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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Determine the pH of a solution that is prepared by dissolving 6.9 g of Ba(OH)2 in 4.5 L water at 25°C. Assume that the volume of the solvent does not change upon addition of the solute. Atomic Weights: Ba = 137.3 g/mol; O = 16.00 g/mol; H = 1.008 g/mol. Express your answer in two decimal places only. Do not put the units.
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
Determine the pH of a solution that is prepared by dissolving 8.6 g of Ba(OH)2 in 1.3 L water at 25°C. Assume that the volume of the solvent does not change upon addition of the solute. Atomic Weights: Ba = 137.3 g/mol; O = 16.00 g/mol; H = 1.008 g/mol. Express your answer in two decimal places only. Do not put the units.
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.
An aqueous solution contains 0.443 M acetic acid. Calculate the pH of the solution after the addition of 2.45×102 moles of sodium hydroxide to 155 ml. of this solution. (Assume that the volume does not change upon adding sodium hydroxide) pH = An aqueous solution contains 0.363 M ammonia. Calculate the pH of the solution after the addition of 3.39×10-2 moles of nitric acid to 255 mL of this solution. (Assume that the volume does not change upon adding nitric acid.) PH =
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
We did an experiment in a lab. We tested for the strength of acids and bases using a conductivity test. Distilled water was used as one of the solutions. the litmus paper and phenolphthalein did not change color. It did not also conduct electricity. Hence it was assumed to be a nonelectrolyte therefore a neutral solution. However, upon searching the internet, it was found that water is not exactly acidic. A pH of 7 at 25°C represents PURE distilled water. Distilled water is considered to be slightly acidic because it absorbed carbon dioxide from the air. The pH of distilled water can range anywhere between 5.5 and 6.9, depending on how long it has been exposed to air. If this is true, then shouldn't the distilled water conduct electricity since acids conduct electricity? Yes or No? please provide an explanation and chemical equation if possible. thank you!
Muscles produce lactic acid, CH, CH(OH)COOH(aq), during exercise. Calculate the percent ionization (deprotonation), pH, and POH of a 0.1075 M solution of lactic acid. The acid-dissociation (or ionization) constant, K₁, of this acid is 8.40 x 10-4. percent ionization = pH = pOH == %
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)
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?

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