A Beer's Law graph obtained by plotting absorbance versus concentration in mol/L for a series of standard solutions, produced a straight line with equation y = 2604.1 x Suppose an unknown SCN solution is treated in exactly the same manner as described in Part B of the procedure. The final diluted solution gives an absorbance reading of 0.270. Determine the [FeSCN2+] in this diluted solution. Determine the SCN concentration in the original (undiluted) unknown solution.
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- A 0.9182 g sample of CaBr2 is dissolved in enough water to give 500. mL of solution. What is the bromide ion concentration in this solution? 20 Multiple Cholce X 0206:02 9.19 x 10-3 M 230 x 10-2 M 272 x 10-3 M 1.84 x 10-2 M 1.25 x 10-1 M Mc Graw Hill Type here to search 近 CA solution contains both NaHCO3 and Na2CO3. Titration of a 50.00 mL portion to a phenolphthalein end point requires 21.25 mL of 0.1385 M HCl. A second 50.00 mL aliquot requires 45.48 mL of the HCl solution when titrated to a bromocresol green end point. Calculate the molar concentration of Na2CO3 in the original solution. (Do not include the unit for molarity. Enter your answer to three significant figures.)A 2.4173 g specimen of a drain cleaner is dissolved and diluted to 75 mL with DI water. A 6.00 mL aliquot is titration with 0.1547 M HCl. It requires 24.87 mL of the HCl to reach the phenophthalein end point. a. Compute the molarity of the 6.00 mL aliquot of the solution assuming the alkali and the HCl react in a 1:1 mole ratio. b. Compute number of grams of alkali originally in 75mL flask assuming that the alkali in the drain cleaner is NaOH. c. Computer the weight-% alkali (expressed at wt-% NaOH) in the specimen of drain cleaner.
- What is the equivalence point volume of 0.140 M NAOH required to neutralize 75.0 mL of 0.350 M HCI? O 188 mL O 38.5 mL O 150 mL 75.0 mL O 126 mLWhich is the correct order of steps in the preparation of a hydrochoric acid standard solution with sodium bicarbonate standard solution. I. Dissolved sodium carbonate (13.25 g) in about 150 mL of distilled water in a beaker II. Solution of sodium carbonate was transferred into a volumetric flask and diluted to mark before mixing. III. Weigh the appropriate amount of the primary standard. IV. Titrate with enough volume of the acid to completely neutralize the base. V. Transfer 10.00 ml primary standard into an erlenmeyer flask and add indicator III, I, II, V, IV III, II, I, V, IV V, III, I, II, IV V, IV, III, I, IIHow many moles of CaF2 will dissolve in 2.7 L of 0.041 M NaF solution? (Ksp for CaF2 = 4.4 × 10–11) 2.38×10-8 moles a) 2.38 x 10^-8 b) 8.81×10^-9 moles c) 6.43×10^-8 moles d) 1.02×10^-9 moles e) 2.76×10^-9 moles
- A solution contains NaHCO₃, Na₂CO₃, and NaOH either alone or in permissible combination. Titration of 25.00 mL portion to a phenolphthalein end point requires 28.78 mL of 0.1107 M HCl. A second 25.00 mL aliquot requires 41.58 mL of HCl when titrated to a bromocresol green end point. a) Show the diagram analysis of the volume of the titrant required for each end points and components. b) Determine the concentrations in mg/mL of the components of the mixture.A solution contains a mixture of Na2CO3 and NaHCO3. Titration of a 30.0 mL portion of the solution to a phenolphthalein end point requires 12.16 mL of 0.306 M HCl. Another 30.0 mL portion of the solution requires 42.76 mL of the 0.306 M HCl when titrated to a bromocresol green end point. Calculate the molarity of the NaHCO3 in the original solution. Please keep your answer in normal number to three decimal places (x.xxx).In an experiment, it requires 34.2 ml of a NaOH solution to titrate 0.500 g of dissolved KHP (molecular weight = 204.22 g/mol) to the phenolphthalein end point. Calculate the molarity of NaOH solution. 0.0176 M A. 0.0415 M OB. 0.0645 M OC. O D. 0.0716 M 0.0312 M OE.
- 1)Calculate the pH of 650. mL of a 0.439-M solution of hypochlorous acid before and after the addition of 0.196 mol of sodium hypochlorite.pH befor addition = pH after addition = 2)A 9.56×10-2-M aqueous solution of C2H5NH2 (ethylamine) has a pH of 11.8. Calculate the pH of a buffer solution that is 9.56×10-2 M in C2H5NH2 and 0.317 M in C2H5NH3+.pH =Question: pH of 50.0 mL acetate buffer + 1.00 mL 0.6 HCl CH3COO- H3O+ CH3COOH before addition Addition after addition (below is the data to answer the answer) Deionized water Acetate Buffer Ammonia Buffer pH of solution 6.62 4.59 9.49 Ph of solution after addition of 1 mL of 0.6 M NaOH 12.41 4.71 9.50 pH of solution after addition of 1 mL of 0.6 M HCl 1.38 3.87 9.24 Preparation of Buffer solutions Mass of sodium acetate in acetate buffer ~ 1.1981 Volume of 3.0 M acetic acid in acetate buffrer ~ 3.81 Mass of ammonium chloride ~ 1.2721 Volume of 5.0 M NH4OH ~ 6.00% 5 T Nal PbS 16 AgCl LICI FeO 6 KOH Ty & 4- 7 * + 00 [Choose] [Choose] soluble in water NOT soluble in water [Choose] [Choose] [Choose] [Choose ] O ( 9 O Y V f11 U + [ insprt sc ← delete backspa