SMARTWORKS FOR CHEMISTRY: ATOMS FOCUSED
2nd Edition
ISBN: 9780393644777
Author: Gilbert
Publisher: MCGRAW-HILL HIGHER EDUCATION
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What change will be caused by addition of a small amount
of Ba(OH)2 to a buffer solution containing nitrous acid,
HNO2, and potassium nitrite, KNO₂?
O The concentration of hydronium ions will increase significantly.
O The concentration of nitrous acid will increase as will the
concentration of hydronium ions.
O The concentration of nitrite ion will decrease and the
concentration of nitrous acid will increase.
The concentration of nitrous acid will decrease and the
concentration of nitrite ions will increase.
1) Write the equilibrium expression for the solid calcium hydroxide and the dissolved ions.
A saturated, aqueous, solution of Ca(OH)2 equation:
Ca(OH)2 (s) ↔ Ca2+ (aq) + 2OH– (aq)
The equilibrium expression for calcium hydroxide:
Ksp = [Ca2+][OH–]2
If the solubility of silver carbonate (Ag2CO3) is 1.3 x 10-4 mol/L, what is the concentration of the Ag+ ion?
Chapter 16 Solutions
SMARTWORKS FOR CHEMISTRY: ATOMS FOCUSED
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- Consider 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_forwardWhen 250 mg of SrF2, strontium fluoride, is added to 1.00 L of water, the salt dissolves to a very small extent. SrF2(s)Sr2+(aq)+2F(aq) At equilibrium, the concentration of Sr2+ is found to be 1.03 103 M. What is the value of Ksp for SrF2?arrow_forwardSolubility is an equilibrium position, whereas Ksp is an equilibrium constant. Explain the difference.arrow_forward
- What is the difference between the ion product, Q, and the solubility product, Ksp? What happens when Q Ksp? Q Ksp? Q = Ksp?arrow_forwardCalcium 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)arrow_forwardThe solubility of Mg(OH)2 in water is approximately 9.6 mg/L at a given temperature. Calculate the Ksp of magnesium hydroxide. Calculate the hydroxide concentration needed to precipitate Mg2+ ions such that no more than 5.0 μg Mg2+ per liter remains in the solution.arrow_forward
- Some 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 Ksp value for radium sulfate, RaSO4, is 4.2 1011. If 25 mg of radium sulfate is placed in 1.00 102 mL of water, does all of it dissolve? If not, how much dissolves?arrow_forwardA solution saturated with a salt of the type M3X2 has an osmotic pressure of 2.64 102 atm at 25C. Calculate the Ksp value for the salt, assuming ideal behavior.arrow_forward
- Although silver chloride is insoluble in water, it readily dissolves upon the addition of ammonia. AgCl(s)+2NH3(aq)Ag(NH3)2+(aq)+Cl(aq) a What is the equilibrium constant for this dissolving process? b Ammonia is added to a solution containing excess AgCl(s). The final volume is 1.00 L and the resulting equilibrium concentration of NH3 is 0.80 M. Calculate the number of moles of AgCl dissolved, the molar concentration of Ag(NH3)2+, and the number of moles of NH3 added to the original solution.arrow_forwardA concentration of 10–100 parts per billion (by mass) of Ag+ is an effective disinfectant in swimming pools. However, if the concentration exceeds this range, the Ag+ can cause adverse health effects. One way to maintain an appropriate concentration of Ag+ is to add a slightly soluble salt to the pool. Calculate the equilibrium concentration of Ag+ in parts per billion thatwould exist in equilibrium with (a) AgCl, (b) AgBr, (c) AgI.arrow_forwardSwimming pool disinfectants produce hypochlorous acid upon dissolution. The weak acid ionizes as follows: HClO (aq) ⇄ H+ (aq) + ClO‒ (aq) Ka=3.0 x 10 ‒8 As strong oxidizing agents, both acid and its conjugate base kill bacteria. However, too high [HClO] is irritating to swimmers’ eyes and too high [ClO‒] will cause the ions to decompose in sunlight. The recommended pH to circumvent both problems is 7.8. Determine the ratio of the weak acid and its conjugate base at this pH.arrow_forward
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