Which is the best acid to use in the preparation of a buffer with pH = 9.3? can someone show me how to get the answer? thank you so much Answer choices: NH2OH (Kb = 9.1 x 10^-9) CH3NH2 (Kb = 3.7 x 10^-4) NH3 (Kb = 1.8 x 10^-5) C6H5NH2 (Kb = 4.3 x 10^-10)

Q: 40. If you add 8.0 mL of 0.10 M HCl to 25 mL lactic acid/lactate buffer that is 0.10 M lactic acid…

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Q: A 25.0 mL sample of 0.100 M NH3(aq) is titrated with 0.100 M HCl(aq). What is the pH at the…

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Q: The Ka of hyperchlorous acid, HClO is 3.50 X 10-8. How many grams of NaClO (molar mass = 74.5…

A: Given, Ka of hyperchlorous acid is 3.50 X 10-8 Therefore, pKa = - log(Ka)…

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

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Q: A solution containing 50.0 mL of 0.180 M NH3 (Kb = 1.77 x 10¯5) is being titrated with 0.360 M HCl.…

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Q: What is the pH of a buffer made with NH3 ( 0.200M) and NH4Cl  (0.300M). Ka NH4+ = 5.68 x 10 -10  (…

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Q: Which of the following acids should be used to prepare a buffer with a pH of 3.4? CH3COОН, Ка - 1.8…

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Q: What is the pH of a buffer made using 45.0 mL of 0.750 M HC3H5O2 (propanoic acid, Ka = 1.3×10–5) and…

A: Given that: Concentration of HC3H5O2 = 0.750 MConcentration of NaC3H5O2 = 0.700 MVolume of HC3H5O2 =…

Q: A beaker with 155 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total…

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Q: What is the pH of a buffer made by combining 0.89 moles HNO2 with 0.96 moles NaNO2 in a 100.00mL…

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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: A chemistry graduate student is given 450.mL of a 1.20M propanoic acid  (HC2H5CO2) solution.…

A: The formula for the calculation of pH of an acidic buffer solution is given below.

Q: What will be the pH of the solution prepared by dissolving 8.35 g of aniline hydrochloride (C6H5NH3…

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Q: Which of the following acid/base conjugate pairs could you use to make a buffer solution with a pH…

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Q: Calculate the pH of 100.0 mL of a buffer that is 0.0800 M  NH4Cl and 0.135 M  NH3 before and after…

A: NH4Cl is salt and NH3 is a base. pKa of NH3 = 4.75

Q: What is the pH of a buffer solution that is 0.20 M propionic acid, HC3H5O2 and 0.16 M sodium…

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Q: Calculate the pH of a base buffer solution composed of 0.20 M NH3 and 0.15 M NH4Cl after the…

A: The formula to calculate the pH of the solution is, pOH+pH=14pH=14-pOH Given, The concentration of…

Q: Which of the following acid/base pairs would be best for making a buffer with a pH of 3.50? H2CO3…

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Q: 25.0-mL sample of 0.100M Ba(OH) 2 is titrated with 0.125M HCl. How many milliliters of HCl will be…

A: Interpretation: A 25.0 mL sample of 0.100 M Ba(OH)2 is titrated with 0.125 M HCl. The volume of HCl…

Q: A buffer is prepared by mixing 206 mL of 0.452 M HCl and 0.500 L of 0.400 M sodium acetate,…

A: Given: Molarity of HCl = 0.452 M Volume of HCl = 206 mL Molarity of sodium acetate = 0.400 M Volume…

Q: A student titrates 20.0 mL of 1.84 M HCl with a weak base (Kb = 2.33 x 10−6). The weak base and HCl…

A: Given values: Volume (V1) of HCl = 20 mL Molarity (M1) of HCl = 1.84 M Kb = 2.33 × 10-6 Volume (V2)…

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

A: We can find the volume of benzoic acid and sodium benzoate to prepare buffer solution as given…

Q: For the titration of 20.0 mL of 0.150 M acetic acid (CH₂COOH, K₂ = 1.8x105) with 0.150 M NaOH, what…

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Q: 3. A 100.0 mL sample of 0.10 M NH3 is titrated with 0.20 M HNO3. Determine the pH of the solution…

A: in this reaction NH3 and nitric acid both are limiting reagent because they are in same quantity so…

Q: Which of the following mixture would result in a buffer solution. Give a brief explanation. (Image)…

A: Solution: By the definition of buffer solution, we know, the solution of weak acid with its…

Q: Which aqueous solutions are buffers?  Show your reactions and reasoning for each one.   100 M NaCl…

A: Buffer solution- It is a chemical added during chemical reaction for control of pH of reaction. For…

Q: A chemistry graduate student is given 300.mL of a 1.10M hydrocyanic acid  (HCN) solution.…

A: The formula for the calculation of pH of the given buffer solution is given below.

Q: 15 The K₂ of oxalic acid (H₂C204) is 5.37 x 10-2. What is the pH of a buffer solution that is…

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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: Suppose you need a buffer with a pH of 4.9. Which conjugate acid-base pair should you use? O sodium…

A: To find the appropriate buffer of given solution we need to find the buffer range of each conjugate…

Q: Which of the following combination can be used to prepare a buffer with a pH of 7?     K2HPO4 and…

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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 (pKa = 4.20)…

A: Given Molarity of benzoic acid = 0.100 M Molarity of sodium benzoate = 0.240 M pH of buffer = 4…

Q: Which of the following has the highest pOH ?   0.2 M NaOH…

A: The concentration of the hydroxide ion in the solution can be defined by the pOH of the solution.…

Q: 1) You want to prepare a buffer with a pH of 3.6. Which weak acid should you use and what else…

A: 1. To prepare a buffer of pH 3.6, the superior choice is HNO2 acid. Because HNO2 has pKa value =…

Q: A chemistry graduate student is given 450. mL of a 1.70M chloroacetic acid (HCH,CICO,) solution.…

A: Buffer Question and solving for the amount of Salt needs to dissolve in Acid to form a buffer of pH…

Q: 1- Calculate the pH of 0.1 M KHCO3.

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Which of the following compounds could be used to create a buffer with a pH of 3.80? Nitrous acid…

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Q: and 0.500 M sodium acetate. What is the pH if 0.100 mol of KOH is added to 1.00 L of the buffer…

A: Given, Moles of acetic acid = 0.500 mol Moles of sodium acetate = 0.500 mol Ka = 1.8×10-5 pKa = 4.74…

Q: Calculate the pH of a buffer system containing 0.280 M NH3 and 0.430 M NH4Cl at 298.15K…

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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: A chemistry graduate student is given 500.mL of a 0.80M chloroacetic acid (HCH2ClCO2) solution.…

A: Given, pH to be made - 3.08 Ka - 1.3 × 10-3  chloroacetic acid taken - 500 mL of 0.80 M

Q: Which of the following aqueous mixtures will result in a buffer with a pH higher than 7.0? (For…

A: Correct answer is option d. 10 mL of 0.1 M NH3 + 5.0 mL of 0.1 M HCl

Q: A chemistry student is asked to maked a buffer of pH = 4.0. Which of the following acids would be…

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Q: Q 1(h) Which buffer system will have the greatest buffer capacity at pH 5.5? Acetic acid/sodium…

A: h) Buffer capacity is more when it's pKa is nearer to its pH. pH = -log(H+) and  pKa= - log (Ka)…

Q: in NH3 and 0.5 M in HCl is (Kb for NH3 = 1.8 x 10¯5):   (A) a solution with a pH less than 7 that…

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Q: 1] A 50.00 mL aliquot of O.1000 M NaOH is titrated with O.1000 M HCI. Calculate the pH of the…

A: When a strong acid and strong base are titrated neutralization reaction takes place. In a…

Q: What mass of sodium benzoate should you add to 150.0 mLmL of a 0.16 molL−1molL−1 benzoic acid…

A: A numerical problem based on Henderson equation, which is to be accomplished.

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

A: Given,

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

A: Buffers are classified based on their pH values. If pH lies in between of 0 to 7, buffer must be…

Q: What mass of sodium benzoate, C6H5COONa should you add to 150 mL of a 0.15 M benzoic acid solution…

A: Introduction: Molarity of benzoic acid = 0.15 M  Volume of benzoic acid = 150 ml  pH = 4.25  Ka =…

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.