Atmospheric CO2 levels have risen by nearly 20%over the past 40 years from 315 ppm to 380 ppmPart AGiven that the average pH of clean, unpolluted rain today is 5.4, determine the pH of unpolluted rain40 years ago. Assume that carbonic acid (H2CO3) formed by the reaction of CO2 and water is theonly factor influencing pH.CO2(g)+NO11) = HgCO(aq)Express your answer using one decimal place.pH = 5.4✓ CorrectPart BPrevious AnswersWhat volume of CO2 at 25 °C and 1.0 atm is dissolved in a 13.0-L bucket of today's rainwater?Express your answer using two significant figures.Η ΕΠΙ ΑΣΦVco₂ =0?SubmitPrevious Answers Request AnswermL1015

Part B: Pressure P= 1.0atmVolume of rain water = 13 L.Temperature: 25oC = 25+273.15 = 298.15K.…

Answered: Atmospheric CO2 levels have risen by…

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...

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Hydrazine, N₂H4, is used as a rocket fuel, but also as a reactant in organic chemistry. The K, of hydrazine is 9.1 x 10-7. If 4.75 x 10-3 mol of hydrazine are added to water to make up 0.500 L of solution, what is the pH of the solution? Select the correct answer below: 6.5 10.0 11.6 13.0
For each of the following entities • Identify it as a strong or weak acid. • Select the correct arrow to show the changes that occur when the acids are placed in water. • Select the approximate pH for each resulting solution. HCI(aq) is classified as a + acid. The reaction equation with water utilizes which of the following arrows? Choice A Choice B 7 >>7 H2SO3(aq) is classified as a The reaction equation with water would utilize which of the following arrows? Choice A Choice B < 50% H2SO3(aq) + H20(I) • HSO3 (aq) + H30*(aq) The approximate pH of the solution would be
A chemist must prepare 800.0 mL of potassium hydroxide solution with a pH of 12.90 at 25 °C. She will do this in three steps: • Fill a 800.0 mL volumetric flask about halfway with distilled water. Weigh out a small amount of solid potassium hydroxide and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the mass of potassium hydroxide that the chemist must weigh out in the second step. Round your answer to 2 significant digits.
A chemist must prepare 400.0 mL of hydrochloric acid solution with a pH of 1.20 at 25 °C. He will do this in three steps: • Fill a 400.0 mL volumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (8.0M) stock hydrochloric acid solution and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the volume of concentrated hydrochloric acid that the chemist must measure out in the second step. Round your answer to 2 significant digits. |mL x10
A chemist must prepare 700.0 mL of sodium hydroxide solution with a pH of 12.30 at 25 °C. She will do this in three steps: • Fill a 700.0 mL volumetric flask about halfway with distilled water. • Weigh out a small amount of solid sodium hydroxide and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the mass of sodium hydroxide that the chemist must weigh out in the second step. Round your answer to 2 significant digits. Ox10
At 25°C the value of Kw is 1.0 x 1014. At 60°C the value of Kw is 1.0 x 1013. Is the reaction exothermic or endothermic? Explain briefly. Calculate [H3O] and pH in a neutral solution at 60°C. 2H,0 0 H,O* (12)+OH (2)
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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−, 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 ions. Does the change in pH from 8.2 to 8.1 result in an increase or decrease in the availability of carbonate ions?
A chemist must prepare 800.0 mL of potassium hydroxide solution with a pH of 12.80 at 25 °C. She will do this in three steps: • Fill a 800.0 mL volumetric flask about halfway with distilled water. • Weigh out a small amount of solid potassium hydroxide and add it to the flask. Fill the flask to the mark with distilled water. Calculate the mass of potassium hydroxide that the chemist must weigh out in the second step. Round your answer to 2 significant digits. ☐ g ☐ x10
A chemist must prepare 550.0 mL of sodium hydroxide solution with a pH of 13.00 at 25 °C. He will do this in three steps: • Fill a 550.0 mL volumetric flask about halfway with distilled water. • Weigh out a small amount of solid sodium hydroxide and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the mass of sodium hydroxide that the chemist must weigh out in the second step. Round your answer to 2 significant digits.

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