The acidity of the stomach is maintained by the H*/K* ATPase in parietal cells of the gastric mucosa. These cells have an internal pH = 7.4. The H/K ATPase transports H* across the cellular membrane into the stomach where pH = 0.8. (a) Given a membrane potential of 65 mV (inside negative), calculate AG in kJ/mol for the transport of H* into the stomach at 37 °C. Show your work.
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- The parietal cells of the stomach lining contain membrane “pumps” that transport hydrogen ions from the cytosol (pH 7.0) into the stomach,contributing to the acidity of gastric juice (pH 1.0). Calculate the free energy required to transport 1 mol of hydrogen ions through these pumps. Assume a temperature of 37 °C.Determine the values of Km and Vmax for the decarboxylation of β-keto acid given the following data. Please show and label your plot. Show your calculations and box your final [S] in mol/l V in mM/ min 2.500 0.588 1.000 0.500 0.714 0.417 0.526 0.370 0.250 0.256What is the concentration of B expressed in terms of A if the Kd is 33.0 uM, and the concentration of AB is 56.0 uM? A + B AB OB= 1850/A OB= 23 - A OB=23+ A OB= 0.589/A
- The equation of the double reciprocal plot is y = 0.5294 x + 1.4960. What is the value of vmax (in M/s)? The substrate concentration is given in units of molarity (M) and reaction velocity has units of molarity per second (M/s). (Report to three significant figures)Substrate Concentration (mol L1) Velocity (mM min-1) 2.500 0.588 1.000 0.500 0.714 0.417 0.526 0.370 0.250 0.256 Determine the values of Km and Vmax for the decarboxylation of a 훃-keto acid given the followingdata. You have to plot the graph by using excel and please include the scope of graphFor the following results of Thermodynamics of Borax Solubility, the volume of Borax solution titrated by HCI is 8.00 mL. Table 1. Volumes of hydrochloric acid required to titrate a saturated borax solution at varying temperatures. The hydrochloric acid was a solution standardized at 0.2912 M. Borax Volume added (mL) Temp. (°C) 8.00 8.00 8.00 8.00 8.00 HCI Volume (mL) 50.5 33.75 40.7 27.02 30.0 17.95 20.2 13.43 10.3 8.55 Using Thermodynamic formula (R= 8.31 J/K•mol) and the above results, (d) AH˚ = (kJ/mol) Type your answer....
- In vitro experiments are conducted at pH = 7.4 to simulate physiological conditions. A phosphate buffer system is often used. H₂PO → H₂PO¹²¯ +H+ pK₁ = 7.2 a. What must be the ratio of the concentrations of HPO to H₂POд ions? b. What mass of NaH2PO4 must be added to 500.0 mL of 0.10 M Na₂HPO4 (aq) in the preparation of the buffered solution?For the following results of Thermodynamics of Borax Solubility, the volume of Borax solution titrated by HCI is 8.00 mL. Table 1. Volumes of hydrochloric acid required to titrate a saturated borax solution at varying temperatures. The hydrochloric acid was a solution standardized at 0.2912 M. Borax Volume added (mL) Temp. (°C) 8.00 8.00 8.00 8.00 8.00 HCI Volume (mL) 50.5 33.75 40.7 27.02 30.0 17.95 20.2 13.43 10.3 8.55 Using Thermodynamic formula (R= 8.31 J/K•mol) and the above results, (e) AS° = (J/K⚫mol) Type your answer...For the following results of Thermodynamics of Borax Solubility, the volume of Borax solution titrated by HCI is 8.00 mL. Table 1. Volumes of hydrochloric acid required to titrate a saturated borax solution at varying temperatures. The hydrochloric acid was a solution standardized at 0.2912 M. Borax Volume added (mL) Temp. (°C) 8.00 8.00 8.00 8.00 8.00 HCI Volume (mL) 50.5 33.75 40.7 27.02 30.0 17.95 20.2 13.43 10.3 8.55 Using Thermodynamic formula (R= 8.31 J/K⚫mol) and the above results, (b) What is the y-intercept of the best fitting line for this data? Type your answer...
- Calculate the concentration of an EDTA solution of which 24.22 mL were needed to titrate the Ca2+ions present in a 50.00 mL solution containing 246.7 mg CaCO3. Express your answer in terms of (a) molar concentration of EDTA (b) Ca Titer (mg Ca per mL of EDTA) MM Ca= 40.078 solve it in a way that it is in one equation already and cancelling all the values just like given in th epictureHeart and muscle cells, where myoglobin resides, maintains an intracellular pO2 of about 2.5 torr. Calculate the fractional saturation (for human myoglobin) if a small change (1 torr) in oxygen partial pressure occurs in either direction (ie what happens at 1.5 torr, what happens at 3.5 torr?) and explain how a small change in oxygen pressure dramatically changes the myoglobin oxygen binding.For the following concentrations, determine the equivalent of a. 75ug/mg lyophilized protein in ppm b. 6.3 x 10° mg/L of glycogen in % (w/v)