You want to prepare 100.0 mL of a buffer solution with a pH of 4.95 by mixing appropriate volumes of 0.10 M CH3CO2H and 0.10 M NaCH3CO2. How many milliliters (mL) of the acetic acid and sodium acetate solution are needed? (CH3CO2H has Ka = 1.8 x 10–5)          (A) 75.0 mL of 0.10 M CH3CO2H + 25.0 mL of 0.10 M NaCH3CO2;          (B) 62.0 mL of 0.10 M CH3CO2H + 38.0 mL of 0.10 M NaCH3CO2;          (C) 38.0 mL of 0.10 M CH3CO2H + 62.0 mL of 0.10 M NaCH3CO2;          (D) 25.0 mL of 0.10 M CH3CO2H + 75.0 mL of 0.10 M NaCH3CO2;

Q: 1. Why was it important to use "flat" soft drinks for your titrations? Would your calculations of…

A: Here we are titrating soft drink which contains acids with strong base, NaOH to find the citric acid…

Q: A buffer is made using 100.0 mL of 0.200 M CH3 CH2 COOH (propanoic acid) and 100.0 mL of 0.100 M…

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Q: A chemistry graduate student is given 300mL of a 1.10M acetic acid solution. Acetic acid is a weak…

A: From given data Concentration of acetic acid = 1.10 M  Ka=1.8×10-5 pH of buffer = 5.14 Volume of…

Q: An environmental chemist needs a carbonate buffer of pH 10.00 to study the effects of the acid rain…

A: Answer - Henderson - Hasselbach equation - According to Henderson-Hasselbach equation, when the…

Q: The Ka of formic acid HCOOH is 1.77 x 10-4. A 0.60 M formic acid solution of 40.0 mL is titrated…

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Q: given 250. ml. of a 0.80 M diethylamine (C2H5)2NH2Br solution. Diethylamine-3 is a weak base with K,…

A: Given, Volume of Base  = 250. ml = 0.250 L Concentration of Base = 0.80 M   Mole of Base =0.80 ×…

Q: A lactic acid/sodium lactate (HC3H5O3/NAC3H5O3) buffer is prepared to 0.104 mol L-1 HC3H5O3 and…

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Q: A 300 mL buffer is prepared in which [HCO3- ] = 0.2 M and [CO32- ] 0.075M a) What is the pH of this…

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Q: A 350.0-mL buffer solution is 0.150 M in HF and 0.150 M in NaF. What mass of NaOH can this buffer…

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Q: You add 100.0 mL of 0.50 M NaOH to 50.0 mL of 1.00 M NH4CI. What is the pH of the resulting…

A: Ammonia(NH3) is a weak base whose base dissociation constant is given as Kb=1.8×10-5 while ammonium…

Q: 1. Calculate the volume at which the pH= pKa if 30.00mL of weak acid with a concentration of…

A: Since you have posted a question with multiple questions, we will solve first question for you. To…

Q: What is the pH of a buffer prepared by combining 0.36 moles of a weak acid, HA, with 0.69 moles of…

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Q: .Suppose polyprotic acid H3X with Ka1=10-2, Ka2=10-5, Ka3 =10-10 . Answer the following questions…

A: From the question it is clear that the given acid is triprotic and its respective first, second and…

Q: A chemistry graduate student is given 300. mL of a 1.00M trimethylamine ((CH, N solution.…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: Suppose you wanted to make a buffer of exactly pHpH 7.00 using KH2PO4KH2PO4 and Na2HPO4Na2HPO4. If…

A: Henderson – Hasselbalch equation can be used here, i.e pH=pKₐ+log₁₀([A⁻]/[HA])

Q: 3.  What is the pH of a buffer made by mixing 1.00 L of 0.020 M benzoic acid, HC7H5O2, with 3.00 L…

A: Given, the molarity of benzoic acid = 0.020 MMolarity of sodium benzoate = 0.060 MThe total volume…

Q: In order to standardize a solution of NaOH, 1.05 mL of NaOH is titrated with 0.100 M oxalic acid…

A: Given,Volume of NaOH = 1.05 mL = 1.05 × 10-3 L    (1 mL = 10-3 L)Volume of H2C2O4 = 295 µL = 295 ×…

Q: A buffer solution is made that is 0.371 M in HCN and 0.371 M in NaCN . (1) If Ka for HCN is…

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

Q: Phosphorous acid, H, PO, (aq), is a diprotic oxyacid that is an mportant compound in industry and…

A: a.) Before any KOH is added , there is only acid , so we would draw an ICE table and use Ka value to…

Q: A 100.0-mL buffer solution is 0.100 M in NH3 and 0.125 M in NH4Br. What mass of HCl can this buffer…

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Q: A propanoic acid/potassium propanoate (C2H5COOH/KOOCC2H5) buffer is prepared to 1.03×10-2 mol L-1…

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Q: A chemistry graduate student Is glven 100. mL of a 0.70M trimethylamine ((CH,) N solution.…

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Q: A chemistry graduate student is given 250. mL of a 0.50M trimethylamine ((CH N solution.…

A: Given: Concentration of trimethylamine = 0.50M Volume of trimethylamine = 250 mL = 0.250 L Kb = 7.4…

Q: Q5) Choose two of the following branches:- 1-What is the pH of a 0.100 M solution of sodium acetate?…

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Q: 2. [A] = day of birth [B] = month of birth I was born December 8th, so for me [A] = 8 [B] = 12 Use…

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Q: The major component of vinegar is acetic acid, CH3COOH. Its Ka is 1.8 × 10-5 . One student used…

A: The question is based on the concept of titrations. We have to calculate molarity of the acid and Ph…

Q: A chemistry graduate student is given 300. mL of a 0.20M hydrocyanic acid (HCN) solution.…

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Q: Pls help ASAP.

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Q: Q7. Given the following Ka values for the weak acids and bases: CH;COOH/CH3CO0 HCO3/CO,2- H2PO4…

A: To find the pair that will be appropriate as buffer of given range we use the buffer range of each…

Q: Consider the reaction of a 20.0 mL of 0.220 M C₅H₅NHCl (Ka = 5.9 x 10⁻⁶) with 12.0 mL of 0.241 M…

A: When CsOH ( a base ) is added to C5H5NHCl ,  It will act as an acid and lose H+ ions and give its…

Q: You are making a buffer solution in the lab by combining the weak acid H2PO4- with its conjugate…

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Q: If the actual mass of a base used (sodium citrate dihydrate) in a buffer solution is 1.5 g, and the…

A: Given,  Actual mass of base (sodium citrate dihydrate) = 1.5 g  Concentration of the acid (ammonium…

Q: Solve this?

A: pH = 9.2 pH + pOH = 14 pOH = 14-9.2 = 4.8

Q: Calculate the pH at equivalence.

A: In this titration weak acid (Propanoic acid) is titrated with strong base NaOH, so salt of a weak…

Q: Calculate the pH of a solution containing 18 mL of 0.43 M of a weak weak base B OH, like NH,OH, or…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: What is the pH of a buffer that is 0.15 M in lactic acid [CH3CH(OH)COOH, or HC3H5O3] and 0.10 M in…

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Q: How will you prepare 500 ml of 0.750 M citrate buffer with a pH of 4.25 from solid citric acid…

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Q: Which of the following is/are TRUE about equivalence and end points? I. The end point of a…

A: 1.) b.ll only    l statement is wrong because it is not the end point but the equivalence point…

Q: 2.  The ionization constant for acetic acid is 1.8 x 10-5. How many grams of NaC2H3O2 must be added…

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

Q: Given the values of Ka and Kh below, which of the systems given would be most suitable to use to…

A: The pH of a buffer solution remain close to the pKa value of its acid in weak acid / base and its…

Q: Propanoic acid that, along with its sodium salt, can be used to make a buffer that has a pH of 5.25.…

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Q: A chemistry graduate student is given 500. mL of a 1.50M trimethylamine ((CH3)¸N) solution.…

A: This is a buffer consisting of a weak base and salt of the same base with strong acid. pOH = pKb +…

Q: -4 What A chemistry graduate student is given 100. mL of a 1.10 M trimethylamine ((CH,) N) solution.…

A: From the buffer solution of (CH3)3N and (CH3)3NHBr: [Salt]: Salt concentration. [base]: base…

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: Consider the following buffer system: 1.03 M H3PO4 and 0.93 M H₂PO4-. What is the pH of such a…

A: Acidic buffer :-  A mixture of weak acid and its salt with strong base is known as acidic buffer…

Q: a) The Ka value for phenolphthalein is 8 x 10-10. What is the concentration of hydrogen fon when…

A: The dissociation of phenolphthalein indicator (HIn) can be represented as follows: HIn (aq)⇌H+…

Q: 9) A 50.0 mL of a 0.100 M ammonia (NH,) solution is titrated with 0.150 M HCI. The k of ammonia is…

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Q: What is the pH of a solution when 100.0 mL of a 0.1M HCN solution (Ka = 6.2 x 10 -10) is titrated…

A: The reaction between HCN and NaOH is as follows: HCN+NaOH→NaCN+H2O Calculation of no. of mol of HCN:…

Q: A 25.0 mL solution of quinine was titrated with 1.00 M hydrochloric acid, HCl. It was found that the…

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

Q: find the acidity function when adding 5 ml of NaOH Calculate the pH value when titrated between 25…

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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.