What is the pH of an aqueous solution of 4.16×10-2 M hydrochloric acid? pH =

Q: What concentration of potassium hydroxide is needed to give an aqueous solution with a pH of 9.770?…

A: pH = 9.770   pH + pOH = 149.770 + pOH = 14pOH = 14 - 9.770pOH = 4.230   pOH = - log [OH-]4.230 = -…

Q: If the hydronium ion concentration of a weak acid is 6.32 x 10 M what is the pH?

A: Given :- concentration of hydronium ion = 6.32 x 10-4 M  To calculate :- pH of the solution

Q: What is the pH of an aqueous solution of 1.59x102 M hydrochloric acid? pH =

A: pH = -log[H+]

Q: what is the pH of a 0.015-M aqueous solution of barium hydroxide?

A:

Q: The pH of an acidic solution is 2.19. What is [OH]?

A: The question is best on the concepts of PH. we have to calculate hydroxide Ion concentration.

Q: What is the pH of an aqueous solution of 4.96x102 M hydrobromic acid? pH

A:

Q: If the Hydrogen ion concentration of a solution is 1.00 x 10^-4 M, what is the hydroxide ion…

A: Hydrogen ion concentration = 1.00 × 10-4 M. Hydroxide ion concentration = ?

Q: Classify each of the following as a strong acid or a weak acid. Indicate how each should be written…

A:

Q: Determine the pH for each of the following solutions: a. [H3O+] = 2.0 x 10-8 M b. [H3O+] = 5.0 x…

A:

Q: What is the pH of a 2.8 x 10-4 M solution of NaOH? What is the hydronium ion concentration of the…

A:

Q: Calculate the pH of an aqueous solution of 0.1340 M potassium sulfite. pH = ||

A:

Q: What is the pH of a solution with a pOH of 10?

A: Given that,  pOH of a solution = 10

Q: What is the pH of a 1.5x10-7 NaOH solution?

A: Given , Solution is NaOH Molarity = 1.5×10-7  { I am considering the the solution expressed in…

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: Classify the following aqueous solutions as strongly acidic, weakly acidic, neutral, weakly basic,…

A: (a) battery acid, pH 0  ----> strongly acidic. (b) lime juice, pH 2.7  -----> strongly acidic.…

Q: A solution has a hydroxide-ion concentration of 0.043 M. What is its pH?

A:

Q: What is the pH of an aqueous solution with a hydrogen ion concentration of [H+]=1.6×10^−4 M?   pH=

A: The pH of an aqueous solution can be calculated using equation (1). In this equation [H+] represents…

Q: In an aqueous solution the  [OH-] is 1.0 x 10- 6 M. What is the [H+]

A: At 25oC, the mathematical relation between molarities of H+ and OH- is given as: [H+][OH-]=1.0×10-14…

Q: What is the pOH of an aqueous solution of 0.144 M hydrochloric acid? pOH =

A: In this question, we have to determine the pOH of aqueous solution of 0.144 M hydrochloric acid. pOH…

Q: A sample of TANG juice has a hydronium-ion concentration of 1.7 x 10^-4 M. What is the pH? Is the…

A:

Q: A solution contains [OH-] = 4.88 x 10-6 M. What is the pH of the solution?

A: Given   The concentration of OH- is 4.88×10-6 M.

Q: What is the pH of a 0.0050 M solution of hydrochloric acid?

A: The pH of a solution is calculated by,

Q: What is the concentration of barium hydroxide in an aqueous barium hydroxide solution with a pH of…

A: Given information: pH = 10.20

Q: Classify each of the following species as a Brønsted acid or base, or both: (a) H,0, (b) OH¯, (c)…

A:

Q: What is the pH

A:

Q: What is the pOH of a solution with a pH of 1.80? The answer should be put to the proper number of…

A: Applying formula PH+POH= 14

Q: What is the pH of a solution of 3.7 M HBr?

A: We can calculate pH of a solution by using following equation pH = - log [H+]

Q: What is the pH of an aqueous solution of 1.89×10² M barium hydroxide? pH %3!

A: As barium hydroxide is a strong base. So dissociation takes place like:- Ba(OH)2 -------------->…

Q: the concentration of H3O+ of seawater is 3.16 x 10-9. what is the pH of seawater?

A: Ph depends on concentration of H+ ions...

Q: What is the pH of the following solutions? [OH-] = 9.1 × 10-3 M

A: We can only Calculate the pH of solution if we know the Hydrogen ion concentration of solution. To…

Q: What is the pH of a solution with a pOH of 2.4? Is the solution acidic or basic?

A: We have pOH as 2.4 , we have to calculate pH as well as nature of solution.

Q: What is the pH of an aqueous solution of 2.15×102 M nitric acid? pH =

A:

Q: 2. Complete the following table: [H;O*] [OH] pH Solution is acidic, basic or neutral 4.56 X 102 3.5…

A: In the given problem we are required to complete the table in which we have to calculate the pH,…

Q: what is the ph of a solution that has [OH-]= 6.9x10^-12

A: Given :- concentration of OH- ions = 6.9 × 10-12 M  To calculate :- pH of the solution

Q: What is the pH of an aqueous solution with a hydroxide ion concentration of 4.20 x 10-4 M?

A:

Q: What is the pH of an aqueous solution of 6.78x102 M barium hydroxide? pH =

A:

Q: what is the pH of a solution that has the following H+ concentraion? 1.75 x 10^-5 mol/L

A:

Q: What is the pH of an aqueous solution of 1.99×102 M perchloric acid? pH =

A: The pH of a solution can be calculated by using formula pH = -log10[ H+]

Q: A solution has a hydrogen ion concentration of 1 x 10^6 M. What is the pH?

A: The negative logarithm of concentration of hydrogen ion is known as pH. pH = – log [H+]

Q: What is the pH of an aqueous solution of 1.56x10² M perchloric acid? pH =

A:

Q: What is the pH of a 1.2 x 10-4 M solution of KOH? What is the hydronium ion concentration of the…

A: The concentration of the KOH solution is = 1.2×10-4 M The hydronium ion concentration of the…

Q: Which of the following are strong acids? HI HNO 3 HE HBr

A:

Q: What is the pH and pOH of a solution with a [OH]] of 7.79 X 10S M? Is the solution acidic, basic or…

A: The solution with a pH less than 7.00 will be acidic. The solution with a pH more than 7.00 will be…

Q: The OH- ion concentration of a blood sample is 2.5 x 10-7 What is the pH of the blood?

A: First from given OH- ion concentration the pOH value is calculated.

Q: Calculate the pH of the following solutions 0.0040 M Ba(OH)2

A:

Q: You have a 7.4x10-4M Sr(OH)2 solution. What is the pH of this solution?

A: First of all we will calculate pOH then pH

Q: What is the pH of an aqueous solution with a hydrogen ion concentration of (H*] = 4.1 x 10-5 M? pH =

A: Given information,      [H+] = 4.1 × 10-5 M

Q: Which of the following chemical formulas corresponds to a base? HCl; KOH; H2SO4; HNO3

A: Acids are H+ (proton) donors and bases donate the OH- ions.

Q: The pH of a solution is 3.10. What is the OH- concentration in the solution?

A:

Q: In a solution, [H+ ] = 3.25 x 10-10 M. What is its pH and is it considered an acid or a base?

A: A solution can be classified as acidic or basic or neutral depending on the pH value. For a solution…

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.