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- acid-base titration lab Use Ka (calculate this first) to find the initial pH for your sample and compare the calculated and experimental results. Possible hint: calculate the concentration of the KHP at the start of the titration by assuming that the measured amount of KHP was dissolved in 50mL of water (provided in screenshot) I found the calculated experimental Ka = 8.7096 x 10^-6 Refresher: from datapoints, I found equivalenct point and halfway point, found pKa since pH = pKa. found Ka by 10-KaTrial 1: Initial pH= 3.92mL Mass of KHP and Paper= 0.868g Mass of paper= 0.357g Mass of KHP= 0.511g Trial 2: Initial pH= 4.09ml Mass of KHP and Paper= 0.870g Mass of paper= 0.359g Mass of KHP= 0.511g 1)Use Kb, the number of moles of C8H4O4^2- at the equivalence point, and the total volume at that point to calculate the pH for each sample at the equivalence point. Compare these calculated results with the experimental results.Please answer it ALL ASAP and CORRECTLY for an upvote. PROVIDE YOUR FULL SOLUTION. You prepared a buffer solution by mixing 68 ml of 0.17 M ammonia and 42 ml of 0.13 M ammonium chloride. The dissociation constant of ammonia is 1.8x10^-5 What is the total volume of the buffer? What is the final concentration of the base? What is the final concentration of the salt? What is the acid strength of the solution? What is the pH of the buffer solution?
- 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].Please help me fill out this table! Answering just one of the columns is good enough, thank you! Concentration of Standardized NaOH - 1.00 mol/L Mass concentration of acetic acid - 2.40 g/L Trial 1 Trial 2 Measured pH of the acetic acid solution 3.07 3.05 Mass of acetic acid solution taken for titration 20.0 g 20.0 g Initial buret reading of NaOH titrant 0.00 mL 0.00 mL Final buret reading of NaOH titrant 0.82 mL 0.79 mL Net volume of NaOH 0.82 mL 0.79 mL Millimoles of NaOH to end point of titration _?_mmol _____mmol Millimoles of acetic acid in sample _?_mmol ______mmol Molar concentration of acetic acid solution _?_mol/L ______mol/LConsider the titration of 25 mL of 0.200 M N2H4 with 0.100 M HCl. Determine the pH of the solution at 20.00, 47.50, and 55.00 mL added HCl solution. pKb for N2H4 is 5.90. You do not have to write the full Kb expression for this problem, but it and other expressions may be helpful.
- A student titrates 29.00 mL of 0.2250 M pyridine (Kb = 1.7*10-9) with 0.3750 M HBr. Calculate the pH after the addition of 6.50 mL, 8.70 mL, 9.90 mL, 10.00 mL, 10.80 mL, 15.00 mL, 17.40 mL, 18.70 mL and 36.00 mL of HBr. Plot the results of your calculations as pH versus mL of HBr addedAn automatic titration of Cola product was analyzed and the following results were produced: Volume of Standardized NaOH Titrant used to achieve the first equivalence point in titration: Trial #1: 1.300 mL Trial #2: 1.137 mL Trial #3: 1.140 mL May you explain why trial #1 was skewed; for example, if pipetting of the 25.00 mL was done incorrectly, how would the molarity change if the volume examined was supposed to be 24.50 mL?Let's determine the concentration and the pH of a H2CO3 solution that was prepared by using standard NaOH solution with a concentration of 0.125 M using the following data. Trial 1 Trial 2 Trial 3 Volume of H2CO3 19.80 mL 20.05 mL 19.95 mL Initial volume of NaOH (mL) 1.90 16.88 31.98 Final volume of NaOH (mL) 16.88 31.98 47.00 What is the Molarity and the pH of the H2CO3 ?
- In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was diluted with 9 mL of water. The pH was taken again and is now around 3.8 a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict the pH of the sample.c) Using…In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was diluted with 9 mL of water. The pH was taken again and is now around 3.8 d) Based on your answer in a) and c), do you think the unknown is really a strong acid or is it a weak acid instead? Defend your answer in one sentence.e)…Consider the titration of 100.0 mL of 0.100 M NaOH with 1.00 M HBr. Find the pH at the following volumes of acid added. VOLUME OF TITRANT (ML) PH (MUST BE IN 2 DECIMAL PLACES) ROUND OFF CORRECTLY 0 9.9 10 10.1 15