A student needs to prepare a buffer solution with a pH of 4.21. Assuming a pK, of 4.15, how many mL of 0.1 M B¯ would need to be added to 22.0 mL of 0.1 M HB prepare this buffer? Please include a proper (abbreviated) unit. HINT : Use pH = pKa + log ([B minus]/[HB]) or, if %3D concentrations are the same, pH = pka + log (Volume of B minus/ Volume of HB) %D

Q: A student needs to prepare a buffer solution with a pH of 4.65. Assuming a pKa of 4.57, how many mL…

A: Given: pH of buffer = 4.65  pKa of acid = 4.57  Concentration of HB = 0.1 M Volume of HB solution =…

Q: A 117.0 mL sample of 0.100 A methylamine (CH₂NH₂; K-3.7 x 10-) is strated with 0.205 M HNOS.…

A: The objective of the question is to calculate the

Q: How many grams of dry NH4Cl need to be added to 2.0 L of a 0.300 mol L-1 solution of ammonia, NH3,…

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Q: a Calculate the pH at the following points in a titration of 40. mL (0.040 L) of 0.121 M barbituric…

A: Answer:When conjugate base of weak acid is added in water then it gets hydrolysed to produce OH-…

Q: Suppose you have 150 mL of a buffer containing 0.100 M acetic acid and 0.0500 M sodium acetate.…

A: Given,  Volume of the buffer = 150 mL  Molarity of CH3COOH = 0.100 M Molarity of CH3COONa = 0.0500 M…

Q: EXTRA. What mass (g) of potassium fluoride (MW = 58.10 g/mol) must be added to 450. mL of a 0.100 M…

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Q: A buffer is prepared such that [CH3COOH]0 = [CH3COO−]0 = 0.050 M. Calculate the volume of 0.10 M…

A: Buffer capacity is used to determine the buffer solutions resistance to changes in pH when a strong…

Q: What is the hydronium ion concentration in a buffer solution prepared by mixing 50.00 mL of 0.10 M…

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Q: A 1.0-LL buffer solution initially contains 0.30 molmol of NH3NH3 (Kb=1.76×10−5)(Kb=1.76×10−5) and…

A:

Q: ou are to prepare exactly 100 mL of 0.200 M acetate buffer, pH 5.00, starting with pure liquid…

A: The solution is provided in the next step:

Q: A student needs to prepare a buffer solution with a pH of 5.20. Assuming a pKą of 4.52, how many mL…

A: I have attached the detailed solution to the question below.

Q: A 100. mL buffer solution is 0.200 M in HAc and 0.150 M in NaAc. Calculate the pH of the solution…

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Q: 6. a) 25.0 mL of 0.50 mol/L hydroiodic acid (HI) is titrated with 0.50 mol/L pyridine,C,H,N.…

A: Introduction

Q: A solution is prepared that is initially 0.40M in propanoic acid (HC₂H₂CO₂) and 0.14M in sodium…

A: Note: we are authorized to answer one question at a time, since you have not mentioned which…

Q: A student needs to prepare a buffer solution with a pH of 5.52. Assuming a pK₂ of 4.07, how many mL…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: Be sure to answer all parts. What is the [H3O+] and the pH of a benzoic acid-benzoate buffer that…

A: Thank you.

Q: How many grams sodium formate (HCOONa), 68.0069 g/mol) do you need to add to 250 mL of0.40 M formic…

A: required mass of sodium formate = 3.808 gExplanation:Given Ka = 1.77 × 10 -4Molarity of formic acid…

Q: To prepare 1-L buffer solution with pH = 5.05, how many moles of C6H5COONa (sodium benzoate) should…

A: Given: pH of solution = 5.05  Moles of C6H5COOH = 0.86 mol. And Ka of C6H5COOH = 6.3 × 10-5

Q: What is the pH of a buffer prepared by combining 0.76 moles of a weak base, B, with 0.47 moles of…

A: Given data set: Moles of weak base= 0.76 mol Moles of acidic salt = 0.47 mol Volume of solution= 684…

Q: A 100. mL buffer solution is 0.200 M in HAc and 0.150 M in NaAc.  Calculate the pH of the solution…

A:

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A: In this titration when 75.0 mL of 1.35 M base, B, is titrated with 1.25 M hydrochloric acid, HCl the…

Q: Calculating the pH at equivalence of a titration 0/5 Izabella A chemist titrates 80.0 mL of a…

A: pH = 5.90Explanation:Given: V(CH3​)2​NH​=80.0mL;[(CH3​)2​NH]=0.7536M;[HBr]=0.0940M;pKb​=3.27at the…

Q: A 360.0 mL buffer solution is 0.160 mol L¹ in HF and 0.160 mol L¹ in NaF. K. (HF) = 6.3 x 10-4 Part…

A: Henderson-Hasselbalch equation is used for the pH of buffer solution. pH=pKa +log[F-][HF]

Q: ming equal concentratic JO suope N2OCI / HOCI (K a= 3.2 x 10-8) NH 3/ NH 4CI (K a=5.6 x 10-10) NANO…

A: Buffer is an aqueous solution of a weak acid and its conjugate base or weak base and its conjugate…

Q: 1. 0.02 mole of HCl is added to one liter of buffer containing 0.05 mole of NH,OH and 0.03 mole of…

A: Moles of NH4 OH = 0.05mol Moles of NH4 Cl =0.03 mol Moles of HCl is 0.02 mol Now,  NH4 OH + H+…

Q: 141480 4. A student needs to prepare a buffer solution with a pH of 5.59. Assuming a pka of 4.54,…

A: Given,pH of the buffer solution = 5.59The pKa of buffer = 4.54Concentration of NaOH solution = 0.1…

Q: If 1. ml of 0.50 M formic acid (HCOOH) is titrated with the strong base of 0.50 M. KOH (Ka for…

A: The pH for the equivalence point : Balance chemical equation :…

Q: Calculate the pH of a buffer solution after the addition of 20.20 mL of 0.135 M NaOH to 50.0 mL of…

A:

Q: You are required to prepare a buffer (pH = 5.30) using propionic acid and sodium propionate. The…

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

Q: c) A student titrated 50.0 mL of a 0.10 M solution of a certain weak acid with NaOH. The results are…

A: Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid being titrated…

Q: You are to prepare exactly 100 mL of 0.200 M acetate buffer, pH 5.00, starting with pure liquid…

A: Formula used  Handerson- Hasselbalch equation  pH = pKa + log[CH3COONa/CH3COOH]  pH= 5.00 , pKa =…

Q: A student needs to prepare a buffer solution with a pH of 4.67. Assuming a pkg of 4.69, how many ml…

A: According to Henderson Hasselbalch equation, the pH of a buffer is given by, pH = pKa + log Volume…

Q: What is the H30* | and the pH of a benzoic acid-benzoate buffer that consists of 0.15 M C6H5COOH and…

A: Given, [C6H5COOH] = 0.15M [C6H5COONa] = 0.38M

Q: You are asked to prepare a buffer with a pH = 3.00. Starting with 1.25 L of 0.80 M HF, how many…

A:

Q: A student needs to prepare a buffer solution with a pH of 5.10. Assuming a pka of 4.37, how many mL…

A: Since concentration of HB and B- are the same (both at 0.1 M), we'll use the second expression for…

Q: A buffer contains 0.175 moles C2H5NH3NO3 and 0.225 moles C2H5NH2 in 800.0 mL water. Kb (C2H5NH2) =…

A: Calculation of pKb: pKb=-log Kb=-log 4.3×10-4=3.37 Calculation of initial pOH:…

Q: genow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator%=Dassignment-take, [References) How…

A: pH is calculated if buffer solution using Henderson equation.

Q: A student needs to prepare a buffer solution with a pH of 4.54. Assuming a pK, of 4.58, how many ml…

A:

Q: part a: A 0.500-L buffer solution was made with 0.25 M NH3 (Kb = 1.8 × 10-5) and 0.40 M NH4Cl. What…

A: Buffer solution is a type of solution that resists the change in its pH on adding small quantity of…

Q: A 1.00 L buffer solution is 0.200 mol L-1 in C6H5COOH and 0.250 mol L-1 in C6H5COOLİ. The Ka for…

A: Given: Volume of buffer solution = 1.00L Concentration of benzoic acid C6H5COOH = 0.200 mol L-1…

Q: How many mL of 1.0 M NaOH must be added to 100. mL of 0.050 M HC2H3O2 to make a buffer with a pH =…

A: We have given that pH = 5.0 Ka = 1.8×10-5 Pka = -log(1.8×10-5) = 4.74 Concentration of Acetic Acid =…

Q: Consider the titration of 40 mL of 0.2 M NH3 with 0.5 M HCI. Calculate the pH after addition of the…

A: In this question it is ask that what is the pH of resultant solution when addition of HCl in NH3 as…

Q: A student needs to prepare a buffer solution with a pH of 5.86. Assuming a pką of 4.30, how many mL…

A: Given: pH = 5.86 pKa = 4.30 Concentration of NaOH = 0.1 M Concentration of HB = 0.1 M Volume of HB =…

Q: You have 10 mL of a buffer that is 0.1 M acetic acid and 0.1 M sodium acetate. How many mLs of 0.025…

A: The number of moles of acetic acid and sodium acetate in the 10.0 mL of buffer is;…