Q: Justify why the Henderson-Hasselbalch equation would be useful for making buffers in the laboratory?…
A: Hello. Since your question has multiple parts, we will solve the first question for you. If you want…
Q: Differentiate the Carbonate buffer and phosphate buffer systems in terms of pH and pKa. Give…
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Q: Which of the following statement is incorrect regarding buffer solutions: O Buffer capacity…
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Q: Differentiate the carbonate buffer and phosphate buffer systems in terms of pH and pKa. Give…
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Q: Using the table of pH indicators and their respective pKas. Determine which indicator would be best…
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Q: Why a mixture of HCl and KCl does not function as a buffer where as a mixture of CH3COOH and…
A: Buffer solutions are those solutions that resist the change in pH upon the addition of a small…
Q: Calculate the pH of each of the following points by titrating 50 mL of 0.40M imidazole (pKa = 6.993)…
A: The required volume of 0.41 M KOH base to reach equivalence point is; 50 mL×0.40 M=0.41…
Q: A student was required to prepare 250.0 mL of a cyanoacetic acid/sodium cyanoacetate buffer in which…
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A: Solution -
Q: An alternative way of preparing the imidazolium buffer involves preparing solutions of imidazole (A)…
A: Note - Since you have asked multiple questions, we will solve the first question for you. If you…
Q: A student needs to prepare a buffer solution with a pH of 4.21. Assuming a pK, of 4.15, how many mL…
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Q: Why is there a discrepancy between the calculated pH and the experimental pH of a prepared buffer…
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Q: The titration of a weak acid with NaOH showed two equivalence points. Using only this information…
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A: Solution: The buffer: Acetic acid (CH3COOH) and Sodium acetate (NaCH3COO).The (CH3COOH) is weak acid…
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Q: The maximum buffering capacity is nearest to the pKa of the buffer. Explain why?
A: A buffer solution is capable of resisting a pH change on addition of small amounts of acid or base…
Q: Explain how does a solution butanoic acid and potassium butanoate can function as a buffer solution?…
A:
Q: The potentiometric titration of a weak acid against a stong base is shown below. For A) calculate…
A: "Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: Can someone explain to me why this example is a buffer? I don't understand it.
A: Buffer solutions are the solutions that resist a change in pH on dilution or on addition of small…
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A: The given plot is:
Q: Calculate the ph of at second equivalence point when 0.10M trisodium arsenate is titrated with 0.20…
A: trisodium arsenate, Na3AsO4(aq) is a deprotonated form of H3AsO4(aq), which is a tribasic acid. The…
Q: 4.0 6.0 8.0 10.0 Volume (mL) nce that is a weak acid. Determine the pK, of this compound.
A: 1- pH = 8.15 is the pH at equivalence point, in this pH Solution was completely neutralizated.
Q: Calculate the pH of the following buffers:a) A solution containing 0.425 molar benzoic acid and…
A: Calculate the value of pKa: Ka of benzoic acid is 6.50 × 10-5.
Q: Consider a buffer solution containing an acid with a pKa of 2.3 and an acid concentration that is…
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Q: Estimate the Ka of the weak acid being titrated in this curve.
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Q: Which of these statements is true? (a) If you add strong acidor base to a buffer, the pH will never…
A: The statement (a) is false as the addition of strong acid or base to a buffer changes the pH. The…
Q: When the pH is below the pKa, is the buffer species more or less than 50% protonated? Explained in…
A: Given -> pH is below the pKa value.
Q: Which of the following three solutions has the largest buffer capacity? Ka values are all the same,…
A: Buffer capacity is the amount of H+ or OH- needed to change the pH of the solution by a factor of 1…
Q: A student needs to prepare a buffer solution with a pH of 5.63. Assuming a pką of 4.49, how many mL…
A: Given: pH = 5.63 pKa = 4.49 Let M1 & V1 be molarity & volume of B- and M2 & V2 be those…
Q: Nonphysiological buffers such as HEPES and PIPES have come into because O they are inexpensive they…
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Q: a). What are acids, bases and buffers? b) What are the different types of buffers? Describe the…
A: Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: Hydrofluoric acid is titrated with potassium hydroxide. Determine the pH at the equivalence point.
A: Interpretation- pH at equivalence point. Concept introduction- pH - pH is defined as negative…
Q: Give the name of another weak acid that will have a similar titration curve. Briefly explain the…
A: To chake the similarities between two weak acid we have to chake the dissociation constant value and…
Q: Explain in details what happens in a buffer solution, taking note of the changes and the buffer…
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Q: are
A: According to the question, we need to determine the pH of buffer solution of benzoic acid and sodium…
Q: A student needs to prepare a buffer solution with a pH of 6.00. Assuming a pKą of 4.86, how many mL…
A: pH = 6.00 ; pka = 4.86 Concentration of B- = 0.1 M Concentration of HB = 0.1 M Volume of HB =…
Q: Draw the titration curve, when 40.00 mL of 0.22 M ammonia solution is titrated with 0.50 M HCl. As…
A: Given: 40.00 mL of 0.22 M ammonia solution 0.50 M HCl Ammonia is weak base and HCl is strong acid.…
Q: What is the relationship between the buffer range and the buffer-component concentration ratio?
A: The relationship between the buffer range and the buffer-component concentration ratio has to be…
Q: is the point at which the titration is complete Endpoint equivalence point Boiling point none of…
A: Given, ..................................is the point at which the titration is complete ? Options…
Considering the figure, write an equation in terms of pH and pKa that defines buffer range.
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- Chemistry Rx Cocaine HCl 1.5% (E = 0.16) Eucatropine HCl 1.5% (E = 0.18) Chlorobutanol 0.5% (E = 0.24) Make isotonic Disp: 30 mL a) How much sodium chloride should be added to make the above solution isotonic? b) If boric acid (E = 0.52) was used to make the solution isotonic how many grams should be used?A sample is analyzed for chloride using the Volhard method. What is the percentage chloride as NaCl using the following data? Weight of sample: 303.0 mg AgNO3 used: 40.00 mL of 0.1234 M KSCN used: 12.20 mL of 0.0930 MStandardization of Sodium Thiosulfate Solution Primary Standard used: Potassium Dichromate Formula mass of 1o standard: __________________ % Purity of 1o standard: 99.80% Trials 1 2 3 Weight of K2Cr2O7 (g)Weight of K2Cr2O7 (g) 0.0315 0.0331 0.0380 Final Volume Reading Na2S2O3 (ml) 27.50 27.50 34.90 Initial Volume Reading Na2S2O3 (ml) 1.10 0.00 1.00 Net Volume Na2S2O3 used (ml) Molarity of Na2S2O3
- 19 g of unknown organic sample was dissolve in 640 mL of Dicloromethane (DCM). The boiling point of benzene was increased by 3.78oC. Determine the molecular weight of the unknown sample? Kb of DCM = 2.42oC/m Bb of benzene = 39.6 oC density of benzene = 1.33 g/mL at 25 °C Round your answer to the nearest whole number, no units required.1. A 50.00 mL stock CaCl2 solution was diluted with water in a 250.0-mL volumetric flask. A 25.00 mL aliquot of this was further diluted to a final volume of 100.0 mL. Finally, 20.00-mL aliquot of the resulting solution was analyzed and found to contain 0.1500 M CaCh2 Solve for the concentration of the stock solution in M. 2. A 50.00 mL stock CaCl2 solution was diluted with water in a 250.0-mL volumetric flask. A 25.00 mL aliquot of this was further diluted to a final volume of 100.0 mL. Finally, 20.00-mL aliquot of the resulting solution was analyzed and found to contain 0.1200 g CaCl2 Solve for %w/v CaCl2 in the stock solution.MULTIPLE CHOICE: Choose the letter of the best answer Please answer all questions correctly 1. The standardization of volumetric solution does not require hydrochloric acid. A. Permanganometry B. Cerimetry C. Iodimetry D. lodometry E.All of the choices 2. In the standardization of its volumetric solution, the primary standard is dried to constant weight, which means drying shall be continued until two consecutive weighings do not differ by more than 0.50 mg. A. Permanganometry B. Cerimetry C. Iodimetry D. lodometry E.All of the choices 3. In the standardization of its volumetric solution, potassium iodide was added to A. Permanganometry B. Cerimetry C. Iodimetry D. lodometry E.All of the choices 4. Starch is the indicator of choice for these procedures because it forms intense blue coloration with the solution. A. Permanganometry B. Cerimetry C. Iodimetry D. lodometry E. C and D 5. In the standardization of its volumetric solution, the reaction needs to be…
- The first goal is to make the oxalic acid standard solution. You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. Molar mass of H2C2O4•2H2O = 126.07 g/mol Mass of H2C2O4•2H2O = 1.5232g Volume of H2C2O4•2H2O solution = 250.0mL What is the Molarity H2C2O4 standard solution ?A 18 g of unknown organic sample was dissolve in 756 mL of benzene. The boiling point of benzene was increased by 3.36oC. As the first step of analysis, determine the moecular weight of the unknow sample? Kb of benzene= 2.64oC/m Bb of benzene = 80.09 oC density of benzene = 0.874 g/mL at 25 °C Answer in whole number, no units required.Prepare 250 mL stock acetic acid solutions and from this solution prepare 100 mL of eachstandard solutions (you have pippette with sensitivity of 0.1 mL). (0.015 M 0.030 M 0.060 M 0.090M 0.12 M 0.15 M)
- AURALGAN Otic Drops contain: Antipyrine 5.4% Benzocaine 1.4% Acetic acid0.01% u-Polycosanol 410 0.01% Glycerin, ad 10 mL (a) What would be thecontent of antipyrine, in mg/mL? (b) If a patient used 5 drops of the otic solution,equivalent to 0.25 mL, how many milligrams of benzocaine would have beenadministered? (c) How many microliters of acetic acid would be used to preparethe 10 mL of drops? (d) What would be the equivalent ratio strength (v/v) of u-polycosanol 410?sing the pictures please help me with these questions.-Volume of unknown acid___-Average molarity of NaOH from above__-mL of NaOH at equivalence point__-molarity of unknown acid__(there was only one trial so average molarity and standard deviation are not required)What's the differences between two questions? Q1) How much calcium would you ingest by drinking one 8 oz glass of your tap water? Show all calculations. -->Tap water 8Oz = 8 x 0.0296L = 0.2368L Hardness = 66.73ppm = 66.73mg/L CaCO3 1L has 66.73mg CaCO3 0.2368L has 66.73mg x 0.2368 = 15.8017mg MW of CaCO3 = 100g/mol MW of Ca = 40g/mol 100g CaCO3 has 40gf of Ca 15.8017mg CaCO3 has 40/100 x 15.8017mg Ca We would ingest 6.321mg of Ca. Q2) What percentage of the recommended daily dose of calcium (1,150 mg/day) does 1.0 L of your water provide? Show all calculations. --> 66.73mg/1150mg x 100 = 5.80% My Question) Why this calculation is wrong? I think this calculation is same with question 1. Isn't it? CaCO3 = 100g/mol, Ca = 40g/mol 100g CaCO3 has 40g Ca. 66.73 CaCO3 has 40/100 x 66.73mg Ca Ca = 26.70mg 26.70mg/1150mg x 100 = 2.32%