Calculate the final concentrations of K+(aq), C2O4 2- (aq), Ba 2+ (aq), and Br- (aq) in...

Calculate the final concentrations of K+(aq), C2O4 2- (aq), Ba 2+ (aq), and Br- (aq) in a solution prepared by adding 50mL of 0.2M K2C2O4 to 100 mL of 0.3M BaBr2. (For BaC2O4 Ksp= 2.3x10^-8) (Hint: assume all solid forms, then redissolves in a common ion problem)

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queen_honey_blossom answered 2 years ago

Calculate the concentrations of H2C2O4, HC2O4^ -, C2O4^ -2, and H^+ species in a 0.430 M...

Calculate the concentrations of H2C2O4, HC2O4^ -, C2O4^ -2, and H^+ species in a 0.430 M Oxalic Acid Solution (Ka1 = 6.5 x 10^-2) (Ka2 = 6.1 x 10^-5) Be sure to answer in correct number of significant figures. H2C2O4 = ________ M HC2O4^- = _________ M C2O4^2- = _________ x 10 ^ (scientific notation) H^+ = ____________ M

In the precipitation reaction Na2(C2O4)2- (aq) + CaCl2 (aq) -----> Ca(C2O4) (s) + 2NaCl (aq), how...

In the precipitation reaction Na2(C2O4)2- (aq) + CaCl2 (aq) -----> Ca(C2O4) (s) + 2NaCl (aq), how do I determine how many grams of the reactants I need to yield 5 grams of the precipitate?

Calculate the Eocell for: Fe(s) + Br2(g) → Fe2+(aq) +Br-(aq) ; is this electrolytic or voltaic?...

Calculate the Eocell for: Fe(s) + Br2(g) → Fe2+(aq) +Br-(aq) ; is this electrolytic or voltaic? A. -1.52V ; voltaic B. 1.52V ; electrolytic C. -1.52V ; electrolytic D. 1.52V ; voltaic

A) A solution of Ba(OH)2 has a molarity of 0.00617 mol/L. Calculate the final pH of...

A) A solution of Ba(OH)2 has a molarity of 0.00617 mol/L. Calculate the final pH of the solution. B) Consider the reaction: CaBr2(s) → Ca(s) + Br2(l) Which of the following statements is correct? Select all that apply. Bromide Ion is reducing agent NOT a spontaneous reaction Ca is oxidized Br is Oxidized Br is Reduced Ca is Reduced Calcium Ion is the Reducing Agent IS a spontaneous reaction Br ion is the oxidizing agent. Ca ion is the oxidizing...

Find the Net ionic Equation of: Ba(NO3)2 (aq) + Pb(NO3)2 (aq) --> ???

Phosphoric acid, H3PO4(aq), is a triprotic acid. Calculate the pH and concentrations of H3O + (aq),...

Phosphoric acid, H3PO4(aq), is a triprotic acid. Calculate the pH and concentrations of H3O + (aq), H3PO4(aq), H2PO4 − (aq), HPO4 2− (aq), PO4 3− (aq), and OH− (aq) in a 0.100-M phosphoric acid solution at 25°C.

Given: AgBr(s) <--> Ag+(aq) + Br -(aq) and Ag+(aq) + 2NH3(aq) <--> Ag(NH3)2+(aq) a) What would...

Given: AgBr(s) <--> Ag+(aq) + Br -(aq) and Ag+(aq) + 2NH3(aq) <--> Ag(NH3)2+(aq) a) What would be the value of K for AgBr(s) + 2NH3(aq) <--> Ag(NH3)2+(aq) + Br -(aq) ? b) What would be the molar solubility of silver bromide in 2.00 M aqueous ammonia?

Consider the equilibrium shown. PbBr2(s)−⇀↽− Pb2+(aq)+2Br−(aq)Ksp=2.10×10−6 Determine the concentrations of Pb2+ and Br− in a saturated...

Consider the equilibrium shown. PbBr2(s)−⇀↽− Pb2+(aq)+2Br−(aq)Ksp=2.10×10−6 Determine the concentrations of Pb2+ and Br− in a saturated solution of PbBr2 in pure water (assume μ=0 M). [Pb2+]= M [Br−]= M Determine the concentrations of Pb2+ and Br− in a saturated solution of PbBr2 in a solution with an ionic strength of 0.010 M. [Pb2+]= M [Br−]= M Determine the concentrations of Pb2+ and Br− in a saturated solution of PbBr2 in a solution with an ionic strength of 0.10 M. [Pb2+]=...

Consider the reaction: 2HCl(aq) + Ba(OH)2(aq) ! BaCl2(aq) + 2 H2O(l) deltaH = "118 kJ A)...

Consider the reaction: 2HCl(aq) + Ba(OH)2(aq) ! BaCl2(aq) + 2 H2O(l) deltaH = "118 kJ A) Calculate the heat produced when 700.0 mL of 0.500 M HCl is mixed with 300.0 mL of 0.500 M Ba(OH)2. Note: One of the solutions is the limiting reagent. B) Calculate the final temperature if both solutions were initially at 25.0° C, and they were mixed together in a calorimeter with a heat capacity of 180.3 J/C° Note: The density specific heat capacity of...

Calculate the value of K in the following reaction: HCN (aq) + F- (aq) <-------> CN-...

Calculate the value of K in the following reaction: HCN (aq) + F- (aq) <-------> CN- (aq) + HF (aq) Ka for HCN = 6.2 x 10^-10 Ka for HF = 7.2 x 10^-4

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