A chemist mixes 10.0 mg of Ca(NO3)2 to a 100.0 mL sample of 0.010 M Na2C2O4 at 25 oC. Assume the volume of solution does not change. Given that for CaC2O4, Ksp = 2.7 x 10-9 at 25 oC, determine a) the value of Qsp (number and magnitude) of CaC2O4 dissolution and b) whether a precipitate should form.
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A chemist mixes 10.0 mg of Ca(NO3)2 to a 100.0 mL sample of 0.010 M Na2C2O4 at 25 oC. Assume the volume of solution does not change. Given that for CaC2O4, Ksp = 2.7 x 10-9 at 25 oC, determine a) the value of Qsp (number and magnitude) of CaC2O4 dissolution and b) whether a precipitate should form.
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- Consider a saturated solution of barium iodate in 0.025 M BaCl2. For the salt: Ba(IO3)2(s) ⇌ Ba2+ + 2IO3- Ksp = 1.57 \times× 10-9 at 25 deg C What is the activity coefficient of Ba2+? Consider a saturated solution of barium iodate in 0.025 M BaCl2. For the salt: Ba(IO3)2(s) ⇌ Ba2+ + 2IO3- Ksp = 1.57 × 10-9 at 25 deg C What is the activity coefficient of Ba2+?. 0.439 0.364 0.276 0.405Describe the effect, if any the following procedural errors would have on the calculated value of the Ksp. Is the dissolution of Ca(IO3)2 in water endothermic or exothermic? Write an equation for the process, including the heat of reaction.Calculate the value of the reaction quotient, Q, of silver iodate (AgIO3) when 10.0 mL of 0.018 M AgNO3 is mixed with 10.0 mL of 0.018 M NaIO3. (Please give your answer with 2 significant figures.)
- Calculate the solubility at 25°C of BaCrO4 in pure water and in a 0.0050M BaCl2 solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. Ksp of BaCrO4 = 1.17 x 10^-10A team of geologists discovered a new basic salt, MgX2(OH)4, where X is a newly discovered metal. Given MgX2(OH4) <-> Mg2++2x2+4OH- Given that the molar solubility of this salt is 1.07×10-3 M, calculate Ksp. Show all of your work.Consider a saturated solution of barium iodate in 0.025 M BaCl2. For the salt: Ba(2IO3)^2(s) = Ba2+ + 2IO3^- Ksp= 1.57 × 10-9 at 25 deg C What is the activity coefficient of Ba2+? 0.276 0.439 0.405 0.364
- Why is high relative supersaturation undesirable in a gravimetric precipitationA student performed titrations of samples of borax at different temperatures to determine the KSP at each temperature. After graphing the 1/T (K-1 ) versus ln(KSP), the student obtained the trend line and R2 value. Use this information to answer the following questions: a. What is deltaH? b. Is this dissolution endothermic or exothermic? c. What is deltaS? d. Determine deltaG at 298K.Calculate the solubility at 25°C of BaCrO4 in pure water and in a 0.0180M BaCl2 solution. You'll find Ksp data in the ALEKS Data tab. ksp for Ba Cr04 =1.17×10−10 Round both of your answers to 2 significant digits. solubility in pure water: gL solubility in 0.0180 M BaCl2 solution: gL
- 50.0 mL of 1.0 M HCl (at 22.0ºC) and 50.0 mL of 1.5 M NaOH (at 22.0ºC) are mixed. The solution temperature rises to 28.9ºC. What is ΔHrxn for the reaction?Why is high supersaturation undesirable in a gravimetric precipitation?Calculate the solubility and molar solubility of Cu3(PO4)2 (MW=380.58 ; Ksp=1.4x10-37).