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A: Explanation given as follows
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Q: At 25°C, water dissolves 0.8108g of PbCl2 per liter, calculate the Kgp of PBCI2 at 25°C.
A: "Since, you have posted multiple question . We will solve first question for you. If you want any…
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Q: 10) How many miligrams of BaSO4 are dissolved in a 225 mL sample of BaSO4(aq)? (Hint: calculate the…
A: BaSO4 (s) ------> Ba2+ (aq) + SO42- (aq) Ksp = [Ba2+][SO42-]
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A: The neutralization reaction is given below.
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- The Ksp of Fe(OH)3(s) is 3x10-39. What concentration of Fe3+ can exist in solution at pH 3.0?What is the solubility of Pb3(PO4)2 if it's Ksp is 3.000e-44?6. Some sulfuric acid is spilledon a lab bench. You can neutralizethe acid by sprinkling sodiumbicarbonate on it and then moppingup the resultant solution. The sodiumbicarbonate reacts with sulfuric acidas follows:2 NaHCO3(s) + H2SO4(aq)Na2SO4(aq) + 2H2O(l) + 2CO2(g)Sodium bicarbonate is added until thefizzing due to the formation of CO2(g)stops. If 27 mL of 6.0 M H2SO4 wasspilled, what is the minimum mass ofNaHCO3 that must be added to thespill to neutralize the acid?
- (a) I f t he molar solubilit y o f CaF2 at 35 °C i s1.24 x 10-3 mol/L, what is Ksp at this temperature? (b) It isfound that 1.1 x 10-2 g SrF2 dissolves per 100 mL of aqueoussolution at 25 °C. Calculate the solubility product forSrF2. (c) The Ksp of Ba(IO3)2 at 25 °C is 6.0 x 10-10. What isthe molar solubility of Ba(IO3)2?If the solubility of Li2CO3(s) is 1.3 x 10-4 mol/L, what is its Ksp?A solution contains S 2– and SO 42– ions. In what order dowe add Ag(NO 3 )(aq) and Ba(NO 3) 2(aq) to separate eachanion independently? Which precipitates form?
- instead of dissolving Ag2SO4 (ksp = 7.8x10^-11) in water, you decide to dissolve it in a 2.0x10^-2 mol/L solution of AgNO3. What is it's solubility in this solution?Consider the reaction of 25.0 mL of 0.20 M AgNO3(aq) with 25.0 mL of 0.20 M NaBr(aq) to form AgBr(s) at 25 °C. What is ΔG for this reaction? The Ksp of AgBr is 5.0 × 10-13 at 25 °CKsp for Pb(IO3)2 is 2.5x10-13. What weight of Pb(IO3)2 will dissolve in 200 mL of water?
- (a) Given the Ksp of calcium phosphate, Ca3(PO4)2 is 1.3 ×10-32. Calculate the concentrations of Ca2+ and PO43- respectively.(b) If a hard water contains 75 mg/L of Ca2+, at what concentration of PO43− would a precipitate of Ca3(PO4)2 begin to appear?Was wondering how to solve this hw problem? Calcium Flouride (dissociation) K@25 C = 3.94 *10^-11 Calcium fluoride is not very soluble in water. ** Its dissociation is: CaF2 (s) Ca²+ (aq) + 2 F¯ (aq) a. At 25°C, how many milligrams of CaF2 would dissolve in 2.0 L of water? b. What were your initial and final values of Q?A sample of impure NaOH, which has been partially converted to Na2CO3 by exposure to CO2, is analyzed by titrating a 188.5 mg sample with 0.1065 M HCl. The volume required to reach phenolphtalein end point is 39.19 ml while the volume required to reach bromocresol green end point is 40.67 ml. Calculate the percentages of NaOH (MWt= 40 g/mole) and Na2CO3 (MWt=83 g/mole) in the sample.