Which of the following aqueous solutions, when mixed with an equal volume of 0.10 M CH3COOH(aq), will produce a buffer solution? (Select all that apply.) HINT: Consider dilution upon mixing and possibly a neutralization reaction . 0.20 М СНзСOONa 0.20 М НСІ 0.050 М НСI None of these 0.10 М СН3CООН 0.050 М NaОН

Which of the following aqueous solutions, when mixed with an equal volume of 0.10 M CH3COOH(aq), will produce a buffer solution? (Select all that apply.) HINT: Consider dilution upon mixing and possibly a neutralization reaction . 0.20 М СНзСOONa 0.20 М НСІ 0.050 М НСI None of these 0.10 М СН3CООН 0.050 М NaОН

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.32QAP

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You want to prepare 1.00 L of a buffer solution with a pH of 3.5. You are given an 0.45 M solution of nitrous acid, HNO2, and an 0.68 M solution of NaOH. What volume of each of these solutions must be mixed in order to get the desired buffer solution? Use the simultaneous equations method to solve this problem. If the buffer solution prepared in a. also contained ~10-6M Ni2+ and ~10-6 M Pb2+ , could those metal ions be separated from each other by saturating the solution with H2S? Explain your answer by showing the necessary calculations.
A buffer is prepared by using 0.20 mole of C6H5COOH and 0.40 mole of C6H5COO- in 1.00 liter of aqueous solution. Is the buffering capacity of this solution great enough to maintain its pH within ±1 when 15 g of HNO3 is added? Group of answer choices No, the concentration of benzoic acid (C6H5COOH) in this buffer solution is not high enough. Yes, the concentration of benzoate ions (C6H5COO-) in this buffer solution is great enough. Yes, the concentration of benzoic acid (C6H5COOH) in this buffer solution is great enough. No, the concentration of benzoate ions (C6H5COO-) in this buffer solution is not high enough.
10. One characteristic of blood that we rarely give a thought to is its pH. The pH of blood must be held remarkably constant, varying only by a few hundredths of a pH unit from 7.36 to 7.40. Blood pH is kept constant primarily through the buffering action of the bicarbonate ion, HCO3-, and dissolved carbon dioxide, commonly represented as H2CO3. The second ionization is negligible in blood so that H2CO3 can be treated as a monoprotic acid. A) If the Ka1 for H2CO3 is 4.2 * 10-7, what ratio of HCO3- to H2CO3 is necessary to produce a buffer of pH 7.40? B) What is the pH of a buffer that is 1.0 M NaHCO3 and 1.0 M H2CO3? C) If you have 1.00 L of the buffer described above (1.0 M NaHCO3 and 1.0 M H2CO3) and 10.0 mL of 0.100 M HCl is added to it, what is the new pH? D) Just to prove that the buffer helps minimize changes in pH, calculate the pH of a solution prepared by adding 10.0 mL of 0.1 M HCl to 1.00 L of pure water.
Benzoic acid, C6H5COOH, dissociates in water as shown in the equation below. A 40.0 mL sample of an aqueous solution of benzoic acid with a concentration of 0.50 M is titrated using standardized 0.25 M NaOH. a.State whether the solution at the equivalence point of the titration is acidic, basic, or neutral. Explain your reasoning. b.How many mL of 0.25 M NaOH need to be added in order to make the ideal buffer solution?
Limestone is a common rock used for road constructions. A construction company extracted 5 tons of the rock near a river on a rainy season. The rain washed away 2% of the rock into a nearby river which flows to a 10 acre and 15 feet deep lake in the area. With the help of relevant chemical equations, data, and calculations, explain how the washing of the rocks into the lake alters the pH of the lake.explain calculations of the final expected pH of the water in the lake
Consider the 25.0 mL portion of pH=4.45 buffer solution prepared as described in question 4. Calculate the buffering capacity of it for the hydrochloric acid of known concentration (M = 0.123 mol/L). Hint: you are calculating how much of the strong acid (HCl in this case) you can add to the buffer portion before you see a significant pH change, so start with deciding which component of the buffer will be the buffering species against the strong acid. Then calculate how much of that species is present in the 25.0 mL portion of this buffer. For the sake of these calculations, consider the buffering capacity to be the maximum volume of the strong acid that can be added to the portion of your buffer before the buffering species in it is completely used up, and the buffer is ‘overwhelmed’. Provide the answer in millilitres, mL. Don't include units.
Calculate the pH of a solution containing a salt B Cl derived from a strong acid (HCl) and a weak Base (B OH), like NH4Cl, CH3NH3I, Ph-NH3Br and so on. In this case two processes have to be considered: 1. Dissociation of the salt, within the assumption that the salt is a strong electrolyte: B Cl → B + + Cl-, for instance: NH4Cl → NH4+ + Cl- 2. the hydrolysis of the water B + + H2O ⇌ B OH + H+, for example: NH4+ + H2O ⇌ NH4OH + H+ (often shown as NH4+ ⇌ NH3 + H+ ) knowing that the initial concentration of the salt is 1.67 M, and the base dissociation constant, Kb , is 8.43e-7.
Which solution below would have the greatest buffering capacity? The solution was prepared from a weak base and the salt of its conjugate acid. 0.197 M HOC2H4NH2 and 0.197 M HOC2H4NH3Cl, Kb = 3.20e-5 0.0966 M NH2OH and 0.0966 M NH3OHF, Kb = 9.10e-9 0.1214 M NH2OH and 0.1214 M NH3OHNO3, Kb = 9.10e-9 0.1157 M HOC2H4NH2 and 0.1157 M HOC2H4NH3Br, Kb = 3.20e-5
propionic acid, ?a=1.34×10−5,Ka=1.34×10−5, 3.00 M sodium propionate, CH3CH2COONa 1. The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid must be 0.100 M. Based on this information, what mass of solid conjugate base should the student weigh out to make the buffer solution with a pH of 5.00? ( in g) 2. Based on this information, what volume of acid should the student measure to make the buffer solution? (in ml)
Which of these apply to the Image (attached)? There should be 4 total answers: A. High End pH B. High Initial pH C. Vertical Line with Equivalence Point Tall D. Equivalence Point Not at pH 7 E. Equivalence point at pH 7 F. low end pH G. low initial pH H. Vertical Line with Equivalence Point Short Using the info identified above, what type of analyte and tirant combo are in the image. Options for Analyte and Titrant: - Weak base - Strong Acid - Strong Base - Weak Acid
The course is specifically quantitative analysis, I figured that would just fall under chemistry. The issue I'm having with this one is that I have absolutely no idea how to even begin. I figure benzoic acid wouldn't affect the pH of NaOH that much since it's a weak acid and NaOH is a strong base, but I don't think it'd be right to just take the pH using solely the concentration of NaOH. What approach should I take to solve this? 220 mL of 0.03 M NaOH were added to 200 mL of 0.03 M benzoic acid (pKa = 4.2). What is the pH of the resulting solution?
You are asked to prepare a buffer solution with a pH of 3.50. The following solutions, all 0.100 M, are available to you: HCOOH, CH3COOH, H3PO4 , NaCHOO, NaCH3COO, and NaH2PO4. What ratio of [conjugate base]/[acid] would yield the best result for the required buffer solution created in the question above? ENTER YOUR ANSWER AS ONE NUMBER ROUNDED TO TWO DECIMAL PLACES.