alkalinity Assume 25°C, 1 atm, ideal conditions (I=0, y→1) in all problems. If you employ simplifyingassumptions when you solve the problems, please provide the rationale for your assumption.1) The dissolved carbonate system refers to the combination of dissolved carbonic acid (H2CO3")and its conjugate base species bicarbonate (HCO;) and carbonate (CO3²). In aquatic systems,the equilibrium distribution of these three species can be described by the following aciddissociation reactions.H2CO3* HCO3¯+ H*HCO3 + CO3²- + H*Kal = 10-6.35Ka2 = 10-10.33where the total inorganic carbon concentration Cr= [H2CO3*]+ [HCO3]+[CO;²].a) Describe two different reasons why the dissolved carbonate system is important foraquatic systems relevant to environmental scientists and engineersb) Identify the pH range where each species (i.e., H2CO3", HCO3', CO3²') is dominant formof CT.c) Calculate the equilibrium pH of a solution that was prepared by dissolving carbonic acidH2CO3* into water to a concentration of CT= 103 M.(You have the option of employing a simplifying assumption to solve the problem. If youdo so, please justify and check your assumption.)2) Calculate the alkalinity (in units of eq/L) of groundwater containing CT = 104 M; pH 6.4(closed system)3) The finished water at a drinking water treatment plant contains an alkalinity of 1.5 meq/L anda pH of 7.2 (due to dissolved carbonate species). What is the total dissolved carbonateconcentration (i.e., Cr)? Assume that no water-gas exchange occurs.

The objective of this question is to show the dissolved carbonate system is important for aquatic…

Answered: alkalinity

Science

Chemistry

alkalinity

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The titration below was performed by placing 10.00 mL solution in an Erlenmeyer flask and titrating it with 0.1000 M HCl. What is the concentration of the solution being titrated? 0.02500 M 0.0500 M 0.0750 M 0.100 M 0.200 M
A 0.8040-g sample of an iron ore is dissolved in acid. The iron is then reduced to Fe²+ and titrated with 47.22 mL of 0.02242 M KMn 04 solution. Calculat the results of this analysis in terms of % Fe (55.847 g/mol).
Please write a balanced equations and indicate the state. HCl(aq) + NH4Cl
An aqueous solution of NaCl was electrolyzed with a current of 2.50 amps for 15.0 minutes. What volume (in mL) of 0.500 M HCl would be required to neutralize the resulting solution? (Hint: H2 is produced at the cathode and Cl2 at the anode.)
For the reaction KClO4⟶KCl+2O2 assign oxidation numbers to each element on each side of the equation.
Balance the following chemical equation (if necessary): FeCl₃(aq) + Na₂S(aq) → Fe₂S₃(s) + NaCl(aq)
What are the products and balanced equation of aqueous solutions of ferrous sulfate and ammonium sulfide
Write the balanced NET ionic equation for the reaction when aqueous KBr and aqueous AgC₂H₃O₂ are mixed in solution to form aqueous KC₂H₃O₂ and solid AgBr
All iron in 4.00 g of iron ore sample, which was dissolved in an acid solution, was converted to Fe2+ which was then titrated with 0.200 M KMNO4 solution. In this titration all iron is oxidized to Fe3+ and MnO4 to Mn2+. If 27.45 mL of KMNO4 solution is required to the end point, determine 1. How many grams of iron content is in the iron ore sample. 2. The yield percentage of iron in the sample. 3. If the iron in the sample is present as Fe2O3, what is the mass percentage of Fe2O3 in the sample.
The hydroperoxide ion, HO2–(aq), reacts with permanganate ion, MnO4–(aq) to produce MnO2(s) and oxygen gas. Balance the equation for the oxidation of hydroperoxide ion to O2(g) by permanganate ion in a basic solution.