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Using the experimental data at 1/2 the equivalence point volume, calculate the Ka of acetic acid.
Volume of NaOH at Equivalence point for HCl Trial = 5.083ml
Equivalence point pH for HCl Trial = 6.57
pH 1/2 Equivalence point for HCl Trial = 3.285
Volume of NaOH at Equivalence point for HC2H3O2 Trial= 4.025ml
Equivalence point pH for HC2H3O2 Trial = 4.13
pH 1/2 Equivalence point for HC2H3O2 Trial = 2.065
When acetic acid reacts with NaOH, the following reaction occurs:
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- 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.find Ka for acetic acid from following half equivalence data point of half equivalence : 5 mLhalf equivalence pH value: 0.88concentration of NaOH: 0.99/ mol L-1 Volume of NaOH at equivalence point: 10mLVolume of acetic acid/mL: 40 mLwhy is it necessary to test the ph? EXTRME DETAIL PLEASE PROCEDURE To a six inch test tube was added thiamine hydrochloride (0.65 g), followed by water (2mL). The mixture was gently shaken until homogeneous, and then ethanol (7.5 mL)was added. Finally, sodium hydroxide (10%, 1.5 mL) was added and the mixture wasgently stirred to ensure complete mixing.Benzaldehyde (3.8 mL) was then added at room temperature in one portion with gentlestirring. The pH of the resulting reaction mixture was determined and adjusted to >10by dropwise addition of 10% sodium hydroxide.
- 4. The molar absorptivities of the indicator weak acid HIn (K_{a} = 1.42 * 10 ^ - 5) and its conjugate base In at 570 were determined as epsilon(HIn) = 7120 and ε(In) = 961. The optical length b = 1.00 cm. (a) What is the absorbance of an unbuffered indicator solution having total indicator concentration 8.0 * 10 ^ - 5 (b) What is the absorbance of a buffered indicator solution having total indicator concentration 8.0 * 10 ^ - 5 and pH = 6.5 .Using the known value for the Ka for acetic acid (1.76x10^-5),calculate the expected ph of an acetic acid solution with a concentration equal to that found in this experiment(I.e the concentration you determined) which was .8604Please answer with complete solutions. Do not use spreadsheet. Thank you A series of solutions containing NaOH, Na2CO3, and NaHCO3, alone or in compatible combination, was titrated with 0.1202 M HCl. Tabulated below are the volumes of acid needed to titrate 25.00-mL portions of each solution to (1) a phenolphthalein and (2) a bromocresol green end point. Use this information to deduce the composition of the solutions. In addition, calculate them molar concentration. (1) Phenolphthalein End Point (2) Bromocresol Green End Point a 22.42 22.44 b 15.67 42.13 c 29.64 36.42 d 16.12 32.23 e 0.00 33.33
- Please answer with complete solutions. Do not use spreadsheet. Thank you A series of solutions containing NaOH, Na2CO3, and NaHCO3, alone or in compatible combination, was titrated with 0.1202 M HCl. Tabulated below are the volumes of acid needed to titrate 25.00-mL portions of each solution to (1) a phenolphthalein and (2) a bromocresol green end point. Use this information to deduce the composition of the solutions. In addition, calculate the mass in milligrams of each solute per milliliter of solution.MUST ANSWER BOYH SUBPARTS A AND B A 1.161g sample of pure maleic acid (H2M, 116.1 g/mol) with Ka1 and Ka2 values of 1.42 × 10-2 and 8.57 ×10-7, respectively, was contained in a 100.0 mL solution with a pH of 5.0. In solution, maleic acid can dissociate into HM- and M2- species. The three species (H2M, HM- and M2-) exist in the solution at varying concentrations that depend on the pH of the solution. a) Calculate the values of α1 (alpha 1) and α3 (alpha 3). b) Calculate the concentration of HM- in the above solution.Full acid, HOOC = CH-COOH is a biphatic acid and we will label it as H2M. Acid constant data for the two protonation phases of the acid: K H.M+H2O = H, 0++HM- HM +H2O = H, 0++M2– a1 = 1.3x10-2 K.2 = 5.9 x 10-7 Measure 0.1 ml of 0.100 M of malic acid with 0.100M NaOH and measure the H variability as a function of the added base volume. A. Calculate the PH value at the beginning of the titration. B. Calculate the pH value at the first equivalent point. C. Calculate the pH value at the second equivalent point. D. Draw the titration curve in the graph. Indicate in the graph titles and units for the axes.
- Double indicator titration of 1.000g powdered sample containing either alone or any compatible mixture of NaOH/Na2CO3/NaHCO3 and the rest are inert components. The sample was dissolved in 20 ml water then titrated with 0.50 M HCl and reach phenolphthalein endpoint at burette volume of 25.55 ml. Continuing titration, it reached methyl orange endpoint at burette volume of 9.45 ml. Calculate the percentage mass of the possible alkaline component/s.Please determine the equivalence point for each trial. The ones highlighted in yellow are the endpoints. Analyte/Standard acid: 0.1M HCl Titrant/Base: 0.1M NaOHLet'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 ?