If the pH of a 1.00 in. rainfall over 1700 miles^2 is 3.40, how many kilograms of sulfuric acid, H2SO4, are present, assuming that it is the only acid contributing to the pH? For sulfuric acid, Ka1 is very large and Ka2 is 0.012. The presence of SO2 in the atmosphere and thesulfuric acid that it produces result in the phenomenonof acid rain. Uncontaminated rainwater is naturallyacidic and generally has a pH value of about 5.6. ThepH of acid rain is about 4. This acidity has affectedmany lakes in northern Europe, the northern UnitedStates, and Canada, reducing fish populations andaffecting other parts of the ecological network withinthe lakes and surrounding forests.The pH of most natural waters containing livingorganisms is between 6.5 and 8.5, but freshwater pHvalues are far below 6.5 in many parts of thecontinental United States. At pH levels below 4.0, allvertebrates, most invertebrates, and manymicroorganisms are destroyed. More than 300 lakes inNew York State contain no fish, and 140 lakes inOntario, Canada, are devoid of life. The acid rain thatappears to have killed the organisms in these lakesoriginates hundreds of kilometers upwind in the OhioValley and Great Lakes regions. Some of theseregions are recovering as sulfur emissions from fossilfuel combustion decrease, in part because of the U.S.Clean Air Act of 1990, which required that power plantsreduce their sulfur emissions by 80%.

Height of rainfall = 1.00 inch = 0.0254 m Area of rainfall = 1700 miles² 1 mile² = 2.59×10⁶ m²…

If the pH of a 1.00 in. rainfall over 1700 miles^2 is 3.40, how many kilograms of sulfuric acid, H2SO4, are present, assuming that it is the only acid contributing to the pH? For sulfuric acid, Ka1 is very large and Ka2 is 0.012.

If the pH of a 1.00 in. rainfall over 1700 miles^2 is 3.40, how many kilograms of sulfuric acid, H2SO4, are present, assuming that it is the only acid contributing to the pH? For sulfuric acid, Ka1 is very large and Ka2 is 0.012.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 84AP

See similar textbooks

Related questions

Q: Phosphoric acid, H3PO4 is a triprotic acid. pKa1= 2.16 pKa2=7.21 pKa3=12.32…

A: Given data, Molarity of HPO42-=0.450MpKa1=2.16pKa2=7.21pKa3=12.32

Q: Calculate the pH of water at 25°C and 75°C. The values for pKw at these temperatures are 13.99 and…

A: Pure water has an equal concentration of hydrogen ions and hydroxyl ions. The dissociation of water…

Q: Derive equations that define a0, a1, a2 and a3 for the triprotic acid H3X

A: In the titration of acid H3X, changes in the concentration of various species can be visualized from…

Q: Do you think the pH of 1.0 M tri-methyl ammonium (CH3)3NH", pKa 9.80, will be higher or lower than…

Q: 1. Calculate the pH of the solutions described below and specify if they are acidic, basic, or…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub- parts for…

Q: Carbonic acid, H:COs is a diprotic acid with Ka1 = 4.3 x 10 7 and Ka2 = 5.6 x 10 11 What is the pH…

A: H2CO3 is the weak dibasic acid as it gives two H+ ions. Since, value of Ka1 of H2CO3 is very-very…

Q: The acid-dissociation constants of phosphorous acid (H3PO3) are Ka1 = 7.5 x 10 3, Ka2 = 6.2 x 108,…

A: Dissociation constant are based on ion of H3PO3 .

Q: 2.2 6. (1) Define pH in words. The strong acid HCl has a pH value of 1, use the following equation…

Q: Consider the following data on some weak acids and weak bases: acid base K, K, name formula name…

Q: Calculate the formate ion concentration and pH of a solution that is 0.050 M in formic acid (HCOOH,…

Q: Suppose that ammonia, applied to a field as a fertilizer, is washed into a farm pond containing 3.0…

Q: Consider the following data on some weak acids and weak bases: acid base Bo K, name formula name…

A: The given compounds are salts. So to check their pH , we would determine how these salts are made.…

Q: Phosphoric acid, H3PO4 is a triprotic acid. pKaj= 2.16 pКа237.21 pКаз-12.32 2- Calculate the pH of a…

A: Phosphoric acid will ionize in aqueous solution as--

Q: For propanoic acid (HC3 H5 O2, Ka = 1.3 X 10^5), determine the concentration of all species present,…

A: Given that the propanoic acid (HC3 H5 O2, Ka = 1.3 X 10^5). Since, the Ka power value won’t be in…

Q: Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name…

A: Given the following data on some weak acids and weak bases: We have to rank the following solutions…

Q: The pOH of ammonium hydroxide at 25 C is 5.55. What is the pH and the [H ], [OH ] in mol/L for…

A: At constant temperature, the pH of a solution remains constant. For 250 C, the pH of the solution…

Q: Abbreviating malonic acid, CH2(CO2H)2, as H2M, find the pH and concentrations of H2M, HM, and M2…

A: a.

Q: The pH for 0.0715 M solution of CCl,CO2H is 1.40. Determine the value of Ka for CCl,CO2H. 1 2 Based…

A: pH of Solution = 1.40 [CCl3COO2H] = 0.0715 M Ka for CCl3COO2H =?

Q: Calculate the pH of a 0.0778 M aqueous solution of formic acid (HCOOH, K, = 1.8×10). pH =

A: The value of Ka for the formic acid is 1.8 × 10-4

Q: The pHpH scale for acidity is defined by pH=−log10[H+]pH=−log10⁡[H+] where [H+][H+]is the…

Q: Explain what happens to the ratio of the two common forms of free residua! chlorine as the pH of…

A: Hypochlorous acid, HOCl(aq) is a weak acid with Ka = 2.5*10-8 Hypochlorite, ClO-(aq) is a conjugate…

Q: Calculate [OH–] , [H+] , and the pH of 0.20 M solutions of each of the following amines. a.…

A: Aniline and pyridine both are weak bases. From the equilibrium table we have to determine its…

Q: Maleic acid (H2C4H2O4) is a diprotic acid with ?a1=1.20×10−3 and ?a2=5.37×10−7. Determine the pH of…

A: 1- First we will determine the H+ ion concentration : Most H+ ion comes from first dissociation.…

Q: The pKw of seawater at 25°C is 13.776. This differs fromthe usual pKw of 14.00 at this temperature…

A: Given data contains, pKw of seawater is 13.776. pH in seawater is 8.00. Actual pKw of water is…

Q: Three (3) 0.10 M acid solutions were prepared and their pH values were recorded. Match the solution…

A: The acidic character of an organic compound depends on the stability of the resulting conjugate…

Q: Sulfurous acid, H2SO3, is a diprotic acid Ka1 = 1.3 × 10-2 and Ka2 = 6.3 × 10-8. The acid forms when…

Q: Calculate the pH of the following solutions: a. 0.34 M hydrocyanic acid. b. 1.5 M solution of…

A: pKa of hydrocyanic acid is 9.2

Q: Calculate the pH of a 0.31 M sodium formate solution (HCOONa). Kb for HCOO− = 5.9 × 10−11

A: Given :- [HCOONa] = 0.31 M Kb for HCOO- = 5.9 × 10−11 To calculate :- pH of solution

Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…

Q: Calculate the pH of 0.40 M NH3 solution, Kb = 1.8 x 10° M.

A: Given :- concentration of NH3 solution = 0.40 M kb for NH3 = 1.8 × 10-5 M To be calculated :- pH…

Q: Why is rainwater always acidic, even in the absence of polluting gases such as SO3?

A: The rain water is acidic due to the presence of carbon dioxide, sulphur dioxide and nitrogen dioxide…

Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…

A: Solution -

Q: The pH of a 0.05 M NaOH solution at 25 °C is: O 10.3 O 12.7 O 11.5 O 13.1 O13.8

A: pH of solution is calculated using relation pH + pOH = 14

Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…

A: For first ionization : pH = 0.5pKa1 - 0.5logC ..(1) Here, pKa1 = -logKa1 = -log(8*10^-5) = 4.097 C…

Q: HClO is a weak acid (Ka=4.0×10−8Ka=4.0×10−8) and so the salt NaClO acts as a weak base. What is the…

A: Ka of HClO is given as 4 x 10-8. It is required to calculate the pH of solution that is 0.029M in…

Q: The value pKw is 11.05 at 78 °C. What is the pH of a neutral solution at the same temperature? Enter…

Q: Thiamine hydrochloride (vitamin B1 hydrochloride, HC12- H17ON4SCl2) is a weak acid with Ka = 3.4 ×…

A: Molar Mass of thiamine hydrochloride is 337.3 g/mol. Mass of thiamine hydrochloride is 3×10-5…

Q: Which of the following solutions would have the lowest pH? Assume that they are all 0.10 M in acid…

A: If the acid has larger Ka, it indicates that the acid can dissociate very well and so it is a strong…

Q: Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name…

A: The compounds given are KCN, C6H5NH3Br, NaNO2 and KBr.

Q: Calculate the pH of a 0.085 M solution of acetic acid, HC2H302. (ka=1.9x10-5) HC2H302 - H* + C2H3O2…

A: pH measures the strength of acids and base that how the solution is acidic and basic lower the pH…

Q: What is the final pH of a 0.012 M solution of sulfuric acid? Ka1 >>1 Ka2 = 1.1 x 10 2 %3D Although…

Q: The Kb of dimethylamine [(CH3)2NH] is 5.90x10–4 at 25°C. Calculate the pH of a 0.103 M solution of…

A: Given : Concentration of (CH3)2NH = 0.103 M And Kb of (CH3)2NH = 5.90 X 10-4 Since (CH3)2NH is a…

Q: At pH = 3.9, a weak acid has a concentration of 0.75 M. If the pKa = 4.5, what is the concentration…

Q: Calculate the pH of an aqueous KOH solution that is made by dissolving 654 mg of solid KOH in enough…

Q: What concentration of acetic acid would produce an aqueous solution with a pH = 3.275? (Ka for…

A: Provided pH of acetic acid=3.275 Provided Ka of acetic acid=1.76×10-5 Since, pH = -log[H+] By using…

Q: If the pH of a 1.00-in. rainfall over 1800 miles^2 is 3.90, how many kilograms of sulfuric acid,…

A: Given: pH = 3.90Area= 1800 miles2Ka2 = 0.012.

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

The presence of SO2 in the atmosphere and the
sulfuric acid that it produces result in the phenomenon
of acid rain. Uncontaminated rainwater is naturally
acidic and generally has a pH value of about 5.6. The
pH of acid rain is about 4. This acidity has affected
many lakes in northern Europe, the northern United
States, and Canada, reducing fish populations and
affecting other parts of the ecological network within
the lakes and surrounding forests.
The pH of most natural waters containing living
organisms is between 6.5 and 8.5, but freshwater pH
values are far below 6.5 in many parts of the
continental United States. At pH levels below 4.0, all
vertebrates, most invertebrates, and many
microorganisms are destroyed. More than 300 lakes in
New York State contain no fish, and 140 lakes in
Ontario, Canada, are devoid of life. The acid rain that
appears to have killed the organisms in these lakes
originates hundreds of kilometers upwind in the Ohio
Valley and Great Lakes regions. Some of these
regions are recovering as sulfur emissions from fossil
fuel combustion decrease, in part because of the U.S.
Clean Air Act of 1990, which required that power plants
reduce their sulfur emissions by 80%.

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

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

List and discuss the basicity of the following compounds.
Let's assume that there is 400 μatm of pCO2 in our atmosphere. Assumingthere is nothing else in the water coming from the atmosphere, what is the pH of rainwater in equilibrium with this atmospheric CO2?Assume KH = 5.4x10-2 mol kg-1 atm-1. KC1 = 3.47×10-7 mol2 kg-2 for freshwater rain.Hint: Because rainwater is acidic, it has little/no alkalinity, thus the (H+] = Alk = [HCO3-]
How many grams of sodium hydroxide do yiu need to neutralize 500mL of the acidic solution (pH 2.6)?
Acid Rain Acid rain is a growing worldwide environmental problem. Naturally, rainwater should have a pH of not less than 5.5, but in the northeastern United States, for example, the average pH of rainwater is about 4.5. The increased acidity of the rain kills plants and animals in lakes and streams, causes increased weathering and decomposition of limestone in statues and on buildings (posing a major threat to Greek antiquities), and creates problems with the production of fruit and vegetable crops. The major chemical involved is sulfur dioxide, SO2SO2, which combines with rainwater to form sulfuric acid. Atmospheric SO2SO2 has many sources, with volcanoes being the primary natural contributor. However, the burning of fossil fuel as the result of human industrialization has led to a significant increase in atmospheric SO2SO2 levels. The number of moles nnn of SO2SO2 released from a coal-burning power plant can be determined from the density ρρrho, volume VVV, and the molar mass…
A large volume of 0.1760 M H2SO3(aq) is treated with enough NaOH(s) to adjust the pH of the solution to 5.55. Assuming that the addition of NaOH(s) does not significantly affect the volume of the solution, calculate the final molar concentrations of H2SO3(aq), HSO3−(aq), and SO32-(aq) in solution given that the Ka1 and Ka2 values are 1.50×10−2 and 1.20×10−7 , respectively.
The pKa of Cl3CCO2H is 0.64. What is the pH of a 0.580 M solution? What percentage of the Cl3CCO2H is dissociated?
The pH of human blood is steady at a value of approximately 7.4 owing to the following equilibrium reactions: Acids formed during normal cellular respiration react with the HCO3- to form carbonic acid, which is in equilibrium with CO2(aq) and H2O(l). During vigorous exercise, a person’s H2CO3 blood levels were 26.3 mM, whereas his CO2 levels were 1.63 mM. On resting, the H2CO3 levels declined to 24.9 mM. What was the CO2 blood level at rest?
When a solution is prepared by dissolving one pellet of KOH weighing 128 mg in 500 ml of dH2O (distilled water) what will be pH of this solution? (Mw of KOH: 51.1 g/mol)
Explain which is the stronger acid, H3PO4 or H2SO3; CCl3CH2COOH or CCl2FCH2COOH. [Draw possible Lewis structure models]
Predict the acid strengths of the following compounds: H2O, H2S & H2Se
Explain the difference in acidity of the following compounds.
Bronsted-Lowry acid/base strengths are dictated by the proton donor/acceptor propertiesof the reaction media. With this in mind, write out chemical reactions emphasizingproton transfers occurring in the following processes:a) Phosphoric acid (H3PO4) functions as base in concentrated H2SO4. b) Perchloric acid (HClO4) and nitric acid (HNO3) are both strong acids in water. In glacialacetic acid HClO4 functions as a strong acid whereas HNO3 is substantially weaker. c) Oxalic acid (HOOC-COOH) is a weak acid in water (Ka1 = 5.6×10-2; Ka2 = 1.5×10-4). Itbehaves as a strong monoprotic acid in liquid ammonia. d) Hydrogen fluoride (H-F) functions as a base in liquid anhydrous HClO4.