A 50.00 mL sample of white dinner wine required 28.54 mL of 0.03867 N NaOH to achieve a phenolphthalein endpoint. Express the acidity of the wine in terms of %w/v of tartaric acid (H2C4H4O6, MW=150.09g/mol).
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A: 25.87 ml of 0.03291 M NaOH is required Molar mass of H2C4H4O6 is 150.09 g/mol 0.03291 M means…
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A 50.00 mL sample of white dinner wine required 28.54 mL of 0.03867 N NaOH to achieve a phenolphthalein endpoint. Express the acidity of the wine in terms of %w/v of tartaric acid (H2C4H4O6, MW=150.09g/mol).
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- A 50.00-mL sample of a white dinner wine required 25.87 mL of 0.03291 M NaOH to achieve a phenolphthalein endpoint. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL.A 50.00-mL sample of white wine required 24.57 mL of 0.03291M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated.)Use the modified H-H shown below to calculate the blood plasma pH under the following conditions: [HCO3-] = 0.022 M and pCO₂ = 46 mmHg. Provide your answer to two decimal places. Do not enter units. Dissociation Constant pH = 6.1 Bicarbonate (mmol/L) HCO 0.03 x PCO₂ CO₂ Solubility Constant CO₂ Partial Pressure (mmHg)
- The disinfectant phenol, C₆H₅OH, has a pKₐ of 10.0 in wa-ter, but 14.4 in methanol. (a) Why are the values different? (b) Is methanol is a stronger or weaker base than water? (c) Write the dissociation reaction of phenol in methanol. (d) Write an expres-sion for the autoionization constant of methanol.Hw.144.A solution contains formic and tartaric acids. A 25.00 mL aliquot portion is treated with 50.00 mL of a 0.1663 mol/L solution of cerium(IV) in 12 molL sulfuric acid; after boiling for one hour, it is cooled to room temperature and the excess cerium(IV) is titrated with 8.24 mL of iron(ll) 0.1108 molL. Under these conditions all organic acids are oxidized to carbon dioxide. Another 25.00 mL aliquot portion of the acid solution is treated with 20.00 mL of 0.2383 molL cerium(IV) in 4 molL perchloric acid and heated at 50°C for 20 minutes. The solution was then titrated with 14.65 mL of 0.1012 mol/L oxalic acid. Under these conditions all organic acids are oxidized to formic acid. (a) Calculate the concentration of formic acid in g/L (b) Calculate the concentration of tartaric acid in g/L
- please explain the process and answer Mouthwash acts to clean and disinfect mouths. Two important considerations when designing a mouthwash solution are the pH, which should ideally not be too acidic (where saliva has a normal pH range of 6.2–7.6 and below pH 5.5 erosion may occur), and the resistance of the solution to changes in pH. One example of a buffering system used in mouthwash is based on the compound H3PO4 which has PKa values of 2.1, 7.2 and 12.3. i. Hand-draw the structure of the main phosphorus species at pH 7.0, as well as a balanced equilibrium equation showing the structures of the two main phosphoric acid species at pH 7.0.Atmospheric CO2 levels have risen by nearly 20% over thepast 40 years from 320 ppm to 400 ppm. (a) Given that theaverage pH of clean, unpolluted rain today is 5.4, determinethe pH of unpolluted rain 40 years ago. Assume thatcarbonic acid (H2CO3) formed by the reaction of CO2 andwater is the only factor influencing pH.CO2(g) + H2O(l) ⇌ H2CO3(aq)(b) What volume of CO2 at 25 °C and 1.0 atm is dissolvedin a 20.0-L bucket of today’s rainwater?When the 2.5M NaOH (15mL) solution is added to the solution of 50:50 mixture of benzophenone and benzocaine acid (2.001g) , in diethyl ether (30 mL), a reaction takes place between NaOH and one of the components in the mixture. Draw a scheme that shows that reaction. Include electron-push arrows
- The concluctivity of a 0,05 M solution of acetic arid of 18°℃ is 4.4×10" si'cm'. A of acti ecelic acid ett the same temperature is 327 ST'cm. Calculate the dissociation constant (Kg) of acetic acid?Each row represents an experimental “run” (in this case, averaged sample of mango wine). Column A shows the run number; Column B shows the percentage of ethanol; Column C shows the amount of glycerol (in g/L); Column D shows the amount of acid (in g/L); Column E shows the temperature of the run (in °C); and Column F shows the pH of the run. Y represents Ethanol of mango wine. 1. Create a scatterplot of the ethanol data for all 20 runs a. Draw a graphical representation of the model that you chose to use. b. Comparing the model to your data, evaluate its fit in one or two sentences. (Not sure what this question is getting at. I've provided all the information given) c. Replace the generic Yi = β0 + ε with the information you have here. Please help. I have no idea what this even means or where to start. HERE is the attached dataset to start with; a b c d e f Run Ethanol Glycerol Acidity Temp pH 1 4.8 3.5 0.84 24 3.8 2 9.6…Petanoic (or valeric) acid is a weak organic acid with an unpleasant odour. Like other small carboxylic acids, it is used to make pleasant smelling esters that are used in perfumes, cosmetics, and food additives. Completed Part D In Part B, a 20.00 mL aliquot of a 0.195 mol L-1 pentanoic acid solution was titrated to its equivalence point with 19.7 mL of 0.198 mol L- 1 NaOH solution. At the equivalence point, all of the weak acid, pentanoic acid, is converted to its weak conjugate base, pentanoate. In part A, the Ka for pentanoic acid was determined to be 1.48×10-5. What is the pH at this equivalence point? 5.089 6.997 pentanoic acid 9.170 4.830 The pka of pentanoic acid is 4.830. 8.911
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