Concept explainers
(a)
Interpretation:
Net ionic equations for precipitation of PbCl2(s) from a solution containing Pb2+ should be written.
Concept introduction:
The net ionic equation shows only the chemical species which involve in the
(b)
Interpretation:
Net ionic equations for the dissolution of
Concept introduction:
The net ionic equation shows only the chemical species which involve in the chemical reaction.
(c)
Interpretation:
Net ionic equations for the dissolution of
Concept introduction:
The net ionic equation shows only the chemical species which involve in the chemical reaction.
(d)
Interpretation:
Net ionic equations for the precipitation of
Concept introduction:
The net ionic equation shows only the chemical species which involve in the chemical reaction.
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GENERAL CHEMISTRY(LL)-W/MASTERINGCHEM.
- Calculate the solubility of aluminum hydroxide, Al(OH)3, in a solution buffered at pH 11.00.arrow_forwardA volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of MgCl2. What mass of NH4Cl must be added to the resulting solution to prevent the precipitation of Mg(OH)2?arrow_forwardA few drops of each of the indicators shown in the accompanying table were placed in separate portions of a 1.0-M solution of a weak acid, HX. The results are shown in the last column of the table. What is the approximate pH of the solution containing HX? Calculate the approximate value of Ka for HX. Indicator Color of Hln Color of ln pKa of Hln Color of 1.0 M HX Bromphenol blue Yellow Blue 4.0 Blue Bromcresol purple Yellow Purple 6.0 Yellow Bromcresol green Yellow Blue 4.8 Green Alizarin Yellow Red 6.5 Yellowarrow_forward
- What must the ratio of H2PO4 to HPO42 be to have a buffer with a pH value of 7.00?arrow_forwardA saturated solution of magnesium hydroxide is prepared and the excess solid magneisum hydorixed is allowed to settle. A 25.0 mL aliquot of the saturated solution is withdrawn and transfered to a flask, two drops of inficator are added. A 0.00053 M HCL is dispensed from a buret into a solution. The solution changes color after the addition of 13.2 mL. What is the molar solubility of magnesium hydroxide?arrow_forwardThe permanganate ion (MnO4- ) is often used in redox titrations. The strongly colored (violet)the permanganate ion forms the slightly pink Mn2+ ion upon reaction in acidic solution.Permanganate solutions are prepared by dissolving solid potassium permanganate. Atpreparation and storage of the solution, however, often forms brownstone (MnO 2 (s)) which mustfiltered before use. The concentration of the solution is therefore determined directly beforeuse by titration in sulfuric acid solution against sodium oxalate (Na2 C2 O4 ;easily soluble salt that serves as the primary standard) whereby the oxalic acid forms carbon dioxide (gas).Calculate the concentration of a potassium permanganate solution from the following data.0.6501 gram of sodium oxalate is weighed and consumes 20.00 mL of the preparedthe potassium permanganate solution.arrow_forward
- Calculate the solubility of AgBr in a 1.00 M aqueous solution of ammonia, given: AgBr(s) ⇌ Ag+(aq) + Br-(aq) Ksp = 7.7 x 10-13 Ag+(aq) + 2 NH3(aq) ⇌ Ag(NH3)2+(aq) Kf = 1.7 x 107 [Hint: combine these reactions into a single reaction].arrow_forwardCalculate the solubility of AgBr in a 1.00 M aqueous solution of ammonia, given: AgBr(s) ⇌ Ag+(aq) + Br-(aq) Ksp = 7.7 x 10-13 Ag+(aq) + 2 NH3(aq) ⇌ Ag(NH3)2+(aq) Kf = 1.7 x 107arrow_forwarda.) What is the precipitation pH in gravimetric sulfate determination? Why is precipitation not done in a strongly acidic medium? What inconvenience does it cause if the heating process is over 800 °C?b.) What is the K2SO4 content of a sample that gives 0.699 g of precipitate in HCl with BaCl2 solution? (BaSO4: 233; K2SO4: 175).arrow_forward
- 134 grams of potassium sorbate KCH3 (CH)4CO2 is fully dissolved in 100.00 mL of water, which is carefully transferred to a conical flask. Then 100.00 mL of 0.240 M HNO3 is added dropwise to this solution from a burette. Given: Ka (sorbic acid) = 1.7 × 1O^-5 Showing all your calculations and reasoning, determine the pH of the solution that results after the addition of all the acid mentioned above. Suppose that the titration continues. Determine the pH of the solution in the flask at theequivalence pointarrow_forwardThe concentration of Ag+ ion in a saturated solution of Ag2C2O4 is 2.3 x 10-4 mol/L. Calculate the solubility product Ksp for this salt.arrow_forwardWhat is the molar solubility of manganese carbonate in water? The solubility product constant for MnCO3 is 5.0 x 10^-10 at 25 degrees Celsiusarrow_forward
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