Calculate the pH of a 0.14 M ammonium chloride, NH4Cl, solution. The Kb of ammonia, NH3, is 1.8 × 10−5 M.

Q: Predict whether aqueous solutions of the following salts are acidic, basic, or neutral, and write an…

A: ACIDS: A chemical substance which tends to donate protons is known as an acid. An acid is a compound…

Q: The pH of an aqueous solution of 0.415 M aniline (a weak base with the formula C,H&NH,) is

A:

Q: Calculate the pH of a 1.88 M NH3 (Kb = 1.8 x 10^–5) solution

A: The pH is a scale that is widely used to measure the acidity or basicity of a solution. The pH is…

Q: What is the pH of a 0.65 M solution of pyridine, C5H5N?

A: Given,  The concentration of C5H5N is 0.65M The kb value of C5H5N is 1.7×10-9 To solve: pH of 0.65M…

Q: The pH of a white vinegar solution is 2.57. This vinegar is an aqueous solution of acetic acid with…

A: The pH of a solution is given by, pH=-log10H+if the pH of the solution is 2.57, then…

Q: What is the pH of a solution that is 2.0 M HF and 2.0 M F–?  Does your answer make sense?

A: The Henderson Hasselbalch equation for acidic buffer is given as :

Q: What are the pOH and the pH of a 0.0125-M solution of potassium hydroxide, KOH?

A: KOH is a strong mono basic base in nature which dissociates completely. Here the given concentration…

Q: Calculate pH, pOH, [OH-(aq)] and [H;O*(aq)] of a 350.0 mL aqueous solution containing 1.20 g calcium…

A:

Q: Calculate the pH of a 0.210 M solution of sodium benzoate

A: Benzoate is the conjugate base of benzoic acid. In water, benzoate hydrolyses as follows...…

Q: Example: - Calculate the pH and pOH of a 1.0 x 107 solution HCI? HCI H+ + Cl-

A:

Q: Calculate the pH of the following solutions a)1 L 0,100 M malonic acid b)100 ml 0,100 M malonic…

A:

Q: 2. At 25°C , find the pH of (a) an ideal, 3.7 x 10³ M HCl solution; (b) an ideal, 1.00 x 10° M HCl…

A:

Q: If you mix 350 grams of NACN in 640 ml of water, what is the pH? How many grams of its conjugate…

A:

Q: Determine the pH of a 0.16M NH3 where kb = 2.4 x 10-6  follow the format: a) [OH-] in 0.16M NH3…

A:

Q: Calculate the pH of each of the following solutions of a strong acid in water. a. 0.10 M HCl b. 5.0…

A: The question is based on the concept of PH  calculations.   pH is defined as negative logarithmic of…

Q: 10. What is the pH of a 0.4M ammonia solution? The ionization constant of ammonia is 1.8 X 10.

A: Given: Concentration of ammonia solution = 0.4 M Kb of ammonia = 1.8×10-5

Q: Determine the [OH ], [H3O*], pH and pOH in a 1.0 x 103 M Ba(OH)2 solution.

A:

Q: calculate the ph of an aqueous solution that contains 8.5x10-2 M hydroxide ion

A:

Q: The pH of 30 cm^3 of an acidic solution is 2.89. Calculate the concentration of hydrogen ions and…

A:

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: Calculate the pH, pOH, [H*], & [OH] of a 0.025M Ba(OH)2 solution.

A:

Q: Can you show me an example of how to calculate an answer similar with a pH of 9.5?

A: We know that when pH is in between 0-7 then the solution is acidic and when it is in between 7-14…

Q: The pH of an aqueous solution of 9.69×10- M ammonium chloride, NHĄC1 (aq), is This solution is

A: NH4Cl is a salt of strong acid (HCl) and weak base (NH3) hence pH this solution  is given by the…

Q: HCl is a strong acid.  What is the pH of a solution of concentration 1 x 10-3M?

A:

Q: What is the pH of a 0.16 M solution of methylammonium chloride, CH;NH; Cl? What is the concentration…

A:

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: Calculate pH, pOH, [OH-(aq)] and [H30*(aq)] of a 350.0 mL aqueous solution containing 1.20 g calcium…

A: Mass of Ca(OH)2 = 1.20 g  Molar mass ( MM ) of Ca(OH)2 ,         = MM of Ca +2×  MM of O + 2 × MM oH…

Q: At 10°C, the ion-product constant of water, K w, is 6.88 × 10 –15. What is the pH of pure water at…

A: Autoionization of water takes place as follows: The product of the concentration of the hydronium…

Q: The pH of aqueous 0.10 M pyridine (C5H5N) ion is 9.29. What is the Kb of this base

A: Given , Concentration of pyridine (C) = 0.10 M pH of pyridine solution = 9.29 Dissociation constant…

Q: calculate the pH of a 0.10 M perchloric ,HCIO4, solution.

A: pH :-  The negative logarithm to the base 10 of hydrogen ion concentration, [H+] expressed in mol/L…

Q: 8. K/U Write the acid-dissociation constant expressions for each of the following weak acids: a.…

A:

Q: Explain how you determine the pH of 0.500 M HOCI (Ka = 3.6 x 10) www m

A: pH  = - log [H3O+] HOCl is a weak acid and doesn't undergo complete dissociation in solution. Thus,…

Q: solution is made by dissolving 0.0699 mole of calcium hydroxide (Ca(OH)2) in 500 mL of water.…

A: Given: moles of calcium hydroxide Ca(OH)2 = 0.0699 mol Volume = 500mL = (500/1000)L = 0.5L Thus,…

Q: NH3 is a weak base (Kb=1.8×10−5 M), so the salt NH4Cl acts as a weak acid. What is the pH of a…

A:

Q: Identify the Lewis acid and Lewis base from among the reactants in the equation. Fe3+ (aq) + 6H2O…

A: Given, Chemical Reaction ::  Fe3+ (aq) + 6H2O (l) -->  Fe(H2O)63+ (aq) Lewis acid :? Lewis base :…

Q: The acid dissociation constant K, of carbonic acid (H,CO3) is 4.5 x 10. Calculate the pH of a 3.4M…

A: All details  explained  in Handwritten solution

Q: Determine the pH of a solution in which the hydronium ion concentration was determined to be 3.70 x…

A: Given information: [H3O+] =3.70 x 10-4 moles/liter

Q: A 0.025 M solution of an unknown organic acid has a pH of 2.75. By means of a full calculation,…

A: Given: Concentration of acid HA = 0.025 M And pH of the acid solution = 2.75. Since pH = -log[H+ ]…

Q: What is the pH of a solution that is prepared by adding 4.0 mL of 0.50 M NAOH(aq) and 4.0 mL of 0.40…

A:

Q: Calculate the pH of a 0.0015 M solution of the strong base Sr(OH)2

A:

Q: Calculate the size of the pH change when the ratio HA] changes from 10 to 1.

A: We can calculate it from dissociation constant of acid and we should do comparisons which is…

Q: Enough water is added to 0.35g of benzoic acid to make 1000 mL of a solution. What is the pH?…

A: Given: Mass of benzoic acid=0.35 g Volume of solution=1000 mL =1 L Ionization constant for benzoic…

Q: What is the pH of a solution that is 0.041 M in NH4Cl?

A: NH4Cl salt can be formed from weak base NH4OH and strong acid HCl. So it is a salt of strong acid…

Q: What is the concentration of hydroxide ion in a 0.150 M aqueous solution of hydroxylamine, NH,OH?…

A: NH4OH is a weak base, hence it can't dissociate completely, hence equilibrium is established between…

Q: The pH of a solution of M(OH)2 is 13.08 .  What is the molarity of the M2+ ion?

A:

Q: Estimate the pH of a 0.016 M aqueous lead (II) chloride.

A:

Q: The pH of an aqueous solution of pyridine (C5H5N) is 10.0 at room temperature. What is the initial…

A: Weak acid or base are those substance which does not dissociate 100%. The value of degree of…

Q: Explain how you determine the pH of 0.500 M HOCI (Ka 3.6 x 108)

A:

Q: Explain how a set of weak bases, all with approximately the same 0.1 molarity, can have different pH…

A: Answer

Q: The base protonation constant K, of ammonia (NH,) is 1.8 x 10. Calculate the pH of a 1.2 M solution…

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.