The maximum buffering capacity is nearest to the pKa of the buffer. Explain why?

Q: on 4. A weak acid (HA) has a pKa of 5. Suppose you have 120 mL of a HA and its conjugate base A- at…

A: Given,The pKa of the weak acid = 5The pH of the buffer= 5.6The volume of solution= 120 mLThe volume…

Q: Explain why you can prepare a buffer from a mixture of NH4Cl and NaOH but not from NH3 and NaOH.

A: Buffer is a solution which is formed by weak acid and its conjugate base or weak base with conjugate…

Q: A student wishes to make a buffer that has a pH of 4.65.  The student has HNO2 and NaNO2.  Nitrous…

A: A buffer mixture is formed by the mixing of weak acid with its conjugate base or mixture of weak…

Q: A student needs to prepare a buffer solution with a pH of 5.83. Assuming a pKą of 4.76, how many mL…

A: Molarity - ratio of number of moles of solute to the volume of solution in litres. Formula is,

Q: What will be the pH of a buffer solution containing an acid with a pKa of 2.2 with an acid…

A:

Q: The pH of this solution is equ HCN. The pK, value of HCN will d is added. The cyanide ion…

A: As concentration of HCN is double the concentration of NaCN. Now, if we add strong base in the…

Q: 9) HB has a Ka of 5.2 x 10-5 and HC has a Ka of 4.6 x 10-4 . Which solution will have a lower pH,…

A: Given : Ka of HB = 5.2 X 10-5  Ka of HC = 4.6 X 10-4  And concentration of HB = concentration of HC…

Q: Amino acids with the general formula below can behave as buffers(R is some number of CH2 groups)…

A: (1)A buffer system is a solution that resists a change in pH when acids or bases are added to it. In…

Q: Identify the principal conjugate acid/base pair and calculate the ratio between them in a solution…

A: Sulfurous acid (H2SO3) is a diprotic acid.The dissociation reaction for H2SO4 is as follows: H2SO3…

Q: Calculate the pH of a buffer solution containing [NH3] = 0.08 M and [NH4Cl] = 0.15 M?

A: Buffer solution:The buffer solution is an aqueous solution consisting of a mixture of a weak acid…

Q: buffer system has 3[HA]=[A-]. Given that the pKa is 7.2, what is the pH of the buffer solution at…

A: Given,  3[HA]=[A-]  [A-]/[HA] = 3  pKa = 7.2  It is Acidic buffer,   pH = pKa + log([A-]/[HA])

Q: A general chemistry student measured the pH of a 0.12 M aqueous solution of an unknown weak acid HA…

A: The question is based on the concept of equilibrium. we have to calculate PKa of a weak acid whose…

Q: Using the Henderson-Hasselbach equation predict under which of the following conditions will the pH…

A: A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate…

Q: A 0.13 M solution of a weak acid HA dissociates such that 95.2% of the weak acid remains intact…

A: A weak acid ionizes partially to produce the H+ ions in an aqueous solution.

Q: [CN A buffer solution made from HCN and KCN has a pH of 9.59 . If pK, for HCN is 9.40 , what is the…

A: Acidic Buffer solution :-  A mixture of weak acid and its salt with strong base is called as acidic…

Q: Which of the following 1:1 mixtures would be best suited to form a buffer closest to a pH of 3.70?

A: In order to prepare a buffer closest to a pH value of 3.70, the buffering range of the resulting…

Q: In the buffer system pictured below, which compound acts to maintain pH in the presence of added HCl…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…

Q: A buffer solution containing 0.19 M methylammonium and 0.22 M of the conjugate base, methylamine,…

A: Answer: option c. 10.70 is the pH of the buffer solution

Q: Pyrazolium Chloride is a weak acid (C3H4N2HCl; Ka=1.4x10-3). How many grams of Pyrazole (conjugate…

A: Given: Ka of C3H4N2HCl = 1.4 X 10-3  Concentration of C3H4N2HCl = 0.3 M And pH of buffer solution =…

Q: For a weak acid, when does the pH equal the pKa?

A: Answer: For this we need to know Henderson-Hasselbalch equation . Explanation:…

Q: What is the of the ratio of conjugate base to weak acid that is necessary to make a buffer solution…

A: We have to find the ratio of conjugate base to weak acid( conjugate base /acid ). According to…

Q: Which of the following is true of a buffer solution that contains equivalent amounts of acid and…

A: buffer solution that contains equivalent amounts of acid and conjugate base means [Conjugate base ]…

Q: Calculate chloride buffered solutions with the following pH value (This problem requires values in…

A:

Q: which of the following should have the weakest IMF CH3F, n2, co, hcl

A: Ion-ion > ion-dipole > hydrogen bonding > dipole-dipole > Van der Waals forces

Q: ou need to produce a buffer solution that has a pH of 5.03. You already have a solution that…

A: Explanation:      Your buffer solution contains acetic acid,   CH 3 COOH  , a weak acid, and the…

Q: 2. Given the H3PO4 - NaH₂PO4 buffer system, which of the following is false when KOH is added into…

A: 2.  Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: The fumarate ion is a dibasic base with pKb values of 9.52 and 10.98. What is the concentration of…

A: Given the pH of the solution = 5.21 Total concentration of both the buffer parts = 0.100 M

Q: I am extremely confused as to the logic behind these conceptual/theory problems can you please add a…

A: Any solution having weak acid+conjugate salt reflects that solution is "acidic buffer". Acidic…

Q: Which of the following can behave as Bronsted-Lowry bases in aqueous solution? Ca(OH)2 NaOH NH4+ I…

A: According to Bronsted and Lowry concept an Acid is a substance that has the tendency to donate a…

Q: Why is the pH at the equivalence point slightly different from that of the end point? Explain.

A: To explain: pH at the equivalence point is slightly different from that of the endpoint.

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.