For an acetic acid-sodium acetate buffer solution to have a pH of 4.97, what molar ratio of CH3COONa to CH3COOH is needed? (Ka for CH3COOH is 1.8x10-5)

Q: 1. Calculate [H+], [OH-], pH and pOH of: a. 0.1 M HNO3 b. 2.00 M (weak acid) HF (Ka=6.8 x 10^-4)

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Q: what is the change in when 15,0ml of °* 100M NgOH is added to Eeoml of Genis eh Formic acid/ Sodium…

A: The change in pH is 0.044

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: The normal pH of blood is 7.40± 0.05 and is controlled inpart by the H₂CO₃/HCO₃⁻ buffer system.(a)…

A: The value of Ka of H2CO3 is not given. Thus, is taken from internet. The value of Ka of H2CO3 is…

Q: How would you prepare a benzoic acid/benzoate buffer with pH = 4.25, starting with 5.0 L of 0.050 M…

A: Given Values: Molarity of sodium benzoate solution = 0.05 M The volume of sodium benzoate solution =…

Q: the following reaction of thiol analysis in drug R-SH + AGNO3 R-SAg + HNO3 It can be analyzed by…

A: Gravimetric analysis is method of analytical chemistry which is used to determine the quantity of…

Q: Calculate the pH of 0.391 L of a 0.25 M acetic acid - 0.27 M sodium acetate buffer before (pH1) and…

A: Given data,Molarity of acetic acid=0.25 MMolarity of sodium acetate=0.27 MVolume of buffer=0.391…

Q: Why is it needed to cover the buffer solutions until their pH is determined? For a buffer prepared…

A: Generally we cover a buffer solution untill the pH is determined because-

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: What is the pH of a buffer solution made with 0.789M benzoic acid with Ka = 6.5 x 10^-5 and 0.659M…

A: Ka = 6.5 × 10-5  So, pKa =  - log (6.5 x 10-5)          = 4.187 By using Henderson Hasselbalch eqn ,…

Q: It is desired to buffer a solution at pH = 4.30. What molar ratio of CH3COOH to NaCH3CO0 should be…

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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: Vitamic C, aka ascorbic acid (H₂C₆H₆O₆) is a weak diprotic acid. Which of the following aqueous…

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Q: What is the pH of a buffer that is 0.12 M in lactic acid [CH3CH(OH)COOH, or HC3H5O3] and 0.10 M in…

A: Buffer solution consists of mixture of weak acid and its conjugate base.

Q: A biochemist needs to preserve anenzy.me 250 mL 0.50 M acetate buffer at in pH 5.5. (Ka of acetic…

A: pKa of acetic acid pKa = -log Ka         = - log (1.8 * 10-5)         = 5 - log 1.8         = 5 -…

Q: You wish to prepare an HC2 H3 O2 buffer with a pH of 4.14. If the pKa of HC2H3 O2 is 4.74, what…

A: Given :-   pH of buffer solution = 4.14  pKa value for HC2H3O2 = 4.74  To calculate :-  Ratio of…

Q: What is the buffer component ratio, (CH3COO-)/(CH3COOH) of an acetate buffer that has a pH of 4.75.…

A: pH  = 4.75 Ka = 1.8 x 10 —5

Q: A) A Buffer Solution of cH3 Cood and NaoH whose PH=5, and the Concentration of CH3 CoONa (o -IM).…

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Q: If 100 mls of 0.02 M HCl added to 400 mls of 0.5 M glycine buffer at pH10.4, what is the resultant…

A: A buffer solution is the solution composed of acid and conjugate base in such a way so that the pH…

Q: What amount of sodium formate must be added to a 1.00 L solution containing 1.28 moles of formic…

A: Given: Volume of solution = 1.00L moles of formic acid = 1.28 moles pH = 4.10 pKa= 3.74 To find: The…

Q: What is the pH of a buffer solution with 0.21 M Pyridine (C5 H5 N) and 0.35 M pyridine chloride ( C5…

A: • Given that the concentration of pyridine base is 0.21 M in buffer solution. • And the…

Q: How many grams of hyrogen phosphate and Sodil dinydrogen phosphate are heeded to make 100 mL of a…

A: Since you have asked multiple questions, we will answer only first question for you. In order to get…

Q: The Ka of CH3COOH is 1.8 x 10-5. Calculate the pH of a solution containing both 0.20 M CH3COOH and…

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Q: Consider a titration of 40.00 mL of 0.1250 M Na2CO3 with 0.4000 M HCl.  Carbonic acid (H2CO3) has a…

A: We know V1S1 = V2S2  Where, V = volume   S = Strength or concentration

Q: A 25.0 mL sample of a 0.100M solution of aqueous trimethylamine is titrated with a 0.125M solution…

A: Strong acid + weak base ---> salt + water pH = 1/2(pkw - pkb- log C) Molarity = no. of moles of…

Q: Consider the following reaction: Ksp of CaCO3 = 4.9 × 10-9 Ka of HCO3¯= 4.7 × 10-11 CaCO3 (s) +…

A: K for the reaction is; CaCO3s↔Ca2+aq+CO32-aq, Ksp=Ca2+CO32- ...... iCO32-aq+H+aq↔HCO3-aq,…

Q: What is the ratio of HEPES/HEPES-H+ in aHEPES buffer at pH 7.9?

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Q: 1. In Acidic Buffer solution (HNO;J/INO,] when the value of pH - pka +1, the ratio of (HNO,/[NO,] is…

A: You have posted multipart of question as per the guidelines i have solved first three kindly asked…

Q: A chemist titrates 80.0 mL of a 0.8628 M trimethylamine ((CH N) solution with 0.2165 M HBr solution…

A: This is titration of weak base and strong acid. pH at equivalence point will be less than 7

Q: How many moles of NaOH must be added to 1.0 L of 2.0 M HC2H302 (Acetic Acid, Ka = 1.8x10^-5) to…

A: Buffer is solution which have tendency to resist pH change when small amount of strong acid or…

Q: A buffer solution contains 0.10M benzoic acid (C6H5COOH, Ka = 6.3 x 105) and 0.10M assium benzoate…

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Q: What is the pka of the weak acid that gives the following pH curve when titrated with NaOH? 14.00…

A: The value of pH for titration of weak acid with strong base is calculated by Henderson-Hasselbalch…

Q: . The acetate buffer contains 0.200 M acetic acid and 0.0500 M sodium acetate. Given that the Ka of…

A: PH of buffer solution is calculated by using Henderson Hasselbalch equation

Q: A Fajans titration of a 0.7908-gg sample required 45.32 mL of 0.1046 M AGNO3. Express the results of…

A: Express the results of this analysis in terms of the percentage of BaCl2·H2O.

Q: You have 0.600 L of an 0.300 M acetate buffer solution (i.e. [HC2H3O2] + [C2H3O2] = 0.300 M) at pH…

A: We are provided with 0.600 L of 0.300 M acetate buffer solution having a pH of 5.30. We are required…

Q: What [NH4Cl] is needed to prepare 1.000 L buffer solution at pH 8.8 using a stock concentration of…

A: Given :  [NH3]  = 0.3500 M  pH = 8.80  Volume of buffer solution = 1.00 L  Kb of NH3 = 1.8 x 10-5

Q: How would you prepare a benzoic acid/benzoate buffer with a pH pf 4.25, starting with 5.0 L of 0.050…

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Q: If all the N in 10.0 mmols urea, CO(NH2)2, is converted to NH4HSO4, and if, with excess NaOH, the…

A: MilliMoles of urea = 10 mmol 1 mole of urea = 2 moles of nitrogen 10 mmol of urea =(2 ×10) mmoles of…

Q: the [CH4COO-]/[CH3COOH] ratio in an acetate buffer at pH 5.00

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Q: [A | [HA] 5. What ratio HA will create an acetic acid buffer of pH 5.0? Ka acetic acid is 1.75 x…

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Q: 65. Boric acid with sodium tetraborate and potassium chloride: Atkins and Pantin's Buffer Sorensen's…

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Q: If 100 mls of 0.02 M HCl added to 400 mls of 0.5 M glycine buffer at  pH10.4, what is the resultant…

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Q: 5. What would be the pH of a 100.0 mL solution containing 0.24 M formic acid [HCHO₂; Ka = 1.8x10-4)…

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Q: Given that the Ka for acetic acid is 1.8 x 10-5.  What is the pH of a buffer solution made from 0.20…

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Q: What is the pH of a buffer that is 0.12 M in lactic acid [CH3CH(OH)COOH, or HC3H5O3] and 0.10 M in…

A: The acid ionization constant for lactic acid is 1.4×10 -4.

Q: Calculate the ph of a buffer solution prepared by mixing 75ml of 1.0M lactic acid and 25ml of 1.0M…

A: Henderson's equation for calculating pH of a buffer consisting of a weak acid and slat of the same…

Q: What is the [CH3CO2-]/[CH3CO2H] ratio necessary to make a buffer solution with a pH of 4.34?…

A: The pKa value of acid can be calculated as follows-

Q: What is the pH of a buffer solution prepared by mixing 20.0 mL of 0.0600 mol L-' NaOH with 20.0 mL…

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Q: If the solubility of Li2CO3 is 1.32 g/100 mL, what is its Ksp at room temperature?

A: Solubility (S) :-  The amount of solute that can be dissolved in one litre of solvent is defined as…

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.