Question: A buffer solution is prepared in such
A buffer solution is prepared in such a way that the concentration of propanoic acid is 2.00 3 1021 M and the concentration of sodium propanoate is 4.00 3 1021 M. If the buffer equilibrium is described by 
Ka = 1.34 × 10-5 use the Henderson-Hasselbalch equation to calculate the pH of the solution.
Transcribed Image Text:
C,H;COOH(aq) + H2O(1)=H,O* (aq) + C,H;COO (aq) Propanoic acid Propanoate anion
> Calculate the number of mol corresponding to: a. 15.0 g NH3 b. 16.0 g O2
> For gasoline, isooctane, 2,2,4-trimethylpentane, is the standard of excellence. Write a balanced equation for the complete combustion of isooctane.
> Why are ionic substances more likely to be water-soluble?
> Suggest a protocol for radioactive waste disposal.
> Would the use of concrete rather than wood paneling help to protect workers in other parts of the clinic? Why?
> Would wearing a lab apron lined with thin sheets of lead have a positive effect? Why?
> Would wearing gloves have any significant effect? Why?
> Why do high-altitude jet flights increase a person’s exposure to background radiation?
> Radioactive molybdenum-99 is used to produce the tracer isotope, technetium-99m. Write a nuclear equation for the formation of molybdenum-99 from stable molybdenum- 98 bombarded with neutrons.
> Describe an application of each of the following isotopes: a. iodine-131 b. thallium-201
> Describe how medically useful isotopes may be prepared.
> Calculate the number of ATP molecules produced by the complete b-oxidation of eicosanoic acid.
> Describe how radioactive tracers are used in the diagnosis of disease.
> What type of nuclear reaction fuels our solar system?
> In what way are beta particles and positrons similar?
> Why are cadmium rods used in a fission reactor?
> What are the major disadvantages of a fission reactor for electrical energy production?
> Which type of nuclear process combines small nuclei to release energy?
> What property of carbon enables us to assess the age of a painting?
> The hydronium ion concentration in the blood of three different patients was: Patient.. [H3O1] A.. 5.0 x 10-8 B. 3.1 x10-8 C.. 3.2 x 10-8
> A patient receives 9.0 ng of a radioisotope with a half-life of 12 h. How much will remain in the body after 2.0 days, assuming that radioactive decay is the only path for removal of the isotope from the body?
> Would you predict lithium-9 to be stable? Explain your reasoning.
> Note the major accomplishment of each of the following: a. Thomson b. Rutherford c. Geiger d. Bohr
> Would you predict cobalt-59 to be stable? Explain your reasoning.
> Phosphorus-31, known to bioaccumulate in the liver, decays by beta emission. Write a balanced nuclear equation for this process.
> Cobalt-60 has a half-life of 5.3 years. How many half-lives occur after 21.2 years?
> Explain why the binding energy of a nucleus is expected to be large.
> Element 106 was named seaborgium (Sg) in honor of Glenn T. Seaborg, a pioneer in the discovery of lanthanide and actinide elements. Seaborgium-263 decays by alpha emission. Write a balanced nuclear equation for this process.
> Write a balanced nuclear equation for positron emission by manganese-52.
> Write a balanced nuclear equation for alpha decay of bismuth-212.
> Element 109 was synthesized by bombarding bismuth-209 with iron-58. Write the equation for this process if one product is a neutron.
> Complete the following nuclear equation: ? −−−→ (90 ^ 214) Th + (2 ^4) HE
> Complete the following nuclear equation: (78 ^ 190) Pt −−−→ a + ?
> a. Write the sequence of steps that would be followed for one round of b-oxidation of hexanoic acid. b. Calculate the number of ATP molecules produced by complete b-oxidation of hexanoic acid.
> Complete the following nuclear equation: (92 ^ 238) U + (7 ^14) N−−−−→?6(0 ^1) n
> Write a nuclear equation to represent radium-226 decaying to radon-222 plus an alpha particle.
> Samarium-147 is one of many rare earth isotopes that undergo alpha decay. Write a balanced nuclear equation for this process.
> How many protons and neutrons are contained in each of the three isotopes of carbon?
> How many protons and neutrons are contained in the nucleus of uranium-235?
> Write the nuclear symbol for carbon-14.
> Rank the four major types of radiation in order of size, speed, and penetrating power.
> What is the major difference between beta and gamma radiation?
> Write the nuclear symbol for a beta particle.
> We can control the rate of chemical reactions. Can we control the rate of natural radiation?
> Observed increases in global temperatures are caused by elevated levels of carbon dioxide. Is this statement a theory or a scientific law? Explain your reasoning.
> What are the major differences between alpha particles and gamma radiation?
> What is the composition of a positron?
> What is alpha decay?
> How does the energy of gamma radiation compare with that of other regions of the electromagnetic spectrum?
> Barium-131 is a radioisotope used to study bone formation. A patient ingested barium-131. How much time will elapse until only one-fourth of the barium-131 remains, assuming that none of the isotope is eliminated from the body through normal processes? T
> Calculate the pH of a buffer system containing 1.0 M NH3 and 1.0 M NH4Cl. (Ka of NH4+, the acid in this system, is 5.6 × 10-10.)
> What is the pH of the solution described in Question 8.101? Question 8.101: What is [H3O+] for a buffer solution that is 0.200 M in acid and 0.500 M in the corresponding salt if the weak acid Ka = 5.80 × 10-7?
> What is meant by the term lethal dose of radiation?
> The half-life of strontium-87 is 2.8 h. What percentage of this isotope will remain after 8 h and 24 minutes (min)?
> What are the roles of DNA, RNA, and protein in information flow in biological systems?
> Write the equilibrium constant expression for the reaction described in Question 7.96. Question 7.96: N2 (g) + O2 (g)↽−−−−⇀2NO(g)
> Will an increase in pressure increase, decrease, or have no effect on the concentration of NO(g) in the reaction: N2 (g) + O2 (g)↽−−−−⇀2NO(g)
> Which of the following are capable of forming a buffer solution? a. HBr and MgCl2 b. H2CO3 and NaHCO3
> Write out each step of the dissociation of chromic acid, H2CrO4.
> Use the equilibrium constant expression you wrote in Question 7.87 and the equilibrium constant you calculated in Question 7.88 to determine the equilibrium concentration of H2S if: Question 7.87: Write the equilibrium constant expression for the react
> Using the equilibrium constant expression in Question 7.87, calculate the equilibrium constant if: Question 7.87: Write the equilibrium constant expression for the reaction: 2H2 (g) 1 S2 (g)↽−−&a
> Chromic acid, H2CrO4, is a polyprotic acid. How many protons can it donate?
> Rewrite the equation in Question 8.82 as a net, balanced ionic equation. Question 8.82: Write an equation to represent the neutralization of an aqueous solution of HCl with an aqueous solution of KOH.
> Write an equation to represent the neutralization of an aqueous solution of HCl with an aqueous solution of KOH.
> What are the products of a neutralization reaction?
> Calculate formula mass and the molar mass of each of the following formula units: a. S8 b. (NH4)2SO4 c. CO2
> Two nitrogen atoms in a nitrogen molecule are held together more strongly than the two chlorine atoms in a chlorine molecule. Explain this fact by comparing their respective Lewis structures.
> The hydroxide ion concentration in a sample of urine was determined to be of 1.0 × 10-8 M (at 250C). Calculate the hydronium ion concentration of this aqueous solution.
> In a neutralization reaction, how many mol of NaOH are needed to react with 3 mol of HCl?
> Calculate the pH of a solution that has [OH-] = 6.7 × 10-9 M.
> Calculate the pH of a solution that has [H3O+] = 6.6 × 10-5 M.
> Distinguish between the rate constant and the equilibrium constant for a reaction.
> Can a dilute solution of a strong acid ever have a higher pH than a more concentrated solution of a weak acid? Why or why not?
> Write the rate law for the reaction: H2S(aq) + Cl2 (aq)↽−−−−⇀S(s) + 2HCl(aq) Represent the order as n, n', and so forth.
> A 6.00-mL portion of an 8.00 M stock solution is to be diluted to 0.400 M. What will be the final volume after dilution?
> A 50.0-mL sample of a 0.250 M sucrose solution was diluted to 5.00 × 102 mL. What is the molar concentration of the resulting solution?
> Identify the conjugate acid-base pairs for the reversible reactions in Question 8.4. Question 8.4: Write an equation for the reversible reactions of each of the following with water. a. H3PO4 b. CH3NH2
> Explain the differences between leading strand and lagging strand replication.
> Calculate [H3O+] for a solution of hydrochloric acid for which: a. pH = 2.00 b. pH = 3.00
> How many g of sodium hydroxide are present in 675 mL of a 0.500 M solution?
> Select one enzyme from a later chapter in this book and describe its biochemical importance.
> What is the concentration of hydronium ions in an aqueous solution of acetaminophen if the concentration of hydroxide ions is 2.5 × 10-9 M?
> Calculate the [OH-] of an aqueous solution that is: a. 1.0 × 10-6 M in H3O+ b. 1.0 × 10-8 M in H3O+
> Calculate the [H3O+] of an aqueous solution that is: a. 1.0 × 10-9 M in OH- b. 1.0 × 10-5 M in OH-
> Label each of the following as a strong or weak base: a. KOH b. CN- c. SO42-
> Of the following diagrams, which one represents: a. a concentrated strong acid b. a dilute strong acid c. a concentrated weak acid d. a dilute weak acid H+ x- H+ x- X- H+ x- H+ H+ x- H+ x- X- H+ x- H+ H+x-H+x=x¯H+ H+ H-X X- Н-X H-X H-X Н-X H-X H-X X
> Identify the conjugate acid-base pairs in each of the following chemical equations: a. HCOOH (aq) + NH3(aq) ↽−−−−−−⇀ HCOO-(aq) + NH4+(aq) b. HCl(aq) + OH-(aq) ↽−−−−−−⇀ H2O(l) + Cl-(aq)
> Which is the stronger base, F2 or CH3COO-?
> Distinguish between the term’s formula mass and molar mass.
> Write an equation for the reversible reactions of each of the following with water. a. H3PO4 b. CH3NH2
> Which is the stronger acid, HNO3 or HCN?
> Write the formula of the conjugate acid of F-.
> Write the formula of the conjugate base of HCOOH.
> Write the formula of the conjugate acid of Br-.
> Write an equation for the reaction of each of the following with water: a. HNO3 b. HCOOH c. CH3CH2CH2NH2
> Classify each of the following as either a Brønsted-Lowry acid, base, or as amphiprotic. a. H2SO4 b. HSO4- c. SO42-
> Classify each of the following as either a Brønsted-Lowry acid, base, or as amphiprotic. a. NH4+ b. NH3 c. CH3CH2CH2NH3+
> Why is ammonia described as a Brønsted-Lowry base and not an Arrhenius base?
> a. Define a base according to the Arrhenius theory. b. Define a base according to the Brønsted-Lowry theory.
> Describe the reaction catalyzed by each of the enzymes listed in Question 22.37. Question 22.37: Match each of the following enzymes with the class of enzyme to which it belongs. (Hint: An enzyme classification may be used more than once or not at all.
