In a lab, dissociation constant, K, of an acid-base indicator is measured. A 1.00 x 104 M solution of the indicator buffered at pH 6.00 shows an absorbance of 0.26 at 520 nm in a 1.00-cm cuvette. Given the acidic form of this indicator has a molar absorptivity of 5000 and its basic form has a molar absorptivity of 150O L cm1 mol1, K, is found to be

In a lab, dissociation constant, K, of an acid-base indicator is measured. A 1.00 x 104 M solution of the indicator buffered at pH 6.00 shows an absorbance of 0.26 at 520 nm in a 1.00-cm cuvette. Given the acidic form of this indicator has a molar absorptivity of 5000 and its basic form has a molar absorptivity of 150O L cm1 mol1, K, is found to be

Chemistry

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Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 132IP: A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in...

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A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
A 0.400-M solution of ammonia was titrated with hydrochloric acid to the equivalence point, where the total volume was 1.50 times the original volume. At what pH does the equivalence point occur?
Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
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.
K4 for acetic acid is 1.7 105 at 25C. A buffer solution is made by mixing 52.1 mL of 0.122 M acetic acid with 46.1 mL of 0.182 M sodium acetate. Calculate the pH of this solution at 25C after the addition of 5.82 mL of 0.125 M NaOH.
A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
In the titration of 50.00 mL 0.0200M weak base B using 0.0150 M HCI, which indicator is the best one to be used? (pK, of the weak base B is 10.50). Indicator 4: Thymolthalein: pH transition = 8.5-10.5 OIndicator 5: Indigo Carmine: pH transition= 11.6- 14.0 Indicator 3: Cresol red: pH transition 7.2-8.8 Indicator 1: Cresol purple: pH transition = 1.2-2.8 Indicator 2: Methyl red: pH transition = 4.8-6.0
The indicator methyl red has a pKHIn = 4.95. It changes from red to yellow over the pH range from 4.4 to 6.2. If the indicator is placed in a colourless buffer solution of pH = 4.55, what percent of the indicator will be present in the acid form, HIn?
A professor prepares a buffer solution that they need for the purification of protein from human cell lysates. They did mix weak acid and conjugate base and obtained the initial solution, which is characterised by these parameters. Final volume: 200mltotal buffer compound concentration: 150mMIntitial concentration weak acid: 0.03MInitial concentration conjugate base: 0.12MInitial pH 6.9buffer compound pka 6.3
What molar ratio of base/salt is required to prepare an ammoniaammonium chloride buffer solution having a pH of 11.0? The Kbvalue of ammonia ammonia is 1.80 x 10-5 at 250C. Also express theresult in mole percent. The molar ratio of Sodium acetate to acetic acid in a buffer solutionhaving a pH of 5.76 is 10:1. Assuming that the total bufferconcentration is 2.2 x 10 -2 mole /liter, how many grams of sodiumacetate (MW=82g/mole) and how many grams of acetic acid(MW=60g/mole) should be used in preparing a liter of the solution?
Nites

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