 M NH4NO3? Kb for NH3 is 1.86e-5.

A: Given: kb for NH3 = 1.86 * 10-5 concentration of NH4NO3 =  0.1563 M

Q: Morphine is an effective painkiller but isalso highly addictive. Codeine is a popular…

A: The pH of a solution is calculated by equation (1) in which H+ is the concentration of hydronium ion…

Q: The ionization constant of water at a temperature above 25°C is 1.7 10-14. What is the pH of pure…

A: Given data,  Ionization constant of water, Kw = 1.7 × 10-14

Q: What is the pH of a solution obtained by adding 158 mL of 0.206 M HCl to 926 mL of an HNO3 solution…

A: Volume of HCL =158mL Concentration of HCL =0.206M Volume of HNO3=926mL pH of HNO3 =2.550

Q: How would I the conjugate acid and the base including ions pair and electron

A: Conjugate acid is a species able to donate proton and formed by accepting a proton of a acid.…

Q: What is the pH of a 0.300 M NH3 solution that has Kb = 1.8 × 10-5? The equation for the dissociation…

A: We have given the balance chemical equation                                      NH3(aq)     +…

Q: The Bronsted-Lowry (B-L) definition of acids and bases was developed mainly because there were…

A: Arrhenius acid/base concept :- According to the Arrhenius acid/base concept ,  the acids are those…

Q: HCN has a K, of 4.9 X 10-10. What is the pH of a solution which contains 0.350 M NaCN? CN (aq) + H,O…

A: The pH of a solution helps to determine the acidity and alkalinity of a solution. The solution maybe…

Q: Calculate the size of the pH change when the ratio HA] changes from 10 to 1.

A: We can calculate it from dissociation constant of acid and we should do comparisons which is…

Q: the PH of a solution of HCl that is 1.0x10^-9 M at 25c is  a) 9.00 b) less than 7 c) 7.00 d) less…

A: The concentration of HCl acid is very very less i.e 1.0 X 10-9  So we can not directly say that the…

Q: 35. Calculate the pH of a solution that is 0.15 M in formic acid (HCOOH) and 0.20 M in sodium…

A: Concentration of formic acid = [HCOOH] = 0.15 M Concentration of sodium formate= [HCOONa] = 0.20 M…

Q: Acid Ka HC3HSO3 1.4 x 104 HOCN 3.5 x 104

A: Given acids,      Lactic acid - HC3H5O3      Cyanic acid - HOCN

Q: The pain reliever codeine is a weak base with a Kb equal to 1.6x10-6. What is the pH of a 0.75 M…

A:

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.