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Concept explainers
(a)
Interpretation:
The
Concept Introduction:
The equilibrium constant used for the partially soluble salt in water is termed as solubility product constant
The expression for
Generally, the concentration of solid is taken as constant. Therefore the expression for
(b)
Interpretation:
The
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
The
Concept Introduction:
Refer to part (a).
(d)
Interpretation:
The
Concept Introduction:
Refer to part (a).
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Chapter 16 Solutions
FOUND.OF COLLEGE CHEMISTRY
- What must be the concentration of chromate ion in order to precipitate strontium chromate, SrCrO4, from a solution that is 0.0034 M Sr2+?arrow_forwardSome barium chloride is added to a solution that contains both K2SO4 (0.050 M) and Na3PO4 (0.020 M). (a) Which begins to precipitate first: the barium sulfate or the barium phosphate? (b) The concentration of the first anion species to precipitate, either the sulfate or phosphate, decreases as the precipitate forms. What is the concentration of the first species when the second begins to precipitate?arrow_forwardThe solubility product constant for calcium oxalate is estimated to be 4 109. What is its solubility in grams per liter?arrow_forward
- How 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_forwardConsider the reaction BaF2(s)+SO42(aq)BaSO4(s)+2 F(aq) (a) Calculate K for the reaction. (b) Will BaSO4 precipitate if Na2SO4 is added to a saturated solution of BaF2?arrow_forwardBecause 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?arrow_forward
- Crystals of AgBr can be removed from black-and-white photographic film by reacting the AgBr with sodium thiosulfate. AgBr(s)+2S2O32(aq)[Ag(S2O3)2]3(aq)+Br(aq) a What is the equilibrium constant for this dissolving process? b In order to dissolve 2.5 g of AgBr in 1.0 L of solution, how many moles of Na2S2O3 must be added?arrow_forwardLead(II) chromate, PbCrO4, was used as a yellow paint pigment (chrome yellow). When a solution is prepared that is 5.0 104 M in lead ion, Pb2, and 5.0 105 M in chromate ion, CrO42, would you expect some of the lead(II) chromate to precipitate?arrow_forwardIf the concentration of Zn2+ in 10.0 mL of water is 1.63 104 M, will zinc hydroxide, Zn(OH)2, precipitate when 4.0 mg of NaOH is added?arrow_forward
- Acrylic 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_forwardA scientist was interested in how soluble rust is in acidic soils, so she set up an idealized problem to get an initial feel for the situation. A fairly acidic soil has a pH of 4.50. Also, rust is essentially Fe(OH)3. Therefore, she considered the following problem: Suppose a 1.00-g sample of iron(III) hydroxide is exposed to 1.00 L of a buffer with a pH of 4.50. She then calculated the nanograms of Fe3+ that dissolve in a liter of this buffer. Show how you would do this problem. Explain your work.arrow_forwardSolid lead nitrate is added to a solution that is 0.020 M in OH- and SO42-. Addition of the lead nitrate does not change the volume of the solution. (a) Which compound, PbSO4 or Pb(OH)2 (Ksp=2.81016), will precipitate first? (b) What is the pH of the solution when PbSO4 first starts to precipitate?arrow_forward
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