1. Indicator dyes are often used to measure the hydrogen-ion concentration. From the measured spectra of an indicator in solution, the ratio of acid to base species and the pH can be calculated: Hin In + H* The molar extinction coefficients are the following: Hin E (300 nm) 10,000 E (400 nm) 2000 In 500 4000 (a) Calculate the ratio of concentrations [In-]/[HIn] for a solution of the indicator that has A (300 nm) = 1.2 in a 1-cm cell and A(400 nm) = 0.7 in a 0.1-cm cell. (b) What is the pH if the pK of the indicator is 5.0?
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- Q4. The acid base indicator HIn undergoes the following reaction in dilute aqueous solution 10 H+ + In HIn When a 5x10-4 M solution of HIn put in 0.1 M NaOH and in 0.1 M HCl, the following data were obtained. Note that all the indicator will be existing as HIn in 0.1 M HCl and existing as In in NaOH, Solution 0.1 M NaOH 0.1 M HCI A at 485 nm 0.052 0.454 A at 625 nm 0.823 0.176 Calculate a) The molar absorptivity of HIn and In" at 485 and 625 nm b) The acid dissociation constant (Ka) if a small amount of the indicator at pH 5 gave A = 0.472 at 485 nm and A = 0.351 at 625 nm.3. Complete neutralization of 10 ml of phosphoric acid solution by NaOH 0.I N in the presence of phenol phthalein until the appearance of purple color (pH, = 9) 11 ml. of NaOH is consumed. (a) What is the concentration of phosphoric acid? (b) Calculate the indicator error. pk2.1 pK. - 7.2 pK - 124Please complete the calculation of the pH of the equivalence point below. Concentration of NaOH solution = 0.1 mol dm-3. Mean titre (NaOH solution) = 18.95 cm3. Amount of NaOH = 0.00189 moles. Molar ratio of NaOH:aspirin = 1:1. Amount of aspirin = 0.00189 moles. Mass of aspirin (in titration) = 0.341 g. |Mass of aspirin (per tablet) = 0.341 g.
- For sulfurous acid, H2SO3, the two dissociation constants are: KI=1.25x10-2 and KII= 5.6x10-8. Calculate the concentration of all species in a solution for a concentration of 0.5M NaHSO3.182 183 134 185 F A B E D C 1. Using calculated molarity of acid (line 3, Table 2) and measured pH of the acid before titration (line5,table 1)use a RICE table and Henderson-Hasselbalch equation to calculate the Ka of the acid. Compare the results of your calculations with the graphical 186 187 188 400 190 191 192 193 195 Reaction Initial conc. / M: Change in conc. at equilibrium /M: Equilibrium conc. / M: pH HA(aq) + H₂O(l) 0.1979 2.946990323 -2.2E-04 2. Use your data and the Henderson-Hasselbalch pH=pka + log[A]/[HA] and 1.98E-01 Ka = 2.5E-07 pKa pH-log[A]/[HA] = pka H3O*(aq) 0 5.9E+00 2.2E-04 2.2E-04 + equation to perform the calculation and find Ka at any pH during titration. Ka = 10 Ka A (aq) Ꮕ Ka 2.2E-04 2.2E-04 1.3E-06 Hints: Use ExCommercial phosphate buffers are sold to maintain fish tanks at a pH of 7. Use a table of acid dissociation equilbrium constants to find all the K, values for H, PO,. AjA BIUS Calculate the pka values from the Ka values. Remember that pX = -logX. pKi = pK = pk3 = What two chemical species are primarily found in solution in a phosphate buffer with a pH of 7? о Н РО, аnd PО H,PO, and HPo HPO; and PO- о Н РО, and H,РО,
- When 2.3 moles of HBrO2 is dissolved in 2 liters of solution it is found at equilibrium that [H3O+] = . 067, calculate ki for HBrO2Explain why the indicator cresol red changes color when the pH is lowered from 10 to 6. What colors will be observed at pH 10, 8, and 6? Why does the color transition require ,2 pH units for completion?2. DETAILS PREVIOUS ANSWERS NCSUGENCHEM202LABV1 7.POST.02. Given that carbonic acid, H₂CO3, has a pka1 = 6.37 and a pka2 = 10.33, answer the following. (a) If you wanted to make a pH 7 buffer solution starting with NaHCO3(aq), would you add 0.10 M HCl or 0.10 M NaOH? O 0.10 M HCI 0.10 M NaOH (b) If you began with 7.0 mL of 0.17 M NaHCO3, how many mL of your choice from (a) would you need to add to get a pH 7 buffer? 3.94 XML
- 1. Calculate [H+], [OH-], pH and pOH of:a. 0.1 M HNO3 b. 2.00 M (weak acid) HF (Ka=6.8 x 10^-4) 2. In the preparation of the standard curve for protein analysis, 50 mnBSA (bovine serum albumin) dissolved in H2O to a final volume of 5mL was used as stock solution. What is the weight of BSA in 0.1 mL ofstock solution? In 0.2 mL? 3. . The above mentioned aliquots (#9) which were diluted with enoughwater to a final volume of 1 mL were assayed colorimetrically andyielded the following absorbance readings:mL stock mL H2O Absorbance0.2 0.8 0.1000.4 0.6 0.2000.6 0.4 0.3000.8 0.2 0.4001.0 0.0 0.500 i. Tabulate mg BSA vs. absorbance readingii. Draw the curve where mg BSA is on x-axis and absorbance ony-axis (use graphing paper).iii. Calculate the slope of the curveiv. If a sample solution has an…Prepared buffer solution GivenAmmonia Volume = 68 mL | Ammonia Concentration = 0.17 MAmmonium Chloride Volume = 42 mL | Ammonium Chloride Concentration = 0.13 MDissociation Constant of Ammonia: 1.8x10-5What is the final concentration of the baseC6H4NH₂COOH, para-aminobenzoic acid (PABA) is used in some sunscreens. Calculate the concentrations of hydronium ion and para-aminobenzoate ion, C6H4NH₂COO- in a 0.055 mol dm-³ solution of the acid. Ka-2.2 x 10-5