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Questions and Answers of Chemical Principles

Determine the \(\mathrm{pH}\) of a \(0.100 \mathrm{M}\) solution of \(\left(\mathrm{NH}_{4}ight)_{2} \mathrm{C}_{2} \mathrm{O}_{4}\).
Calculate the \(\mathrm{pH}\) of a solution initially with \(0.10 \mathrm{M}\) \(\mathrm{NaHSO}_{4}\) and \(0.10 \mathrm{M} \mathrm{NH}_{3}\).
A chemist dissolves \(0.135 \mathrm{~mol}\) of \(\mathrm{CO}_{2}(\mathrm{~g})\) in \(2.50 \mathrm{~L}\) of \(0.105 \mathrm{M} \mathrm{Na}_{2} \mathrm{CO}_{3}\). Calculate the \(\mathrm{pH}\) of the
Calculate the \(\mathrm{pH}\) of \(6.0 \times 10^{-4} \mathrm{M} \mathrm{NaNO}_{2}\).
Calculate the \(\mathrm{pH}\) of a solution prepared by mixing equal volumes of \(1.0 \times 10^{-4} \mathrm{M} \mathrm{NH}_{3}\) and \(1.0 \times 10^{-4} \mathrm{M} \mathrm{HCl}\).
Calculate \(\left[\mathrm{OH}^{-}ight]\)in a \(3.0 \times 10^{-7} \mathrm{M}\) solution of \(\mathrm{Ca}(\mathrm{OH})_{2}\).
" Captain Kirk, of the Starship Enterprise, has been told by his superiors that only a chemist can be trusted with the combination to the safe containing the dilithium crystals that power the ship.
We found that the equilibrium concentration of H+ in a 1.0 M HF solution is 2.7 × 10–2 M and the percent dissociation of HF is 2.7%. Calculate [H+] and the percent dissociation of HF in a solution
A buffered solution contains 0.50 M acetic acid (HC2H3O2, Ka = 1.8 × 10–5) and 0.50 M sodium acetate (NaC2H3O2).a. Calculate the pH of this solution.b. Calculate the change in pH that occurs when
A buffered solution contains 0.25 M NH3 (Kb = 1.8 × 10–5) and 0.40 M NH4Cl.a. Calculate the pH of this solution.b. Calculate the pH of the solution that results when 0.10 mol of gaseous HCl is
Calculate the pH of a buffered solution containing 3.0 × 10–4 M HOCl (Ka = 3.5 × 10–8) and 1.0 × 10–4 M NaOCl.
Calculate the change in pH that occurs when 0.010 mol of gaseous HCl is added to 1.0 L of each of the following solutions.Solution A: 5.00 M HC2H3O2 and 5.00 M NaC2H3O2Solution B: 0.050 M HC2H3O2 and
A chemist needs to prepare a solution buffered at pH 4.30 using one of the following acids (and its sodium salt):Calculate the ratio of [HA]/[A–] required for each system to yield a pH of 4.30.
Hydrogen cyanide gas (HCN) is a powerful respiratory inhibitor that is highly toxic. It is a very weak acid (Ka = 6.2 × 10–10) when dissolved in water. If a 50.0-mL sample of 0.100 M HCN is
A chemist has synthesized a monoprotic weak acid and wants to determine its Ka value. To do so, the chemist dissolves 2.00 mmol of the solid acid in 100.0 mL of water and titrates the resulting
Bromthymol blue, an indicator with a Ka value of 1.0 × 10–7, is yellow in its HIn form and blue in its In– form. Suppose we put a few drops of this indicator in a strongly acidic solution. If
Calculate the pH of a 1.0 M solution of NaH2PO4. (For H3PO4, Ka1 = 7.5 × 10–3, Ka2 = 6.2 × 10–8, and Ka3 = 4.8 × 10–13.)
Calculate the Ksp value for bismuth sulfide (Bi2S3), which has a solubility of 1.0 × 10–15 mol/L at 25°C.
The Ksp value for copper(II) iodate [Cu(IO3)2] is 1.4 × 10–7 at 25°C. Calculate its solubility at 25°C.
A solution contains 1.0 × 10–4 M Cu+ and 2.0 × 10–3 M Pb2+. If a source of I– is added to this solution gradually, will PbI2 (Ksp = 1.4 × 10–8) or CuI (Ksp = 5.3 × 10–12) precipitate
Calculate the concentrations of Ag+, Ag(S2O3)–, and Ag(S2O3)23– in a solution prepared by mixing 150.0 mL of 1.00 × 10–3 M AgNO3 with 200.0 mL of 5.00 M Na2S2O3. The stepwise formation
You have two salts \(\mathrm{AgX}\) and \(\mathrm{AgY}\) with very similar \(K_{\mathrm{sp}}\) values. You know that the \(K_{\mathrm{a}}\) value for \(\mathrm{HX}\) is much greater than the
Under what circumstances can the relative solubilities of two salts be compared by directly comparing values of their solubility products?
Calculate the \(\mathrm{pH}\) of each of the following solutions.a. \(0.100 \mathrm{M}\) propanoic acid \(\left(\mathrm{HC}_{3} \mathrm{H}_{5} \mathrm{O}_{2}, K_{\mathrm{a}}=1.3 \times
Calculate the pH after 0.020 mol of HCl is added to 1.00 L of each of the four solutions in Exercise 19.Data from Exercises 19Calculate the pH of each of the following solutions.0.100 M propanoic
Calculate the \(\mathrm{pH}\) after \(0.020 \mathrm{~mol}\) of \(\mathrm{NaOH}\) is added to \(1.00 \mathrm{~L}\) of each of the four solutions in Exercise 19.Data from Exercises 19Calculate the pH
The results of Exercises 19-21 illustrate an important property of buffered solutions. Which solution in Exercise 19 is the buffered solution and what important property is illustrated by the
Calculate the \(\mathrm{pH}\) of a solution that is \(0.60 \mathrm{M} \mathrm{HF}\) and \(1.00 \mathrm{M} \mathrm{KF}\).
Calculate the \(\mathrm{pH}\) of a solution that is \(0.100 \mathrm{M} \mathrm {HONH}_{2}\) and \(0.100 \mathrm{M} \mathrm {HONH}_{3} \mathrm{Cl}\).
Calculate the \(\mathrm{pH}\) after \(0.10 \mathrm{~mol}\) of \(\mathrm{NaOH}\) is added to 1.00 L of the solution in Exercise 23, and calculate the \(\mathrm{pH}\) after \(0.20 \mathrm{~mol}\) of
Calculate the \(\mathrm{pH}\) after \(0.020 \mathrm{~mol}\) of \(\mathrm{NaOH}\) is added to \(1.00 \mathrm{~L}\) of the solution in Exercise 24, and calculate the \(\mathrm{pH}\) after \(0.020
Calculate the \(\mathrm{pH}\) of a buffered solution prepared by dissolving \(21.5 \mathrm{~g}\) of benzoic acid \(\left(\mathrm{HC}_{7} \mathrm{H}_{5} \mathrm{O}_{2}ight)\) and \(37.7 \mathrm{~g}\)
How many moles of \(\mathrm{NaOH}\) must be added to \(1.0 \mathrm{~L}\) of \(2.0 \mathrm{M} \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) to produce a solution buffered at each \(\mathrm{pH}\) ?a.
Calculate the number of moles of \(\mathrm{HCl}(\mathrm{g})\) that must be added to \(1.0 \mathrm{~L}\) of \(1.0 \mathrm{M} \mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) to produce a solution
Calculate the \(\mathrm{pH}\) after \(0.010 \mathrm{~mol}\) of gaseous \(\mathrm{HCl}\) is added to \(250.0 \mathrm{~mL}\) of each of the following buffered solutions.a. \(0.050 \mathrm{M}
a. Carbonate buffers are important in regulating the \(\mathrm{pH}\) of blood at 7.40. What is the concentration ratio of \(\mathrm{CO}_{2}\) (usually written \(\mathrm{H}_{2} \mathrm{CO}_{3}\) ) to
Which of the following mixtures would result in a buffered solution when \(1.0 \mathrm{~L}\) of each of the two solutions are mixed?a. \(0.1 \mathrm{M} \mathrm{KOH}\) and \(0.1 \mathrm{M}
In Section 8.3 an equation was derived for the exact treatment of HA/NaA-type buffers. What would be the expression for \(\mathrm{B} / \mathrm{BHCl}\)-type buffers stated in terms of
Consider a weak acid HA with a \(K_{a}\) value of \(1.6 \times 10^{-7}\). Calculate the \(\mathrm{pH}\) of a solution that is \(5.0 \times\) \(10^{-7} \mathrm{M} \mathrm{HA}\) and \(5.0 \times
A \(25.0-\mathrm{mL}\) sample of \(0.100 \mathrm{M}\) lactic acid \(\left(\mathrm{HC}_{3} \mathrm{H}_{5} \mathrm{O}_{3}, \mathrm{pK}ight.\) =3.86) is titrated with \(0.100 \mathrm{M} \mathrm{NaOH}\)
Two drops of indicator HIn \(\left(K_{\mathrm{a}}=1.0 \times 10^{-9}ight)\), where HIn is yellow and \(\mathrm{In}^{-}\)is blue, are placed in \(100.0 \mathrm{~mL}\) of \(0.10 \mathrm{M}
Indicators can be used to estimate the \(\mathrm{pH}\) values of solutions. To determine the \(\mathrm{pH}\) of a \(0.01 \mathrm{M}\) weak acid (HX) solution, a few drops of three different
Consider the titration of \(100.0 \mathrm{~mL}\) of a \(0.0500 \mathrm{M}\) solution of the hypothetical weak acid \(\mathrm{H}_{3} \mathrm{X}\left(K_{\mathrm{a}_{1}}=1.0 \timesight.\) \(10^{-3},
Consider \(100.0 \mathrm{~mL}\) of a \(0.100 \mathrm{M}\) solution of \(\mathrm{H}_{3}\mathrm{~A}\) \(\left(K_{\mathrm{a}_{1}}=1.5 \times 10^{-4}, K_{\mathrm{a}_{2}}=3.0 \times 10^{-8},
A 0.200 -g sample of a triprotic acid (molar mass \(=165.0\) \(\mathrm{g} / \mathrm{mol}\) ) is dissolved in a \(50.00-\mathrm{mL}\) aqueous solution and titrated with \(0.0500 \mathrm{M}
A student was given a \(0.10 \mathrm{M}\) solution of an unknown diprotic acid \(\mathrm{H}_{2} \mathrm{~A}\) and asked to determine the \(K_{\mathrm{a}_{1}}\) and \(K_{\mathrm{a}_{2}}\) values for
The titration of \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) with \(\mathrm{HCl}\) has the following qualitative profile:a. Identify the major species in solution as points A-F.b. For the titration of
Consider \(100.0 \mathrm{~mL}\) of a solution of \(0.200 \mathrm{M} \mathrm{Na}_{2} \mathrm{~A}\), where \(\mathrm{A}^{2-}\) is a base with corresponding acids \(\mathrm{H}_{2} \mathrm{~A}\)
Calculate the solubility of each of the following compounds in moles per liter and grams per liter. (Ignore any acid-base properties.)a. \(\mathrm{Ag}_{3} \mathrm{PO}_{4}, K_{\text {sp }}=1.8 \times
The concentration of \(\mathrm{Ag}^{+}\)in a solution saturated with \(\mathrm{Ag}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(s)\) is \(2.2 \times 10^{-4} M\). Calculate \(K_{\text {sp }}\) for
The solubility of \(\mathrm{Ce}\left(\mathrm{IO}_{3}ight)_{3}\) in a \(0.20 \mathrm{M} \mathrm{KIO}_{3}\) solution is \(4.4 \times 10^{-8} \mathrm{~mol} / \mathrm{L}\). Calculate \(K_{\text {sp }}\)
Explain the following phenomenon. You have a test tube with about \(20 \mathrm{~mL}\) of silver nitrate solution. Upon adding a few drops of sodium chromate solution, you notice a red solid forming
A solution is prepared by mixing \(75.0 \mathrm{~mL}\) of \(0.020 \mathrm{M}\) \(\mathrm{BaCl}_{2}\) and \(125 \mathrm{~mL}\) of \(0.040 \mathrm{M} \mathrm{K}_{2} \mathrm{SO}_{4}\). What are the
A solution is prepared by mixing \(50.0 \mathrm{~mL}\) of \(0.10 \mathrm{M}\) \(\mathrm{Pb}\left(\mathrm{NO}_{3}ight)_{2}\) with \(50.0 \mathrm{~mL}\) of \(1.0 \mathrm{M} \mathrm{KCl}\). Calculate
A solution contains \(1.0 \times 10^{-5} \mathrm{M} \mathrm{Na}_{3} \mathrm{PO}_{4}\). What is the minimum concentration of \(\mathrm{AgNO}_{3}\) that would cause precipitation of solid
Given the following data,calculate the value for the overall formation constant for \(\mathrm{Mn}\left(\mathrm{C}_{2} \mathrm{O}_{4}ight)_{2}{ }^{2-}\)
The overall formation constant for \(\mathrm{HgI}_{4}{ }^{2-}\) is \(1.0 \times 10^{30}\). That is,\[1.0 \times 10^{30}=\frac{\left[\mathrm{HgI}_{4}{
A solution is prepared by adding \(0.090 \mathrm{~mol}\) of \(\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}ight]\) to \(0.60 \mathrm{~L}\) of \(2.0 \mathrm{M} \mathrm{NaCN}\). Assuming no volume
Consider a solution made by mixing \(500.0 \mathrm{~mL}\) of 4.0 \(M \mathrm{NH}_{3}\) and \(500.0 \mathrm{~mL}\) of \(0.40 \mathrm{M} \mathrm{AgNO}_{3} . \mathrm{Ag}^{+}\)reacts with
Solutions of sodium thiosulfate are used to dissolve unexposed \(\mathrm{AgBr}\) in the developing process for black-andwhite film. What mass of \(\mathrm{AgBr}\) can dissolve in \(1.00 \mathrm{~L}\)
The equilibrium constant for the following reaction is \(1.0 \times 10^{23}\) :EDTA is used as a complexing agent in chemical analysis. Solutions of EDTA, usually containing the disodium salt
Calculate the concentration of \(\mathrm{Pb}^{2+}\) in each of the following.a. a saturated solution of \(\mathrm{Pb}(\mathrm{OH})_{2} ; K_{\mathrm{sp}}=1.2 \times 10^{-15}\)b. a saturated solution
The solubility rules outlined in Chapter 4 say that \(\mathrm{Ba}(\mathrm{OH})_{2}, \mathrm{Sr}(\mathrm{OH})_{2}\), and \(\mathrm{Ca}(\mathrm{OH})_{2}\) are marginally soluble hydroxides. Calculate
When phosphoric acid is titrated with a \(\mathrm{NaOH}\) solution, only two stoichiometric points are seen. Why?
For solutions containing salts of the form \(\mathrm{NH}_{4} \mathrm{X}\), the \(\mathrm{pH}\) is determined by using the equation\[\mathrm{pH}=\frac{\mathrm{p}
Consider the titration of \(100.0 \mathrm{~mL}\) of a solution that contains a mixture of \(0.050 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) and \(0.20 \mathrm{M}\) \(\mathrm{H}_{2} \mathrm{C}_{6}
a. Show that the solubility of \(\mathrm{Al}(\mathrm{OH})_{3}\), as a function of \(\left[\mathrm{H}^{+}ight]\), obeys the equation\[S=\left[\mathrm{H}^{+}ight]^{3} K_{\mathrm{sp}} / K_{\mathrm{w}}{
Consider the titration of \(100.0 \mathrm{~mL}\) of a \(1.00 \times 10^{-4} \mathrm{M}\) solution of an acid HA \(\left(K_{\mathrm{a}}=5.0 \times 10^{-10}ight)\) with \(1.00 \times\) \(10^{-3}
Consider a solution formed by mixing \(200.0 \mathrm{~mL}\) of \(0.250 \mathrm{M} \mathrm{Na}_{3} \mathrm{PO}_{4}, 135.0 \mathrm{~mL}\) of \(1.000 \mathrm{M} \mathrm{HCl}\), and \(100.0
Calculate the \(\mathrm{pH}\) of a solution prepared by mixing 500.0 \(\mathrm{mL}\) of \(0.50 \mathrm{M} \mathrm{Na}_{3} \mathrm{PO}_{4}\) and \(500.0 \mathrm{~mL}\) of \(0.10 \mathrm{M}
In the titration of \(100.0 \mathrm{~mL}\) of a \(0.0500 \mathrm{M}\) solution of acid \(\mathrm{H}_{3} \mathrm{~A}\left(K_{\mathrm{a}_{1}}=1.0 \times 10^{-3}, K_{\mathrm{a}_{2}}=5.0 \times 10^{-8},
A 225-mg sample of a diprotic acid is dissolved in enough water to make \(250 . \mathrm{mL}\) of solution. The \(\mathrm{pH}\) of this solution is 2.06. A saturated solution of calcium hydroxide
Predict the signs of \(q\) and \(w\) for the process of boiling water.
In the equation \(w=-P \Delta V\), why is there a negative sign?
You have an ideal gas with an initial volume of \(1.0 \mathrm{~L}\) and initial pressure of \(1.0 \mathrm{~atm}\). You decide to change the conditions such that \(P_{\text {final }}=2.0
What is the difference between \(\Delta H\) and \(\Delta E\) at constant \(P\) ?
For the process \(\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{H}_{2} \mathrm{O}(g)\) at \(298 \mathrm{~K}\) and 1.0 atm, \(\Delta H\) is more positive than \(\Delta E\) by \(2.5 \mathrm{~kJ}
In a coffee cup calorimeter \(50.0 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{AgNO}_{3}\) and \(50.0 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{HCl}\) are mixed. The following reaction
Consider the dissolution of \(\mathrm{CaCl}_{2}\) :\[\mathrm{CaCl}_{2}(s) \longrightarrow \mathrm{Ca}^{2+}(a q)+2 \mathrm{Cl}^{-}(a q) \quad \Delta H=-81.5 \mathrm{~kJ}\]An 11.0-g sample of
Consider the reactionCalculate the heat when \(100.0 \mathrm{~mL}\) of \(0.500 \mathrm{M} \mathrm{HCl}\) is mixed with \(300.0 \mathrm{~mL}\) of \(0.100 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\).
Calculate the molarity of a solution prepared by bubbling 1.56 g of gaseous HCl into enough water to make 26.8 mL of solution.
Calculate the number of moles of Cl– ions in 1.75 L of 1.0 × 10–3 M AlCl3.
Typical blood serum is about 0.14 M NaCl. What volume of blood contains 1.0 mg of NaCl?
To analyze the alcohol content of a certain wine, a chemist needs 1.00 L of an aqueous 0.200 M K2Cr2O7 (potassium dichromate) solution. How much solid K2Cr2O7 must be weighed out to make this
Using the solubility rules in Table 4.1, predict what will happen when the following pairs of solutions are mixed.a. KNO3(aq) and BaCl2(aq)b. Na2SO4(aq) and Pb(NO3)2(aq)c. KOH(aq) and Fe(NO3)3(aq)
For each of the following reactions, write the molecular equation, the complete ionic equation, and the net ionic equation.a. Aqueous potassium chloride is added to aqueous silver nitrate to form a
Calculate the mass of solid NaCl that must be added to 1.50 L of a 0.100 M AgNO3 solution to precipitate all the Ag+ ions in the form of AgCl.
When aqueous solutions of Na2SO4 and Pb(NO3)2 are mixed, PbSO4 precipitates. Calculate the mass of PbSO4 formed when 1.25 L of 0.0500 M Pb(NO3)2 and 2.00 L of 0.0250 M Na2SO4 are mixed.
Phosphorite, also called phosphate rock, is a mineral containing PO43– and OH– anions and Ca2+ cations. It is treated with sulfuric acid in the manufacture of phosphate fertilizers (see Chapter
What volume of a 0.100 M HCl solution is needed to neutralize 25.0 mL of a 0.350 M NaOH solution?
In a certain experiment 28.0 mL of 0.250 M HNO3 and 53.0 mL of 0.320 M KOH are mixed. Calculate the amount of water formed in the resulting reaction. What is the concentration of H+ or OH– ions in
An environmental chemist analyzed the effluent (the released waste material) from an industrial process known to produce the compounds carbon tetrachloride (CCl4) and benzoic acid (HC7H5O2), a weak
Assign oxidation states to all of the following atoms.a. CO2 b. SF6 c. NO3–
Because metals are so reactive, very few are found in nature in pure form. Metallurgy involves reducing the metal ions in ores to the elemental form. The production of manganese from the ore
Cerium(IV) ion is a strong oxidizing agent that accepts one electron to produce cerium(III) ion:A solution containing an unknown concentration of Sn2+ ions was titrated with a solution containing
Iron ores often involve a mixture of oxides and contain both Fe2+ and Fe3+ ions. Such an ore can be analyzed for its iron content by dissolving it in acidic solution, reducing all the iron to Fe2+
You have a sugar solution (solution A) with concentration \(x\). You pour one-third of this solution into a beaker and add an equivalent volume of water (solution B).a. What is the ratio of sugar in
Which of the following must be known to calculate the molarity of a salt solution (there may be more than one answer)?a. The mass of salt addedb. The molar mass of the saltc. The volume of water
Consider separate aqueous solutions of \(\mathrm{HCl}\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}\), each with the same molar concentration. An aqueous solution of \(\mathrm{NaOH}\) is added to each
Which of the following statements is (are) true? Correct the false statements.a. A concentrated solution in water will always contain a strong or weak electrolyte.b. A strong electrolyte will break

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