If the K of a weak base is 2.4 x 10-6, what is the pH of a 0.47 M solution of this base? pH =

Q: A 0.010 M solution of a weak acid, HA, has a pH of 3.10. What is the K, of the acid? 6.3 x 106 6.3…

A: pH is the negative logarithm of the hydronium ion concentration of a solution. Given:- pH = 3.10…

Q: What is the pH of a 2.35 x 10-2 M HCl acid solution?

A:

Q: What is the pH of a solution of 8.2 x 10-5 M HCl?

A: GivenConcentration of HCl = 8.2 x 10-5 MHCl a strong electrolyte completely dissociate solutionHCl →…

Q: If the K of a weak base is 8.5 x 10-6, what is the pH of a 0.27 M solution of this base? pH =

A:

Q: HCIO is a weak acid (Ka = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: Ka of HClO = 4.0 × 10-8 Concentration of the solution of NaClO = 0.089 M pH =?

Q: The OH concentration in an aqueous solution at 25 °C is 7.9 x 10-3. What is [H]?

A: pH of a solution measures acidity or basicity of solution. pH less than 7 indicates solution is…

Q: Butyric acid  ( C3H7COOH) is a weak acid . What is the pH of a 0.0250 M solution of this acid. Ka =…

A: For weak acids, ions dissociation is very small that results in small H+ ions amount. Their…

Q: If the Ka of a monoprotic weak acid is 5.8 × 10-6, what is the pH of a 0.47 M solution of this acid?

A: Given: Ka=5.8×10-6 Molarity of acid = 0.47 M

Q: If the K, of a monoprotic weak acid is 7.5 x 10, what is the pH of a 0.42 M solution of this acid?…

A: Given: Ka=7.5×10-6 C=0.42M

Q: The pH of a 0.0833 M ethanoic acid (Ka=1.8x10-5) solution is

A:

Q: A certain weak base has a Kp of 7.30 x 10-'. What concentration of this base will produce a pH of…

A: Given data, Kb =7.30×10-7 pH =10.37 Let us consider the weak base is B. It react with water as,…

Q: What is the pH of a solution containing 0.225 M weak base, B', with a K, of 3.8 X 10-7? в (аq) + Н,О…

A:

Q: For a given acid, Ka is 7.2  x 10−4. This means that it is: a strong acid B a weak base C a weak…

A:

Q: What is the pH of a 0.139 M solution of HF? Ka for Hf is 6.6 x 10-4

A:

Q: If the K of a weak base is 7.0 × 10-6, what is the pH of a 0.37 M solution of this base? pH :

A: We make an ICE table then equilibrium constant expression is written ,since we have weak acid so we…

Q: pH

A:

Q: Lactic acid is produced in the tissues by anaerobic metabolism of glucose. Lactic acidosis occurs at…

A:

Q: Determine the pH of a solution of a weak acid (HA) that is 0.17 M. The Ka of the weak acid is 7.5 x…

A: Given a concentration of weak acid (HA) =0.17M Acid dissociation constant value =        7.5 x 10-5…

Q: A weak base has a base hydrolysis constant, K, of 3.2 x 10-6. What is the pH of a 0.18 M solution of…

A:

Q: a value of 7.2 x 10*. What is the pH to 2 decimal -f hydrofluoric acid with a concentration of 0.537…

A: We will calculate pH

Q: What is the pH of a 75.0 mL solution that is 0.049 M in weak base and 0.055 M in the conjugate weak…

A: The pH can be calculated by using Henderson equation  poH =pkb +log10 [ conjugate acid]/ [weak base]

Q: The ionization constant for NH3 in water is 1.8 x 10 - 5. Determine the hydrox concentration and the…

A: The dissociation of ammonia in aqueous solution can be represented as: The ionization constant for…

Q: If the K, of a monoprotic weak acid is 1.4 x 10-6, what is the pH of a 0.14 M solution of this acid?…

A: Given:   The concentration of acid is 0.14 M. The Ka of a monoprotic weak acid is 1.4×10-6.

Q: If the K of a monoprotic weak acid is 1.4 x 10-6, what is the pH of a 0.14 M solution of this acid?…

A: Given : Ka of monoprotic acid (assuming HA) = 1.4 X 10-6  And Concentration of acid = 0.14 M Since…

Q: What is the pH of a solution which is 0.023M in weak base and 0.039 M in the conjugate weak acid (Ka…

A: This question can be solved using Henderson-Hasselblach equation. The equation is, pH=pKa+…

Q: Based on the Kb determined in the previous part, what is the pH of the initial 1.0 M base solution?…

A:

Q: The Ka of a weak monoprotic acid is 1.85 x 10-5. What is the pH of a 0.0761 M solution of this acid?

A: First, we have calculated the concentration of [H+] with the help of Ka and the concentration of the…

Q: If the K of a weak base is 8.0 × 10-6, what is the pH of a 0.48 M solution of this base? pH

A: Weak base dissociated less in aqueous solutions

Q: If the K, of a weak base is 2.4 x 10-6, what is the pH of a 0.27 M solution of this base? pH =

A: Given,  Base dissociation constant of base (say B) = Kb= 2.4 x 10-6  Molarity of base (B) = 0.27 M…

Q: Calculate the pH of the following solutions: (a) 0.0500 M NaOH (b) 0.0500 M sodium acetate (c)…

A: A)   0.05 M  NaOH    As NaOH is a strong base, it will dissociate completey.   NaOH (aq) → Na+ (aq)…

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

A:

Q: HCIO is a weak acid (K, = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: given  HClO Ka=4.0 x 10-8  concentration of  NaClO IS 0.027  PH =?

Q: If the Kh of a weak base is 6.2 × 10-6, what is the pH of a 0.24 M solution of this base? pH =

A:

Q: HCN has a K, of 4.9 X 10-10. What is the pH of a solution which contains 0.350 M NaCN? CN (aq) + H,O…

A: The pH of a solution helps to determine the acidity and alkalinity of a solution. The solution maybe…

Q: The K₂ of a weak monoprotic acid is 1.74 x 10-5. What is the pH of a 0.0939 M solution of this acid?…

A:

Q: A particular base has Kb= 4.4*10^-4. What is the pH of 0.35M solution of this base ?

A: Since the Kb value is less so the dissociation of base is very less and it is assumed that the…

Q: What is the pH of 5.04 x 10-3 M HI? Is it acidic, basic, or neutral?

A: HI is a strongest acid it dissociates completely .

Q: A certain weak base has a Kp of 8.60 × 10-'. What concentration of this base will produce a pH of…

A: Kb = 8.40x10-7 pH= 10.37 Concentration of base=?

Q: what is the pH of a 7.1 x 10^-3 M solution of H^+?

A: Given : [H+ ]  = 7.1  x 10-3 M

Q: If the Ką of a monoprotic weak acid is 1.4 × 10-6, what is the pH of a 0.42 M solution of this acid?…

A: Given data, ka = 1.4 × 10-6  Concentration of Weak acid = 0.42 M

Q: If the K of a weak base is 5.6 × 10-6, what is the pH of a 0.40 M solution of this base? pH

A: Given:  Kb = 5.6×10-6 Concentration = 0.40 M Since, the value of Kb and concentration of base is…

Q: Calculate the pH of a solution that is 0.450 M HC2H2O2 and 0.730 M NaC2H3O2. The Ka for acetic acid…

A: This problem is solved by using Henderson Hassel baltch equation.

Q: If the Ka of a monoprotic weak acid is 1.6 x 10-6, what is the pH of a 0.37 M solution of this acid?…

A:

Q: Determine the pH of a solution of a weak acid (HA) that is 0.0072 M. The Ka of the weak acid is 1.9…

A: Given ,  Weak acid is HA Concentration of weak acid (C) = 0.0072 M Dissociation constant (Ka) of the…

Q: HCIO is a weak acid (K, = 4.0 x 10-) and so the salt NaCIO acts as a weak base. What is the pH of a…

A:

Q: HCIO is a weak acid (K. = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A:

Q: If the Ka of a monoprotic weak acid is 4.7 x 10-6, what is the pH of a 0.49 M solution of this acid?…

A: Given Ka = 4.7 x 10-6 C = 0.49 M

Q: HCIO is a weak acid (K, = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: pH = 7 +12 (pka + log c)

Q: What is the hydronium ion concentration [H3O+] of a 0.010 M acetic acid solution in water? (Ka for…

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.