7. If the equilibrium constant of binding of NADH to an enzyme [E] is 2.7=2,7 v Ko = [NADH][E]/[E-NADH] = 1.5 x 10-6 M, and solution concentrations of [E] and [NADH] are 10 nM and 1.0 µM, respectively, what is the concentration of the [E-NADH] complex? %3D 51210 (a) 16 µM0.:0 (b) 0.62 x 109 M 1.5 E-NADH (c) 62 nM .0000000 (d) None of the above. 5 -2.51x

What is the [Cr^3+] in the solution?

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1. In this experiment we measured K, for borax Na,B,O,(OH), 8H,0(s)=2Na*(aq)+B,0,(OH),² (aq)+8H,0(1) write down K, for this reaction in terms of reactants/product sp concentrations We measured the concentration of the borate by titrating it with HCl to make boric acid B,O,(OH), (a) + 2 HCI( aq) + 3 H,O(I) → 4 H,BO, + 2CI (ag) the pH at the equivalence point is pH = 4. 2. What indicator did we use, and what color was the indicator at the equivalence point? 3. At 48.2°C, 5.00ml of the saturated solution of bo ax was titrated with 0.235M HCI. It took 23.00 mL of the a id to reach the equivalence point. 1. What is the molarity of the tetra-borate anion in t e solution? 2. What is Kn for borax at this temperature?

AgNazt Cu-Agt_Cu[(103)2 Acidic Solution

Part 1 out of 4   (a) Write equilibrium constant expressions for Kc for the following process.  2CO2(g)      2CO(g) + O2(g) Kc=

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For AgOH, Ksp = 1.5 x 108. What is the molar solubility of AgOH in a solution containing 0.1 M of NH3 buffered at pH = 7? (KĘ[Ag(NH3)2*]= 1.6 x 107). %3D A. 0.20 M B. 0.025 M C. 0.25 M D. 0.05 M

Experiment 3: The Equilibrium State Introduction In this experiment, you will quantitatively assess the equilibrium constant for the reaction of the iron (III) cation complexing with a thiocyanate anion (SCN–) to form the red iron (III) thiocyanate complex, Fe(SCN)2+.                                                                              (1) If Kc is a large number (>1), then the chemical equilibrium favors the formation of product (large numerator). If Kc is a small number (<1), then the chemical equilibrium favors the formation of reactants (large denominator).  In this simulated experiment, several solutions of varying initial concentrations of reactants (and product) are to be evaluated.  Despite the different concentrations, the equilibrium constants calculated from their equilibrium concentrations should be the same, as long as the temperature is kept constant.

A solution is prepared such that the initial concentration of A2+ is 1.50x103 M and the initial concentration of X is 4.60x10-3 M. A2+ and X are allowed to react as shown below to establish equilibrium with the complex AX2+. In a colorimetry experiment, the equilibrium concentration of the complex AX2+ is determined to be 8.9x10-4 M. A2* (aq) + X (aq) =Ax2+ (aq) %3D Complete the ICE table below by selecting the correct value or expression to place in the ICE table from the drop-down menu. A2+ (aq) X (ад) АХ2+ (aq) Initial concentration Change in concentration Equilibrium concentration expression Equilibrium concentration value