Balance the equation below for the reaction under acidic aqueous conditions. Cr20 (aq) (ag) Cr3+ (aq) 12(s) What is the coefficient for the Cr+ ions? Select one: O a 2 b. d. 9. 7
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- The molarity of a solution is 0.15 M in NaI (aq) at 298.15 K. A large excess of HgI2 (s) to the solution. What is the solubility (in grams) of HgI2 (s) at saturation? HgI2 (s)<------->Hg2+ (aq) + 2I- (aq) Ksp= 2.7 × 10^-29HgI2 (s) + 2I- <------> [HgI4]2- (aq) Kf= 0.75 MThe solubility, s, of calcium carbonate, CaCO3 at 25 °C is [s] = 6.90 •10-5 The reaction is: CaCO3 (s) D Ca2+(aq) + CO32-(aq) a) Calculate the concentration of Ca2+ and CO32- at equilibrium. _____________________ [Ca2+] ___________________ [CO32-] b) Calculate the equilibrium constant for the dissolution reaction. (This equilibrium constant is also known as the solubility product, Ksp.) Keq (or Ksp) = ___________Copper (II) Phosphate is extremely insoluble, but forms a complex ion with CN- that can drive the Copper (II) solubility through Le Chatlier’s principle. Given the two reactions below, determine KT. Cu3(PO4)2 (s) --> 3 Cu2+ (aq) + 2 PO43- (aq) K1=2.05x10-35 Cu(CN)42- (aq) --> Cu2+ (aq) + 4 CN- (aq) K2=1.0x10-25 Cu3(PO4)2 (s) + 12 CN- (aq) --> 3 Cu(CN)42- (aq) + 2 PO43- (aq) KT=??? 3b. Of the 4 special types of reaction, which one is depicted by K1 and which one is depicted by the reverse of K2?
- Copper (II) Phosphate is extremely insoluble, but forms a complex ion with CN- that can drive the Copper (II) solubility through Le Chatlier’s principle. Given the two reactions below, determine KT. Cu3(PO4)2 (s) -->3 Cu2+ (aq) + 2 PO43-(aq) K1=2.05x10-35 Cu(CN)42- (aq) -->Cu2+ (aq) + 4 CN- (aq) K2=1.0x10-25 Cu3(PO4)2 (s) + 12 CN- (aq) --> 3 Cu(CN)42- (aq) + 2 PO43- (aq) KT=???I need help with part c. I included the rest of the problem incase additianal info is needed. Consider the solubility of calcium oxalate (oxalate = C2O42-) in water: CaC2O4(s) ⟺ Ca2+(aq) + C2O42-(aq) a) Write the equilibrium expression for the reaction as written. b) Calculate the [Ca2+] from the dissolution of calcium oxalate in pure water. pKsp = 7.90 c) Calculate the [Ca2+] from the dissolution of calcium oxalate in a solution that contains 0.250 M ammonium oxalate.A chemist at a pharmaceutical company is measuring equilibriumconstants for reactions in which drug candidatemolecules bind to a protein involved in cancer. The drugmolecules bind the protein in a 1:1 ratio to form a drug–proteincomplex. The protein concentration in aqueous solutionat 25 °C is 1.50 x 10-6 M. Drug A is introduced into the proteinsolution at an initial concentration of 2.00 x 10-6 M.Drug B is introduced into a separate, identical protein solutionat an initial concentration of 2.00x 10-6 M. At equilibrium,the drug A–protein solution has an A–protein complexconcentration of 1.00 x 10-6 M, and the drug B solutionhas a B–protein complex concentration of 1.40 x 10-6 M.Calculate the Kc value for the A–protein binding reactionand for the B–protein binding reaction. Assuming that thedrug that binds more strongly will be more effective, whichdrug is the better choice for further research?
- Consider the following reaction between oxides of nitrogen: NO2(g)+N2O(g)→3NO(g) a) Using the value of Ka , calculate ΔG∘ for the dissociation of nitrous acid in aqueous solution. b) What is the value of ΔG at equilibrium? c)What is the value of ΔG when[H+] = 6.0×10−2M, [NO2−] = 6.2×10−4M and [HNO2] = 0.20 M ?The UV/Vis allows you to determine the concentration of a colored compound. Calculate the value of K using the following values. Vol of 0.002 M KSCN-5.00 mL Vol of 0.002 M Fe(NO3)3- 2.71 mL Vol water- 2.29mL Abs after mixing-0.553 Hint: 1- convert absolute to concentration of FeNCS 2- determine the equilibrium concentrations of KSCN and Fe(NO3)3 3- calculate K Then multiply calculationsMath toolbox: ax2+bx+c =0 solve ; 1 cm3 = 0.001 dm3 The equilibrium constant is calculated Keq = 0.36 for the reaction @ 400 K when using M (mol/dm3) as the unit for the gasses. note: not the pressure unit. PCl5 (g) <=> PCl3 (g) + Cl2 (g) When using M as the units, the Keq is unitless with unit canceled to CѲ= 1 M. Giving that 5.365 g of PCl5 (Mw = 208 g/mol) was initially placed in a reaction vessel of volume V = 250 cm3. When reach equilibrium, determine the molar concentrations of PCl3 in the mixture assuming ideal gasses for all. concentration of PCl3 = ______ M. 3 sig. fig.
- Hypothetical reaction A2 <--> A The In Kp = -33.47 at 2000K while deltaH0 = 205200 +4.94T - 0.888*10-3 T2 . At equilibrium, what will be the partial pressure of each component at a temperature of 8000K and 2atm total pressure?2. Calculate Kc for each reaction. a. I2(g)⇌2I(g)Kp=6.26×10−22I2(g)⇌2I(g) Kp=6.26×10−22 (at 298 KK)Express your answer to three significant figures. b. CH4(g)+H2O(g)⇌CO(g)+3H2(g) Kp=7.7×1024CH4(g)+H2O(g)⇌CO(g)+3H2(g)Kp=7.7×1024 (at 298 KK)Express your answer to two significant figures c. N2(g)+O2(g)⇌2NO(g) Kp=4.10×10−31N2(g)+O2(g)⇌2NO(g)Kp=4.10×10−31 (at 298 KK)Express your answer to three significant figures.It is found that 8.70e-09 g of Ga(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Ga(OH)3.The Ksp of Y2(CO3)3 at 25 oC is 1.03e-31. What is the molar solubility of Y2(CO3)3?
