An aqueous solution of benzoic acid and sodium benzoate has a pH of 5.1. The dissociation constant of benzoic acid is 6.5 x 10^-5.

Q: Dilute phosphoric acid(K1 = 7.5 x 10-3) solution is titrated with standard NaOH solution to form…

A: Which indicators is used not used for this titration are given below.

Q: For CO2 in the atmosphere at 25 degrees C, kH = 3.4 x 10-2 mol L-1 atm-1 and the partial pressure of…

A: Given Data: Henry's constant, kH = 3.4 x 10-2 mol L-1 atm-1 Partial pressure of CO2 = 0.000405 atm =…

Q: What is the ratio of concentrations of acetate ion and undissociated acetic acid in a solution that…

A: Ethanoic acid is a weak acid and the dissociation of acetic acid is given by: CH3COOH   ⇌  CH3COO-…

Q: Calculating percent dissociation of a weak acid A student prepares a 0.55 M aqueous solution of…

A: Observing the table shows that trimethylacetic acid has only one pKa value hence one proton from it…

Q: Carbonic acid (H2CO3) and the anions which result from its dissociation provide the molecular basis…

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Q: 9- The acid dissociation constant K, of trimethylacetic acid (HC (CH,),CO, is 9.33 x 10. Calculate…

A: Since trimethyl lactic acid is a weak monoprotic acid. hence it will dissociate partially as per the…

Q: Which acid would you choose to combine with its sodium salt to make a solution buffered at pH 4.25?…

A: To choose the best acid, look for it's .The acid with closest to the given is the best choice.

Q: You are asked to go into the lab and prepare an acetic acid – sodium acetate buffer solution with a…

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Q: You are asked to prepare a buffer for an experiment. You have access to the following dolutions of…

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Q: An employer is interviewing 4 applicants for a job as a laboratory technician and asks each of them…

A: Buffer solution is defined as a solution that oppose changes in pH while adding little amount of…

Q: A monoprotic weak acid (HA) has a pKa value of 3.493. Calculate the fraction of HA in each of its…

A: Given: pKa of HA = 3.493 And pH = 4.829

Q: Write the chemical reactions whose equilibrium constants are K, and K, for imidazole (C, H, N,) and…

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Q: Define pKa for a weak acid. What is the relationship between the value of the pKa and the strength…

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Q: Write the Henderson-Hasselbalch equation for a propanoic acid solution (CH,CH, CO,H, pKa = 4.874).…

A: The given pKa value for a propanoic acid solution is 4.874. Henderson-Hasselblach equation is given,…

Q: What is the ratio of acetate ion to acetic acid (Ka = 1.76×10–5) in a solution containing these…

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Q: What is the pKa of the acid? Solve using the Henderson-Hasselbalch equation.  What is the…

A: 1- We will used the Henderson equation,  pH = pKa + log( [salt] / [acid] )  5.1 = pKa + log( 0.20M /…

Q: What is the pH of a solution

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Q: A 50.0 ml of acidic solute (K. = 1.20 x 10-2) is titrated with a 2.50 mL of x 10-5 M NaOH solution.…

A: Given: Ka of acid solute = 1.20 X 10-2  Volume of acid solution = 50.0 mL = 0.050 L…

Q: For each value of Ka, calculate the corresponding value of pKa. Which compound is the stronger acid?…

A: pKa of any acid can be calculated as: pKa=-logKa Ka is dissociation constant of an acid. Larger the…

Q: 1. Calculate the pH of a 1 L solution containing 6 mL of 1.5 M acetic acid and 5 ml of 0.4 M sodium…

A: According to Henderson- hasselbalch equatlon.pH=pKa+log[salt ][acid]..........1stGiven,pKa=4.766ml…

Q: Write down the reaction between [Cr(C2O4)2(H2O)2] and dilute potassium hydroxide.

A: Introduction: [Cr(C2O4)2(H2O)2] is a chromium (|||) complex in which C2O4 oxalate ion has a charge…

Q: What is the ratio of conjugate base to undissociated acid for a weak acid with a pk, of 4.4 at a pH…

A: Given :  pKa = 4.4  pH = 9  To determine :  Ratio of conjugate base to weak acid

Q: What is the ratio of acetate ion to acetic acid (Ka = 1.76×10–5) in a solution containing these…

A:

Q: What is the pH of a balsamic vinegar having an acetic acid (M.W. = 60.05g/mol; Ka = 1.8 x 10^-5)…

A: Given, M.W. of acetic acid HC2H3O2 = 60.05 g/mol Ka of acetic acid = 1.8 × 10-5 w/v (weight of…

Q: The pKa for the first protonation of nicotine (2) is 8.02. What is the pH and the fraction of…

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Q: Which acetic acid plus acetate solution has the greatest buffering capacity? 0.335M HC2H3O2 and…

A: The more the concentration of acid and its conjugate base, the greater is the buffering capacity.

Q: 0.100M solution of monoprotic weak acid has a pH of 3.00. What is the pKa of this acid?

A: Let , weak monoprotic acid = HA  pH = 3.00  [HA] = 0.100 M

Q: Estimate the pH and percentage of dissociation of 0.010 M CH3CH(OH)COOH(aq) (lactic acid). pKa of…

A: For a weak acid:                                     HA           =            A-        +       H+…

Q: The pH of a solution containing 0.010 M lactic acid and 0.087 M lactate is 4.80. Calculate the pKa…

A: Given:Concentration of lactic acid = 0.010 M Concentration of lactate = 0.087 M  pH of the solution…

Q: A buffer solution of 0.1 M concentration with a buffering zone of 3.74-5.74 pH value , specify what…

A: The considered buffer solution is 0.1M in concentration. The buffering zone is mentioned to range…

Q: Calculate the pH of a buffer prepared by dissolving 0.80 moles acetic acid (CH3COOH) and 0.40 moles…

A: pH of acidic Buffer solution is calculated Handerson   equation that is    pH = pKa +…

Q: The base protonation constant K, of allantoin (C,H,N;03NH,) is 9.12 × 10 °. Calculate the pH of a…

A: Given:

Q: solution that is 0.150 M chloroacetic acid and 0.250 M sodium chloroacetate, after the addition of…

A: Answer p oh = 10.2

Q: What volume of 1.50 M NaOH must be added to 200.0 mL of 1.00 M glycolic acid (HC2H3O3) to produce a…

A: We have to calculate the volume of base needed.

Q: Methyl Amine (CH3NH2) is a weak base with a Kb of 4.38 x 10-4. What would be the pH of a solution of…

A: The above salt is a mixture of weak base and strong acid. When it dissolves in water it forms an…

Q: Acetic acid (pKa = 4.75) is contained in vinegar.  1. Calculate the pH of an 0.1500 M aqueous…

A: As per our guidelines, we can only solve one question at a time. Please post other questions as next…

Q: to prepare a 10.0 mL 0.02 M acetate buffer with pH of 5.5. How will you prepare this? Note that the…

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Q: What is the reason for finding the 1/2 equivalence point? Select one: a. To determine the moles of…

A: The half-equivalence point is the point at which half of the acid has reacted with the base for…

Q: pH

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Q: Calculate the pH of a 2.2 M solution of pyridine salt (Ko (pyridine) = 1.7 x 10°) %3D

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Q: After a buffer solution of carbonic acid (with pKa of 3.75) was added with 1ml of sulfuric acid, the…

A: Buffer solution is that which resist the change in pH value pH of a weak acid and it's conjugate…

Q: Consider the HNO2-KNO2 buffer system, which species would react if a dilute aqueous KOH solution…

A: The buffer solution of HNO2-KNO2 formed by combination of weak acid nitrous acid HNO2 and it's salt…

Q: To find the pKb of the conjugate base of a weak acid, one must subtract the pKa of the weak acid…

A: Ka and Kb are the dissociation constant of weak acid and weak base respectively. pKa is the -log of…

Q: How many moles of sodium acetate must be added to 500 mL of 0.25 M acetic acid solution to produce a…

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Q: The amino acid tyrosine has pKa = 2.20 for deprotonation of its carboxylic acid group. What are the…

A: Henderson-Hasselbalch equation establishes a relationship between pH of the solution and the acid…

Q: Calculate the sodium acetate/acetic acid ratio to prepare a buffered solution with a pH of 5.06.…

A: The ratio can be found by using Henderson-Hasselbach equation: pH = pKa + log[salt][acid]…

Q: A compound have pKa 3 , what will be its dissociation constant at pH 10 and at pH 1 ?

A: The formula that can be used to calculate Ka (acid dissociation constant) from pKa and pH is…

Q: You decide to put your growing knowledge of chemistry to profit by making and selling boutique soaps…

A: Soaps are salts of fatty acids (weak acid) and strong base. The salt hydrolysis formula for the…

Q: The Kb of pyridine, C5H5N, is 1.7 x 10−9.  What is the %dissociation of pyridinium in a 0.124 M…

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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.