One strategy for dealing with the acidification of lakes is periodically to add powered limestone (CaCO3) to them, resulting in pH of 10.95. Calculate the Ca2+ concentration in the lake. CO2 in atmosphere 370 ppm KH,CO2 = 0.033 mol/(L∙atm) Ka1 = 10-6.3 Ka2 = 10-10.3 Ksp,CaCO3 = 4.57 x 10-9

One strategy for dealing with the acidification of lakes is periodically to add powered limestone (CaCO3) to them, resulting in pH of 10.95. Calculate the Ca2+ concentration in the lake. CO2 in atmosphere 370 ppm KH,CO2 = 0.033 mol/(L∙atm) Ka1 = 10-6.3 Ka2 = 10-10.3 Ksp,CaCO3 = 4.57 x 10-9

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section: Chapter Questions

Problem 116IL: Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H)...

See similar textbooks

Related questions

Q: The pH of the river adjacent to the site is governed by the carbonic acid/bicarbonate buffer system…

A: According to answering guidelines only first question is to be answered. It is requested please post…

Q: A bottled carbonated mineral water (i.e. closed system) has a pH of 4.9 and an alkalinity of 4×10-³…

Q: Carbon dioxide dissolves in water to form carbonic acid, which is primarily dissolved CO,. Dissolved…

A: Given partial pressure = 6.8x10-4 bar. Atmospheric pressure = 0.9869 bar. Determine the mole…

Q: Suppose that the solubility of Ca(OH)2 in water is 0.3g/0.1L. What is the pH of an aqeous saturated…

A: Given that: Mass of calcium hydroxide = 0.3 g Volume…

Q: You dissolve 6.31 g of potassium formate in 250 mL of 0.25 M formic acid (HCOOH). This solution was…

A: Given, Mass of KHCO2 = 6.31 g Molar mass of KHCO2 = 84.12 g/mol Molarity of HCOOH = 0.25 M…

Q: A solution (total volume = 1L) of 0.4 M NH3 contains 12.78 g of NH4CI (MW = 53.491 g/mol). Kb = 1.8…

A: First we would Calculate initial pH of solution before adding HCl. Then pH after adding HCl is…

Q: 134 grams of potassium sorbate KCH3 (CH)4CO2 is fully dissolved in 100.00 mL of water, which is…

Q: The solubility of CO2(g) in water at 25 °C and under a pressure of 1.00 atm is 1.45 g/L. If the air…

Q: Chlorine gas used for disinfection combines with water to form hypochlorous acid (HOCI). The HOCI…

A: Given, Reversible reaction : HOCl ⇌ H+ + OCl- K=2.7×10-8

Q: A buffer solution with a pH of 4,9, consists of 0,25 mol∙dm–3 acetic acid (HC2H3O2; Ka= 1,8 x 10–5)…

Q: Calculate the pH of a saturated Co(OH)2 solution. Ksp = 1.1 × 10^-15?

A: Solubility product constant: The equilibrium constant of partially soluble ionic compound in…

Q: A biochemist working with bacteria requires a culture buffered at a pH of 3.6. Which of the…

A: Given that: pH = 3.6 Buffer solution is mixture of weak acid and its conjugate base . Buffer…

Q: The pH and Kh of 0.1N NH4CI solution, if Kb for NH4OH at 25°C is 1.8x10-5 will be respectively equal…

A: pKb = - log Kb = - log ( 1.8 x 10-5) = 5 - 0.26 = 4.74 C = 0.1 N For salt NH4Cl pH = 0.5 (pKw - pKb…

Q: The Ksp for Zn(OH)2 is 5.0 × 10-17. Determine the molar solubility of Zn(OH)2 in a solution with a…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: 2. The solubility product for the dissolution of calcium carbonate in water (ar pH-7, 20 C) is K4.8…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Given the identity of the base, its concentration and pKb, determine the pH of a solution of the…

A: Whenever a weak acid and strong base reacts with each other than they form a weak acid strong base…

Q: The solubility of iron(II) hydroxide, Fe(OH)2, is 1.43×10–3 gram per liter at 25 °C. Write a…

Q: NH3 is a weak base (Kp = 1.8 x 10³) and so the salt NHĄCI acts as a weak acid. What is the pH of a…

A: At Temperature 25°C Kb (NH3) = 1.8 × 10-5 [NH4Cl] = 0.028 M

Q: Acetic acid is a weak acid that partially dissociated in water according to equation B1-2, with an…

Q: Hydrogen sulfide is characterized by a rotten egg smell. This odorous gas can be removed from…

A: Solution given: Reaction : H2S ⇔H+ + S- Ka = 0.86 x 10-7 Fraction of H2S is given by :…

Q: 5. Magnesium hydroxide (Mg(OH)2) has a pKsp value of 11.25. In a solution at pH 10, what is the…

A: Given, pKsp of Mg(OH)2 = 11.25 pH = 10 What is the maximum Mg2+ concentration in µmol/L = ? What…

Q: 1. Compare the pH values of boiled and unboiled distilled H2O. 2. The Henderson-Hasselbalch…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.00? Ksp for Mg(OH)2 is…

A: Molar Solubility is the total no. of moles of a compound that can dissolve in 1 liter of solution…

Q: Calculate the change in pH that results from adding 0.160 mol NaNO2 to 1.00 L of

A: Ka = 7.2 ×10-4 pKa = -log(Ka) = -log(7.2×10-4) = 3.14 initially, weak acid HNO2 is present So,…

Q: What is the pH of an acidic mixture containing 0.062 M hydrazoic acid (Ka = 1.9 * 10-5) and 0.062 M…

A: Henderson-Hasselbalch equation explains the relationship between of solution and of acid. For a…

Q: Calculate the pH of a solution of magnesium hydroxide, Mg(OH)2 (Ksp = 5.6 × 10−12), made by…

A: Solubility Product : For a sparingly soluble salt , the product of Solubility (mol/lit) of all the…

Q: The leaves of the rhubarb plant contain high concentrations of diprotic oxalic acid (HOOCCOOH) and…

A: Diprotic acid have two acidic hydorgen atoms. It can donate two hydrogen atoms. Carbonic acid is…

Q: A buffer solution was made by dissolving 10 g of sodium acetate (CH3COONa) in 100 ml of 1.0 M Acetic…

Q: The weak acid, HA, has a Ka of 3.00 x 10-8. What is the Kp of its conjugate base, A"?

A: Given :- Ka for weak acid HA = 3.00 × 10-8 To calculate :- Kb for conjugate base A-

Q: Calculate the solubility of zinc (II) hydroxide in a solution maintained at (i) pH= 5.3 (ii) pH=…

Q: Lakes have a natural buffering capacity, especially in regions where limestone gives rise to…

A: Sulphuric acid in the lake contains H3O+ ions. when acid rain falls in the lake that contains…

Q: which is tribasic(H3Y). 25cm^3 of lemon juice was diluted to 250cm^3. 25cm^3 of the solution was…

A: The question is based on the concept of solutions. we have to quantitatively estimate the citric…

Q: For an open system with PCO2=10−3.5 atm what fraction of the total carbonate is in the form of CO32−…

A: Given: Partial pressure of carbon dioxide= 10-3.5 atm . To find: Total fraction of carbonate ion…

Q: Calculate the molar solubility of X(OH)3 within water. Ksp X(OH)3 = 8.3 x 10–34 2.6 x 10–9 M…

Q: What is the molar solubility of calcium fluoride in water? The Ksp is 3.9 x 10-11 at 25 °C. O 2.1 x…

A: Answer:- (A) 2.1×10-4 Given Ksp of CaF2 is 3.9×10-11 We can determined molar…

Q: determination of formic acid by neutralization volumetry, an analyst calculated the pH as a function…

A: pH is a scale used to specify the acidity or basicity of an aqueous solution. pH is defined as the…

Q: What is the pH of the solution that results from the mixing of 250.0 mL of 0.350M HCl and 100.0 mL…

Q: . Upon investigating the pH of different ponds, you found out that a sertain pond measures 4.2 which…

Q: What is the pH of a solution that results from diluting 0.30 mol acetic acid (CH;CO,H) and 0.20 mol…

Q: Calculate the pH of a 0.22 M solution of a weak acid (HA). Ka for HA = 3.0 x 10-4.

A: The pH of a solution is a measure of hydrogen (H+) ion concentration, which is, in turn, a measure…

Q: ?For Cu(OH)2, Ksp = 1.6 x 10-19. What is the molar solubility of Cu(OH)2 2.7 x 10-11 M .a 5.1 x…

A: Correct option C. 3.4 x 10-7 M

Q: You are on one of Saturn's many moons and discover a substance, Y2O that undergoes autoionization…

A: Applying similar concept of kw and pH as like water because it also involves in auto ionisation like…

Q: A volume of 100.0 mL of 3.016 M strontium nitrate was added to 200.0 mL of a 3.644 M solution of…

Q: One can calculate the molar solubility of a conic marble sample, predominantly made of CaCO3, when…

A: A numerical problem based on Ksp, which is to be accomplished.

Q: If 360 mL of 2.66 x 10-4M Pb(NO3)2 is added to 275 mL of 8.37 x 10-5 M NaI (in aqueous solution)…

Q: Consider the titration of 25.0 mL of 0.124 M acetic acid (CH₂COOH, pK, = 4.75) with 0.125 M NaOH.…

A: #1. Calculation for initial pH: Initial [CH3COOH] = 0.124 M pKa = 4.75

Q: Phosphate buffered saline (PBS) is buffered to a pH of 7.40, the pH of human blood, with the H₂PO4…

A: Given: pH=7.40Ka=6.31×10-8

Q: Sulphuric acid (H2SO4 ), used in the manufacture of fertilizers, undergo decomposition and the acid…

A: Given First acid dissociation constant of H2SO4 = Ka1 = 1 x 103 Second acid dissociation constant…

Q: Aniline, C6H7N (molar mass = 93.13 g/mol), is a weak base that is used as a precursor in the…

A: The solution is given below -

Question

One strategy for dealing with the acidification of lakes is periodically to add powered limestone (CaCO₃) to them, resulting in pH of 10.95. Calculate the Ca²⁺ concentration in the lake.

CO₂ in atmosphere 370 ppm

K_H,CO2 = 0.033 mol/(L∙atm)

K_a1 = 10^-6.3

K_a2 = 10^-10.3

K_sp,CaCO3 = 4.57 x 10^-9

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

Lakes have a natural buffering capacity, especially in regions where limestone gives rise to dissolved calcium carbonate. Write an equation for the effect of a small amount of acid rain containing sulfuric acid if it falls into alake containing carbonate (CO3-2 ) ions. Discuss how the lake will resist further pH changes. What happens if a large excess of acid rain is deposited?
Calculate the pH, pOH, and fraction of solute protonated or deprotonated in the following aqueous solutions: (a) 0.150 M CH3CH(OH)COOH(aq) (lactic acid), (b) 2.4 x 10-4 M CH3CH(OH)COOH(aq), (c) 0.25 M C6H5SO3H(aq) (benzenesulfonic acid). The appropriate values for pKa or pKb are given inthe table.
You are given a 27 % (w/v) solution of psicose. Molar mass: psicose (C6H12O6) = 180.156 g/mol. You dissolve 6.31 g of potassium formate in 250 mL of 0.25 M formic acid (HCOOH). This solution was then made up to a total volume of 500 mL with distilled water. Potassium formate (KHCO2): molar mass = 84.12 g/mol Calculate the pH of this solution given the pKa of formic acid = 3.77.
For CO2 in the atmosphere at 25 degrees C, kH = 3.4 x 10-2 mol L-1 atm-1 and the partial pressure of CO2 is .000405 atm: Calculate the concentration of dissolved H2CO3 (aq) air-saturated rainwater. Determine the pH expected for rainwater on the basis of the first dissociation constant of the carbonic acid, H2CO3 (aq), from the dissolved CO2. The pKa values of carbonic acid are pKa1 = 6.35 and pKa2 = 10.33 at 25 C.
Give the pH of 0.005 M C6H5O- (aq) at 298 K of the Ka for C6H5OH at the given T is 1.0 x 10-10
Consider the titration of 100.0 mL of 0.200 mol/L ethanoic acid, HC2H3O2(aq) (Ka = 1.8 x 10-5), by 0.100 mol potassium hydroxide solution. Calculate the pH of the resulting solution when 150.0mL of potassium hydroxide solution has been added?
A 0.025 M solution of an unknown organic acid has a pH of 3.23. 2.1 By means of a full calculation, determine the value of the ionisation constant of the conjugatebase of this acid..- You may use “HA” to denote the formula of the acid.- You may make certain assumptions to simplify your calculations2.2 A certain amount of the sodium salt of the conjugate base of the acid was added to the system.Will the pH of the resulting solution increase or decrease, compared to the original given value? Explain your answer in a short sentence or two.
In some water softening operations, Mg2+ must be removed from solution along with Ca2+. What is the minimum pH required to lower TOTMg to 10 mg/L as CaCO3 by precipitation of Mg(OH)2(s)?
A 0.3654 g portion of pure formic acid (CH2O2, FW=46.03 g/mol, Ka=1.77 x 10-4) is dissolved in 50.00 mL of water and is titrated with 0.1086 M NaOH. What is the expected pH during this analysis when the titration is complete?
the solubility (in M) of cobalt(II) hydroxide, Co(OH)2(s) in H2O. Ksp = 1.70×10-16 at a specific temperature=3.49x10^-6 What is the pH of this solution of cobalt(II) hydroxide?
In the determination of the water hardness of a river water sample, the pH of the sample was adjusted to 12 instead of 10. Is there a positive error, negative error, no effect, or error could not be determined In terms of the ppm CaCO3 of sample?
A 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was added