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chemistry
organic chemistry

Questions and Answers of Organic Chemistry

Explain why an acid–base reaction favors the weaker acid.
A 1.00-L aqueous solution contained 6.78 g of barium hydroxide, Ba(OH)2. What was the pH of the solution at 25°C?
A certain sample of rainwater gives a yellow color with methyl red and a yellow color with bromthymol blue. What is the approximate pH of the water? Is the rainwater acidic, neutral, or basic? (See
A drop of thymol blue gave a yellow color with a solution of aspirin. A sample of the same aspirin solution gave a yellow color with bromphenol blue. What was the pH of the solution? Was the solution
Identify each of the following as an acid or a base in terms of the Arrhenius concept. Give the chemical equation for the reaction of the substance with water, showing the origin of the acidity or
Which of the following substances are acids in terms of the Arrhenius concept? Which are bases? Show the acid or base character by using chemical equations. a. P4O10 b. K2O c. N2H4 d. H2Se
Write a reaction for each of the following in which the species acts as a Brønsted acid. The equilibrium should favor the product side. a. H2O2 b. HCO3 c. NH4+ d. H2PO4
Write a reaction for each of the following in which the species acts as a Brønsted base. The equilibrium should favor the product side. a. H2O b. HCO3 c. NH3 d. H2PO4
For each of the following, write the complete chemical equation for the acid–base reaction that occurs. Describe each using Brønsted language (if appropriate) and then using Lewis language (show
For each of the following, write the complete chemical equation for the acid–base reaction that occurs. Describe each using Brønsted language (if appropriate) and then using Lewis language (show
Complete the following proton-transfer reaction. Decide on the basis of relative acid strengths whether the reaction is more likely to go in the direction written or in the opposite direction.
Give two important factors that determine the strength of an acid. How does an increase in each factor affect the acid strength?
Complete the following reaction. Decide on the basis of relative acid strengths whether the reaction is more likely to go in the direction written or in the opposite direction.
List the following compounds in order of increasing acid strength: HBr, H2Se, H2S.
List the following compounds in order of increasing acid strength: HBrO2, HClO2, HBrO.
A solution is 0.25 M KOH. What are the concentrations of H3O+ and OH in this solution?
A solution is 0.35 M Sr(OH)2. What are the concentrations of H3O+ and OH in this solution?
A wine has a hydronium-ion concentration equal to 1.5 × 10–3 M. What is the pH of this wine?
A sample of lemon juice has a hydronium-ion concentration equal to 2.5 × 10–2 M. What is the pH of this sample?
A sample of apple cider has a pH of 3.15. What is the hydroxide-ion concentration of this solution?
A sample of grape juice has a pH of 4.05. What is the hydroxide-ion concentration of this solution?
A 2.500-g sample of a mixture of sodium hydrogen carbonate and potassium chloride is dissolved in 25.00 mL of 0.437 M H2SO4. Some acid remains after treatment of the sample. a. Write both the net
Lactic acid, HC3H5O3, is found in sour milk, where it is produced by the action of lactobacilli on lactose, or milk sugar. A 0.025 M solution of lactic acid has a pH of 2.75. What is the ionization
What is the concentration of formate ion, CHO2, in a solution at 25°C that is 0.10 M HCHO2 and 0.20 M HCl? What is the degree of ionization of formic acid, HCHO2?
One liter of solution was prepared by dissolving 0.025 mol of formic acid, HCHO2, and 0.018 mol of sodium formate, NaCHO2, in water. What was the pH of the solution? Ka for formic acid is 1.7 × 10-4.
What is the pH of a buffer prepared by adding 30.0 mL of 0.15 M HC2H3O2 (acetic acid) to 70.0 mL of 0.20 M NaC2H3O2 (sodium acetate)?
Suppose you add 50.0 mL of 0.10 M sodium hydroxide to 1 L of the solution described in Exercise 16.11. What would be the pH of the result?
What is the pH of a solution in which 15 mL of 0.10 M NaOH has been added to 25 mL of 0.10 M HCl?
What is the pH at the equivalence point when 25 mL of 0.10 M HF is titrated by 0.15 M NaOH?
An 80.0-mL sample of 0.200 M ammonia is titrated with 0.100 M hydrochloric acid. Kb for ammonia is 1.8 × 10-5. Calculate the pH of the solution at each of the following points of the titration: a.
What are the concentrations of hydrogen ion and acetate ion in a solution of 0.10 M acetic acid, HC2H3O2? What is the pH of the solution? What is the degree of ionization? See Table 16.1 for the
What is the pH of an aqueous solution that is 0.0030 M pyruvic acid, HC3H3O3? (Pyruvic acid forms during the breakdown of glucose in a cell.)
Sulfurous acid, H2SO3, is a diprotic acid with Ka1 = 1.3 × 10-2 and Ka2 = 6.3 × 10-8. The acid forms when sulfur dioxide (a gas with a suffocating odor) dissolves in water. What is the pH of a 0.25
Quinine is an alkaloid, or naturally occurring base, used to treat malaria. A 0.0015 M solution of quinine has a pH of 9.84. The basicity of alkaloids is due to a nitrogen atom that picks up protons
What is the hydronium-ion concentration of a 0.20 M solution of ammonia in water? See Table 16.2 for Kb.
Consider solutions of the following salts: a. NH4NO3; b. KNO3; c. Al(NO3)3. For each, state whether the solution is acidic, basic, or neutral.
Calculate the following, using Tables 16.1 and 16.2:a. Kb for F;b. Ka for C6H5NH3+ (conjugate acid of aniline, C6H5NH2).
Benzoic acid, HC7H5O2, and its salts are used as food preservatives. What is the concentration of benzoic acid in an aqueous solution of 0.015 M sodium benzoate? What is the pH of the solution? Ka
You have prepared dilute solutions of equal molar concentrations of HC2H3O2 (acetic acid), HNO2, HF, and HCN. Rank the solutions from the highest pH to the lowest pH. (Refer to Table 16.1.)
A base B is placed into a beaker of water with the result depicted below (water molecules have been omitted for clarity). Write the ionization reaction for this base and classify the base as being
Which of the following aqueous solutions has the highest pH and which has the lowest? a. 0.1 M NH3; b. 0.1 M NH4Br; c. 0.1 M NaF; d. 0.1 M NaCl
You add 1.5 mL of 1 M HCl to each of the following solutions. Which one will show the least change of pH? a. 15 mL of 0.1 M NaOH b. 15 mL of 0.1 M HC2H3O2 c. 30 mL of 0.1 M NaOH and 30 mL of 0.1 M
The beaker on the left below represents a buffer solution of a weak acid HA and its conjugate base, A. (Water molecules and spectator ions have been omitted for clarity.) a. Which beaker on the
Write an equation for the ionization of hydrogen cyanide, HCN, in aqueous solution. What is the equilibrium expression Ka for this acid ionization?
Do you expect a solution of anilinium chloride (aniline hydrochloride), C6H5NH3Cl, to be acidic or basic? (Anilinium chloride is the salt of aniline and hydrochloric acid.) Write the equation for the
Calculate the base-ionization constants for PO43 and SO42. Which ion is the stronger base?
Calculate the pH of a 0.15 M aqueous solution of aluminum chloride, AlCl3. The acid ionization of hydrated aluminum ion is and Ka is 1.4 × 10-5.
Calculate the pH of a 0.15 M aqueous solution of zinc chloride, ZnCl2. The acid ionization of hydrated zinc ion is and Ka is 2.5 × 10-10.
An artificial fruit beverage contains 11.0 g of tartaric acid, H2C4H4O6, and 20.0 g of its salt, potassium hydrogen tartrate, per liter. What is the pH of the beverage? Ka1 = 1.0 × 10–3.
A buffer is made by dissolving 13.0 g of sodium dihydrogen phosphate, NaH2PO4, and 15.0 g of disodium hydrogen phosphate, Na2HPO4, in a liter of solution. What is the pH of the buffer?
Blood contains several acid–base systems that tend to keep its pH constant at about 7.4. One of the most important buffer systems involves carbonic acid and hydrogen carbonate ion. What must be the
Codeine, C18H21NO3, is an alkaloid (Kb = 6.2 × 10-9) used as a painkiller and cough suppressant. A solution of codeine is acidified with hydrochloric acid to pH 4.60. What is the ratio of the
Calculate the pH of a solution obtained by mixing 456 mL of 0.10 M hydrochloric acid with 285 mL of 0.15 M sodium hydroxide. Assume the combined volume is the sum of the two original volumes.
Calculate the pH of a solution made up from 2.0 g of potassium hydroxide dissolved in 115 mL of 0.19 M perchloric acid. Assume the change in volume due to adding potassium hydroxide is negligible.
Find the pH of the solution obtained when 25 mL of 0.065 M benzylamine, C7H7NH2, is titrated to the equivalence point with 0.050 M hydrochloric acid. Kb for benzylamine is 4.7 × 10-10.
What is meant by the common-ion effect? Give an example.
What is the pH of the solution obtained by titrating 1.24 g of sodium hydrogen sulfate, NaHSO4, dissolved in 50.0 mL of water with 0.175 M sodium hydroxide until the equivalence point is reached?
Ionization of the first proton from H2SO4 is complete (H2SO4 is a strong acid); the acid ionization constant for the second proton is 1.1 × 10–2. (a) What would be the approximate hydronium-ion
Ionization of the first proton from H2SeO4 is complete (H2SeO4 is a strong acid); the acid ionization constant for the second proton is 1.2 × 10–2. (a) What would be the approximate hydronium-ion
Methylammonium chloride is a salt of methylamine, CH3NH2. A 0.10 M solution of this salt has a pH of 5.82. a. Calculate the value for the equilibrium constant for the reaction b. What is the Kb
Sodium benzoate is a salt of benzoic acid, C6H5COOH. A 0.15 M solution of this salt has a pOH of 5.31 at room temperature. a. Calculate the value for the equilibrium constant for the reaction b.
Each of the following statements concerns a 0.010 M solution of a weak acid, HA. Briefly describe why each statement is either true or false. a. [HA] is approximately equal to 0.010 M. b. [HA] is
Each of the following statements concerns a 0.10 M solution of a weak organic base, B. Briefly describe why each statement is either true or false. a. [B] is approximately equal to 0.10 M. b. [B] is
A 0.288-g sample of an unknown monoprotic organic acid is dissolved in water and titrated with a 0.115 M sodium hydroxide solution. After the addition of 17.54 mL of base, a pH of 4.92 is recorded.
A 0.239-g sample of unknown organic base is dissolved in water and titrated with a 0.135 M hydrochloric acid solution. After the addition of 18.35 mL of acid, a pH of 10.73 is recorded. The
(a) Draw a pH titration curve that represents the titration of 50.0 mL of 0.10 M NH3 by the addition of 0.10 M HCl from a buret. Label the axes and put a scale on each axis. Show where the
The pH of 0.10 M CH3NH2 (methylamine) is 11.8. When the chloride salt of methylamine, CH3NH3Cl, is added to this solution, does the pH increase or decrease? Explain, using Le Châtelier's principle
(a) Draw a pH titration curve that represents the titration of 25.0 mL of 0.15 M propionic acid, CH3CH2COOH, by the addition of 0.15 M KOH from a buret. Label the axes and put a scale on each axis.
The equilibrium equations and Ka values for three reaction systems are given below.a. Which conjugate pair would be best for preparing a buffer with a pH of 2.88?
The equilibrium equations and Ka values for three reaction systems are given below.a. Which conjugate pair would be best for preparing a buffer with a pH of 6.96? Why?
A 25.0-mL sample of hydroxylamine is titrated to the equivalence point with 35.8 mL of 0.150 M HCl.
A 25.00-mL sample contains 0.562 g of NaHCO3. This sample is used to standardize an NaOH solution. At the equivalence point, 42.36 mL of NaOH has been added. a. What was the concentration of the
A solution made up of 1.0 M NH3 and 0.50 M (NH4)2SO4 has a pH of 9.26. a. Write the net ionic equation that represents the reaction of this solution with a strong acid. b. Write the net ionic
A solution is prepared from 0.150 mol of formic acid and enough water to make 0.425 L of solution. a. Determine the concentrations of H3O+ and HCOO in this solution. b. Determine the H3O+
An important component of blood is the buffer combination of dihydrogen phosphate ion and the hydrogen phosphate ion. Consider blood with a pH of 7.44. a. What is the ratio of [H2PO4–] to
An important component of blood is the buffer combination of bicarbonate ion and carbonic acid. Consider blood with a pH of 7.42. a. What is the ratio of [H2CO3] to [HCO3]? b. What does the pH
Tartaric acid is a weak diprotic fruit acid with Ka1 = 1.0 × 10–3 and Ka2 = 4.6 × 10–5. a. Letting the symbol H2A represent tartaric acid, write the chemical equations that represent Ka1 and
Define the term buffer. Give an example.
Malic acid is a weak diprotic organic acid with Ka1 = 4.0 × 10–4 and Ka2 = 9.0 × 10–6. a. Letting the symbol H2A represent malic acid, write the chemical equations that represent Ka1 and Ka2.
A quantity of 0.25 M sodium hydroxide is added to a solution containing 0.15 mol of acetic acid. The final volume of the solution is 375 mL and the pH of this solution is 4.45. a. What is the molar
A quantity of 0.15 M hydrochloric acid is added to a solution containing 0.10 mol of sodium acetate. Some of the sodium acetate is converted to acetic acid, resulting in a final volume of 650 mL of
How is acid rain defined? What is the source of the low pH of acid rain?
A 30.0-mL sample of 0.05 M HClO is titrated by a 0.0250 M KOH solution. Ka for HClO is 3.5 × 10-8. Calculate (a) The pH when no base has been added; (b) The pH when 30.00 mL of the base has been
A 0.108 Msample of a weak acid is 4.16% ionized in solution. What is the hydroxide concentration of this solution?
A generic base, B, is added to 2.25 L of water. The pH of the solution is found to be 10.10. What is the concentration of the base B in this solution? Ka for the acid HB at 25°C is 1.99 × 10-9.
Calculate the pH of a solution made by mixing 0.60 L of 0.10 M NH4Cl with 0.50 L of 0.10 M NaOH. Kb for NH3 is 1.8 × 10-5.
Cyanic acid, HOCN, is a weak acid with a Ka value of 3.5 × 10-04 at 25°C. In a 0.293 M solution of the acid, the degree of ionization is 3.5 × 10-02. Calculate the degree of ionization in a 0.293
What is meant by the capacity of a buffer? Describe a buffer with low capacity and the same buffer with greater capacity.
The Kb for NH3 is 1.8 × 10-5 at 25°C. Calculate the pH of a buffer solution made by mixing 65.1 mL of 0.142 M NH3 with 39.2 mL of 0.172 M NH4Cl at 25°C. Assume that the volumes of the solutions
Ka for formic acid is 1.7 × 10-4 at 25°C. A buffer is made by mixing 529 mL of 0.465 M formic acid, HCHO2, and 494 mL of 0.524 M sodium formate, NaCHO2. Calculate the pH of this solution at 25°C
Ka for acetic acid is 1.7 × 10-5 at 25°C. 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 25°C after
Calculate the pH of a solution made by mixing 7.52 mL of 4.9 × 10-2 M Ca(OH)2 with 22.5 mL of 0.11 M HCl.
A 0.150 M solution of NaClO is prepared by dissolving NaClO in water. A 50.0-mL sample of this solution is titrated with 0.100 M HCl. Calculate the pH of the solution at each of the following points
The pH of a white vinegar solution is 2.45. This vinegar is an aqueous solution of acetic acid with a density of 1.09 g/mL. What is the mass percentage of acetic acid in the solution?
The pH of a household cleaning solution is 11.87. This cleanser is an aqueous solution of ammonia with a density of 1.00 g/mL. What is the mass percentage of ammonia in the solution?
What is the freezing point of 0.92 M aqueous acetic acid? The density of this solution is 1.008 g/cm3.
What is the freezing point of 0.87 M aqueous ammonia? The density of this solution is 0.992 g/cm3.
A chemist needs a buffer with pH 4.35. How many milliliters of pure acetic acid (density = 1.049 g/mL) must be added to 465 mL of 0.0941 M NaOH solution to obtain such a buffer?
Describe the pH changes that occur during the titration of a weak base by a strong acid. What is meant by the term equivalence point?
A chemist needs a buffer with pH 3.50. How many milliliters of pure formic acid (density = 1.220 g/mL) must be added to 325 mL of 0.0857 M NaOH solution to obtain such a buffer?

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