The equilibrium constant for the reaction HASO4 (aq) + SeO32- (aq) =HASO42-(aq) + HSeO3(aq) is K=24....
Find the value of the equilibrium constant for the following equilibrium HAsO42–(aq) + H2O(l) ⇌ H2AsO4–(aq) + OH–(aq) given the acid ionization constants for H3AsO4: pKa1=2.26, pKa2=6.77, pKa3=11.29.
In a Bronsted acid-base reaction, the stronger acid reacts with the stronger base to produce a weaker acid and a weaker base. Thus, whether a reaction “goes” or “does not go” can be used to determine the relative strength of the Bronsted acids and bases in the reaction. From the data below, determine the order of the strengths of the three Bronsted acids. Reaction 1: CH3CO2H + H2AsO3- → H3AsO3 + CH3CO2- goes Reaction 2: H2AsO4- + H2AsO3- → H3AsO3...
B3438 QUESTION 24 What is the equilibrium constant (K) at 350 K for the following reaction? (R= 8.314 J/K.mol, F = 96,500 C-moll) Sn2+ (aq) + Fe(s) Sn(s) + Fe2+(aq) E cell = 0.35 V O 7.1 x 10-11 1.2 x 1010 1.2 x 105 8.6 x 10- 2.3 1023 QUESTION 30 A chemist adds substance A and B to a reaction flask and allows equilibrium to establish A+B=CKc= 1.5 x 10-25 Which of the following describe the contents of...
Write the equilibrium constant expression for this reaction: H2SO4 (aq) → 2H+ (aq) + SO−24 (aq)
Calculate the pH and the equilibrium concentrations of HSeO3- and SeO32- in a 0.1000 M selenious acid solution, H2SeO3 (aq). For H2SeO3, Kal=2.4×10-3 and Ka2=4.8×10-9
What is the equilibrium constant expression, K i, for the following weak acid? H 2SO 3( aq) H +( aq) + HSO 3 -( aq) Ki = [H2SO3] / [H+][HSO3-] Ki = [H+]2 [SO32-]/ [H2SO3] Ki = [H+]2 [HSO3-]/ [H2SO3] Ki = [H2SO3] / [H+]2 [SO32-] Ki = [H+][HSO3-]/ [H2SO3
For the reaction A(aq) + BB(1) - C(s) + (aq) the equilibrium constant, K, can be written as PoD K- A When calculating the equilibrium constant, aqueous solutes must be expressed in moles per liter (M), and gases must be expressed in pressure as bars. This is because they are dimensionless ratios of the actual concentration or pressure divided by standard state concentration, which is M for solutions and 1 bar for gases. these are the only units of concentration...
I just did a lab on determination of an equilibrium constant through the reaction EtAc (aq) + H2O (sln) <-> EtOH (aq) +HAc (aq). For all initial concentrations, K was less than one. Which I know says that equilibrium favors reactants. One of the post lab questions is "After the titration of the solutions at equilibrium, how will the solution return to equilibrium? Which chemicals will increase and which will decrease? (Be careful with acetic acid) " I am not...
I just did a lab on determination of an equilibrium constant through the reaction EtAc (aq) + H2O (sln) <-> EtOH (aq) +HAc (aq). For all initial concentrations, K was less than one. Which I know says that equilibrium favors reactants. One of the post lab questions is "After the titration of the solutions at equilibrium, how will the solution return to equilibrium? Which chemicals will increase and which will decrease? (Be careful with acetic acid) " I am not...
Consider the balanced chemical equation for this equilibrium reaction: A (aq) + B (aq) = AB (aq) To determine the equilibrium constant for this reaction at 298 K, a student mixes two solutions together and allows them to react: • 10.0 mL of 0.60 M A (aq), and, • 40.0 mL of 0.25 MB (aq). When this solution reaches equilibrium, the student measures the equilibrium concentration of AB in the 50.0 mL solution: [AB]E = 0.10 M. Which values should...