A solution is prepared and the resultant pH = 12. What is the pOH of the solution? 12 8 -2 2

Q: The pH of hydrochloric acid solution of 1 x 10-9 M is 6.8 9 7.4

A: Concentration of HCl =1 x 10-9M                                      = 10-9Mor   [HCl] =  10-9M

Q: The [H3O+] in a solution with pOH of 0.253 is ____.

A:

Q: During a lab discussing the effect of pH on food preservative, HCl was added to sodium Benzoate…

A: Sodium benzoate is a chemical commonly used as a food preservative. If sodium benzoate becomes…

Q: The pH of the following solutions will be equal to or less than 7.0 for all of the following…

A: The pH of the following solutions will be equal to or less than 7.0 for all of the following…

Q: 19. Consider the K, values for the following acids: Cyanic acid, HOCN, 3.5 x 10 Formic acid, HCHO2,…

A: Here multiple choice question is given.

Q: 5) What is the pH of a 0.250 M HF solution? The Ka of HF is 3.5 X 104. (2.03) HF (aq) + H2O (1) A…

A: We will calculate pH

Q: Which of the following liquids/solutions is most likely to have the highest pH? a) KOH(aq) b)…

A:

Q: pH indicators are frequently* standardizing agents weak acids or bases O oxidizing agents O reducing…

A: pH indicators are usually Weak acids or weak bases. If we take an Acidic indicator as HInd with…

Q: What is the pHpH of a 0.24 M0.24 M solution of the weak base?

A: pH + pOH = 14  pH = 14 - pOH  pOH = -log[OH-]

Q: Calculate the pH of the solution, where the acetic acid is x10 stronger than acetate.

A: In chemistry, pH is defined as the potential of hydrogen ion. It is the negative logarithm of…

Q: Step by step please

A: The following reaction takes place when NaF dissociates in water,

Q: Calculate the pOH for the solution with a concentration of [H+] = 2.4x10

A:

Q: The pOH of formic acid solution is----- if a 0.1M of the acid is 10 % ionized ---- --

A: The question is based on the concept of equilibrium. we have been given a weak acid formic acid…

Q: Calculate the pH and pOH for each of the solutions with the following hydrogen ion or hydroxide ion…

A: pH is is defined as power of hydrogen  PH = log [H+]

Q: What is the hydronium concentration [H3O+] of a solution with a pOH of 2.47?

A: Given data is as follows: The pOH of the solution = 2.47 As we know that;  pH + pOH =…

Q: The pOH of an aqueous solution of 0.435 M nitrous acid is

A: Formula used :-  pOH = -log[OH]-

Q: 1. IfH ions in the solution increases, a The more basic is the solution. b. The solution becomes…

A: Acidity and basicity of a solution can be measured by using pH scale. pH less than 7 means solution…

Q: A solution contains 5.59×10-2 M potassium fluoride and 0.136 M hydrofluoric acid. The pH of this…

A:

Q: What is the pH of a solution what is formed when 0.035M HCl(aq) is mixed with 0.045M HBr(aq)?

A: Given that, [HCl]= 0.035 M  [HBr]= 0.045 M  pH of the solution = ?

Q: 0.60 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 6.0 L of solution. What is…

A: Molecular weight of NaOH= (23+16+1) = 40 gm/mol  Amount of NaOH taken = 0.6 gm  Moles of NaOH =…

Q: Calculate the pOH in a solution that has [H+]= 4.7x10-8 M.

A:

Q: The pOH of an acidic solution is 10.01. What is [H*]?

A: Find the solution below

Q: What is the the PH and POH of the following solutions: 1. 0.05 M Ba(NO3)2 2. 0.01 M Na2SO4

A: The given solutions are 0.05 M Ba(NO3)2 and 0.01 Na2SO4.

Q: What is the the pH of a H2O + HCl solution. Where there is 6.0 M HCl.

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: The pH of 0.10 M solution of an acid is 6. What is the percentage ionization of the acid?  6.0 %…

A: Given, pH = 6. Concentration of solution = 0.10M. The dissociation of acid can be given as follows:

Q: A sodium hydroxide solution is prepared by dissolving 9.0 g NaOH in 5.00 L of solution. What is the…

A:

Q: . What is the pH of a solution that contains 0.35 mol/L of the strons base NaOH?

A:

Q: 3. If you had 36 ml of a .14M solution HBr that you mixed with 40 ml of a .11M solution of RBOH,…

A:

Q: More HA molecule is added to HA(aq) + H,0(1) A(aq) + H,0"(aq). What will happen to the pH of the…

A: Given : Two reactions are given  To Find: vi) If HA is added to it, what will happen to equilibrium…

Q: A 1.0 M NaCl solution has an initial pH of 7.00 at 25° Using your knowledge of ions that participate…

A: Counter ions of strong acid or base do not hydrolyse.

Q: There are several chemical equilibria taking place in a solution of carbon dioxide in water: 1.…

A: A question based on equilibrium concept that is to be accomplished.

Q: What happens to the pH of the final solution if equal volumes of octimolar nh4oh and CH3COOH…

A: NH4OH is ammonium hydroxide which is a weak base. CH3COOH is acetic acid which is a weak acid. Weak…

Q: Calculate the pH of the resulting solution if 25.0 mL of 0.250 M HCl(aq) is added to15.0 mL of 0.350…

A:

Q: What is the pH of a 0.454 M nitrous acid solution? HNO2 ->

A:

Q: A solution has a pOH of 12.4. What is the pH of this solution?

A:

Q: hydrochloric acid solution has a pH value of 3. Which of the following substances would increase the…

A: On addition of an acid pH of the solution decreases as acid gives H+ ions in the water while on…

Q: A solution formed by dissolving an antacid tablet has a pOH of 4.82. Calculate 3H+4.

A: We know that pH + pOH = 14 Given: pOH = 4.82 So, pH = 14 - 4.82 = 9.18

Q: Calculate the pH and pOH of the: 0.125M potassium hydroxide (KOH) solution

A:

Q: 6. The pH of a solution is 6.5, what is the [H3O*]? What is the pOH? What is the [OH]?

A: pH of solution is defined as the concentration of hydronium ion H3O+in the solution pOH of solution…

Q: Calculate the pH and the pOH of these solutions:

A:

Q: Calculate the OH– concentration & pOH of a 0.075 M NH3 solution (Kb=1.75 × 10–5).

A:

Q: The pH of an aqueous solution of 0.223 M ammonium bromide, NH,Br (aq), is This solution is

A: In this question, we want to determine first the pH of the aqueous solution of NH4Br(aq) and then…

Q: The Kb of hydrazine is 9.1 x 10-7. If 3.12 x 10-3 mol of hydrazine is added to water to make up…

A: Hydrazine (N2H4) is a weak base Concentration of hydrazine is calculated as follows,

Q: Calculate the pOH value of a 0.0150 M solution of pyridine, C5H5N.

A:

Q: A solution has a pOH of 4.5. What is the concentration of H3O+ in the solution in Molarity? Group…

A: pH of solution is defined as the concentration of hydronium ion H3O+in the solution pOH of solution…

Q: The pOH of a solution is 9.05. What is the H* concentration in the solution?

A: [OH-] = 10-pOH  [H+].[OH-] = 10-14  [H+] = 10-14/ [OH-]

Q: What is the pOH of this solution?  What is the pH of this solution?

A:

Q: 0.100 M HCL, what will be the pH of the resulting solution? Ca(OH)2 (aq) + HCl (aq) CaCl2 (aq) + H2O…

A: Applying concept of molarity equation MV= M2V2 -M1V1

Q: Differentiate the Arrhenius acids and bases, Bronsted-Lowry acids and bases, and Lewis acids and…

A: Redox reactions can be defined as the  reaction in which both oxidation and reduction reaction occur…

Q: The pH of an aqueous solution of 0.176 M ammonium bromide, NH Br (aq), is This solution is

A: 1. Solution - According to the question - pH = pH stand for potential of hydrogen, since pH is…

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.