What is the ratio of lactic acid (Ka = 1.37x10-4) to lactate in a solution with pH =4.01? Write your ratio out as a number containing a decimal.
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Q: What is the ratio of lactic acid (Ka = 1.37x10-4) to lactate in a solution with pH =4.09? Write…
A: Given Ka = 1.37 × 10-4 PH = 4.09 [ lactic Acid ][ lactate ] = ?
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A: Given,
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A: Sodium lactate is the salt of strong base and weak acid. Its solution will be basic in nature.
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A: Henderson hasselbalch equation for pH calculation of an acidic buffer:
Q: If an acid has a Ka of 2.12 x 10-3, what is its pKa?
A:
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- 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…The pH of blood is 7.35. This pH is maintained by a natural buffer system of H2CO3 and HCO3. What is the ratio of [ HCO3]/[ H2CO3 ] at this pH if the K, is 4.2 x 107? Give your answer in 2 significant figures.1. Which of the following solutions are acidic? Which are basic? Distilled H2O NaCl NH4Cl NaCH3COO (NH4)2CO3
- Calculate the pH of a 0.025 M solution of propanoic acid (Ka = 1.3 x 10-5). The answer is 1.6The amount of tartaric acid is responsible for the tartness of wine and controls the acidity of the wine. Tartaric acid also plays a very significant role in the overall taste, feel and color of a wine. Tartaric acid is a diprotic organic acid The chemical formula for tartaric acid is C4H6O6 and its structural formula is HO2CCH(OH)CH(OH)CO2H. A 50.00 mL sample of a white dinner wine required 21.48 mL of 0.03776 M NaOH to achieve a faint pink color. Express the acidity of the wine in terms of grams of tartaric acid, H2C4H4O6 (M. M. = 150.10) per 100 mL of wine. Assume that the two acidic hydrogens are titrated at the end point. MM H2C4H4O6 = 150.10 MM NaOH = 40.00 Below is the balanced chemical equation for this titration.Mola and Rity were tasked to analyze the acidity of a 10.0-mL fermented milk sample diluted with water in a 250-mL volumetric flask. Mola obtained a 15.0-mL aliquot of this solution, diluted it to 50.0 mL, and then titrated this diluted sample. Titration data were given to Rity and she found out that the 50.0-mL diluted sample contains 0.21 mmol of lactic acid. What is the lactic acid concentration (in M) of the titrated sample?
- Mola and Rity were tasked to analyze the acidity of a 10.0-mL fermented milk sample diluted with water in a 250-mL volumetric flask. Mola obtained a 15.0-mL aliquot of this solution, diluted it to 50.0 mL, and then titrated this diluted sample. Titration data were given to Rity and she found out that the 50.0-mL diluted sample contains 0.21 mmol of lactic acid. MW: Lactic Acid (90.08) Follow proper significant figure rulesa. What is the lactic acid concentration (in M) of the titrated sample? b. Determine the lactic acid content (in M) of the 10.0-mL fermented milk sample. c. What is the lactic acid concentration (in %w/v) of the 10.0-mL fermented milk sample?Mola and Rity were tasked to analyze the acidity of a 10.0-mL fermented milk sample diluted with water in a 250-mL volumetric flask. Mola obtained a 15.0-mL aliquot of this solution, diluted it to 50.0 mL, and then titrated this diluted sample. Titration data were given to Rity and she found out that the 50.0-mL diluted sample contains 0.21 mmol of lactic acid. MW: Lactic Acid (90.08) a. What is the lactic acid concentration (in M) of the titrated sample? b. Determine the lactic acid content (in M) of the 10.0-mL fermented milk sample. c. What is the lactic acid concentration (in %w/v) of the 10.0-mL fermented milk sample?4. Oleum at a concentration of 110 percent is equivalent to H2SO4 at a concentration of 91.8 percent. true or false
- What is the ratio of lactic acid (Ka = 1.37x10-4) to lactate in a solution with pH =4.09? Write your ratio out as a number containing a decimal. [lactic acid][lactate] =Given that pK₂ = 3.14 at 25 °C for HNO₂, what is the pH of 0.165 mol L-1 NaNO₂(aq) at 25 °C? What is the equilibrium concentration of HNO₂? pH = Number (Give your answer accurate to 2 decimal places.) Number mol L-¹ (Give your answer accurate to 2 signficant [HNO₂]eq figures.) =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
