**Understanding Acid Rain and Its Effects**"Acid rain" forms when rain falls through air polluted by oxides of sulfur and nitrogen, which dissolve to form acids such as \( \text{H}_2\text{SO}_3 \), \( \text{H}_2\text{SO}_4 \), and \( \text{HNO}_3 \). Trees and plants are affected if the acid rain has a pH of 3.5 or lower.**Calculation of Hydrogen Ion Concentration**1. **Problem:** What is the hydrogen ion concentration in acid rain that has a pH of 3.41? \[ \text{[H}^+\text{]} = \] \_\_\_ M2. **Problem:** What is the pH of a solution having twice your calculated hydrogen ion concentration? \[ \text{pH} = \] \_\_\_For these questions, you will calculate the hydrogen ion concentration using the formula for pH and then determine how the concentration change affects the pH.

1) Here given---- pH of the acid rain = 3.41 We know---- pH = - log [H+] Or, [H+] = 10-pH Now…

"Acid rain" forms when rain falls through air polluted by oxides of sulfur and nitrogen, which dissolve to form acids such as H₂SO3, H₂SO4, and HNO3. Trees and plants are affected if the acid rain has a pH of 3.5 or lower. What is the hydrogen ion concentration in acid rain that has a pH of 3.41? [H*] = i What is the pH of a solution having twice your calculated hydrogen ion concentration? pH = M i

"Acid rain" forms when rain falls through air polluted by oxides of sulfur and nitrogen, which dissolve to form acids such as H₂SO3, H₂SO4, and HNO3. Trees and plants are affected if the acid rain has a pH of 3.5 or lower. What is the hydrogen ion concentration in acid rain that has a pH of 3.41? [H*] = i What is the pH of a solution having twice your calculated hydrogen ion concentration? pH = M i

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...

See similar textbooks

Similar questions

This is a multi- answer question. Please type your properly rounded answers in the next three questions ( starting with this one):Calculate the pH of a 0.70 M solution of sodium sulfite, Na2SO3. Also calculate the concentrations of HSO3 and H2SO3. Type the properly rounded pH below:
help please
What is the pH of a 0.0200 M Ba(OH)2 solution? A) 12.6 C) 1.70 B) 12.3 D) 1.40 E) 0.040 A solution has a pH of 5.45. What is the proton concentration, [H*]? A) 5.45 x 10-7 B) 2.82 x 10-9 C) 3.55 x 10-6 D) 8.55 E) 5.45 Benzoic acid, C6H5CO₂H, is a weak organic acid: C6H5CO₂H C6H5CO₂-1 + H+1 Determine the pH of a 0.461 M benzoic acid solution. A) 2.26 C) 11.74 B) 4.52 D) 9.48 E) 5.48
< Which of the following solutions would be expected to have a pH of 7.00? Weak Acid HCN HNO₂ HIO HBrO C6H5COOH Ka 4.9 x 10-1⁰ 4.5 x 10-4 2.3 x 10-¹1 2.5 x 10-⁹ 6.3 x 10-5 Question 4 of 11 Tap here or pull up for additional resources Weak Base HONH, NH3 CoHsNH, H₂NNH₂ C5H5N A) CSIO B) NaF C) LICIO3 D) KNO₂ Submit
Enough of a monoprotic weak acid is dissolved in water to produce a 0.0114 M solution. The pH of the resulting solution is 2.60. Calculate the K₂ for the acid. = K₂ = x10 TOOLS
What are the concentrations of hydrogen ion and hydroxide ion in household ammonia, an aqueous solution of NH3 that has a pH of 11.50? What is the concentration of hydroxide ion in household ammonia, an aqueous solution of NH3 that has a pH of 11.50? M OH- What is the concentration of hydrogen ion in household ammonia, an aqueous solution of NH3 that has a pH of 11.50? M H+
Ethanolamine, HOC2H4NH2, is a viscous liquid with an ammonia-like odor; it is used to remove hydrogen sulfide from natural gas. A 0.84 M aqueous solution of ethanolamine has a pH of 11.70. What is K, for ethanolamine? Calculate the pH of a 0.63 M aqueous solution of ethanolamine.
What is the pH of a 0.2 M solution of each of the following (for this question, assume only the first proton contributes to the solution [H+]). Acetic acid (CH3COOH) Ka = 1.8 x 10^-5 Sodium acetate (NaCH3COO) = 1.7 x 10^-5 Carbonic acid (H2CO3) = 5.0 x 10^-7
Los Angeles has water regulations that requires any wastewater poured down the drain to be between pH = 4.5 and pH = 9.0. In lab, Dr. Smith is feeling lazy and decides to pour waste down the drain instead of going through the appropriate procedure for disposal of chemical waste. The waste contained your 0.250 M solution of HCl. Does this wastewater comply with the Los Angeles water standards? Hint: Recall that strong acids completely dissociate. HCl → H+ + Cl- How is [H+] related to the concentration of the HCl solution? a)No, this solution has pH below the safe range. b)Yes, this solution has pH within the safe range. c)No, this solution has pH above the safe range. d)The pH will depend on the volume (liters) of solution.
Water ionizes by the equation Н20(1) — н+ (аq) + ОH (аq) The extent of the reaction is small in pure water and dilute aqueous solutions. This reaction creates the following relationship between [H*] and [OH ]: Part A At a certain temperature, the pH of a neutral solution is 7.27. What is the value of Kw at that temperature? K, = [H*][OH¯] Express your answer numerically using two significant figures. Keep in mind that, like all equilibrium constants, the value of Kw changes with temperature. • View Available Hint(s) V ΑΣφ. ? Kw %3D Submit Part B What is the pH of a neutral solution at a temperature where Kw 9.9 x 10-14? Express your answer numerically using two decimal places. • View Available Hint(s) V ΑΣφ. pH = Submit
Chemistry 2, Question 2
A chemist dissolves 576. mg of pure nitric acid in enough water to make up 150. mL of solution. Calculate the pH of the solution. Be sure your answer has the correct number of significant digits. 0 X S