The solubility of Ni(OH) 2 in water at 25 °C is measured to be 4.9 × 10 Round your answer to 2 significant digits. -4 g L ☐ ☐ x10 ✗ . Use this information to calculate K sp for Ni(OH)2. Calculate the solubility at 25 °C of PbCO3 in pure water and in a 0.0020M Pb (NO3)2 solution. You'll find Kp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. sp solubility in pure water: solubility in 0.0020 M Pb(NO3)2 solution: ㅁ른 品 □×□ ㅁㅁ

The solubility of Ni(OH) 2 in water at 25 °C is measured to be 4.9 × 10 Round your answer to 2 significant digits. -4 g L ☐ ☐ x10 ✗ . Use this information to calculate K sp for Ni(OH)2. Calculate the solubility at 25 °C of PbCO3 in pure water and in a 0.0020M Pb (NO3)2 solution. You'll find Kp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. sp solubility in pure water: solubility in 0.0020 M Pb(NO3)2 solution: ㅁ른 品 □×□ ㅁㅁ

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.96QE: The concentration of barium in a saturated solution of barium sulfate at a particular temperature is...

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According 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?
Calcium hydroxide, Ca(OH)2, dissolves in water to the extent of 1.78 g per liter. What is the value of Ksp for Ca(OH)2? Ca(OH)2(s)Ca2+(aq)+2OH(aq)
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 /Csp of 1.1 X 10-,<) gives it such low solubility' that it can be safely consumed. What is the molar solubility' of BaSO4. What is its solubility' in grams per 100 g of water?
Magnesium hydroxide, Mg(OH)2, is the active ingredient in die antacid TUMS and has a Ksp value of 8.9 1012. If a 10.0-g sample of Mg(OH)2 is placed in 500.0 mL of solution, calculate the moles of OH ions present. Because the Ksp value for Mg(OH)2 is much less than 1, not a lot of solid dissolves in solution. Explain how Mg(OH)2 works to neutralize large amounts of stomach acid.
Solubility is an equilibrium position, whereas Ksp is an equilibrium constant. Explain the difference.
Sodium chloride is added to water (at 25C) until it is saturated. Calculate the Cl concentration in such a solution. Species G(kJ/mol) NaCl(s) 384 Na+(aq) 262 Cl(aq) 131
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)
The ore cinnabar (HgS) is an important source of mercury. Cinnabar is a red solid whose solubility in water is 5.5 X 10-2 mol L-1. Calculate its \p. What is its solubility' in grams per 100 g of water?
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 â€¢ no precipitate? â€¢ a precipitate of BaCO3 only? â€¢ a precipitate of CaCO3 only? â€¢ 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.
You are given four different aqueous solutions and told that they each contain NaOH, Na2CO3, NaHCO3, or a mixture of these solutes. You do some experiments and gather these data about the samples. Sample A: Phenolphthalein is colorless in the solution. Sample B: The sample was titrated with HCl until the pink color of phenolphthalein disappeared, then methyl orange was added. The solution became pink. Methyl orange changes color from pH 3.01 (red) to pH 4.4 (orange). Sample C: Equal volumes of the sample were titrated with standardized acid. Using phenolphthalein as an indicator required 15.26 mL of standardized acid to change the phenolphthalein color. The other sample required 17.90 mL for a color change using methyl orange as the indicator. Sample D: Two equal volumes of the sample were titrated with standardized HCl. Using phenolphthalein as the indicator, it took 15.00 mL of acid to reach the equivalence point; using methyl orange as the indicator required 30.00 mL HCl to achieve neutralization. Identify the solute in each of the solutions.
The concentration of barium in a saturated solution of barium sulfate at a particular temperature is 1.2 g/mL. Calculate Ksp at this temperature.
The solubility rules outlined in Chapter 4 say that Ba(OH)2, Sr(OH)2, and Ca(OH)2 are marginally soluble hydroxides. Calculate the pH of a saturated solution of each of these marginally soluble hydroxides.