Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is best suited for preparing a buffer solution with pH of 4.74?   Question 2 options:   NH3 / NH4Cl  (Ka = 5.6 × 10–10)   NaNO2 / HNO2  (Ka = 4.5 × 10–4)   CH3COONa / CH3COOH  (Ka = 1.8 × 10–5)   NaCl / HCl   NaOCl / HOCl  (Ka = 3.2 × 10–8)

Q: Consider how best to prepare one liter of a buffer solution with pH = 6.52 using one of the weak…

A: Given: The pH of the buffer solution is 6.52. The volume of the buffer solution is 1.00 L.

Q: 12. Assuming equal concentrations of conjugate base and acid, which of the following mixtures is…

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Q: An analytical chemist is titrating 226.0mL of a 0.8900M solution of diethylamine ((C2H5)2  NH) with…

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

A: The solution is as follows :

Q: A chemist needs a solution buffered at pH 4.30 and can choose from the following acids: A.…

A:

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,…

A:

Q: Consider the following acids and bases: HCO2H    Ka = 1.8 × 10-4 HOBr    Ka = 2.0 × 10-9 (C2H5)2NH…

A: Given :      the values of the dissociation constant for the following acids and bases. HCO2H…

Q: Given 0.1 M aqueous solutions of ammonium chloride (NH4Cl) and ammonia (NH3) to the solution of that…

A: In equation (1), the relation between Ka, Kb, and Kw is shown. The values for Kw and Ka are…

Q: You want to make a 500.0 mL of 0.080 M of phosphate buffer pH = 7.90 from Na2HPO4 and NaH2PO4…

A:

Q: An analytical chemist is titrating 143.9 mL of a 0.6100M solution of acetic acid (HCH3CO₂) with a…

A: Given data : Concentration of HCH3CO2 = 0.6100 M Volume of HCH3CO2 = 143.9 mL Concentration of NaOH…

Q: Calculate the pH at the points indicated below if 50.0 mL of 0.100 M aniline hydrochloride (…

A: Aniline hydrochloride (fC6H5NH3+Cl¯) is a salt of the weak base aniline (C6H5NH2)  and the strong…

Q: A diprotic acid, H2A, has the ionization constants: Ka1 = 1.1 × 10–3 ;Ka2 = 2.5 × 10–6. In order to…

A: for making buffer solution the value of pKa for acid should near equal to the pH value ..

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: ethylamine C2H5NH2 Kb = 4.3×10-4 An aqueous solution contains 0.494 M ethylamine (C2H5NH2). How…

A: Hydroiodic acid is strong acid and ethylamine is a weak acid. 225mL  0.494M  C2H5NH2 =…

Q: Calculate the mL of acetic acid (0.845 M) and baking soda (assume 0.735 M) that need to be mixed to…

A: Buffer are the solutions which prevent any change in the pH of a solution when small amount of an…

Q: 2. Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is…

A:

Q: A buffer was made with HC2H3O2 and its conjugate base. What is the pH of the buffer if at…

A: According to Henderson equation pH= pKa(HC2H3O2)+ log[C2H3O2-1]/ [HC2H3O2]

Q: A 100. mL sample of 0.10 M HCl is mixed with 50. mL of 0.14 M NH3. What is the resulting pH? (Kb for…

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Q: 1. The acid used in the titration is a weak diprotic acid. Briefly explain: 1. how you know it’s…

A: Given :  triration curve between acid and sodium hydroxide base.  To find : Properties of acid that…

Q: Q2.Show in detail how you would prepare 350 ml of 0.12M citrate buffer pH-5.1.(You must use the Ka…

A: Desired pH = 5.1 We chose the conjugate acid/base pair as the buffer solution whose pKa value is…

Q: Mass of NaCl needed for 50.0 mL of 0.200 M NaCl solution. (Show calculation below.) Change in pH…

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Q: You are to prepare a 500.0-mL buffer solution. ou have exactly 0.125 mol of NaO2CCO2H. Prepare a…

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Q: 4.) A 100-mL buffer solution with pH of 4.80 is prepared as a stock solution. Using this stock…

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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: An analytical chemist is titrating 160.3mL of a 0.8600M solution of benzoic acid HC6H5CO2 with a…

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Q: Question 10 Assuming equal concentrations of conjugate base and acid, which one of the following…

A: Option - C would be the correct option when you put value in Equation  pH= pka + log(Salt)/(Acid)…

Q: You were asked to estimate the pH of a 15mL of 0.09N of HCl when 16.9mL of 0.085N NaOH is added to a…

A:

Q: Suppose you wanted to make the best pH = 9.30 buffer you can using the acids listed on the table…

A: Here in the given all 5 cases, the acids are HCN and HClO4. Here the HCN is a weak acid with pka…

Q: Given the equations and constants below, calculate the concentration of Zn(OH)* and of Zn(OH)2(aq)…

A: The solubility product of salt is a constant at a given temperature irrespective of the source from…

Q: An analytical chemist is titrating 83.7 mL of a 0.3300M solution of isopropylamine ((CH,) CHNH,)…

A: Given that : The volume of isopropylamine = 83.7 mL The molarity of isopropylamine = 0.3300 M The…

Q: Using the pKa values and molecular weights from the OneNote Class notebook, show you work to prepare…

A: We need to prepare a phosphate buffer with pH 7.3.

Q: a)  What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.507 mol of NaA…

A: the solution is as follows:

Q: Calculate the pOH of 103.16 mL of a buffer initially consisting of 0.1752 M H2NCH2COOH and 0.1573 M…

A:

Q: Which of the following combinations of acids and conjugate bases would be the best to create a pH…

A: 1- In this question, we will see the best buffer system at pH 7.0  You can see the details…

Q: An analytical chemist is titrating 64.9 mL of a 0.5800M solution of isopropylamine ((CH, CHNH, with…

A: The question is based on the concept of titration. we are titrating a weak base with a strong acid.…

Q: Which of the following acids (listed with Ka values) and their conjugate base should be used to form…

A: Answer: HClO2  Amongst all options, the HClO2 acid and its conjugate is superior choice for the…

Q: A student was given a 0.15 M solution of an unknown diprotic acid H2A and asked to determine the Ka1…

A: The first acid dissociation constant of diprotic acid is calculated as,

Q: An analytical chemist is titrating 109.0 mL of a 0.5400 M solution of isopropylamine ((CH,) CHNH, )…

A:

Q: Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is…

A:

Q: Consider how best to prepare one liter of a buffer solution with pH = 6.52 using one of the weak…

A:

Q: If you have a solution with 1 mole of acetic acid HC2H3O2, which of the following can be added to…

A: We have to predict the chemical added to make a buffer solution.

Q: Calculate the mL of acetic acid (0.845 M) and baking soda (assume 0.735 M) that need to be mixed to…

A: Vinegar is acetic acid solution. For pH 5: Total concentration of buffer = 0.25 M Let, [salt] =…

Q: 14,How many milliliters of 0.1154 M NaOH are required to titrate 10.00 mL of 0.0950M H2SO4 to the…

A:

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: sample of 100.00mL of 0.100 M HC2H3O2 is titrated with 0.100 M NaOH. Find the pH of the solution…

A:

Q: b = 3.00x10-6), C5H5N (Kb = 1.69x10-9)? Grou

A: Buffer solutions are used to maintain a constant pH of the solutions. The pH is maintained by the…

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: Consider how best to prepare one liter of a buffer solution with pH = 3.79 using one of the weak…

A: In the given question, preparation of buffer solution is required with pH = 3.79. The closest pKa…

Q: A student needs to prepare a buffer solution with a pH of 4.18. Assuming a pKa of 4.69, how many mL…

A:

Q: Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is…

A: We have to choose suitable buffer for given pH range.

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.