Chemistry The glucose assay reagent contains NAD (0.5 mM) and ATP (0.7 mM) in TEA buffer. If you add 100 μl of glucose assay reagent to a 10 μl sample, what is the final concentration of (a) NAD? (b) ATP?
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Chemistry
The glucose assay reagent contains NAD (0.5 mM) and ATP (0.7 mM) in TEA buffer. If you add 100 μl of glucose assay reagent to a 10 μl sample, what is the final concentration of
(a) NAD?
(b) ATP?
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- Use the following data to calculate the Ksp value for each solid. (a) The solubility of FeCO3 is 5.6 ✕ 10−4 g/L.(b) The solubility of Cr(OH)3 is 1.3 ✕ 10−8 mol/L.2MnO4−+5H2C2O4+6H+⟶2Mn2++10CO2+8H2O Reaction : Permanganate Ion Reduced by Oxalic Acid If you increase the concentration of oxalic acid in an experiment, what will the molecules and ions be doing? (Simply trying to determine how it will be effected because I don't understand what it would be doing. In the experiment I did, it took longer to notice any changes occur in the color of the test I was doing. )3) One of the main buffer systems found in living organisms is the phosphate buffer system, often used in biological research to mimic cellular conditions. The phosphate equilibrium reactions and their corresponding pKa's are as follows: H3PO4 = H* + H2PO, H2PO, = H+ + HPO?- HPO- = H+ + PO;- pKa1 pКаz —D 7.21 = 12.44 = 2.12 pKa3 (a) Given the above chemical reaction, write out the expression for K, of the buffer system which would predominate at neutral pH conditions. Justify your choice. (b) The human body, and many other lifeforms, prefer an internal pH of 7.2 to maintain homeostasis. However, some more acid-tolerant or basic-tolerant organisms can survive (and sometimes thrive) within different ranges of pH. Calculate the mass and moles of the correct acid and corresponding conjugate base solid (assume you have sodium salts of each base: NaH,PO4, Na,HPO4, and Na PO,) which are needed to make 500 mL of a 0.5 M buffer solution (0.5 M total, including the concentration of acid and base…
- Consider the following equilibrium reaction: 2 CH3OH + CH2O ⇌CH2(OCH3)2+ H2O ΔH = + 46 indicate the direction that the equilibrium will shift when the following changes are made.(No states are provided because the solvent for the reaction is not water, so aq for aqueous would not be appropriate.) (a)Concentration of CH3OH increases (b)H2O is removed from the reaction (c)Reaction is heated2:25 1 Question 17 of 25 Submit Consider the equilibrium system described by the chemical reaction below. A 1.00 L reaction vessel was filled 0.0560 mol O, and 0.200 mol N20 and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO2 present. Determine the concentrations of all species and then calculate the value of Kc for this reaction. 2 N20(g) + 3 O2(g) =4 NO2(g) 1 2 Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. 2 N20(g) + 3 O2(g) = 4 NO2(g) Initial (M) Change (M) Equilibrium (M) 5 RESET 0.0560 0.200 -1.00 -0.0560 0.0200 -0.0200 0.0100 -0.0100 -0.0050 0.0050 0.0150 -0.0150 0.210 0.190 0.0410 0.0710 0.0360 0.180Five moles of an acid HA was dissolved in 5.0 L of solution. After the system had come to equilibrium, the concentration of HA was found to be 0.43 M. Calculate Ka for HA. (Write your answer in scientific notation) Ka = Submit Question 348 45,838 MAY tv L (9) S
- (a) What does it mean when the reaction quotient, Q, is numerically equal to the equilibrium constant, Kc? (b) What does it mean when it is less than the equilibrium constant? (c) What does it mean when it is less than the equilibrium constant?AH = - 1.2 kcal/mol; Kp = 16 nM OH 1 НО AH = - 6.0 kcal/mol; Kp = = 76 nM OH HOllio AH = - 5.5 kcal/mol; Kp = 0.5 nM OH 3 (ii) What is the significance of Kp? Hence, arrange the three molecules in terms of decreasing affinity to their target. O=5. One of the key steps in the tricarboxylic acid (TCA) cycle is the hydration of fumarate to malate: Fumarate-² + H₂O = Malate-2 The standard reaction Gibbs free energy and enthalpy for this reactions are -880 cal/mol and 3560 cal/mol, respectively. (a) What is the equilibrium constant for this reaction (25 °C)? (b) Is the reaction favorable (spontaneous) at 25 °C? (c) What is the equilibrium constant of this reaction under physiological conditions (37 °C)? (d) Is this reaction favorable at 37 °C?
- The value of Ka for acetylsalicylic acid (aspirin), HC,H-O4, is 3.00x10* Write the equation for the reaction that goes with this equilibrium constant. (Use H30* instead of H*.)For the reaction - what effect would adding large amounts of heat have on the equilibrium? (Which way would it shift and why?) Explain in terms of LeChatelier’s Principle. Fe3O4(s) + 4 H2 (g) <_-> 3 Fe (s)+ 4 H2O (g) ΔH = 36 kcal Keq = 2.3 x 10-18 During the process of ketogenesis in the liver, 3-hydroxybutyric acid and acetoacetic acid are in equilibrium with each other. However, acetoacetic acid can decompose to form carbon dioxide and acetone in a nonreversible reaction. Answer the following by using LeChatelier’s Principle. What effect would the nonreversible decomposition of acetoacetic acid have on the equilibrium between 3-hydroxybutyric acid and acetoacetic acid? (i.e. which way would if shift?) What effect would the nonreversible decomposition of acetoacetic acid have on the concentration of 3-hydroxybutric acid? (i.e. would it go up or down)Calculate the Ksp of the following compounds, given their molar solubilities. (a) CoS, 6.31 × 10-11 M (b) Cd(OH)2, 1.21 x 10-5 M (c) Ca3 (PO4)2, 1.14 × 10-7 M