How many mL of 4.50 M sodium hydroxide must be added to 250 mL of a 0.200 M acetic acid solution to make a buffer with pH = 5.00? Look up Ka or Kp in a suitable source - on an exam you would be given the Ka of acetic acid, CH3COOH. Select one: a. 32.01 mL b. 20.22 mL с. 7.17 mL d. 15.02 mL е. 3.94 mL O O OO

Q: 26. What is the pH of a buffer that is 0.12 M in lactic acid, CH3CH(OH)COOH, and 0.10 M in sodium…

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Q: You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid…

A: Henderson Hasselbalch equation, shown below, where pKa is the equilibrium constant for the acid,…

Q: The bicarbonate/ carbonic acid buffer is of extreme importance to our bodies. The pH of importance…

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Q: How many grams of solid potassium acetate should be added to 1.50 L of a 0.283 M acetic acid…

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Q: A chemistry graduate student is given 450. mL of a 0.20M ammonia (NH,) solution. Ammonia is a weak…

A: GivenpH = 9.14pOH + pH = 14pOH + 9.14 = 14pOH = 4.86

Q: Sample student prepares three buffer solutions. Each solution is 1.0 M in one of the acids in the…

A: When NaOH is added to the the buffer solutions , it will react with acidic part of buffer.  So the…

Q: 5. You need to prepare a buffer at pH = 7. A buffer based on which molecule below is most…

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

Q: 1. Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 46.0 mL of 0.300 M HBrO (Ka = 2.5 ×…

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Q: Suppose you need to prepare a buffer with a pH of 5.00. Am 90S a. Which of the buffer systems in the…

A: We have to calculate the value of pKa to find the appropriate buffer systems. The appropriate buffer…

Q: For each solution, calculate the initial and final pH after adding 0.010 mol of NaOH. a. 250.0 ml of…

A: Answer :            Part A : pHi = 7.00   and pHf = 12.60           Part B :  pHi = 3.89   and pHf =…

Q: 1.0 L of acetate buffer is made by combining 0.50 M CH3COOH with 0.50 M CH3COONa. The Ka of CH3COOH…

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Q: A chemist needs to make a buffer at a pH of 4.5. 600 mL of 60mM acid is prepared. pka of acid=4.81…

A: Answer: Buffer solution over here is the mixture of weak acid and its salt which will resist the…

Q: For each solution, calculate the initial and final pH after adding 0.010 mol of NaOH.a. 250.0 mL of…

A: A.) Pure water : pH = 7.00 (initial) moles NaOH = 0.010 So, [OH-]= 0.010 mol/ 0.210 L=0.048 M pOH =…

Q: What is the pH of a buffer made by combining 45.0 mL of 0.30 M nitrous acid and 20.0 mL of 0.35 M…

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Q: In the following example, by changing the titration conditions on a weak acid as compared to a…

A: A question based on acid-base titration, which is to be accomplished.

Q: 2. Phenol (C6H5OH) has a Ka of 1.6*10-10. Starting with a 100.0 mL solution that is 0.300 M phenol,…

A: Given that : Volume of C6H5OH=100mLIts concentration=0.300 MpH = 10Ka of C6H5OH=1.6×10-10So,…

Q: A 50.0 ml sample of 0.200 M HNO2 (weak acid) is titrated with 0.400 M KOH. Calculate the pH after…

A: Given Data: A 50 ml. sample of HNO2 having concentration =0.200 M This HNO2 titrated with the KOH…

Q: What mass of NH,CI must be added to 500 mL of a 0.150M NH3 solution to make a buffer with pH = 9.50?…

A: When NH4Cl (salt) and NH3 (weak base) mixed, then they form a buffer solution. The pH of the buffer…

Q: How many mL of 5.00 M sodium acetate must be added to 1.00 L of a 0.200 M acetic acid solution to…

A: We know  PH = Pka + log [salt]/[acid]

Q: A 30.87 mL solution of a weak acid 0.17 M is titrated with 0.221 M NaOH. The Ka of the acid is 1.3 x…

A: Given, Volume of weak acid = 30.87 mL Concentration of weak acid = 0.17 M Concentration of NaOH =…

Q: You are tasked to preparee three buffers with pH values of: 9.10, 10.45, and 4.65. You have the…

A: Buffer solution is the solution which resist the change in pH of the solution on addition of small…

Q: Calculate the pH of a buffer that is 0.225 M HC 2H 30 2 and 0.162 M KC 2H 30 2. The K a for HC 2H 30…

A: Henderson-Hasselbalch equation Henderson-Hasselbalch equation explains the relationship between pH…

Q: A buffer is prepared by combining 25 mL of 0.50 M NH3(aq) with 25 mL of 0.20 M HCl. What is the pH…

A: Given : Concentration of NH3 = 0.50 M Volume of NH3 solution = 25 mL = 0.025 L…

Q: Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 x 10-5) by 0.100 M KOH .…

A: The question is based on the concept of titrations.   we are titrating  a weak acetic acid with a…

Q: What is the pH of a buffer made by combining 45.0 mL of 0.34 M nitrous acid and 60.0 mL of 0.48 M…

A: Answer

Q: 1.0 L of a buffer solut What is the pH after 0 O a. 9.928 O b.9.602 O c. 9.319 O d. 9.193 Oe. 9.398

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Q: You have 100 mL of an acetic acid/acetate buffer. The solution is comprised of 0.33 M acetic acid…

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Q: You have 500.0 mL of a buffer solution containing 0.250 M acetic acid (CH₂COOH) and 0.240 M sodium…

A: Conc of CH3COOH=0.25MConc. Of CH3COONa= 0.24MKa = 1.80 x 10⁻⁵ for acetic acidFind out PH of buffer…

Q: Calculate the pH of a buffer that is 0.208 M lactic acid, HC3H5O3, and 0.208 M sodium lactate,…

A: Given that:                                                   Molarity of lactic acid = 0.208 M…

Q: Acetic acid has a Ka of 1.8 x 10¬º. Three acetic acid/acetate buffer solutions, A, B, and C, were…

A: pKa = -logKa pH = pKa + log(base/acid)

Q: A 40.0 mL solution of 0.100 mol/L acetic acid, CH,COOH (K, = 1.8 x 10-5), is titrated with 0.100…

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Q: A buffer solution contains 0.100 M fluoride ions and 0.126 M hydrogen fluoride. What is the…

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Q: You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (p?a=4.20)  and…

A: Let y mL benzoic acid and 100-y mL sodium benzoate are mixed. For acidic buffer solution,  pH = pKa…

Q: Calculate the pH at different stage of the titration when 40.0mL of 0.30N acetic acid (Ka =…

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Q: 8. You have 500.0 mL of a buffer solution containing 0.30M acetic acid and 0.20M sodium acetate.…

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.