A 0.0500 M solution of a base is 7.5% ionized. Calculate the base ionization constant Kb.

Q: Determine the pH of the solution. (2 decimals) 0.21 M KCHO 2 (Ka(HCHO₂)=1.8x10-4)

A: Answer:When salt of weak acid and strong base is added in water, due to hydrolysis it produces OH-…

Q: Ką for acetic acid, CH3COOH, is 1.80×10°. Ką for nitrous acid, HNO2, is 4.50×104. Ką for hydrocyanic…

A: Given: Ka for acetic acid, CH3COOH = 1.80×10-5 Ka for nitrous acid, HNO2 = 4.50×10-4 Ka for…

Q: 2. 50 x 10-5 , wha

A: Given data are as follows: Concentration of acidic solution = 0.05 M Ionization constant = 2. 50 x…

Q: If the hydrogen ion concentration of a 0.100 M HClO solution is 0.000 055 M, what is the ionization…

A: The equation for the ionization of HClO is as follows. HClO(aq)↔ClO-(aq)+H+(aq)

Q: A 0.513 M solution of a weak base has a pH of 11.4. What is the Kb of the base?

A: Weak base concentration is given and pH is also given we have to find the Kb.

Q: Enter your answer in the provided box. Determine the K, of a weak base if a 0.29 M solution of the…

A: The pOH of 0.29 M solution is calculated below.

Q: What is [H⁺]?

A: Given :- pH = 11.65  To calculate :- [H+]

Q: Calculate the pH of a solution that is 0.185M benzoic acid and 0.240M sodium benzoate, a salt whose…

A: Henderson Hasselbalch equation for acidic buffer mixture is pH = pKa + log Where pKa = - log ( Ka )…

Q: the pH of a basic solution is 10.47. What is [H+]

A:

Q: Calculate the pH of the following solutions in which the [H+] is a) 0.01, b) 1.0 x 10 –8 , and c)…

A: Given that -  Hydrogen ion concentration , [H+] are -  a) 0.01 b)1.0 x 10 –8  c) 4.67 x 10 –4  Then,…

Q: Calculate the pH of an aqueous solution of 0.0740 M potassium sulfite.

A:

Q: Calculate the pH of an aqueous solution that is 0.70 M sodium hypochlorite.

A: The given compound Sodium hypochlorite (NaClO) is a strong electrolyte. So, it dissociates…

Q: A 0.431 M solution of a weak base has a pH of 10.67. What is the base ionization constant, Kb. for…

A: The objective of this question is to calculate the base ionization constant, Kb, for a weak base…

Q: Calculate the pH of a 0.200 M solution of a weak base, A", given K = 1.11×107. pH =

A: pH = 10.2 (Rounded off.)Explanation:To calculate the pH of a weak base like A-,  Step 1: First, we…

Q: A 0.150 M solution of a weak acid has a pH of 2.65. Calculate the acid ionization constant Ka for…

A: 3.34×10−5Explanation:

Q: Calculate the pH of each of the following solutions of strong acids.

A:

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: Hydrogen selenide (H2Se) reacts with water according to the following equation. H2Se + H2O → SeH– +…

A:

Q: 0.05 Μ of a weak acid solution (HA) ionizes 0.2 percent in water. Find its acid dissociation…

A: Concentration of weak acid, c = 0.05 M Percentage ionisation = 0.2% x = 0.002

Q: Determine the percent ionization of the 9.58 M solution of HIO3. Ka = 0.17.

A:

Q: o simplify the measurement of the acidity or basicity of a solution, the pH (hydrogen potential)…

A: Given[H+] = 0.0000375 pH = To be determined

Q: Calculate The pH 0.09M solution of magnesium hydroxide

A:

Q: -69 The acid dissociation constant K, of hypobromous acid (HBrO) is 2.3x 10. Calculate the pH of a…

A: Consider the dissociation of hypobromous acid is as follows:                       HBrO   →     H+…

Q: A 0.125 M weak acid (HA) solution has a pH of 2.25. Find the acid ionization constant, Ka-

A: Given that : Initial concentration of weak acid = 0.125 M pH = 2.25 The pH can be given by : pH =…

Q: What is the ionization constant of a weak acid [HA], when its conjugate pair has a Kb value of 4.4 x…

A: In the ionization of a weak acid HA, A- is produced as a conjugated base.  HAAcid →Ionization…

Q: Be sure to answer all parts. Please report your answer to the correct number of significant figures.…

A:

Q: Calculate the hydroxide ion concentration of a solution with pH= 2.8

A: Given: pH= 2.8 To find: The concentration of hydroxide ion

Q: Ammonia is a weak base with a ?b of 1.8×10−5. Calculate the initial molar concentration of a…

A: Answer:-This question is answered by using the simple concept of calculation of concentration of…

Q: Question 3 A student is given a concentrated solution that is supposed to contain vinegar, a weak…

A: A weak acid will not be completely dissociated in a solution. However, a strong acid will be…

Q: Calculate the pH of the following solution:

A: Given :- concentration of NaOH = 2.4 x 10-5 M  To calculate :- pH of the solution  pH + pOH = 14

Q: If the K, of a weak base is 1.7 × 10-6, what is the pH of a 0.18 M solution of this base? pH =

A: pH of a substance represents the strength of an acid or base. If the pH is small, it is a strong…

Q: Ph for H3O+ = 2.19 × 10‐11

A: pH is negative logarithm of hydrogen ions

Q: The generic equation for a weak base in water is: ?+?2?⟷??++??−B+H2O⟷BH++OH− A 0.0500 M solution…

A:

Q: Ką for formic acid, HCOOH, is 1.80×10-4. Ką for acetylsalicylic acid (aspirin), HC,H,04, is…

A: ->conjugate base of strong acid is weak base. ->Ka is proportional to acidity. ->conjugate…

Q: The pH of a 2.16 M solution of a weak base B is measured to be 11.00.    Determine the pH of a 2.00…

A:

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: Be sure to answer all parts. Please report your answer to the correct number of significant figures.…

A: Formula: pH + pOH = 14 pOH = - log[OH] For a weak base solution: [OH] = (Kb × C)1/2 Where, C = molar…

Q: Calculate the pH of a 0.37 M solution of sodium hydrogen sulfite,  (6.0x10^-8). pH =

A: The pH of a 0.37 M solution of sodium hydrogen sulfite is to be determined. (Ka = 6.0x10-8).

Q: 1.21 х 103 М HNO3

A: Calculate the pH of each of the following solutions of strong acids.

Q: pH of a 0.30 M solution of a weak base B is 9.02. What is the K, of the base? Be sure your answer…

A:

Q: The pH of a basic solution is 9.77. What is [OH⁻]?

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

Q: Calculate the hydroxide ion concentration of a solution with pH = 6,4.

A: pH of solution is 6.4 We need to determine [OH-]

Q: K, for acetic acid, CH3COOH, is 1.80×10-5. Ką for hypochlorous acid, HC10, is 3.50x10-8. Ką for…

A:

Q: The ionization constant for water (Kw) is 2.9 × 10−14 at 40 °C. Calculate the pH of pure water at 40…

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

Q: 11.) Acid strength decreases in the series HI > HSO4– > HF > HCN. Place the conjugate bases of these…

A: Stronger the acid weaker will be the conjugate base

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.