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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EBK GENERAL CHEMISTRY
- A 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_forwardWhat must the ratio of H2PO4 to HPO42 be to have a buffer with a pH value of 7.00?arrow_forwardCalculate the solubility of aluminum hydroxide, Al(OH)3, in a solution buffered at pH 11.00.arrow_forward
- A 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_forwardThe solubility of cadmium oxalate. CdC2O4, in 0.150 M ammonia is 6.1 103 mol/L. What is the oxalate-ion concentration in the saturated solution? If the solubility product constant for cadmium oxalate is 1.5 108, what must be the cadmium-ion concentration in the solution? Now calculate the formation constant for the complex ion Cd(NH3)42+.arrow_forwardPhosphate ions are abundant in cells, both as the ions themselves and as important substituents on organic molecules. Most importantly, the pKa for the H2PO4 ion is 7.20, which is very close to the normal pH in the body. H2PO4(aq) + H2O() H3O+(aq) + HPO42(aq) 1. What should the ratio [HPO42]/[H2PO4] be to control the pH at 7.40?arrow_forward
- Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 1.00 102 mL of solution and then titrate the solution with 0.108 M NaOH. C6H5CO2H(aq) + OH(aq) C6H5CO2(aq) + H2O() (a) What was the pH of the original benzoic add solution? (b) What are the concentrations of all of the following ions at the equivalence point: Na+, H3O+, OH, and C6H5CO2? (c) What is the pH of the solution at the equivalence point?arrow_forwardThe solubility of zinc oxalate, ZnC2O4, in 0.0150 M ammonia is 3.6 104 mol/L. What is the oxalate-ion concentration in the saturated solution? If the solubility product constant for zinc oxalate is 1.5 109, what must be the zinc-ion concentration in the solution? Now calculate the formation constant for the complex ion Zn(NH3)42+.arrow_forwardCalculate the molar solubility of Sn(OH)2 in a buffer solution containing equal concentrations of NH3 and. NH4+.arrow_forward
- The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)arrow_forwardCalculate the solubility in grams per 100 mL of BaF2 in a 0.10 M BaCl2 solution.arrow_forwardA sample of impure tin of mass 0.530 gg is dissolved in strong acid to give a solution of Sn2+Sn2+. The solution is then titrated with a 0.0448 molL−1molL−1 solution of NO3−(aq)NO3−(��), which is reduced to NO(g)NO(�). The equivalence point is reached upon the addition of 3.91×10−2 LL of the NO3−(aq)NO3−(��) solution. Part A Find the percent by mass of tin in the original sample, assuming that it contains no other reducing agents.arrow_forward
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