Concept explainers
Use the following solubility data to calculate a value of
(a)
(b)
(c)
(d)
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CHEMISTRY-TEXT
- To a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of Na2CO3. After equilibrium is established, will there be • no precipitate? • a precipitate of BaCO3 only? • a precipitate of CaCO3 only? • a precipitate of both CaCO3 and BaCO3? Assume that the volume of the solution is still 500.0 mL after the addition of the salts.arrow_forwardAcrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’. What is the pH of a 0.11 M solution of acrylic acid, CH2CHCOOH?arrow_forwardConsider the reaction AgC2H3O2(s)+Cl(aq)AgCl(s)+C2H3O2(aq)(a) Calculate K for the reaction. (b) Will more AgCl precipitate if H+ ions are added?arrow_forward
- A 1.0-L solution that is 4.2 M in ammonia is mixed with 26.7 g of ammonium chloride. a What is the hydroxide-ion concentration of this solution? b 0.075 mol of MgCl2 is added to the above solution. Assume that there is no volume change. After Mg(OH)2 has precipitated, what is the molar concentration of magnesium ion? What percent of the Mg2+ is removed from solution?arrow_forwardA solution is prepared by mixing 13.00 mL of 0.0021 M aqueous Hg2(NO3)2 with 25.0 mL of 0.015 M HCl. Assume that volumes are additive. (a) Will precipitation occur? (b) Calculate [Hg22+], [Cl-], and after equilibrium is established.arrow_forwardSketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.arrow_forward
- A solution contains 0.00740 M calcium ion. A concentrated sodium fluoride solution is added dropwise to precipitate calcium fluoride (assume no volume change). a At what concentration of F does precipitate start to form? b When [F] = 9.5 104 M, what is the calcium-ion concentration? What percentage of the calcium ion has precipitated?arrow_forwardHow would the solubility of calcium fluoride be affected by the presence of fluoride ion from another source? What is the solubility of calcium fluoride in a saturated solution of barium fluoride? How does this compare with the value of the solubility of calcium fluoride found in Example 17.4? Is this what you expect?arrow_forwardMarble is almost pure CaCO3. Acid rain has a devastating effect on marble statuary left outdoors. Assume that the reaction which occurs is CoCO3(s)+ H+(aq)Ca2+(aq)+HCO3(aq) Neglecting all other competing equilibria and using Tables 15.1 and 13.2, calculate (a) K for the reaction. (b) the molar solubility of CaCO3 in pure water. (c) the molar solubility of CaCO3 in acid rainwater with a pH of 4.00.arrow_forward
- Hydrogen iodide gas decomposes to hydrogen gas and iodine gas: 2HI(g)H2(g)+I2(g)To determine the equilibrium constant of the system, identical one-liter glass bulbs are filled with 3.20 g of HI and maintained at a certain temperature. Each bulb is periodically opened and analyzed for iodine formation by titration with sodium thiosulfate, Na2S2O3. I2(aq)+2S2O32(aq)S4O62(aq)+2 I(aq)It is determined that when equilibrium is reached, 37.0 mL of 0.200 M Na2S2O3 is required to titrate the iodine. What is K at the temperature of the experiment?arrow_forwardConsider a 2.0-L aqueous solution of 4.17 M NH3, where 21.0 g of NH4Cl are dissolved. To this solution, 4.8 g of CaCl2 are added. (a) What is [OH-] before CaCl2 is added? (b) Will a precipitate form? (c) What is [Ca2+] after equilibrium is established?arrow_forwardCalcium nitrate is added to a sodium sulfate solution that is 0.0150 M. (a) At what concentration of Ca2+ does a precipitate first start to form? (b) Enough Ca(NO3)2 is added to make [ Ca2+ ]=0.0075 M. What percentage of the original sulfate ion has precipitated?arrow_forward
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