3. Calculate the pH of a mixture of 0.25 M acetic acid and 0.1 M sodium acetate. pKa of acetic acid is 4.76.

Q: 1. Calculate the pH of an acetate buffer prepared by dissolving sodium acetate (5.21 g) and acetic…

A:

Q: What will be the pH

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Q: When 40 mL of benzoic acid (C.HSCOOH) and 35 mL of potassium hydroxide were titrated, the pH at the…

A: At equivalence point salt potassium benzoate is formed in which C6H5COO- undergoes hydrolysis.…

Q: In the titration of 71.0 mL of 0.400 M HCOOH with 0.150 M LiOH, how many mL of LiOH are required to…

A: The volume of 0.400 M HCOOH used for titration is 71.0 mL. The molarity of LiOH is 0.150 M.

Q: 1.What mass of sodium formate must be added to 500.0 mL of 1.00 M formic acid to produce a buffer…

A: Given: The pH of formic acid is 3.50 The molarity of formic acid is 1 M. The volume is 500 mL. We…

Q: what volume of 0.10 M sodium acetate must be added to 20.0 ml of 0.20 M acetic acid to produce a…

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

Q: 3. Calculate the pH of a mixture of 0.25 M acetic acid and 0.1 M sodium acetate. The pk, of acetic…

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

Q: How to make 100 ml of buffer solution (ammonia - ammonium chloride) with pH = 10?

A: There may be many possibility to make buffer of pH =10 , Here only one possibility is discussed.

Q: How would you prepare a buffer solution ?give the constituent ratio of ph 8 buffering ?

A: Buffer solutions The solution that resists any change in pH is known as buffer solution. There are…

Q: What is the pH of a solution that results from mixing together equal volumes of a 0.130 M  solution…

A: Given, 0.130 M solution of acetic acid 0.065 M solution of sodium hydroxide pKa of acetic acid =…

Q: In a titration of 76.0 mL of a 0.500 M solution of a diprotic acid H,C,H,O, (malonic acid) with…

A: [H2C3H2O4] = 0.500M  Volume = 76.0mL = 76.0mL×1L/1000ml = 0.076L  [NaOH] = 0.255M  Molarity = moles…

Q: 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3 Determine the pH of solution after the…

A: Given, Volume of NH3 = 100.0 mL = 0.100 L   (1mL = 0.001 L) Molarity of NH3 = 0.10 M = 0.10 mol/L…

Q: What is the pKa of a monoprotic, weak acid HA given that a 30.0 mL sample required 15.0 mL 1.50 M…

A:

Q: How did you determine the values of pka1 and pka2 from the titration curve?

A: For the titration of a polyprotic acid with a base, we get more than one equivalence points. We can…

Q: Calculate the pH of a solution prepared by mixing 0.080 0 mol of chloroacetic acid plus 0.040 0 mol…

A: The molarity of chloroaccetic acid and sodium chloroacetate solutions are first determined as shown…

Q: The pH at the equivalence point was 10.99. Find pKa for HA.

A: In chemistry various types of titrations take place. Some time there is titration of strong acid and…

Q: 2. a) Calculate the pH of 0.12 mol/L ethanoic acid (K₂ = 1.7 x 105 mol/L). b) Calculate the mass of…

A: Since the given question is a multipart question, hence I solved first three parts according to…

Q: 4. Consider the titration of 30.0 mL of 0.400 M ethylamine with 0.300 M HBr. Calculate the pH of the…

A: Ethyl amine is a weak base it reacts with HCl to make a buffer solution.

Q: 1. a. What is the pH of a solution prepared by adding 25.0 mL of 0.10 M acetic acid (Ka ) and 20-x:…

A: 25.0 mL of 0.1 M acetic acid and 20 ml of 0.1 M sodium acetate are mixed. Acetic acid is a weak acid…

Q: How many moles of sodium hydroxide would have to be added to 125 mL of a 0.339 M hypochlorous acid…

A:

Q: What is the pH of a solution prepared by mixing 150 mL of 0.10 M HCl with 300 mL of 0.20 M sodium…

A: Given, 150mL of 0.1M HCl 300mL of 0.1 NaOAc

Q: What volume of 0.028 M NaOH must be added to 0.75 L of0.0900 M HCl to achieve a pH of 9.00?

A: Given ,  Molarity of NaOH ( Mb ) = 0.028 M  Volume of NaOH ( Vb ) = ? Volume of HCl ( Va ) = 0.75 L…

Q: In the titration of 90.0 mL of 0.400 M HCOOH with 0.150 M LİOH, how many mL of LIOH are required to…

A:

Q: Calculate the pH of a mixture that contains 0.22 M of HCNO and 0.10 M of HC6H5O. The Ka of HCNO is…

A: Given : Concentration of HCNO = 0.22 M And concentration of HC6H5O = 0.10 M Ka of HCNO = 3.5 X 10-4…

Q: 3. Prepare 100 mL of 0.200 bicarbonate buffer, pH 10 by calculating the mass of sodium bicarbonate…

A: Answer is given as follows using the equation given above

Q: Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter…

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Q: What is the pH of a solution made by adding 23.5 g of KC2H302 to 400 mL of 0.80 M HC2H302? (Ka for…

A:

Q: What is the approximate pH of a solution prepared by mixing equal volumes of 0.05 M methylamine and…

A: Given -  Molarity of methyl amine = 0.05M Molarity of hydrochloric acid  = 0.2M n-  Volume of Methyl…

Q: what is the pH of a solution prepared by mixing 50.0 mL of 0.125 M amonia and 25.0 mL of 0.100 M…

A:

Q: What weight of sodium formate must be added to 400.0 mL of 1.00 formic acid to produce a buffer…

A: Given volume of HCOOH = 400.0 mL  Concentration of formic acid = [HCOOH] = 1.00 M  Concentration of…

Q: he pKa of the indicator is approximately 6, to which of the following equivalence point will it be…

A:

Q: What is the pH after addition of 50.0 mL KOH? pH = What is the pH after addition of 60.0 mL KOH? pH…

A: Find : A) after addition of 50.0 mL of KOH. B) after addition of 60.0 mL of KOH.   Formula : 1) Kb…

Q: Buffer A: Calculate the mass of sodium acetate that must be added to make 100.0 mL of an acetic…

A:

Q: What is the pH of the solution that is prepared when 121 g piperidinium chloride salt is dissolved…

A:

Q: What is the pH at 25°C of a solution that results from mixing equal volumes of a 0.0500 M solution…

A: The pH of a solution is related to the acid dissociation constant by the Henderson-Hasselbalch…

Q: In a titration of 35.0 mL of a 0.500 M solution of the diprotic acid H₂C₃H₂O₄ (malonic acid) with…

A:

Q: How many moles of sodium acetate must be added to 2.5 L of 0.25 M acetic acid to give a solution…

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

Q: Determine the pH at 25°C of a solution prepared by dissolving 0.0250 mole of sodium acetate in 1.00…

A: Molarity (M) is of a solution expressed as the number of moles of solute per litter of solution.The…

Q: Calculate the mass of sodium acetate that must be added to 500.0 mL of 0.760 Macetic acid to form a…

A:

Q: 2. A 0.100 mole quantity of a monoprotic acid HA is added to 1.00 L of pure water. When equilibrium…

A:

Q: What is the pH of the solution of 35 mL 0.20 M formic acid and 55mL 0.10 M sodium formate in 110 mL…

A: Here the pka of formic acid given is 3.75  [Salt] - concentration of salt here salt is sodium…

Q: What volume (in mL) of a 1.0 M solution of imidazolium chloride must be added to a 500 mL solution…

A: Buffer solutions are the solutions which counter the pH change on addition of small amount of acid…

Q: Calculate the pH of the following mixture 500 ml 0.35 M HF + 500 ml 0.25 M KOH

A: The reactants are, HF and KOH. HF is a strong acid and KOH is a strong base. Strong acids and strong…

Q: What is the pH at 25°C of a solution that results from mixing equal volumes of a 0.0500 M solution…

A: The Henderson–Hasselbalch equation shows the pH of a solution which have a mixture of the two…

Q: For the titration of 10 mL of 0.15 M acetic acid with 0.1 M sodium hydroxide, what is the pH when…

A:

Q: Calculate the pH if 0.30M Acetic Acid, with Ka = 1.8 x 10-5 is added to 0.20M Sodium Acetate.

A:

Q: In the titration of 100.0 mL of 0.050 M HCl solution, what will be the pH after adding 30.0 of a…

A: Molarity = number of moles/volume (L)  So, moles = molarity × volume (L)  pH = -log[H+]

Q: 100.0mL sample of 0.10M NH3 is titrated with 0.10M NHO3 . Determine the pH of the solution before…

A: NH3 is a weak base.  Hence, pOH = 1/2pKb-1/2logC ...(1)  Here, pKb = -logKb = -log(1.8*10^-5) = 4.74…

Q: When 16.24 mL of 0.064 3 M KOH were added to 25.00 mL of 0.093 8 M weak acid, HA, the observed pH…

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Q: Calculate the ratio of conjugate base to weak acid, [A−]/[HA], needed to make a buffer at pH = 5.00…

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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.