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Questions and Answers of Chemical Principles

A 230.-mL sample of a 0.275 M CaCl2 solution is left on a hot plate overnight; the following morning, the solution is 1.10 M. What volume of water evaporated from the 0.275 M CaCl2 solution?
You wish to prepare 1L of a 0.02 M potassium iodate solution. You require that the final concentration be within 1% of 0.02 M and that the concentration must be known precisely to the fourth decimal
What volume of 0.100 M NaOH is required to precipitate all of the nickel(II) ions from 150.0 mL of a 0.249-M solution of Ni(NO3)2?
A 450.0-mL sample of a 0.257-M solution of silver nitrate is mixed with 400.0 mL of 0.200 M calcium chloride. What is the concentration of Cl2 in solution after the reaction is complete?
Consider the following apparatus: a test tube covered with a nonpermeable elastic membrane inside a container that is closed with a cork. A syringe goes through the cork.a. As you push down on the
As you increase the temperature of a gas in a sealed, rigid container, what happens to the density of the gas? Would the results be the same if you did the same experiment in a container with a
If you put a drinking straw in water, place your finger over the opening, and lift the straw out of the water, some water stays in the straw. Explain.
Chemicals X and Y (both gases) react to form the gas XY, but it takes a bit of time for the reaction to occur. Both X and Y are placed in a container with a piston (free to move), and you note the
Explain the following seeming contradiction: You have two gases, A and B, in two separate containers of equal volume and at equal pressure and temperature. Therefore, you must have the same number of
You have a balloon covering the mouth of a flask filled with air at 1 atm. You apply heat to the bottom of the flask until the volume of the balloon is equal to that of the flask.a. Which has more
A gauge on a compressed gas cylinder reads 2200 psi (pounds per square inch; 1 atm 5 14.7 psi). Express this pressure in each of the following units.a. Standard atmospheresb. Megapascals (MPa)c. Torr
Calculate the pressure exerted by 0.5000 mole of N2 in a 10.000-L container at 25.08C.a. Use the ideal gas law.b. Use the van der Waals equation.c. Compare the results from parts a and b.d. Compare
A 1.0-L sample of air is collected at 258C at sea level (1.00 atm). Estimate the volume this sample of air would have at an altitude of 15 km (Fig. 5.27). At 15 km, the pressure is about 0.1 atm.
Boyle’s law can be represented graphically in several ways. Which of the following plots does not correctly represent Boyle’s law (assuming constant T and n)? Explain. PV P V P KA 1/P 1/V
A certain flexible weather balloon contains helium gas at a volume of 855 L. Initially, the balloon is at sea level where the temperature is 258C and the barometric pressure is 730. torr. The balloon
One of the assumptions of the kinetic molecular theory is that the volume of a gas particle is negligible. If this were the case, the ratio of the number of collisions of gas particles with the walls
For the reaction H2(g) + I2(g) 34 ⇌ HI(g), consider two possibilities using the same-sized, rigid container:(a) You add 0.5 mole of each reactant, allow the system to come to equilibrium, then add
Given the reaction A(g) + B(g) ⇌ C(g) + D(g), consider the following situations:i. You have 1.3 M A and 0.8 M B initially.ii. You have 1.3 M A, 0.8 M B, and 0.2 M C initially.iii. You have 2.0 M A
Consider the reaction A(g) + B(g) ⇌ C(g) + D(g) in a 1.0-L rigid flask. Answer the following questions for each situation (a–d):i. Estimate a range (as small as possible) for the requested
Consider the following statements: “Consider the reaction A(g) + B(g) ⇌ C(g), at equilibrium in a 1-L container, with [A] = 2 M, [B] = M, and [C] = 4 M. To this 1-L container you add 3 moles of
Consider the same reaction as in Exercise 12. In a particular experiment, 1.0 mole of H2O(g) and 1.0 mole of CO(g) are put into a flask and heated to 3508C. In another experiment, 1.0 mole of H2(g)
At a given temperature, K = 1.3 × 10-2 for the reaction N₂(g) + 3H₂(g)2NH₂(g) Calculate values of K for the following reactions at this temperature a. N₂(g) + H₂(g) →NH3(g) b.
An equilibrium mixture contains 0.60 g solid carbon and the gases carbon dioxide and carbon monoxide at partial pressures of 2.60 atm and 2.89 atm, respectively. Calculate the value of Kp for the
Sketch two graphs: (a) Percent dissociation of weak acid HA versus initial concentration of HA ([HA]0), and(b) Concentration versus [HA]+. Explain both.
Consider a solution prepared by mixing a weak acid HA and HCl. What are the major species? Explain what is occurring in solution. How would you calculate the pH? What if you added NaA to this
You are asked for the H+ concentration in a solution of NaOH(aq). Because sodium hydroxide is a strong base, can we say there is no H+, since having H+ would imply that the solution is acidic?
Fill in the missing information in the following table. Solution a Solution b Solution c Solution d pH 9.63 POH 12.2 [H+] 0.027 M [OH-] 3.9 x 10-6 M Acidic, Basic, or Neutral?
Can the pH of a solution be negative? Explain. True or false: A strong acid solution always has a lower pH than a weak acid solution. Explain.
Will 0.10 M solutions of the following salts be acidic, basic, or neutral?a. Ammonium bicarbonateb. Sodium dihydrogen phosphatec. Sodium hydrogen phosphated. Ammonium dihydrogen phosphatee. Ammonium
Calculate [OH+], [H-], and the pH of 0.40 M solutions of each of the following amines.a. Aniline b. Methylamine
A 0.25-g sample of lime (CaO) is dissolved in enough water to make 1500 mL of solution. Calculate the pH of the solution.
A solution of formic acid (HCOOH, Ka = 1.8 × 1024) has a pH of 2.70. Calculate the initial concentration of formic acid in this solution.
Consider a solution prepared by mixing equal moles of a weak acid HA, HCl, and NaA. Which of the following best describes what happens?a. The H1 from the HCl reacts completely with the A2 from the
Acids and bases can be thought of as chemical opposites (acids are proton donors, and bases are proton acceptors). Therefore, one might think that Ka = 1/Kb. Why isn’t this the case? What is the
The following are representations of acid–base reactions: + 11 呢 + +
You have two solutions of the salts NaX(aq) and NaY(aq) at equal concentrations. What would you need to know to determine which solution has the higher pH? Explain how you would decide (perhaps even
Consider the following illustrations:Which beaker best illustrates what happens when the following acids are dissolved in water?a. HNO2 b. HNO3 e. HC2H3O2c. HCld. HFe. HC2H3O2 H* A B
Is the conjugate base of a weak acid a strong base? Explain. Explain why Cl- does not affect the pH of an aqueous solution
Match the following pH values: 1, 2, 5, 6, 6.5, 8, 11, 11 and 13 with the following chemicals (of equal concentration): HBr, NaOH, NaF, NaCN, NH4F, CH3NH3F, HF, HCN, and NH3. Answer this question
You may need Table 7.2 to answer the following questions.a. Which is the stronger acid, HCl or H2O?b. Which is the stronger acid, H2O or HNO2?c. Which is the stronger acid, HCN or HOC6H5 Table
The salt BX, when dissolved in water, produces an acidic solution. Which of the following could be true? (There may be more than one correct answer.)a. The acid HX is a weak acid.b. The acid HX is a
Classify each of the following as a strong acid or a weak acid. a. b. C. d. H 0 CI S
Why is the pH of water at 258C equal to 7.00?
Consider the following statements. Write out an example reaction and K expression that are associated with each statement.a. The autoionization of water.b. An acid reacts with water to produce the
You may need Table 7.2 to answer the following questions.a. Which is the stronger base, Cl2 or H2O?b. Which is the stronger base, H2O or NO22?c. Which is the stronger base, CN2 or OC6H5?Table 7.2
Write balanced equations that describe the following reactions.a. The dissociation of perchloric acid in water.b. The dissociation of propanoic acid (CH3CH2CO2H) in water.c. The dissociation of
Write the dissociation reaction and the corresponding Ka equilibrium expression for each of the following acids in water.a. HCNb. HOC6H5c. C6H5NH3
Write the reaction and the corresponding Kb equilibrium expression for each of the following substances (acting as bases in water).a. NH3 b. CN2 c. pyridine, C5H5Nd. aniline, C6H5NH2
Consider the reaction of acetic acid in water CH3CO2H(aq) + H2O(l) ⇌ CH3CO22(aq) + H3O+(aq) where Ka 5 1.8 3 1025.a. Which two bases are competing for the proton?b. Which is the stronger base?c. In
The pOH of a sample of baking soda dissolved in water is 5.74 at 258C. Calculate the pH, [H+], and [OH-] for this sample. Is the solution acidic or basic?
At 40.8C the value of Kw is 2.92 3 10214.a. Calculate the [H+] and [OH-] in pure water at 40.8C.b. What is the pH of pure water at 40.8C?c. If the hydroxide ion concentration in a solution is 0.10 M,
Give the conditions for a neutral aqueous solution at 258C, in terms of [H+], pH, and the relationship between [H+] and [OH-]. Do the same for an acidic solution and for a basic solution. As a
Calculate the concentration of all species present and the pH of a 0.020 M HF solution.The solution contains one of the following substances: HCl, NaOH, NH4Cl, HCN, NH3, HF, or NaCN. If the solute
Calculate the [H1] of each of the following solutions at 258C. Identify each solution as neutral, acidic, or basic.a. [OH-] = 1.5 Mb. [OH-] = 3.6 × 10-15 Mc. [OH-] = 1.0 × 10-7 Md. [OH-] = 7.3
Calculate the [OH2] of each of the following solutions at 258C. Identify each solution as neutral, acidic, or basic.a. [H+] =1.0 × 10-7 Mb. [H+] = 8.3 × 10-16 Mc. [H+] = 12 Md. [H+] = 5.4 × 1025
Calculate [H+] and [OH-] for each solution at 258C. Identify each solution as neutral, acidic, or basic.a. pH 5 7.40 b. pH 5 15.3c. pH 5 21.0d. pH 5 3.20e. pOH 5 5.0f. pOH 5 9.60
A solution is prepared by adding 50.0 mL of 0.050 M HBr to 150.0 mL of 0.10 M HI. Calculate [H+] and the pH of this solution. HBr and HI are both considered strong acids.
What mass of HNO3 is present in 250.0 mL of a nitric acid solution having a pH = 5.10?
Using Table 7.3, order the following bases from strongest to weakest.NO3-, H2O, NH3, and C5H5NTable 7.3 Values of K₁ for Some Common Weak
Calculate the pH of a 0.010 M solution of iodic acid (HIO3, Ka = 0.17).
At 258C a saturated solution of benzoic acid has a pH of 2.80. Calculate the water solubility of benzoic acid in moles per liter and grams per 100. mL.
Calculate the pH of a solution that contains 1.0 M HF and 1.0 M HOC6H5. Also calculate the concentration of OC6H5- in this solution at equilibrium.
A solution is made by adding 50.0 mL of 0.200 M acetic acid (Ka 5 1.8 3 1025) to 50.0 mL of 1.00 3 1023 M HCl.a. Calculate the pH of the solution.b. Calculate the acetate ion concentration.
Quinine (C20H24N2O2) is the most important alkaloid derived from cinchona bark. It is used as an antimalarial drug. For quinine pKb = 5.1 and pKb2 = 9.7 (pKb = 2log Kb). Only 1.0 g of quinine will
A 0.15 M solution of a weak acid is 3.0% dissociated. Calculate Ka.
Calculate [CO32-] in a 0.010 M solution of CO2 in water (H2CO3). If all the CO3 2- in this solution comes from the reactionwhat percentage of the H1 ions in the solution is a result of the
You have 100.0 g of saccharin, a sugar substitute, and you want to prepare a pH = 5.75 solution. What volume of solution can be prepared? For saccharin (HC7H4NSO3), pKa = 11.70 (pKa = 2log Ka).
For the reaction of hydrazine (N2H4) in water.H2NNH2(aq) + H2O(l) ⇌ H2NNH3+(aq) + OH-(aq) Kb is 3.0 3 1026. Calculate the concentrations of all species and the pH of a 2.0 M solution of
Calculate the percentage of pyridine (C5H5N) that forms pyridinium ion, C5H5NH+, in a 0.10 M aqueous solution of pyridine (Kb = 1.7 x1029).
The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton?
Calculate the pH of a 0.20 M C2H5NH2 solution (Kb = 5.6 × 1024).
Calculate the pH of a 0.050 M (C2H5)2NH solution (Kb= 5 1.3 × 10-3).
Calculate the pH and [S2-] in a 0.10 M H2S solution. Assume Ka1 = 1.0 × 1027; Ka2 = 1.0 ×10219.
Determine [OH-], [H+], and the pH of each of the following solutions.a. 1.0 M KCIb. 1.0 M KF
An unknown salt is either NaCN, NaC2H3O2, NaF, NaCl, or NaOCl. When 0.100 mole of the salt is dissolved in 1.00 L of solution, the pH of the solution is 8.07. What is the identity of the salt?
Calculate the pH of a 7.0 × 1027 M HCl solution.
Calculate the pH of a 1.0 3 1027 M solution of NaOH in water.
Calculate the value for the equilibrium constant for each of the following aqueous reactions.a. NH3 + H3O+ ⇌ NH4 + H2Ob. NO2- + H3O+ ⇌ HNO2 + H2Oc. NH4 + CH3CO2- ⇌ NH3 + CH3CO2Hd. H3O+ 1 OH2
Complete the table for each of the following solutions: 0.0070 M HNO3 3.0 M KOH [H+] pH POH [OH-]
A solution is prepared by adding 50.0 mL concentrated hydrochloric acid and 20.0 mL concentrated nitric acid to 300 mL water. More water is added until the final volume is 1.00 L. Calculate [H+],
Consider a 0.60-M solution of HC3H5O3, lactic acid (Ka = 1.4 × 1024).a. Which of the following are major species in the solution?i. HC3H5O3ii. C3H5O3iii. H+iv. H2Ov. OH-b. Complete the following ICE
A 10.0-mL sample of an HCl solution has a pH of 2.000. What volume of water must be added to change the pH to 4.000?
A 0.20 M sodium chlorobenzoate (NaC7H4ClO2) solution has a pH of 8.65. Calculate the pH of a 0.20 M chlorobenzoic acid (HC7H4ClO2) solution.
Consider a 0.67-M solution of C2H5NH2 (Kb 5 5.6 3 1024).a. Which of the following are major species in the solution?i. C2H5NH2ii. H+iii. OH-iv. H2Ov. C2H5NH3b. Calculate the pH of this solution.
Rank the following 0.10 M solutions in order of increasing pH.a. NH3b. KOH c. HC2H3O2d. KCle. HCl
Consider 0.10 M solutions of the following compounds: AlCl3, NaCN, KOH, CsClO4, and NaF. Place these solutions in order of increasing pH.
A typical solution of baking soda (sodium bicarbonate, NaHCO3) has a pH that is independent of concentration. The pH of a solution of sodium bisulfate (NaHSO4) does depend on the concentration.a.
A certain acid, HA, has a vapor density of 5.11 g/L when in the gas phase at a temperature of 258C and a pressure of 1.00 atm. When 1.50 g of this acid is dissolved in enough water to make 100.0 mL
How many of the following are buffered solutions? Explain your answer. Counter-ions and water molecules have been omitted from the illustrations for clarity. H+ A™ B
A 0.100 M solution of the salt BHX has a pH of 8.00, where B is a weak base and X2 is the anion of the weak acid HX. Calculate Ka value for HX if the Kb value for B is 1.0 × 10-3.
Determine the pH of a 0.100 M solution of (NH4)2C2O4.
An aqueous solution contains a mixture of 0.0500 M HCOOH (Ka = 1.77 × 1024) and 0.150 M CH3CH2COOH (Ka = 1.34 × 10-5). Calculate the pH of this solution.
A 50.00-mL solution of a weak acid HA (Ka = 5.00 × 10210) in water has a pH = 5.650. Calculate the amount of water that must be added to reach a pH value of 6.650.
Derive an equation to solve for the pH for a dilute weak base in which water is a significant contributor to the pH. Use this formula to calculate the pH of a 100.0-mL sample of 2.0 × 10-5 M B
Calculate the pH of 6.0 × 10-4 M NaNO2.
Calculate [OH+] in a 3.0 × 1027 M solution of Ca(OH)2.
Define a buffered solution. What makes up a buffered solution? Explain how buffers absorb added H+ or OH- with little pH change. A certain buffer is made by dissolving NaHCO3 and Na2CO3 in some
One of the most challenging parts of solving acid–base problems is writing out the correct equation. When a strong acid or a strong base is added to solutions, they are great at what they do and we
Calculate the pH after 0.010 mole of gaseous HCl is added to 250.0 mL of each of the following buffered solutions.a. 0.050 M NH3/0.15 M NH4Clb. 0.50 M NH3/1.50 M NH4Cl Do the two original buffered
An aqueous solution contains dissolved C6H5NH3Cl and C6H5NH2. The concentration of C6H5NH2 is 0.50 M and pH is 4.20.a. Calculate the concentration of C6H5NH3+ in this buffered solution.b. Calculate

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