Give me right solution according to the question Under a 25°C subsurface environment, the groundwater has reached equilibrium withsoil minerals and pore gas. The pH of groundwater equals to 7.4. The major componentof soil minerals is CACO3, with solubility constant pKso = 8.3. The partial pressure ofCO2 in the pore gas is 0.2 atm. Determine [H2CO;], [HCO;], [CO;], [Ca?"]. Give your%3Danswers in molar concentration (M).Hints:Acid constants of H2CO3 at 25°C: pKal = 6.3; pKa2 = 10.3Henry's constant for CO2 at 25°C: KH = 3.39*102 M/atm%3D

Given: pH of ground water = 7.4 pKsol = 8.3; Ksol = 10- pKsol = 10-8.3 = 5.01 x 10-9 CaCO3…

Answered: Under a 25°C subsurface environment,…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter13: Titrations In Analytical Chemistry

Section: Chapter Questions

Problem 13.5QAP

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In some natural systems the pH must be maintained within very narrow limits. e.g. in human blood the pH must remain close to 7.4 or cell deterioration occurs. Blood contains several weak acid/conjugate base equilibria called buffers, which control the pH.One weak acid present in blood is the dihydrogen phosphate ion, H2PO4-(aq), for which the equilibrium in aqueous solution is H2PO4-(aq) +H2O(l) <--> HPO42-(aq) + H3O+(aq). a) What would be the effect on this equillibrium of adding hydrochloric acid solution?b) Write the expression for the equilibrium constant of this reaction.c) If 0.5 mol H2PO4- and 0.5 mol HPO42- are in equilibrium in 1.0L of aqueous solution, calculate the pH of the solution. (Ka for H2PO4-= 6.4 x 10-8)d) 0.010 mol HCl is now added to the 1.0L of the solution in c). Assuming that all the added H+ ions are used up in the equilibrium shift, calculate the concentrations of H2PO4- and HPO42-. Hence calcuate the pH of this solution.e) 0.010 mol HCl has been added…
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