3. An indicator is a dye whose spectrum changes with pH. Consider the following data for the absorption spectrum of an indicator (pK = 4) in its ionized and nonionized form. InH* + In + H* Molar absorptivity, ɛ (M1.cm-1) InH (nm) In 400 10,000 15,000 8,000 420 2,000 8,000 12,000 3,000 440 460 480

ALL INFORMATION NEEDED IS PROVIDED, I NEED FIRST QUESTIONS ANSWERED FIRST BEFORE OTHERS CAN BE ANSWEREDRate = -(Delta[RCl])/Delta t andln[RCl]t=-k*t+ln[RCl]0 < [R-Cl]-time equation Test tube A = 0.30 of 0.10M NaOH(aq), 6.70ml DI H2O & 1 drop of bromophenol bue Test Tube B = 3.00M of 0.10M R-CL in acetone. Mix together in 3 water baths Bath A Trial 1= 20C, 53.6s Trial 2= 20C, 49s for color to changeBath B Trial 1= 32C, 18s Trail 2= 32C, 20s Bath C Trial 1= 10C, 204s Trial B= 10C, 200s average out both trials for each bathcolor change happens after 10% of R-Cl has reacted so In terms of R-Cl this means that 10% of the R-Cl has reacted and ____ of the R-Cl is left Q1. at the time of the color change [R-Cl]t=____[R-Cl]o (Fill in the blank) Q4. Substitute the value of [R-Cl]t into appropriate equation listed above and solve for k in terms of [R-Cl] and t. Q5. Use average time for each temp and determine the value of k (with units) at each temperature Q6. Rearrange the Arrhenius…

Data The following tables include calculated as well as observed and recorded data for Part 1 and Part 2 of the pH study experiment. System I 0.0010 М HC 0.010 М НСl 0.00010 M HCI 0.0010 M NaOH Calculated pH Indicator pH 2 3 4 Meter pH 1.88 2.62 3.25 9.46 System II 0.010 МНАс 0.0010 M HAC 0.00010 M HAC 0.0010 M NH, Calculated pH Indicator pH 3.5 4 8 Meter pH 3.26 3.65 3.67 9.51

9-10. (a) Find the pH of a solution prepared by dissolving 1.00 g of glycine amide hydrochloride plus 1.00 g of glycine amide in 0.100 L. + Cl- H3N H2N. NH2 NH2 Glycine amide hydrochloride (BH†) FM 110.54, pK, = 8.20 Glycine amide (B) FM 74.08 (b) How many grams of glycine amide should be added to 1.00 g of glycine amide hydrochloride to give 100 mL of solu- tion with pH 8.00? (c) What would be the pH if the solution in (a) is mixed with 5.00 mL of 0.100 M HC1? (d) What would be the pH if the solution in (c) is mixed with 10.00 mL of 0.100 M NaOH?

atWhat is [H30+] in a solution of 0.25 M CH3CO2H and 0.030 M NaCH3CO2? CH3CO,H(aq) + H,0(1) E H30*(aq) + CH3CO,¯(aq) Ka = = 1.8 × 10-5

4. The molar absorptivities of the indicator weak acid HIn (K₁ = 1.42 x 105) and its conjugate base In at 570 were determined as ε(HIn) = 7120 and ɛ(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%. (b) What is the absorbance of a buffered indicator solution having total indicator concentration 8.0 x 105 and pH = 6.5.

Please answer A & B pH  See full Question.

Subject- chemistry

✓ ?? 14. Two groups of students were asked to check the concentration of ammonia in a particular brand of cleaning product because there had been complaints about that brand. The students placed a 25.0mL sample of cleaning product in a volumetric flask and made it up to 250mL using distilled water. They then performed a titration by using 25.0mL of the diluted ammonia solution in a conical flask and 0.10 moll-¹ standardised hydrochloric acid in a burette. One group used bromocresol green (pH range 4.0-5.6) as the indicator and obtained the following results: Titration Volume of acid 1st 23.2 added (mL) 2nd 22.9 3rd 22.8 4th 22.9 a) Calculate the concentration of the diluted sample. b) Calculate the concentration of ammonia in 1L of the original sample.

Calculate the pH of a saturated solution of Mg(OH)2. Ksp [Mg(OH)2] = 1.8 × 10-¹1. Express your answer to two decimal places. View Available Hint(s) pH = Submit IVE ΑΣΦ ?