A 1.2 g sample of mixture of NaOH and Na:CO, containing inert impurities s dissolved and titrated cold with 0.5N HCI. With phenolphthalein as indicator the solution turns colorless after the addition of 30.0 ml of the acid. Methyl orange is then added and 12 ml more of the acid is required before this inclicator changes color. What is the percentage of NaOH and of Na;CO, in the sample ? 5.

A 1.2 g sample of mixture of NaOH and Na:CO, containing inert impurities s dissolved and titrated cold with 0.5N HCI. With phenolphthalein as indicator the solution turns colorless after the addition of 30.0 ml of the acid. Methyl orange is then added and 12 ml more of the acid is required before this inclicator changes color. What is the percentage of NaOH and of Na;CO, in the sample ? 5.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 93QRT: When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence...

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Marble is almost pure CaCO3. Acid rain has a devastating effect on marble statuary left outdoors. Assume that the reaction which occurs is CoCO3(s)+ H+(aq)Ca2+(aq)+HCO3(aq) Neglecting all other competing equilibria and using Tables 15.1 and 13.2, calculate (a) K for the reaction. (b) the molar solubility of CaCO3 in pure water. (c) the molar solubility of CaCO3 in acid rainwater with a pH of 4.00.
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 buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?
Calculate the pH change when 10.0 mL of 0.100-M NaOH is added to 90.0 mL pure water, and compare the pH change with that when the same amount of NaOH solution is added to 90.0 mL of a buffer consisting of 1.00-M NH3 and 1.00-M NH4Cl. Assume that the volumes are additive. Kb of NH3 = 1.8 × 10-5.
Methyl red has a pk, of 5.0 and is red in its acid form and yellow in its basic form. If several drops of this indicator are placed in a 25.0-mL sample of 0.100 M HCI, what color will the solution appear? If 0.100 M NaOH is slowly added to the HCI sample, in what pH range will the indicator change color?
pH of solution made by mixing 200 mL of 0.2 M CH3COONa and 400 mL 0.1 M CH3COOH is [pKa(CH3COOH) = 4.7] %3D 3.2 4.7 5.2 6.8
In an air pollution analysis, 3 L of polluted air is passed through 50 mL of 0,0116 M Ba(OH)2 solution and the carbon dioxide (CO2) in it is precipitated as BaCO3. The excess of the base is titrated with 23.6 mL 0.0108 M HCl in addition to the phenol phthalate indicator. Calculate the CO2 concentration in this air sample in ppm.(Take the density of CO2 as 1.98 g/L, C=12, O=16 g/mol).
25.0 mL of 0.25 M HCN (for HCN; Ka = 6.2 x 10-10) sample is titrated with 0.50 M NaOH. Calculate the pH of the mixture, a) at the half equivalence point. b) List the major species in equilibrium in part (a) c) at the equivalence point. d) after adding 20.0 mL of 0.50 M NaOH.
A white solid dissolves in water to form a neutral solution. No precipitate forms when this solu- tion is treated with a solution of NH Cl/NH, buffer, nor when (NH),S is added. When the solu- tion is acidified with HC,H,0, and K,CrO, is added, a yellow precipitate forms. This precipitate dissolves upon addition of concentrated HCl. Acidification of a solution of the solid with HNO, followed by addition of AgNO, causes formation of a white precipitate. What is the identity of the original solid? 6.
You are given a solution of 0.20M CoCl3, 0.15M SnCl2, 0.35M CuCl2, and 0.25M AgCl.Giventhe following table, calculatethe hydroxide concentration needed to precipitate each metal individually so they can be recovered. You do not want more than one metal to precipitate at one time or when you filter the precipitate you will get a mixture.(Optional; calculate the volume of a 0.25M NaOH solution needed to cause this precipitation) b.) Hydroxide needed to precipitate Sn(OH)2 c.) Hydroxide needed to precipitate Cu(OH)2 d.) Hydroxide needed to precipitate AgOH
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 titration curve is constructed by plotting the pH of the analyte solution versus the volume ofthe reagent added as the titration progresses. As the equivalence point is approached, there is arapid change in the pH. Titration curves enable us to explain how end points are detected andtheir relationship to equivalence points. They can also serve as guides for choosing the properindicators for a particular acid-base titration. Explain how each plot can be used to interpret the acid-base titration.

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