. A 25 °C, 1 L water sample has the following species present in addition to other ions: [H*]=108.3 mol/L, [HCO3]=10² mol/L, [Mg²+]=104 mol/L. a. To what pH must the water be adjusted to precipitate Mg(OH)2, Ksp for Mg(OH)2 is 10-10.74 b. How many moles of OH must be added to reach the pH for precipitation of Mg(OH)2. Ronuc Ouoctionı

. A 25 °C, 1 L water sample has the following species present in addition to other ions: [H*]=108.3 mol/L, [HCO3]=10² mol/L, [Mg²+]=104 mol/L. a. To what pH must the water be adjusted to precipitate Mg(OH)2, Ksp for Mg(OH)2 is 10-10.74 b. How many moles of OH must be added to reach the pH for precipitation of Mg(OH)2. Ronuc Ouoctionı

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 76QAP

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A solution is made up by adding 0.632 g of barium nitrate and 0.920 g of lanthanum nitrate, to La(NO3)3 enough water to make 0.500 L of solution. Solid sodium iodate, NalO3, is added (without volume change) to the solution. (a) Which salt will precipitate first? La(IO3)3 (Ksp=7.501012) or BAIO3 (Ksp=4.0109)? (b) What is [IO3-] when the salt in (a) first begins to precipitate?
59. Iron(II) hydroxide, Fe(OH)2, has a solubility in water of 6.0 x 10¹ mg/L at a given temperature. (a) From this solubility, calculate the Ksp of iron(II) hydrox- ide. Explain why the calculated K differs from the experimental value of 8.0 X 10-16. (b) Calculate the hydroxide concentration needed to precip tate Fe²+ ions such that no more than 1.0 µg Fe²+ per liter remains in the solution. 1x 10¹, in
142.)What is the molar solubity of Al(OH)3 in s solution containing 6.81x10^-3 M NAOH? Ksp (Al(OH)3) =4.6x10^-33 what is the molar solublity
A student titrates 20.0 mL of 1.0 M NaOH with 2.0 M formic acid, HCOOH (K, = 1.8 x 104). Hypochlorous acid is an unstable compound and one of the decomposition products is chlorine gas, Cl2. The composition of the acid lowers its concentration over time. What effect will the decomposition of one-fourth of the acid have on the agreement between the endpoint of the titration and the equivalence point during a titration with standard sodium hydroxide? It is impossible to determine The endpoint would be before the ideal equivalence point The endpoint would be after the ideal equivalence point The endpoint will rema eerthe ideal egvaleacepolnt
5. DETAILS UCSCGENCHEML1 10.RQ.005. A saturated solution of Pb(OH)2 was found to contain 4.1x10-8 mol OH in 100.0 mL. Calculate the Kep of Pb(OH)2. If an ionic solid is very insoluble, will the saturated solution have relatively low or relatively high concentrations of the aqueous ions? o relatively low o relatively high
The generic metal hydroxide M(OH)2M(OH)2 has KspKspK_sp = 8.05×10−12. (NOTE: In this particular problem, because of the magnitude of the KspKsp and the stoichiometry of the compound, the contribution of OH−OH− from water can be ignored. However, this may not always be the case.) Part A) What is the solubility of M(OH)2M(OH)2 in pure water? Part B) What is the solubility of M(OH)2M(OH)2 in a 0.202 MM solution of M(NO3)2M(NO3)2?
Lead (II) bromide, PbBr2, has Ksp = 4.6 x 10–6. (a) Will precipitate of PbBr2 form when 20.0 mL of 0.10 M Pb(NO3)2 is reacted with 30.0 mL of 0.10 M NaBr? (b) Determine the concentration of Pb2+, NO3–, Na+, and Br–, respectively, in the saturated solution at equilibrium. (c) How many grams of PbBr2 precipitate are formed at equilibrium? (Hint: use successive approximation method to determine concentrations of Pb2+ and Br– at equilibrium.)
Lead (II) bromide, PbBr2, has Ksp= 4.6 x 10–6. (a) Will precipitate of PbBr2 form when 20.0 mL of 0.10 M Pb(NO3)2 is reacted with 30.0 mL of 0.10 M NaBr? (b) Determine the concentration of Pb2+, NO3–, Na+, and Br–, respectively, in the saturated solution at equilibrium. (c) How many grams of PbBr2 precipitate are formed at equilibrium? (Hint: use successive approximation method to determine concentrations of Pb2+and Br–at equilibrium.)
1. Which of these statements about the common-ion effect is most correct? (A) the solubility of a salt MA is decreased in a solution that already contains either M+ or A- (B) common ions alter the equilibrium constant for the reaction of an ionic solid with water. (C) the common ion effect does not apply to unusual ions like SO32-. (D) the solubility of a salt MA is affected equally by the addition of either A- or an uncommon ion. Group of answer choices Statement (C) is most correct. Statement (A) is most correct. Statement (B) is most correct. Statement (D) is most correct.
Magnesium sulfate,MgSo4 is added to 165 mL of 9.60x10^-2 M NaOH, sodium hydroxide, until precipitate just forms. How many grams of magnesium sulfate were added? Assume that the volume of the solution is not changed significantly by the addition of magnesium sulfate. Ksp (Mg(OH)2) = 1.8x10^-11
One way to reduce the presence of lead in water is to add a phosphate corrosion inhibitor, which forms an insoluble saltwith lead, coating the pipes with a protective mineral later: Pb3(PO4)2(s) ⇌ 3Pb2+(aq) + 2PO43-(aq) Kc=9.9 x 10-55 a.) Calculate the solubility of lead (Pb2+) in g/L when Pb3(PO4)2 is dissolved in water. b.) The acceptable level of lead in water is less than 1x10-6g/L. If phosphate is added to drinking water, does it keep the lead levels below the allowed limit? c.) In 2014, the city of Flint, MI, changed water sources to a system that didn’t include phosphate. Instead, it used chlorine to treat water. The Ksp of lead chloride is 1.5x10-5. The switch increased the levels of lead in the drinking water and significantly affected the community. Explain why switching water sources increased the lead levels in Flint’s drinking water.
For calcium fluoride, CaF2, Ksp = 4.0 x 10-11. What is the minimum concentration of Ca2+needed to precipitate CaF2 from a 0.20 M solution of sodium fluoride, NaF?

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