KConsider a situation in which acid rain has heavily polluted a lake to a level of pH 4. Anunscrupulous chemical company dumps some acid into the lake illegally. Assume that thelake contains 250 million gallons of water and that the company dumps 250,000 gallons ofacid with pH 2. Complete parts (a) through (d) below.a. What is the hydrogen ion conentration, [H*], of the lake polluted by acid rain alone?410 (Type your answer using exponential notation.)b. Suppose that the unpolluted lake, without acid rain, would have a pH of 7. If the lakewere then polluted by company acid alone (no acid rain), what hydrogen ion concentration[H], would it have? Round to the nearest power of ten, as necessary.(Type your answer using exponential notation.)X +View an exampleGet more help -ViClear allMoreCheck answerX

The pH of a solution is expressed in terms of hydrogen ion concentrations and its formula is- pH =…

10 (Type your answer using exponential notation.) b. Suppose that the unpolluted lake, without acid rain, would have a pH of 7. If the lake were then polluted by company acid alone (no acid rain), what hydrogen ion concentration [H], would it have? Round to the nearest power of ten, as necessary. (Type your answer using exponential notation.)

10 (Type your answer using exponential notation.) b. Suppose that the unpolluted lake, without acid rain, would have a pH of 7. If the lake were then polluted by company acid alone (no acid rain), what hydrogen ion concentration [H], would it have? Round to the nearest power of ten, as necessary. (Type your answer using exponential notation.)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 9RQ: What is a salt? List some anions that behave as weak bases in water. List some anions that have no...

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Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?
What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.
Find [OH-] and the pH of the following solutions. (a) 0.25 g of Ba(OH)2 dissolved in enough water to make 0.655 L of solution. (b) A 3.00-L solution of KOH is prepared by diluting 300.0 mL of 0.149 M KOH with water. What is the molarity of the diluted solution? What is the effect of a tenfold dilution on the pH?
Students are often surprised to learn that organic acids, such as acetic acid, contain OH groups. Actually, all oxyacids contain hydroxyl groups. Sulfuric acid, usually written as H2SO4, has the structural formula SO2(OH)2, where S is the central atom. Identify the acids whose structural formulas are shown below. Why do they behave as acids, while NaOH and KOH are bases? a. SO(OH)2 b. ClO2(OH) c. HPO(OH)2
Calculate the maximum volume in mL of 0.15 M HCl that each of the following antacid formulations would be expected to neutralize. Assume complete neutralization. (Show work.) a) a tablet containing 250 mg Al(OH)3 and 150 mg Mg(OH)2 b) a tablet containing 850 mg of CaCO3
Consider two lakes, North Lake and South Lake. North Lake has a granite base, and South Lake has a limestone base. Each of them is exposed to acid deposition, primarily from nitric acid. Both lakes have volumes of 3 × 106 m3, surface areas of 1.0 × 105 m2, and are fed by springs that have no nitric acid and have flow rates of 75 m3/day. a. Calculate the pH of North Lake if it experiences a nitric acid deposition rate of 1.5 × 10–10 mol m–2 day–1 . Remember, granite lake beds do not buffer acids. The pH could be very low, due to the lack of any nitric acid removal processes other than its dissociation and dissolution processes. b. Calculate the pH of South Lake if it experiences the same nitric acid deposition rate. This time, there is limestone to buffer the nitric and carbonic acids.
Over the past 250 years, the average upper-ocean pH near the Pacific Northwest has decreased by about 0.1 units, from about 8.2 to 8.1. This drop in pH corresponds to an increase in acidity of about 30%. When CO2 levels in seawater rise, the availability of carbonate ion, CO32−, This makes it more difficult for marine organisms to build and maintain shells and other body parts from calcium carbonate. Calculate H3O+ and OH− concentrations at pH levels of 8.2 and 8.1. Demonstrate by calculations that this decrease in pH corresponds to an increase in acidity of about 30%. Explain the relationship between the pH of seawater and the availability of carbonate ion. Does the change in pH from 8.2 to 8.1 result in an increase or decrease in the availability of carbonate ion?
Rain with a pH below 5.6 is considered acid rain. The principal cause of acid rain is coal-burning electrical power plants (sulfurous and sulfuric acids are formed in the atmosphere from this). Any combustion reaction that produces high temperature can also produce acid rain (nitrous and nitric acid are produced in the atmosphere from this). Thus, automotive engines are also an important contributor to acid rain. Acid rain harms both living and nonliving things in a variety of ways. What solution/s can you propose to combat acid rain?
Determine the pH of a 0.650 M solution of magnesium nitrite, Mg(NO2)2 at 25 °C. A solution containing 7.50 g of this salt is diluted with water until it reaches a pH of 8.18.What is its final volume? Give one example of a salt whose solution is expected to be acidic and briefly explain why. Give one example of a salt whose solution is expected to be basic and briefly explain why. You cannot reuse the compound in a) and b) to answer c) and d).
Aluminum has been implicated as a neurotoxic agent for Alzheimer’s patients and is known as harmful for renal failure patients. In 1985, the medical community recommended that no more than 10 mg/L Al3+ be present in drinking water used for dialysis patients. At what pH is the maximum Al3+ concentration equal to 10 mg/L, assuming that the only source of Al3+ is Al(OH)3? How does this compare with the allowable pH of drinking water of 7.8; would we expect to observe this concentration in drinking water?
find the volume of 0.675 m HCl is required to neutralize 30 ml of 0.0035 m Ba(OH)2?