The pH of normal human blood is in the range of 7.35 to7.45. Compute the range of the concentration of H3O+and the range of the OH- concentration in normal blood.
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The pH of normal human blood is in the range of 7.35 to
7.45. Compute the range of the concentration of H3O+
and the range of the OH- concentration in normal blood.
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- For an acid HA, the concentrations of HA and A are 0.075 and 0.025, respectively, at pH 6.0. What is the p K a value for HA?Normal arterial pH is 7.35 to 7. 45. Both metabolic and respiratory alkalosis have pH more basic compare to the normal arterial pH. The difference is 0.5 units. What is pH value in alkalosis? Niemann-Pick type C disease is a progressive neurological disease; symptoms include unsteady walking with uncoordinated limb movements, slurred speech, a difficulty in swallowing, epilepsy and tremor. This condition is due to the abnormal functioning of a lysosome. State the normal functions performed by this organelle.Consider the following pH titration curve of a diprotic acid. What is the approximate values for pka 1 and pka 2? the curve is attached below.
- Describe the preparation of 2.00 L of 0.100 M glycine buffer, pH 9.0, from glycine and 1.00 M NaOH. What mass of glycine is required, and what volume of 1.00 NaOH is required? The appropriate pKa of glycine is 9.6Quinine ( C20 H24 N2 O2) is the most important alkaloid derived from cinchona bark. It is used as an antimalarial drug. For quinine, pK, = 5.1 and pK, = 9.7 ( pKp = – log Kp). Only 1 g quinine will dissolve in 1920.0 mL of solution. Calculate the pH of a saturated aqueous solution of quinine. Consider only the reaction | Q+ H2O= QH+ + OH- described by pK, where Q = quinine. pH =Describe the preparation of 2.00 L of 0.100 M glycine buffer, pH 9.0, from glycine and 1.00 M NAOH. What mass of glycine is required, and what volume of 1.00 NaOH is required? The appropriate pK, of glycine is 9.6.
- What mass of sodium glycolate (NaC2H3O3) should be added to 400.0 mL of 1.00 M glycolic acid to produce a buffer solution with a pH of 4.00? Ka = 1.47 x 10-4. Please indicate the full solutions.Calculate the [OH-] and the pH of a solution with an [H] = 5.6 x 10-¹0 M at 25 °C. [OH-] = pH = Calculate the [H*] and the pH of a solution with an [OH-] = 0.059 M at 25 °C. pH = Calculate the [H] and the [OH] of a solution with a pH = 2.70 at 25 °C. [H*] = MHow is Ka defined? Write the equation for Ka for the generalized acid HA.