None Hardness is defined as the total concentration of divalent cations (primarily Ca2+ and Mg2+ ). On method used bymunicipalities to soften water (i.e., to remove the Ca and Mg ions) is lime - soda softening. In this process, the pH is firstraised by adding lime (CaO) which causes brucite (Mg(OH) 2) to precipitate. In the second step, soda ash (Na2CO3) isadded to cause CaCO3 to precipitate. This problem concerns the removal only of the Mg2+. The pH of a 250 C1groundwater containing 10 -4 mo of Mg2+ is raised to 12 with strong base. No further base is added. What will be theLequilibrium pH and Mg 2+ concentration? Ignore activity corrections and the possible precipitation of species other thanbrucite (Mg(OH) 2) as well as the possible complexation of Mg2+ by ligands other than OH - .

To solve this problem, we will analyze the removal of Mg2+ in water softening and determine the…

Answered: Hardness is defined as the total…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.97QE

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Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
Marble is almost pure CaCO3. Acid rain has a devastating effect on marble statuary left outdoors. Assume that the reaction which occurs is CoCO3(s)+ H+(aq)Ca2+(aq)+HCO3(aq) Neglecting all other competing equilibria and using Tables 15.1 and 13.2, calculate (a) K for the reaction. (b) the molar solubility of CaCO3 in pure water. (c) the molar solubility of CaCO3 in acid rainwater with a pH of 4.00.
A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?
A 1.0-L solution that is 4.2 M in ammonia is mixed with 26.7 g of ammonium chloride. a What is the hydroxide-ion concentration of this solution? b 0.075 mol of MgCl2 is added to the above solution. Assume that there is no volume change. After Mg(OH)2 has precipitated, what is the molar concentration of magnesium ion? What percent of the Mg2+ is removed from solution?
The titration of 0.100 M acetic acid with 0.100 M NaOH is described in the text. What is the pH of the solution when 35.0 mL of the base has been added to 100.0 mL of 0.100 M acetic acid?
The following figure represents solutions at various stagesof the titration of a weak acid, HA, with NaOH. (The Na+ions and water molecules have been omitted for clarity.) Towhich of the following regions of the titration curve doeseach drawing correspond: (a) before addition of NaOH,(b) after addition of NaOH but before the equivalencepoint, (c) at the equivalence point, (d) after the equivalencepoint?
Calculate pH for a weak acid/strong base titration. Determine the pH during the titration of 59.5 mL of 0.436 M nitrous acid (K₂ = 4.5x10-4) by 0.436 M NaOH at the following points. (a) Before the addition of any NaOH (b) After the addition of 15.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 89.3 mL of NaOH
Calculate pH for a weak acid/strong base titration. Determine the pH during the titration of 71.4 mL of 0.302 M hydrofluoric acid (K₂ = 7.2×10¯4) by 0.302 M KOH at the following points. (a) Before the addition of any KOH (b) After the addition of 16.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 107 mL of KOH
Please answer both the parts otherwise I'll downvote
Sêtting up A solution is prepared that is initially 0.36M in trimethylamine ((CH,),N), a weak base, and 0.19M in trimethylammonium chloride ((CH,) NHCI Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in OH . You can leave out the M symbol for molarity. [(CH.),N] [(cH.),NH] [oH] initial change final Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Ac 17 MacBook Air
You are required to prepare a buffer (pH sodium propionate. The concentration of the propionate must the concentration of the acid be? K, = 1.3 × 105 5.30) using propionic acid and 0.6M. Which one

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