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Chapter 16
Aqueous Ionic Equilibrium
| The antidote for ethylene glycol poisoning is the administration of ______________. | ethyl alcohol (alcoholic drinks) |
| An important buffer in the blood is a mixture of _______________. | carbonic acid and bicarbonate ion |
| Identify a good buffer. | significant amounts of both a weak acid and its conjugate base |
| A buffer is most resistant to pH chane when | [acid] = [conjugate base] |
| Define buffer capacity. | the amount of acid or base that can be added to a buffer w/o destroying its effectiveness |
| The equivalence point is where | the amount of acid equals the amount of base during any acid-base titration. |
| When titrating a strong monoprotic acid and KOH at 25 C, the | pH will be equal to 7 at the equivalence point |
| When titrating a weak monoprotic acid and NaOH at 25 C, the | pH will be greater than 7 at the equivalence point |
| When titrating a monoprotic strong acid and a weak base at 25 C, the | pH will be less than 7 at the equivalence point |
| Stalacites and stalagmites form us ______________ precipitates out of the water evaporating in underground caves. | calcium carbonate |
| Give the equation for an unsaturated solution in comparing Q w/ Ksp. | Q<Ksp |
| Give the equation for an saturated solution in comparing Q w/ Ksp. | Q=Ksp |
| Give the equation for an supersaturated solution in comparing Q w/ Ksp. | Q>Ksp |
| A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 in NaCl. What will happen once these solutions are mixed? Ksp(AgCl) = 1.77 x 10^-10 | Silver chloride will precipitate out of solution, leavig a saturated AgCl soultion |
| A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 4.75 x 10^-5 M in AgNO3 and 0.075 in NaCl. What will happen once these solutions are mixed? Ksp(CaC2O4) = 2.3 x 10-9 | Nothing will happen since Ksp > Q for all possible precipitants |
| A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 3.5 x 10-4 M in calcium ion and 2.33 x 10-4 M in oxalate ion. What will happen once these solutions are mixed? Ksp(CaC2O4) = 2.3 x 10-9 | A precipitate will form since Q>Ksp for calcium oxalate |
| Which of the following solutions is a good buffer system? | A solution that is 0.10 M HCN and 0.10 M LiCN A solution that is 0.10 M HC2H3O2 and 0.10 M LiC2H3O2 |
| A buffer resists pH change by | neutralizing added acids and bases |
| The pH does not increase drastically b/c the NaOH reacts with the ______________ present in the buffer solution. | hydrazoic acid |
| The pH does not decrease drastically b/c the HCl reacts with the ______________ present in the buffer solution. | chloroacetate ion |
| The highest pH for an effective buffer occurs when the base is how many times as concentrated as the acid? | 10 |
| Which of the following acids (listed w/ pKa values) and their conjugate base would form a buffer w/a pH of 8.10? | HClO, pKa = 7.54 |
| Which of the following acids (listed w/ Ka values) and their conjugate base would form a buffer w/ a pH of 2.34? | HClO2, Ka = 1.1 x 10-2 |
| A 1.0 L buffer solution is 0.250 M HC2H3O2 and 0.050 M LiC2H3O2. Which of the following actions will destroy the buffer? | adding 0.050 moles of HCl |
| A 1.0 L buffer solution is 0.250 M HC2H3O2 and 0.250 M NaC2H3O2. Which of the following actions will destroy the buffer? | adding 0.050 moles of KOH |
| Identify the pH of normal blood. | 7.4 |
| Identify the most common indicator. | phenolphthalein |
| Identify the indicator that can be used at the lowest pH. | crystal violet |
| Identify the indicator that has two endpoints | alizarin |
| Identify the indicator that can be used at the highest pH. | alizarin yellow R |
| Which of the following compounds will have the highest molar solubility in pure water? | MgCO3, Ksp = 6.82 x 10-6 Fe(OH)3, Ksp = 2.79 x 10-39 |
| Which of the following compounds will be more soluble in acidic solution than in pure water? | Fes |
| Identify the salts that are in hard water. | CaCO3 and MgCO3 |
| Which of the following compounds solubility will bot be affected by a low pH in solution? | AgCl |
| Determine the molar solubility of CaSO4 in a solution containing 0.12 M Na2SO4. Ksp(CaSO4) = 2.4 x 10-5 | 2.0 x 10-4 M |
| Give the expression for the stability product constant for PbCl2 | [Pb2][Cl-]2 |
| Give the expression for the stability product constant for BaF2 | [Ba2+][F-]2 |
| Give the expression for the stability product constant for Ca3(PO4)2 | [Ca2+]3[PO4^3-]2 |
| Give the expression for the stability product constant for Cr2(CO3)3 | [Cr3+]2[CO3^2-]3 |
| Identify the compound that is acid-insoluble. | As2S3 |
| Identify the compound that is base-insoluble | ZnS |
| Define entropy. | a thermodynamic function that increases w/ a number of energetically equivalent ways to arrange the components of a system to achieve a particular state. |
| Define the second law of thermodynamics | For any spontaneous process, the entropy of the universe increase |
| Give the standard state for a gas | 1 atm |
| Give the standard state for a liquid | 1 atm;25 C |
| Give the standard state for a solid | 1 atm;25C |
| Give the standard state for a solution | 1 M;1 atm |
| Define the thrid law of thermodynamic | The entropy of a perfect crystal at absolute zero (0 K) is zero |
| Define allotrope | two or more forms of an element existing in the same size |
| A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 M HCl. | AgCl |
| A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 M HCl, then H2S and 0.2 M HCl. | CuS |
| A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 M HCl; H2S and 0.2 M HCl; and OH- to a pH of 8. | MnS |
| A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the precipitate after the addition of 6 M HCl; H2S and 0.2 M HCl; OH- to a pH of 8; and (NH4)2HPO4 with NH3. | Ca3(PO4) |
| A sample contains Ba3(PO4)2, CdS, AgCl, NH4Cl, and ZnS. Identify the soluble ions after the addition of 6 M HCl; H2S and 0.2 M HCl; OH- to a pH of 8; and (NH4)2HPO4 with NH3. | NH4Cl |
| A ligand is a molecule or ion that acts as a | Lewis base |
| Describe the solubility of Al(OH)3 with respect to pH | soluble at low pH, insoluble in pH-neutral solution, and soluble at high pH |
| Gives what happens at low pH for aluminum hydroxide. | Al(H2O)63+ dissolves |
| Gives what happens at neutral pH for aluminum hydroxide | Al(OH)3 precipitates |
| Gives what happens at high pH for aluminum hydroxide | Al(H2O)2(OH)4- dissolves |
| pH = 7 | equivalence point of a strong acid/strong base titration |
| pH = pKa | half-way to equivalence point of a weak acid/strong base titration |
| pH > 7 | equivalence point of a weak acid/strong base titration |
| pH < 7 | equivalence point of a weak base/strong acid titration |
| pH = pKa2 | 3/4 of the way to second equivalence point of a diprotic acid/strong base titration |
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