Calculate the pH for 0.43 M NH4ClO4

Q: Determine the pH of 6.49 M CH3COOH

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

Q: Why is the ph of NH4C2H3O2 nearly 7

A: The question is based on the concept of salt hydrolysis . we need to calculate pH of ammonium…

Q: Calculate the pH of a 0.100 M KCN solution.

A: Anionic part of the salt will be hydrolysed and cationic part of the salt will not be hydrolysed.

Q: Calculate the pH of a 6.8 x 10-6 M solution of LiOH

A: Given: Concentration of hydroxide ion =

Q: A solution has a [H3O+] of 0.0015 M. Calculate the [OH-], the pH, and the pOH of the solution. Is…

A: In the question is given that concentration of [H3O]+  is 0.0015. i.e. [H]+ = 0.0015 [OH]- = ? pH =…

Q: Calculate the [H+] or [H3O+] in a solution that has a pH of 8.75.

A: Given: pH = 8.75.

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: Calculate the pH of a 0.67 M NH3 solution.

A: Concentration of NH3 solution = 0.67 M Kb for NH3 =

Q: what is the pH when the H3O concentration is 0.0003M?

A: The pH of a solution can be calculated as given below.

Q: Calculate the H3O+ concentration from each pH: (a) 7.82;    (b) 13.96.

A: FORMULA  We can calculate HydroNium ion concentration  by using formula  [H3O]+ = 1 × 10-PH a) 7.82…

Q: base or acid

A:

Q: Ethanolamine, HOC2H4NH2 , is a viscous liquid with an ammonia-like odor; it is used to remove…

A: Weak base are bases which does not dissociate completely to furnish hydroxide ion when dissolved in…

Q: Calculate the pH of 0.050 M of H+

A: We know that, pH can be expressed as the negative logarithm of hydrogen ion concentration. i.e.…

Q: What is the pH of a 0.845 M solution of KOH?

A:

Q: What is the pH of a solution that is 3.0 M H2SO4

A: Please find the solution below:

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

A:

Q: Calculate the pH of 0.02 M H;PO4

A:

Q: Calculate the hydrogen-ion concentration and pH of 0.010 M HNO3.

A:

Q: In converting from the pH of a solution to the corresponding H3O+ concentration, the following…

A: The answer of the given question is given below

Q: Determine the pH of a 0.500 M HA solution if the Ka of HA is 4.0 x 10.

A: The ionic equation is simply: HA --------> H+ + A- now we can write the Ka formula.

Q: What is the concentration of an HCI solution with a pH = 2.487

A: pH of HCl solution = 2.487  Concentration of HCl solution = ?

Q: What is the pH of 0.160 M HNO2

A:

Q: calculate the {H3O} of the solution of hydrochloric acid with pH = 2.00

A: Given, PH = 2.00 PH is defined as negative logarithm of concentration of [H+] ions.

Q: Distinguish between the terms " weak " and " strong " as they apply to acids

A: The question is based on the concepts of acids. acids and base are two important aspects of the…

Q: Calculate the pH of 0.00756 M HNO3

A: pH Scale: It is common to express the level of acidity of a solution using the pH scale. Most…

Q: What is the pH of a solution if the concentration of H+ is .000284

A: Given :  Concentration of H+ = 0.000284 Therefore [H+] = 0.000284

Q: Calculate the pH if the [OH-] = 2.16 × 10-12

A:

Q: Calculate the pH value of 0.5 M NaCl

A: There can be 4 type of combinations of salt:A salt formed when a strong acid combines with a strong…

Q: Calculate the pH for an aqueous solution having a hydrogen ion concentration of 2.15 × 10-3 M.

A: pH = -log[H+] where [H+] = hydrogen ion concentration  Hence substituting the values we get  pH =…

Q: Calculate the pH of 0.141 M NaOH

A: we have to calculate the pH of solution

Q: HO II OH OH II IV

A: Answer: acidity order in alcohols are . 1>2>3>4 . Then the pH order is the  4 >3…

Q: If the concentration of OH- ions in a solution is 10^-2 M, pH of that solution will be 7 12 14 2

A:

Q: The pH of a 0.0046 M solution of HNO, is

A: Ph is the negative logarithm of the concentration of Hydrogen ion for dilute solutions. Thus, pH is…

Q: Determine the pH of a 0.33 M solution of NH4Br

A: Since we know that, Pkb(NH3) = 4.74.. Since NH4Br is salt of strong acid and weak base..

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: Calculate the concentration of H3O+ and OH- in a sample of pH 3.30 solution?

A: As we know  pH = -log [H+] and pOH = -log[OH-]  and also pH+ pOH = 14

Q: Calculate the concentration of H+ in a solution of pH = 1.25.

A: pH of the solution = 1.25  Concentration of H+ = ?

Q: Ph for H3O+ = 2.19 × 10‐11

A: pH is negative logarithm of hydrogen ions

Q: calculate the ph of the following solution and tellw hether it is acidic, basic, or neutral…

A: Given, [H3O+] = 4.53 ×10-8 M

Q: the pH of a solution with [H3O+] = 2.0×10^-4 M is

A: The pH of a solution is a measure of its acidity or alkalinity. It is defined as the negative…

Q: Calculate the pH value of 0.5 M NaOH

A: As NaOH is very strong electrolyte i.e base so it will dissociate completely  :…

Q: Calculate the pH of 0.0250 M NaOH.

A: NaOH being a strong base easily dissociated into its respective ions in water. NaOH -------> Na+…

Q: Calculate the pH of 0.730 M hydrazine

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.