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- Figure 15-3 outlines the classic scheme for separating a mixture of insoluble chloride salts from one another. Explain the chemistry involved in the various steps of the figure.if concentrations of [H+] in three fluids are 5.2*10-6M, 5.2*10-4M and 5.2*10-2M, what is the pH of each fluid. if the pH level of two fluids are 3.6 and 9.2, what is [H+] for each fluid.Given the chemical equation for the anthocyanin extract of red cabbage as an indicator. HIn + H20 S H;0* + In¯ Using the results from the experiment, identify which of the reactant/product are responsible for the red and green color of the indicator. Notes: solution turns red after adding acid; solution turns blue/green after adding base RED: BLUE/GREEN: Why is the color violet/blue at pH near 7? Answer in 1 sentence. Hint: What is the relationship of the species responsible for the observed colors?
- In the experiment, we used titration to determine the total acid content ofsamples, which we reported in terms of molarity. Reporting acidity through pHmeasurements is quite different, in that we can only measure the amount of theacid in its ionized form. You were tasked to investigate a clear aqueous solutionof an unknown monoprotic acid. You decided to use two methods togather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mLdistilled water. Two drops of phenolphthalein were added and then it was titrated3.54 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 toestimate the pH, which turned out to be around 3.3. Another 1 mL of the samplewas 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 thepH of the sample.c) Using pH strip results,…What is the percentage of total acid expressed as acetic acid in a sample of vinegar if 4.0g of vinegar requires 29.5ml of 0.153N KOH for an endpoint with phenolphthalein indicator? (molar mass of acetic acid: HC2H3O2 = 60.05g/mol a. 3.995% b. 6.776% c. 8.650% d. 12.68%During titration the following data were collected. A 25 mL poretion of an unknown acid soluation was titrated with 1.0 M NaOH. It required 65mL of the base to neutalize the sample. How many moles of acid are present in 3.0 liters of this unknown solution?
- hexamethylenetetramine. Qualitative and quantitative analysis?Consider a solution of 0.00500 M HNO, (K.= 3,98 x 10-4) for nos. 25 - 28. Determine the following: 25. equilibriym molar concentration of H-O* = 0.00141 26. equilibrfummolar concentration of HNO,000359 M. 27. pH = 2.85 28. %ionization =28.2A mixture may contain NaOH, NaHCO3, Na2CO3 or any compatible mixture of these. A sample weighing 0.245 g requires 10.30 mL of 0.0990 N HCl to reach a phenolpthalein endpoint and an additional 26.25 mL to reacha bromcresol green endpoint. a. What are the components of the mixture? Put Yes for the components and NO if the component is not present. a1. NaOH a2. NaHCO3 a3. Na2CO3 b. Determine the composition anf amounts (in w/w) of each components of the mixture. Put 0 for the component which is no present. b1. % NaOH b2. %NaHCO3 b3. %Na2CO3
- Three drops of the phenolphthalein chemical indicator should be added to the acidic analyte sample (KHP or citric acid) before every titration. You will then carefully add the base to the analyte until the solution turns O a. from clear to a very pale pink color. O b. from a pale pink color to totally clear. O. from a dark pink color to totally clear. O d. from clear to a very dark pink color.10:57 H₂O 0.1 NaCl Solution A Solution B Initial pH 7.0 5.D 3.0 10.0 Acid-Base Titration % acidity from vinegar label Molarity of NaOH 2030 Volume of Vinegar (ml) Initial Volume of NaOH (ml) Final Volume of NaOH (mL) Report Table AB.3: Effect of Adding Base pH after 5 Drops NaOH 11.0 9.0 3.0 11.0 Acid/Base Titration, Buffers, and PH Report Sheet pH after 10 Drops NaOH 5% 0.101 Trial 1 Report Table AB.4: Concentration of Acetic Acid in Vinegar 11.0 12.0 3.0 11.0** 5.00 ML 0.00 ML 41.20 ML Total pH Change Trial 2 5,00 ML 000 ML 38.40mL Buffer? (Y or N) Trial 3 Show your calculations for calculating the %(m/v) for acetic acid in vinegar for Trial 1 in Report Table AB.4. X 5.00 ML 0.01 ML 41.30mLCalculate the molar solubility of CaF2 in pure water. Neglect hydrolysis of the fluoride ion. Ksp of CaF2 = 4 x 10-11 Express answer in 2 significant figures. Do not include unit in the answer box. If answer is 1.2 x10-3, write 1.2E-3 If answer is 7.8 x104, write 7.8E4 Answer: