2. 20.0 mL of 0.1000 M Benzoic Acid (HC7H5O2) in a flask is being titrated with 0.1000 M NaOH contained in a burette. Show clearly by calculations the final pH at the end of each of scenario. (ka = 6.4 x 10 5) 1. When no NaOH was added to the acid in the flask.
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- A biochemist needs 750 mL of an acetic acid–sodiumacetate buffer with pH 4.50. Solid sodium acetate(CH3COONa) and glacial acetic acid (CH3COOH) areavailable. Glacial acetic acid is 99% CH3COOH by massand has a density of 1.05 g/mL. If the buffer is to be 0.15 Min CH3COOH, how many grams of CH3COONa and howmany milliliters of glacial acetic acid must be used?If 21.6 mL of 0.107 M acid with a pKa of 5.16 is titrated with 0.105 M NaOH solution, what is the pH of the titration mixture at halfway to the equivalence point?A chemist titrates 120.0mL of a 0.5279M hydrocyanic acid HCN solution with 0.7646M KOH solution at 25°C. Calculate the pH at equivalence. The pKa of hydrocyanic acid is 9.21.
- For Ca2+ and Mg2+ determinations in a tap water sample, two 50 mL aliquots were pipetted and placed in different Erlenmeyer flasks. The first of them had the pH adjusted to 12 (Ca2+ titration) and the second to 10 (Ca2+ +Mg2+ titration). The volumes of EDTA (5.07*10-3 mol/L) used in the first and second titrations were 2.40 and 4.80 mL, respectively. Calculate: a) The concentration of Ca2+ in mg/L in the water sampleb) The concentration of Mg2+ in mg/L in the water sampleGive typed full explanation not a single word hand written otherwise leave it An experiment requires a pH 6.5 buffer. Solid sodium acetate and glacial acetic acid available. Glacial acetic acid is 99% acetic acid by mass and has a density of 1.05 g/mL. If the buffer is to be 0.20 M in acetic acid, how many grams of NaC2H3O2 and how many milliliters of glacial acetic acid must be used?How will you prepare 500 ml of 0.750 M citrate buffer with pH of 4.25 from solid citric acid (C6H8O7) and solid sodium citrate (Na3C6H5O7).The Ka of citric acid is 7.40 x 10-4
- To create a buffer solution, 40.00mL of a 0.100M benzoic acid (Bz) solution are mixed with 20.00mL of 0.100M sodium hydroxide solution. What is the pH of the resulting solution if the Ka of benzoic acid 6.5 x10 -5 and the pKa = 4.19? (Use the Henderson Hasselbach Equation with mmol). Reaction: HOBz + OH- ---> H2O + OBz- From the buffer solution above, youo take a 10.00mL portion of the buffer. Using all of the information provided, how much conjugate acid and conjugate base are in the 10.00mL portion that you took out? Group of answer choices 0.167mmol 0.500mmol 0.222mmol 0.333mmolIf 40.0 mL of formic acid with a concentration of 0.300 M and a Ka of (2.258x10^-5) is titrated with 0.300 M lithium hydroxide what is the pH of the solution after 20.00 ml of base has been added? Note: Your answer is assumed to be reduced to the highest power possible.A. How would you prepare 1.5L of a buffer of pH = 4.00 using 0.25M formic acid and solid sodium salt of theacid? (ignore volume changes) In your answer, indicate the volume of solution you would use and the mass of thesalt you would use. Show all calculations. In order to make the buffer, B. What would the pH of a 50.00 mL sample of the buffer be after the addition of:i. 25.0mL 0.25M NaOH pH = ii. 50.0 mL 0.025M HCl pH =
- A 50.00-mL sample of a 1.00 M solution of the diprotic acid H2A (Ka1 = 1.0 × 10–6 and Ka2 = 1.0 × 10–10) is titrated with 2.00 M NaOH. How many mL of 2.00 M NaOH must be added to reach a pH of 12? Give answer in 15 min.Consider the titration of 20 mL of 0.10 M base with 0.20 M HCl. The analyte is dibasic withpKb1 = 5.00 and pKb2 = 10.00. Calculate the pH at the following volumes of HCl0 mL, 5 mL, 10 mL, 15 mL, 20 mL50 mL sample solution containing Na2CO3 and NaOH is titrated with 0.2 M HCl solution. In the presence of phenolphthalein indicator, the acid consumption is 15 mL. Then, the titration is continued by adding bromocresol green indicator, and in the presence of this indicator, the acid consumption is 10 mL. Accordingly, which of the following is the amount of Na2CO3 (in grams) in the sample? (NaOH: 40 g / mol; NazCO3: 106 g / mol)