In which solution will 0.000015 BaCl2 form a participate? a. 7.0x10^-7 M H2SO4 (ksp of BaSO4 = 1.1x10^-10) b. 0.10 M Pb(NO3)2 (ksp of PbCl2 = 1.7x10^-5) c. 0.010 M NaF (ksp of BaF2 = 1.7x10^-6) d. 5.0x10^-7 M AgNO3 (ksp of AgCl = 1.8x10^-10)
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In which solution will 0.000015 BaCl2 form a participate?
a. 7.0x10^-7 M H2SO4 (ksp of BaSO4 = 1.1x10^-10)
b. 0.10 M Pb(NO3)2 (ksp of PbCl2 = 1.7x10^-5)
c. 0.010 M NaF (ksp of BaF2 = 1.7x10^-6)
d. 5.0x10^-7 M AgNO3 (ksp of AgCl = 1.8x10^-10)
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- 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) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mLThe solubility of AX2 is 0.000047 M What is the Ksp of AX2?1. Find the number of millimoles of solute in a. 226 ?? of 0.320 ? HClO4. b. 25.0 ? of 8.05 ? 10−3 ? K2CrO4. c. 6.00 ? of an aqueous solution that contains 6.75 ??? of AgNO3. d. 537 ?? of 0.0200 ? KOH. 2. Describe the preparation of a. 5.00 ? of 0.0500 ? KMnO4 from the solid reagent. b. 4.00 ? of 0.250 ? HClO4, starting with an 8.00 ? solution of the reagent. c. 400 ?? of a solution that is 0.0250 ? in I2, starting with MgI2. d. 200 ?? of 1.00% (?/?) aqueous CuSO4 from a 0.365 ? CuSO4 solution. e. 1.50 ? of 0.215 ? NaOH from the concentrated commercial reagent [50% NaOH (w/w), ?? ?? = 1.525]. f. 1.50 ? of a solution that is 12.0 ??? in K+, starting with solid K4Fe(CN)6. 3. Exactly 75.00 ?? of a 0.3132 ? solution of Na2SO3 were treated with 150.0 ?? of 0.4025 ? HClO4 and boiled to remove the SO2 formed. a. What was the mass in grams of SO2 that was evolved? b. What was the concentration of the unreacted reagent (Na2SO3 or HClO4) after thereaction was complete?
- In which solution will 0.010 M Pb2+ remain soluble? a. 0.030 M Cl- (Ksp of PbCl2=1.7x10-5) b. 0.0020 M F- (Ksp of PbF2=3.6x10-8) c. 7.0x10-5M SO42- (Ksp of PbSO4=6.3x10-7) d. 3.0x10-11M CrO42- (Ksp of PbCrO4=2.8x10-13)A 370.00 mL solution of 0.00190 M AB5 is added to a 200.00 mL solution of 0.00165 M CD2. What is pQsp for AD5?In order to form Ba(IO3)2, 500 mL of 0.5000 M Ba(NO3)2 was mixed with 500 mL of 0.0500 M NaIO3. Ksp= 1.57x10^-9What is the concentration of the excess reagent?What is the molar solubility of Ba(IO3)2 in this solution? 2.04x10^-5 M 4.07x10^-5 M 6.15x10^-5 M 8.30x10^-5 M
- Consider the following reaction; 2S2O32- + I2 → 2I- + S4O62- If 10.0 mL of 0.10M S2O32- is needed to titrate a 50.0mL solution containing I2, what is the concentration (mol/L) of I2 in the unknown solution?1. What is the molar solubility of PbCl2 in a solution of 0.23 M CaCl2? Ksp = 1.6 ✕ 10-5 for PbCl2. 2. What is the Qsp when 32.0 mL of 6.50 ✕ 10-7 M Na3PO4 are mixed with 41.4 mL of 5.50 ✕ 10-5 M CaCl2? Assume the volumes are additive. Ksp = 2.0 ✕ 10-29. 3. What is the Qsp when 61.0 mL of 1.50 ✕ 10-4 M AgNO3 are mixed with 80.0 mL of 5.20 ✕ 10-3 M CaCl2? Assume the volumes are additive. Ksp = 1.6 ✕ 10-10. 4. What [I-1] is needed to start the precipitation of AgI from a saturated solution of AgCl? Ksp = 2.9 ✕ 10-16 for AgI and Ksp = 1.2 ✕ 10-10 for AgCl.If you have a saturated solution of PBr2 that 1.33x10-5M, what is the Ksp of PBr2?
- Ksp of AgCl = 1.8 x 10^-10, how much volume of water would it take to dissolve 0.019g?A group of wealthy chemistry 1A students had a little too much disposableincome and decided to create the most expensive they could think of. Using various spectroscopictechniques the salt was determined to be rhodium (III) Bromide (RhBr3). When this salt was shaken withpure water at 25°C, the solubility was found to be 0.026 mg/mL. Calculate the Ksp of RhBr3100.0-mL sample of a saturated PbSO4 solution was evaporated until dry. If 24 mg of solidPbSO4 was recovered, what will be the Ksp value for PbSO4?