Write the Henderson-Hasselbalch equation for a propanoic acid solution (CH,CH, CO,H, pKa = 4.874). [A¯] pH pK. + log = [HA] Answer Bank Using the equation to calculate the quotient [A¯]/[HA] at three different pH values. [A¯] pH = 4.232 [HA] [A^] [HA] 1 pH = 4.874 = [A¯] pH = 5.373 [НА]
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- Your goal is to make a buffer with a pH of 4.95 from acetic acid and sodium acetate. Assume the pKa for acetic acid is 4.74. What is the volume of acetic acid added to make your buffer? Report your answer to the tenths place. To do this, we use the Henderson-Hasselbach Equation pH = pkA + log (base/acid) where pkA = 4.74 for acetic acid, pH = target pH and [base] /[acid] = x/(1-x) since we don't know the concentration of the base, we will call it x the acid is just 1-x, assuming the two add up to 100% solve for x, and then you know the mL of base and acid to add.Calculate the pH of two HCl solution based on their concentrations of 0.001 and0.0001 M. Then calculate the pH of a solution when you add each of these to a closed carbonicacid system with mcarb-t = mH2CO3 + mHCO3- + mCO32- = 0.01 m and pH = 6. At that pH, mH2CO3 =10-2.16; mHCO3- =10-2.51; mCO32- is negligible.If a 0.3 M solution of NaOH was used to titrate 100 mL of 0.3 M solution of CH3COOH (Ka =1.8 x 10 -5) and the following volumes of NaOH were recorded: 102, 97, 99, 98, 101, 106 mL. The pH Value is………………when added 99.0 mL of 0.3 M NaOH The pH of the solution at the equivalence point more than 7 Because................................... Calculate the 99% confidence limits of the mean? And use them to decide whether there is any evidence of systematic error? [ hints: For N=6 and the 99 % confidence interval, the value of t is 4.03].
- Students 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?09. Two samples of the same soil is subjected to pH analysis using a pH meter, the first is analysed using 1:1 soil:water ratio and the other with 1:1 soil:KCl ratio, what would be the most probable result? A. Soil analused using 1:1 soil:KCl ratio will register a higher pH compared to that of soil analysed using 1:1 soil water ratio B. Soil analysed using 1:1 soil:KCl will register a lower pH compared to that of soil analysed using 1:1 soil:water ratio C. Soil analysed using 1:1 soil:water ratio will register a lower pH compared to that of soil analysed using 1:1 soil:KCl ratio D. Soil analysed using 1:1 soil:water ratio will have the same pH with that of soil analysed using 1:1 soil:KCl ratioFor the synthesis of maroon dye, Taylor needs to use a primary amine with a pH between 3.00 and 4.00 for optimum yield. In one of her trials, she dissolved 8.22 g of anilinium chloride, C6H5NH3Cl (MM = 129.58 g/mol) in distilled water to make 250.0 mL solution. Given that Kb of aniline (C6H5NH2) is 4.29 x 10-10, calculate the pH of the salt solution. Yes or No. Will Taylor obtain high yield of maroon using C6H5NH3Cl?'
- 1. Predict if an aqueous solution of 0.5 M sodium cyanide, NaCN, would be acidic, neutral, or basic at 298 K. 2. Write the correct hydrolysis reaction that would be used to calculate the pH of the solution. 3. Create and fill in an ICE table below your reaction in part 2, using x as the variable. Do NOT make assumptions about the size of x; include all terms. 4. Which equilibrium constant is needed? Substitute your terms into the expression for the appropriate equilibrium constant. Do NOT make assumptions about the size of x; include all terms. Do NOT look up the value of K, solve for x or calculate the pH; you're done.Determine the Concentration of Ethanoic Acid in Vinegar Equipment / Apparatus: 250-mL conical flasks Clamp Burette Graduated cylinder Pipette Reagents / Materials: Vinegar Phenolphthalein indicator 0.2 M NaOH (standardized) Calculation: Molarity (M) of ethanoic acid The average measured volume of the NaOH from titration: Average volume of NaOH used = (21.5ml + 21.5ml + 21.6ml) / 3 =21.5ml No of mole of NaOH = Concentration of NaOH (0.2M) × Average volume of NaOH used When an acid is completely neutralized: No of moles of CH3COOH = No of moles of NaOH Using the moles of CH3COOH, the molarity of ethanoic acid in the 5.0-mL sample of vinegar is calculated: Molarity (M) CH3COOH = moles CH3COOH / volume of vinegar (0.005 dm3). Calculation: Mass / Volume Percent (m/v) of ethanoic acid To calculate the percent (m/v) of CH3COOH in vinegar, we convert the moles of ethanoic acid to grams using the molar mass of ethanoic acid, 60.1 g/mole. Mass of CH3COOH =…A 1.0-LL buffer solution initially contains 0.30 molmol of NH3NH3 (Kb=1.76×10−5)(Kb=1.76×10−5) and 0.30 molmol of NH4ClNH4Cl. What mass of the correct reagent should you add? Express your answer using two significant figures.
- In this lab, you will make a buffer out of acetic acid, H3CCOOH, and acetate, H3CCOO–. By convention, weak acids are often shortened to HA and their conjugate weak bases are shortened to A–. You will make a pH 5.00 buffer. Use the Henderson-Hasselbach equation to calculate the ratio of conjugate base to acid ([A–]/[HA}) in this buffer. The pKa of acetic acid is 4.75. Enter your answer with three digits.H2PO4- + H2O ======== HPO4^-2 + H3O+ 2. Effect of the ratio of the conjugate base to the weak acid. CASE 1. From the Henderson-Hasselbach equation, calculate the ratio of dihydrogen phosphate (H2PO4-) and monohydrogen phosphate (HPO4-2) components required to produce buffer solution with 1. pH 6.2 2. pH 7.2 3. pH 8.2 CASE 2. From the Henderson-Hasselbach equation, calculate the ratio of acetic acid and acetate required to produce buffer solution with: 1. pH 3.7 2. pH 4.7 3. pH 5.7Using the stock solution provided to you, make 25 mL of each of the buffer solutions assigned to you. Measure and record the pH of each of the buffer solutions. Add 2 mL of 0.1 M NaOH to each of the 25 mL buffer solutions. Record the pH of each buffer solution after addition of alkali. Account for the magnitude of pH shift in each with reference to the direction of pH shift.Calculate the molarity of the acid (HA) and the conjugate base (A- ) . For acetate, use grams-to-mol conversion and divide it by the total volume. For (aceitic acid), use M1V1=M2V2. Consider the total volume of your buffer (50 mL + 10 mL). a) [A-] = b) [HA] = I am not sure how to answer this or if it is related to this info that we were given at the top of the page: "A buffer is made by mixing 2.0 g of sodium acetate (NaA: 1 mol / 82 g) and 10 mL of 3.0 M acetic acid. Then 50 mL of water is added to the mixture. Find the pH of this buffer!"