Calculate the pH of 0.40 M NH3 (Kb=1.8×10−5) Calculate the concentration of NH3 present in 0.40 M NH3 Calculate the concentration of NH4+NH4+ presents in 0.40 M NH3 Calculate the concentration of OH− presents in 0.40 M NH3 Calculate the concentration of H3O+ presents in 0.40 M NH

Q: Consider the generic Lewis dot symbol for an element. Which element could this symbol represent? OF…

A: The number of valance electrons of an element is an important characteristic of an element. The…

Q: What is the pH of a solution if [H+] =  1.50 × 10-4 M

A: Given :- [H+] = 1.50 × 10-4 M  To be calculated :- pH of solution  formula :- pH = -log[H+]

Q: A solution of HNO3 has a pOH = 9.45. Calculate the concentration of H3O+ ions in the solution.

A: Solution - According to the question - Given value -  pOH = 9.45 pH and pOH are related as, pH + pOH…

Q: What is the pH of a 0.0065 M Mg(OH)2 solution?

A:

Q: What is the pH of a 0.0758 M solution of NH4Cl? Kb for NH3 = 1.8 × 10−5

A: NH4Cl is salt of strong acid and weak base

Q: A solution has a pH of 11.35. What is the concentration of [OH*]? 1.0x10-14 M 4.5x10-12 M 1.0x10-7 M…

A: Given data:pH of the solution=11.35We have to find the concentration of [OH−].Given…

Q: Calculate the concentration of H3O* in a solution that contains 5.5 x 10° M OH" at 25°C. Identify…

A: • The values provided in the question are:-      i) Hydroxide ion concentration of a solution,…

Q: Determine the pH of the following solutions: 1.    [H+1] = 2.3 X 10-13 M 2.    [H+1] = 7.3 X 10-3…

A:

Q: Consider the following data on some weak acids and weak bases: name acid hydrofluoric acid HF…

A: The question is based on the concept of salt hydrolysis. We need to arrange given salts in…

Q: Determine the pH of a solution that has an [OH] = 3.2 x 10-8 M. O 7.49 6.51 5.25 8.75

A: The problem is asking us to find the pH of a solution given the concentration of hydroxide ions…

Q: What is the pH of 0.055 M Sr(OH)2? 13.04 12.13 13.39 13.75 12.87

A: 13.04Explanation:Detailed explanation:Step 1: Determine the dissociation of  Sr(OH)2​. Being a…

Q: Determine the pH of each solution. 0.23 M KCHO2 (Ka(HCHO2)=1.8×10−4) 0.18 M CH3NH3I…

A: We need to determine the pH of the each solutions below :1.  0.23 M KCHO2      Ka of HCHO2=1.8×10-4…

Q: To a precision of 2 significant figures, what is the pH of a solution containing a concentration of…

A: Given, Concentration of KOH solution = 1.0x10-14 M pH of the solution = ? Note: KOH is a strong base…

Q: Calculate the hydroxide ion concentration, [OH−][OH−], for a solution with a pH of 9.59

A: We know that pH = – log[H+] pOH = – log[OH–] [OH–] = 10–pOH    Given that pH = 9.59

Q: A sample of a cleaning product containing household amm of 11.50. Determine the hydroxide ion…

A: We will calculate concentration of OH-.

Q: calculate ph of 0.28 M solution of NaOH 0.091 M solution of Ca (OH)2 0.040 M2 solution of HClO4

A:

Q: Determine [H3O+] in a solution where [OH-] = 3.32 × 10-8 M.  Identify the solution as acidic, basic,…

A: Determine [H3O+] in a solution where [OH-] = 3.32 × 10-8 M.  Identify the solution as acidic, basic,…

Q: What is the pH of a solution that has an [H+]=0.0470 M ? 3.06 12.7 1.33 8.42

A: We have to calculate the pH of Solution.

Q: Select a strong acid and explain how you would prepare a dilute solution of the acid. Select a  weak…

A:

Q: what is the pH for   [OH−]M_1 = 2.9×10−7 M [H3O+]M_2 = 4.4×10−3 MM   [H3O+]M_3 = 2×10−4 M

A: Given :-  [OH-] = 2.9×10−7 M [H3O+]= 4.4×10−3 M [H3O+]= 2×10−4 M To calculate :  pH in each part

Q: What is the pH of a 3.21 ×10 -2 M solution of KOH?   1.49 9.97 12.5 6.97

A: Given, Concentration of the KOH solution = 3.21 ×10 -2 M  pH of a 3.21 ×10 -2 M solution of KOH = ?…

Q: he following: (given that Kb% D (given that Ka = 2

A:

Q: Calculate the hydroxide ion concentration, [OH−], for a solution with a pH of 8.52.         [OH−]= M

A: Given pH = 8.52  pH = - log [H+] 8.52 = - log [H+] log [H+] = - 8.52 = -9 + 0.48 log [H+] = log (…

Q: Solution 1 has [H+] = 8.6×10-7 M, and solution 2 has [H+] = 8.6×10-4 M. Calculate pH of both…

A: pH is given by the equation  pH = -log [H+] where  [H+] = concentration of  H+ ions present in the…

Q: Calculate the pH of 0.05 M Ba(OH)2 Group of answer choices 1.3 2.6 1.0 13

A:

Q: Calculate the pH of a 0.10M solution for each substance pH(NH3)=9.3 pH(NH4Cl)=4.03…

A: Given , Concentration of solution = 0.10 M

Q: What are [H3O+], [OH−], and pOH in a solution with a pH of 4.14? H3O+] = ____×10^__ M  [OH−] =…

A:

Q: Calculate the pH of the solution.  Assume 1.0 L of solution. You must identify the type of solution…

A:

Q: Find the concentration and tell if it’s an acid or base 1.[H+]=1.0 X 10^-8 M 2.[OH-]=1.0 X 10^-3 M…

A:

Q: Determine the pH of a 0.0054 M solution of calcium hydroxide. ○ 12.25 ○ 10.97 12.03 O 11.65

A: Step 1: Step 2: Step 3: Hope this helps!

Q: Why do phospholipids spontaneously form a bi-layer in water? O The non-polar head group and the…

A:

Q: For each of the following strong base solutions, determine [OH−],[H3O+][OH−],[H3O+], pH, andOH.…

A:

Q: Determine the [OH-] of a solution that is 0.135 M in CO3 2?   2. Determine the pH of a solution…

A: We have to calculate the pH, pOH and concentration of OH- in the given solution.

Q: Calculate the [H+] and pH of a 0.0040 M hydrofluoric acid solution. The Ka of hydrofluoric acid is…

A: Given: Ka for HF = 6.80 × 10-4Initial Concentration of HF = 0.0040 MRequired: [ H+ ] = ?pH= ?

Q: What is the pH (to two decimal places) of the following solutions, where the concentration of H+ is…

A:

Q: Calculate the hydroxide ion concentration, [OH−]

A: Given :- pH = 7.38  To calculate :- concentration of hydroxide ions i.e. [OH-]  [H+].[OH-] = Kw  KW…

Q: If the pH of a certain soft drink is 3.60, what is the H3O+ concentration in the soft drink?…

A: The objective of this question is to find the concentration of hydronium ions (H3O+) in a soft drink…

Q: What is the [H3O-] and [OH-] ion concentration respectively in a solution that contains 0.155 M…

A: HNO3(aq) ----> H+(aq) + NO3-(aq) [HNO3] = 0.155 M

Q: What is the hydroxide ion concentration [OH-] in a solution that has pH = 3? Assume the solution at…

A:

Q: What is the pH of a solution of 0.35 M Hydrochloric Acid?   60 35 68 7 45 61 75 90 80

A: HCl -------> H+ + Cl- [HCl] =0.35 M pH = -log [H+]

Q: solution has a pH equal to 9.4. Calculate the hydroxide ion concentration in this solution.  Group…

A: In this question we want to determine the value of OH- Concentration. You can see details Solution…

Q: What is the pH of a 0.00075 M HBr solution? O2.61 03.12 5.63 10.87 04.53 the answer is not listed

A:

Q: This statement is true when comparing solutions with a pH of 6 and a pH of 8 The solution with a pH…

A: pH of one solution = 6  pH of second solution = 8  formulae used ;  pH = -log[H+]  or [H+] = 10-pH…

Q: What is the pH of a 0.0001OM solution of HCI? * O 1.0x10-4 0.30 2.0

A: Given The  concentration of HCl=0.00010 M.

Q: Oxalic acid,  H2C2O4,  a poisonous colorless solid, is found in some vegetables such as spinach and…

A: Oxalic acid is the organic acid in which two carboxylic groups are present  The structure of Oxalic…

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.