1. Calculate the H30* and OH concentrations according to the given ph values. Solution pH [H3O] [OH] Unboiled distilled water 9.02 Boiled distilled water 6.54 1.0 M NaCl solution 6.02 1.0 M NaHSO4 solution 0.73 1.0 M Na2CO3 solution 11.48

Q: Determine the pH of 6.49 M CH3COOH

A: The pH of the solution can be given as :…

Q: Calculate the [H+] in a solution that has a pH of 5.66.

A:

Q: A given strong acid has a concentration of 0.065M. The pH of this acid

A: Since you have posted multiple questions, we are entitled to answer the first 3 only.

Q: Determine the pH of a 0.20M CH3NH3I solution.

A: Given that: [CH3NH3I] = 0.20M  CH3NH3I is salt made up of weak base CH3NH2 and strong acid HI.

Q: Name the following molecules.Classify each of the following species as a Brønsted acid or base, or…

A:

Q: Calculate the pH of the following solution: 1.0 M H

A: pH = -log [H^+] Given -> [H^+]=1.0M

Q: Calculate the H+ concentration in a solution with a pH of 2.34

A: Given that,The pH of the solution,The concentration of hydrogen ion,

Q: Determine the [H+] in a solution with a pH of 4.39.

A:

Q: Calculate the pH of a 0.307 M NH3 solution. NH3 has a ?b=1.8×10−5.

A: First of all a balanced reaction should be written for the solution: Here, water concentration is…

Q: Identify the following solution whether acidic, basic, or neutral. kalamansi, pH = 2.2 O BASIC O…

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: base or acid

A:

Q: Write equations that show NH3 as both a conjugate acid and a conjugate base.

A: Conjugate base is formed from acids, when a proton or hydrogen ion is removed. Conjugate acids are…

Q: Calculate the pH of solutions with the following concentrations. [H3O+]= 1×10−8M

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: Given the [H+] values, determine the pH of the following, And state whether acidic basic or neutral…

A: We can determie the PH of the solution by known value of the concentration of H+ ion, [H+] Using the…

Q: Given a solution in which the pH = 4, determine [H+], [OH-] and pOH.

A: Inorganic chemistry.

Q: g) H3P h) КОН

A: H3P=  pka value of PH3 is 27. It means that, pka value is more, so this is weak acid.

Q: Calculate the pH of a 0.45M NH4Cl solution.

A:

Q: The pH Of An Unknown Solution Is 0.46. Calculate [H3O+] In Solution.

A:

Q: Calculate the hydroxide ion concentration, [OH−], for a solution with a pH of 6.02.

A:

Q: Complete the table.    pH [H+] [OH-] pOH  7.0  7.3  7.4  7.5

A: To complete the below table. pH [H+] [OH-] pOH 7.0       7.3       7.4       7.5

Q: If the pH of a solution is 9.0 determine its [-OH] concentrations.

A: pH is the negative logarithm of H+ ion concentration, which indicates the concentration of hydrogen…

Q: calculate the hydroxide ion concentration of a solution with pH =9.9

A: Given : pH = 9.9  Since , pH + pOH = 14  => pOH = 14 - pH = 14 - 9.9 = 4.1  pOH = - log[OH-

Q: 1. The formula for the conjugate base of HF is 2. The formula for the conjugate acid of CN is

A: Given two species , HF and CN– We have to write formula of conjugate base of HF and Conjugate acid…

Q: Given the [H+] values, determine the pH of the following, And state whether acidic basic or neutral…

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: What is the pH of the following solution. 0.035 M HNO3

A: Given data contains, Molarity of nitric acid is 0.035 M.

Q: Calculate the pH of a 0.255 M NH3 solution. NH3 has a ?b=1.8×10−5

A: NH3 is a weak base. It undergoes partial dissociation in water accordinglyKb is the dissociation…

Q: Determine the formula of the conjugate base acid: H3PO4

A: Since the conjugate base is formed by removing 1 H+ ion from the acid  hence removing 1 H+ ion from…

Q: Determine the [H3O'] and pH of a 0.100 M solution of benzoic acid.

A: The pH of a 0.100 M solution of benzoic acid is calculated as,

Q: Given the [H+] values, determine the pH of the following, And state whether acidic basic or neutral…

A: Given is pH=3.75 Are asked to find [H+] and state whether acidic, basic or neutral. pH = -log[H+]…

Q: concentration of H3O+ ions

A:

Q: calculate the pH of a 0.70 M solution of KOH

A: Given that,The concentration of strong base,pH of the solution = ?

Q: What are the H3O+ and OH- concentrations of solutions that have the following pH values? pH4, pH 11

A: Ionic product of water, Kw:                                        Kw=[H3O+][OH-] = 10-14…

Q: Given the [H+] values, determine the pH of the following, And state whether acidic basic or neutral…

A: pH is the power of Hydrogen ion concentration or potenz of Hydrogen ion concentration. It is…

Q: A 0.050 M solution of the salt NB has a pH of 9.00. Calculate the pH of a 0.01 M solution of HB.

A: pOH = 14-pH = 14- 9 =5 pOH = -log[OH-]So[OH-] = 10-pOH[OH-] = 10-5 The  Reaction…

Q: Determine the [H3O+] for solutions having the following pH value. Your answers should include the…

A: Given pH = 9.345 We know that pH = - log[H3O+] [H3O+] = 10-pH

Q: Calculate [OH-] given pH=1.92

A: Acidity of the aqueous solution is given in the term of pH. pH is given as,…

Q: Calculate the pH of a solution where [H3O+] = 4.6x10-4. Is this solution an acid or base?

A:

Q: Write the formula for the conjugate acid of the following. H2O                       NH3…

A: Since, Conjugate acid obtain from adding H+ in the given species. Thus,

Q: What is the pH of a solution if the given is -4 [OH¯] = 4.5x10¬ M?

A: Given that: [OH-] = 4.5×10-4 M

Q: Calculate the pH of each solution. [H3O+] = 6.7×10−8 M [H3O+] = 7.0×10−7 M [H3O+] = 5.2×10−6 M…

A: The pH of the solution can be calculated by using the formula given below as; pH = - log H3O+…

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.