Principles of Modern Chemistry
8th Edition
ISBN: 9781305079113
Author: David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher: Cengage Learning
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Because barium sulfate is opaque to X-rays, it is suspended in water and taken internally to make the gastrointestinal tract visible in an X-ray photograph. Although barium ion is quite toxic, barium sulfate’s Ksp of 1.1 x 10–10 gives it such low solubility that it can be safely consumed.
(a) What is the molar solubility of BaSO4?
(b) What is its solubility in grams per 100 g of water?
(a) If the molar solubility of Mg3(PO4)2 at 25 oC is 6.26e-06 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 0.00336 g of Ag2C2O4 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Ag2C2O4.Ksp = (c) The Ksp of Sc(OH)3 at 25 oC is 2.22e-31. What is the molar solubility of Sc(OH)3?solubility = mol/L
The thermodynamic solubility product of AGCN is 6.0x10-17.
(a) What is [Ag+] in a 0.033 M KNO3 solution?
4.0
7.7e-9
X mol·L-1
(b) What is [Ag+] in a 0.033 M KCN solution?
4.0 1.8e-15
X mol·L-1
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- 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_forwardAccording to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?arrow_forwardnitrous acid is estimated, c) What is the pH of the groundwater sample in which dichromate is oxidized to chromic ion by ethanol, which is simultaneously transformed to dissolved carbon dioxide? Modeling studies show that equilibrium is 1.75 x 107 M, dichromate ion is 7.3 x 10-2 M, chromic ion is 8.2 x 10°, ethanol is 6.8 x 102, and carbon dioxide is 6.4 x 10%. dr for the state of South Carolina, describearrow_forward
- The solubilities of the following compounds are listed below. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for (2) each. (a) BaSeO4, 0.0118 g/100 mL (b) Ba(BrO3)2·H2O, 0.30 g/100 mL (c) NH,MgAsOa•6H2O, 0.038 g/100 mL (d) La2(MoO4)3, 0.00179 g/100 mLarrow_forwardIf the molar solubility of Ag2SOA In water is 1.44 x 102 M, calculate the solubility product, Kn, forAgSO.arrow_forward(a) If the molar solubility of YF3 at 25 °C is 4.23e-06 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found that 0.00100 g of BaCO3 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility-product constant for BaCO3. Ksp = (c) The Ksp of ZnCO3 at 25 °C is 1.46e-10. What is the molar solubility of ZnCO3? solubility = mol/Larrow_forward
- The solubility product for calcium phosphate is Ksp= 1.3 × 10–26. What is the molar solubility of calcium phosphate?arrow_forwardThe molar solubility of magnesium carbonate in a water solution is M.arrow_forwardA buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the0.500 mol·dm–3 HLac solution is mixed with 0.300 dm3 of the 0.300 mol·dm–3 NaLac solutionto prepare the buffer. Ka for lactic acid (HLac) is 1.4 x 10–4 a.Calculate the pH of the buffer solution. [2]b.What will the pH of the above solution be after 5.0 cm3 of 0.200 mol·dm–3 NaOH hasbeen added to only 100.0 cm3 of this bufferarrow_forward
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