What is the concentration of the lactate ion in a 1.00 M lactic acid solution given that the Ka of HCH3H503 is 1.38 x 10 4? 5.26 x 10-5 M 1.38 x 10-4 M 1.17 x 102 M 1.00 M 0.998 M

Q: What is the hydroxide ion concentration in a solution of triethylamine with the concentration of…

A:

Q: The % ionization of a 0.015 M aqueous solution of an acid is 0.14 at 25 °C. What is Ka of this acid…

A: Let the acid be HA. So it will disociate as H+ + A- . Let the concentration of acid be denoted as C…

Q: What is the equilibrium concentration of H2C2O4 in a .542 M oxalic acid H2C2O4 solution? For oxylic…

A:

Q: Determine the concentration of CO32- ions in a 0.18 M H2CO3 solution. Carbonic acid is a diprotic…

A: Carbonic acid is a weak acid and it dissociates partially to release the hydrogen ions.

Q: Determine the ka for each of the different concentrations for Acetic Acid              1.00 M…

A: Given that, (i) Concentration of acetic acid = 1.00 M    pH of the acetic acid solution = 2.65 We…

Q: The pH of a 0.063 M solution of a weak acid is 3.95. What is the value of Ka for this acid. A. 2.5 x…

A: Interpretation: The pH of a 0.063 M solution of a weak acid is 3.95. The value of Ka for this acid…

Q: The value of Kp for the C3H5O2 ion is 7.7 x 10-10. What is the value of Ka for HC3H5O2? Ka =

A:

Q: What is the equilibrium concentration of H2C204 in a 0.170 M oxalic acid, H2C2O4, solution? For…

A: Let α  be the degree of dissociation of H2C2O4:                          H2C2O4    ↔       HC2O4-  +…

Q: Q3/ Calculate the pH of a solution containing (0.1 M) of (Fe+] [Mg+]. knowing that Ksp is for…

A: Dissociation of Fe(OH)3 : Fe(OH)3 → Fe3+ + 3 OH- Ksp = 1 x 10-13 = [Fe3+] [OH-]3   Dissociation of…

Q: In the laboratory, a general chemistry student measured the pH of a 0.461 M aqueous solution of…

A: The acid dissociation constant Ka is the equilibrium constant, which indicates the acidic strength…

Q: A 0.22 M solution of a weak monoprotic acid, HA, has a pH of 3.28. Calculate Ka for the acid. 1.5 ×…

A: Given, pH = 3.28 Concentration of weak monoprotic acid= 0.22M

Q: What will be the [H*] in a 0.50 M solution of HCIO? The Ka of HCIO = 3.5 x 10-8 A) 1.8 x 10-8 M B)…

A:

Q: A weak base has a Kp = 6.4 x 10-5. What is the Ka of its conjugate acid O 6.4 x 10° O 1.6 x 10-10…

A:

Q: A solution is prepared from two weak acids, 0.2 M HA and 0.1 M HB. If the Ka of HA is 1x10-5 and the…

A: pH - It is the negative logarithm of the hydronium ion concentration of a  solution. Equilibrium -…

Q: Calculate the Ka of a 0.400 M acid solution with [H30*]= 1.4x 10 4M O 1.40 x 106 O 1.40 x 10 5 O…

A: Equilibrium constant is defined as products concentrations divided by reactant concentrations to the…

Q: What is the pH of a buffer solution that is 0.26 M chloroacetic acid and 0.17 M sodium…

A: An acidic substance is the substance that can give H+ ions. They are corrosive and sour in nature.…

Q: 4 A solution is made by dissolving 24.7 g of LIC3H5O2 in 500.0 mL of water. a Does Li have any…

A: We are authorised to solve first three subparts of a question. Please post rest of the subparts…

Q: Calculate the Cyanide (CN") ion concentration of a solution that is 0.60 M in HCN and 0.20 M in HCI.…

A: First determine the hydrogen ion concentration of the solution. HCl is strong acid hence the…

Q: What is the pH of a buffer solution that is 0.39 M chloroacetic acid and 0.27 M sodium…

A:

Q: Calculate the percent ionization and the pH of the following solution of benzoic acid, HC7H5O2 (Ka =…

A:

Q: There is a buffer solution containing 0.50 M acetic acid (CH3COOH, Ka= 1.8 X 10-5) and 0.50 M sodium…

A: A buffer is used to maintain the pH of the solution when the addition of acid or base is done. pH of…

Q: arbonic acid is an example of weak acid. Calculate the Ka of the carbonic acid (H2CO3) based on the…

A: Acid dissociation constant can be determined by dividing the equilibrium concentration with initial…

Q: A 0.10 M aqueous solution of acid HA has a pH = 3.15. Determine which will be the value of Ka for…

A: Acid is a substance that donates a H+ion. If an acid on dissolving in water cannot dissociate…

Q: Calculate the pH after the addition of 35 ml of 0.8 M of NaOH to 32 ml of 0.5 M of citric acid.…

A: Given : concentration of citric acid = 0.5 M volume of citric acid = 32 mL moles of citric acid =…

Q: What is the pH of a 0.0013 M solution of niacin? Ka = 1.5x10^-5

A:

Q: What is the pH of a buffer solution that is 0.46 M chloroacetic acid and 0.29 M sodium…

A: Since chloroacetic acid is a monoprotic acid.

Q: 7. The equilibrium constant of acetic acid in an aqueous solution of of concentration is given by :…

A: Since you have posted multiple questions, we will solve first question for you. If you want any…

Q: The pH of 0.100 M Jackmanic Acid, HJa, is 2.24. What is the value of Ka for the acid? a. 4.4 x 10-5…

A: Equation representing dissociation of HJa in water: HJa + H2​O → H3​O++ Ja− Dissociation constant,…

Q: Calculate the pH of a buffer solution in which the acetic acid concentration is 5.8 × 10−1 M and the…

A:

Q: Which of the following solutions will have the lowest pH value 2.0 M CH3COOH (Ka = 1.8 x 10-5) %3D…

A: The concentration of hydrogen ion for acetic acid can be calculated as follows-

Q: Find the pH and percent ionization of a 0.100 M solution of a weak monoprotic acid having the given…

A: The answer for part a) is given below. kindly repost the other subparts as separate question Given:…

Q: Hydrofluoric acid has a Ka value of 7.2 x 10-4 . What is the pH of a 0.04 M solution of HF acid if…

A: pH :-  The negative logarithm to the base 10 of concentration of hydronium ions, [H3O+] expressed in…

Q: Calculate the concentration of the lactate ion in a solutionthat is 0.100 M in lactic acid…

A: Ka of the given solution can be calculated as follows: The reaction for the dissociation of lactic…

Q: Acetic acid has pKa of 4.76. At which pH does it act as the best buffer? A. > 7.0

A: Given: pKa of acetic acid = 4.76.

Q: . The acetate buffer contains 0.200 M acetic acid and 0.0500 M sodium acetate. Given that the Ka of…

A: PH of buffer solution is calculated by using Henderson Hasselbalch equation

Q: Using the Kb for NH3 (from Appendix G: Kb = 1.8 x 10-5), calculate the Ka for the NH4* ion. O 5.6 x…

A: Conjugate acid base pair :-  A pair of acid and base which differs by a proton is called conjugate…

Q: What is the pH number of a buffer solution prepared from 0.05 M ammonium hydroxide (NH4OH) and 0.09…

A: The Given solution is a Basic buffer solution.

Q: we found that the percent ionization of niacin 1Ka = 1.5 * 10-52 in a 0.020 M solution is 2.7%.…

A: Given information, The percent ionization of niacin Ka = 1.5 * 10-52 in a 0.020 M solution is 2.7%…

Q: Given Ka of HClO = 2.9×10-8 Kb of ClO- = 3.4×10-7 Determine the value of K for HClO(aq) + H2O(ℓ) ⇌…

A: Given, HClO(aq) + H2O(ℓ) ⇌ H3O+(aq) + ClO-(aq) Ka of HClO = 2.9×10-8Kb of ClO- = 3.4×10-7 Determine…

Q: If a weak acid has a Ka of 2.04 x 10-7 what is the value of pKb?

A: Given  Ka value of weak acid = 2.04 × 10-7 PKb = ?

Q: Suppose sodium hydroxide is added to a 0.Q120 M solution of zinc nitrate such that the pH of the…

A: The given data contains, Concentration = 0.0120 M. pH = 13.1

Q: Q3/ Calculate the pH of a solution containing (0.1 M) of [Fe+] [Mg+J. knowing that Ksp is for…

A: There are two sparingly soluble hydroxide.   Mg(OH)2 and Fe(OH)3.   When both are dissolved in the…

Q: Hypochlorous acid (HCIO) is a weak acid with pK, 9.21. For a 0.10 M aqueous solution of nitrous…

A: Given :  Concentration of HClO = 0.10 M  pKa of HClO = 9.21

Q: 4-)

A: The equilibrium constant can be written as the ratio of concentration of products to the…

Q: 8) A 0.10 M aqueous solution of a weak acid HA has a pH of 5.00. What is the value of Ka for НА? A)…

A:

Q: What is the pH of a 0.0770 M solution of hydrocyanic acid, HCN (Ka = 4.9 x 10-10)? 1 3 4 C 7 8 9 +/-…

A: PH = -log[H+] [H+] = 0.0770M

Q: What is the pH and percent ionization for a hydrocyanic acid (HCN) solution of concentration 2.0 X…

A:

Q: Calculate the pH of a 0.300 M solution of lactic acid, for which the Ka value is 1.40 x 104. A. 8.67…

A: Lactic acid is a weak acid. Given data is: concentarion of solution = 3.00 M Ka=1.40×10-4 Now, next…

Q: The pH of a solution containing 0,1 M of a weak acid HA is 6. Calculate Ka for this acid. O 1.0 x…

A: Let HA is a weak acid whose concentration is 0.1 M and pH is 6 and the dissociation constant is Ka.…

Q: Decide whether the solution of the salt, ammonium nitrate (NH,NO3), is acidic, neutral, or basic.…

A: The salt given is NH4NO3.

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.