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Carbon dioxide dissolves in water according to the equations:CO2( g) + H2O(l )<----->H2CO3(aq)H2CO3(aq) + H2O(l)<----->HCO3-(aq) + H3O+(aq)Carbon dioxide levels in the atmosphere have increased about 20% over the last century. Given that Earth’s oceans are exposed to atmospheric carbon dioxide, what effect might the increased CO2 be having on the pH of the world’s oceans? What effect might this change be having on the limestone structures (primarily CaCO3) of coral reefs and marine shells?

Identify the TRUE statement about acid rain. O Acid rain dissolves marble statues. O Acid rain contains nitric acid and sulfurous acid O Acid rain comes from hydroelectric power plants. O NO combines with oxygen and water to form nitrous acid, which is a component of acid rain. O Acid rain does not corrode steel bridges.

For each of the following pairs of substances • Classify each of the substances. • Compare their approximate pH levels. • Compare their ability to conduct electricity. • Compare their relative hydronium or hydroxide concentration. Comparison of 1.0 mol/L LIOH(aq) and 1.0 mol/L HOCI(aq) • LIOH(aq) is classified as a • HOCI(aq) is classified as a • HOCI(aq) has a + pH than LIOH(aq) has. . нос(ag) is a + electrical conductor than LIOH(aq) is. LIOH(aq) has a : [OH (aq)] than HOCI(aq) has. Comparison of 1.0 mol/L HCN(aq) and 1.0 mol/L KF(aq) • KF(aq) is classified as a • HCN(aq) is classified as a • HCN(aq) has a : pH than KF(aq) has. • HCN(aq) is a + electrical conductor than KF(ag) is. • HCN(aq) has a + [H30+(aq)] than KF(aq) has.

Consider the following data on some weak acids and weak bases: name K₂ formula HNO₂ 4.5 x 104 acetic acid HCH,CO₂ 1.8x105 acid nitrous acid solution 0.1 M HONHYBT 0.1 M KBr Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. 0.1 M KCH₂CO₂ 0.1 M C₂H₂NHCI PH choose one choose one choose one base choose one K name formula hydroxylamine HONH₂ 1.1 x 107 pyridine CH₂N 1.7×10

Explain how atmospheric nitrogen dioxide (NO2) decreases the pH of water in clouds and rain. In your answer, include balanced chemical equations for reactions of NO2 with water.

Hydrazoic acid, HN3, has an acid dissociation constant of 2.5 x 10-5.  Calculate the equilibrium concentrations of all substances if the initial concentration of HN3 is 0.0750 M. Determine the pH of the solution. Would a 0.0750 M solution of HBr have a higher or lower pH than the 0.0750 M HN3 solution? Explain why.

The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = - log [H*] where [H"] is the hydrogen ion concentration. a If the hydrogen ion concentration in a solution is 1.97 x 10 molL, the pH is b. If the pH of a solution is 3.146, the hydrogen ion concentration is mol/L.

If a limestone sculpture were treated to form a surface layer of calcium sulfate, would this help to slow down the effects of acid rain? Explain.

The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = -log[H¹] where [H] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 5.98 x 10-3 mol/L, the pH is b. If the pH of a solution is 3.171, the hydrogen ion concentration is mol/L.

A scientist is comparing two lakes. She finds that water samples from Lake X have a pH of 3.50 and water samples from Lake Y have a pH of 5.50. Therefore, it can be said that Lake X has a hydronium ion concentration that is times greater than Lake Y.

Laundry detergent most often exhibits basic properties. Calculate the pOH of a sample of laundry detergent if the hydronium ion concentration in a sample of detergent is 2.7 x 10-11 mol/L.   Ammonia is often used as a glass cleaner.  Calculate hydronium concentration of a sample of ammonia that has a pOH of 2.800You MUST show your work, and then record your final answer with the correct number of significant digits and proper units.

The pH scale was designed to make it convenient to express hydrogen ion concentrations that are small in aqueous solutions. The definiton of pH is in terms of base 10 logarithms. pH = - log[H*] where [H*] is the hydrogen ion concentration. a. If the hydrogen ion concentration in a solution is 7.26 x 10 mol L, the pH is b. If the pH of a solution is 3.607, the hydrogen ion concentration is mol L.

Here is ph of the molarity of butyl chloride (C,H,CI) in a reaction vessel during a certain chemical reaction. Use this graph to answer the questions in the table below. у 0.030- 0.0247 olo 0.020- Ar M 0.015- 0.010- 0.005- 500 1000 1500 2000 2500 3000 seconds created x10 Is C,H,Cl being created or destroyed by the chemical destroyed reaction? neither created nor destroyed If C,H,Cl is being created or destroyed, what is the rate at which it is being created or destroyed 1200 seconds after the reaction starts? Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility

Chapter #9, Question #5: The principal anion and cation of Lake Huron, one of the Great Lakes in North America, are, respectively, hydrogen carbonate and calcium.  The concentration of the former is approximately 1.05 mmol L-1.  Calculate the mass of solid calcium carbonate that would remain if 250 mL of Lake Huron water is evaporated to dryness.

Why does  acid rain fall far from the source?  Show the equations  leading  from the combustion  of coal to the formation of acid rain

Name the two ways that remove the most carbon dioxide from the atmosphere.  Carbon dioxide combines with water to form a single product.  Name that product (label it as product #1).  That product #1 reacts with water to produce hydronium ion and product #2.  Name product #2.  BRIEFLY: How do these two reactions affect ocean pH?  BRIEFLY: how does ocean pH affect ocean-dwelling organisms?

1. Nitrogen in an industrial wastewater is primarily in the form of ammonia (NH3) and ammonium (NH4+) ions. The acid/base equilibrium reaction for ammonia and ammonium is given as: NH4+ → H+ + NH3 Ką = 10-9.26 The total nitrogen concentration in wastewater is given as 2 x 10-3 moles/L (or 28 mg N/L), a. Calculate the concentration of ammonia (NH3) and ammonium (NH4*) ions at pH 10. NH3: moles/L NH4*: moles/L Check b. In ammonia stripping, nitrogen is removed from wastewater by volatilization of NH3. Would ammonia stripping be more effective above or below pH 9? Briefly explain your reasoning.

Organic molecules often have polar covalent bonds. How does this provide opportunities for chemical reactions to occur at a specific site in a molecule? How could competitive reactions be controlled by adjusting the acidity/basicity of the chemical system?

10. True or False (use your periodic table/data sheet when appropriate) а. The cation formed from a neutral atom is always smaller than the neutral atom. b. The Celsius temperature of a gas is directly proportional to the average kinetic energy of the gas particles. The H-Br bond is more polar than the H F bond. NO, is the conjugate acid of the base, HNO2. A postulate of “The Kinetic Molecular Theory of Gases" is that gas particles do not attract each other. A solution with a pOH of 7.5 has a greater concentration of hydrogen ions than a solution with a pOH of 5.6. As the volume of a gas decreases, the pressure the gas exerts on its container increases (assume n & T remain constant). Real Gases approach Ideal Gas behavior at low Pressures and low temperatures. A solution with a pH of 6.3 has a greater concentration of hydroxide ions than a solution with a pH of 4.5. HCO3 (aq) is an amphiprotic substance. Vapor is any substance in the gaseous state that is usually a liquid or solid.…

Discuss and give a reason for the pollution problem associated with acid rain?

The pH of a solution is 2.45. What is the molar concentration of hydronium ions in the solution?  The answer should be to the proper number of significant digits.

When coal is burned, it produces ______  which combines with _______  to form _________, SO2. This SO2 then reacts with_______  , which_______  the pH of normal rainwater. This acidic rainwater is also called_______  . It is responsible for dissolving valuable________  nutrients, but also converts normally harmless________  compounds into very toxic varieties. Fill in the Blank!

(b) What will happen if acetic acid (HC2H3O2) is added to water? O An equilibrium will form between its molecular form, HC2H3O2, and the species formed by removal of water, C2H2O. O An equilibrium will form between its molecular form, HC2H3O2, and the species formed by addition of water, H3C2H3O3. O Acetic acid is a strong acid and will ionize completely. O An equilibrium will form between its molecular form, HC2H3O2, and the ionized form, H* and C2H3O2. O Acetic acid is a weak acid and will not ionize completely. Hint Attempts: 1 of 15 used Submit Save for Later TIng I aI system, SOme of UIS energy Can De transieIICU To une su t ST國 ост 15 MacBook Air

A 0.11 M solution of weak acid, HA, has a pH of 4.24.  Write the dissociation reaction of the acid in water.  Write the acid dissociation constant expression.  Given the table below, what is the most probable identity of the acid?  Acid  K​a Hypochlorous acid  3.0 x 10⁻⁸ Nitrous acid  7.1 x 10⁻⁴ Hydrogen cyanide  6.2 x 10⁻10 Propionic acid  1.3 x 10⁻⁵

A)When working in the lab, you are measuring the pH of a system. The pH meter reads 4.34. What is the concentration of [H3O+] in solution? B)You have created a solution of NaOH by dissolving NaOH in water. You determine that the [OH-] concentration in solution is 4.37 x 10-9. What is the pOH of the solution? C)What is the pH of a solution containing an [H3O+] = 9.67 x 10-3?

A 500 mL sample of waste water contains 42.65 ug of mercury, Hg. If the density of the sample is 1.073 g/mL. Calculate the concentration of mercury in parts per billion (ppb) 1. O85.3 2. O48.6 3. O79.5 4. O5.03 5. O34.6

Formic acid, HCOOH, ionizes in water according to the following equation. The equilibrium constant is K = 1.8 × 10–4. $$HCOOH(aq)+H2​O(l)HCOO−(aq)+H3​O+(aq) Calculate the equilibrium concentration of H3O+ in a 0.985 M solution.     M

If the Hydrogen ion concentration [H+] of certain slurry sample of soil with water is 3.5 x 10-6 M, what is the pH of the soil sample? Is the soil acidic, neutral or alkaline. Write your computation in the reply section. Highlight your final answer.

Row 1: Your answer is incorrect. • Row 2: Your answer is incorrect. Row 4: Your answer is incorrect. The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that NH, is a weak base. 1.3 mol of HI is added to 1.0 L of a 1.3MNH, solution. 0.22 mol of HNO, is added to 1.0 1. of a solution that is 1.1M in both NH, and NH Br. ✔ acids: NH, H,O bases: 11,0, NHL, other: I acids: NH H bases: NH, other: NO, Br a S da X 0.0.

Consider the reaction below. Co(H,O),* (aq) + 4 Cl¯ (aq) = COC1," (aq) + 6 H,O (1I) The equilibrium constant expression (K) of the reaction does not include the concentration of H,O even though the reaction produces six moles of water. Explain.

What three strategies that can be used to protect coral reefs from ocean acidification?

Write the chemical formual of acid: Cl-(aq0+HS04-(aq)  HCI(AQ+SO42-(aq)

com/courses/22672/quiz2es/68142/laRU e G My Policy Details O Strongnet l-Notes... P PowerSchool P PowerTeacher IEP Anywhere Claim Status Form Question 2 23.79g of solid sodium hydroxide, NaOH is added to 87.5 ml of a 1.97M solution of iron(Il) chloride, FeC13. This causes iron(III) hydroxide to precipitate out of solution. The reaction is shown below. Determine the limiting reagent then find the mass of the iron(III) hydroxide precipitate. 3NAOH(s) + FeCl3 (aq) - Fe(OH);(s) + 3NaCl(aq) Question 3 The mixture of which two solutions will result in a precipitate being formed? O LIOH(aq) + Na2SO4(aq) O BaCl2(aq) + NAOH(aq) O Pb(NO3)2(aq) + NaC2H3O2(aq) O Al(NO3)2(aq) + BaCl,(aq) O Al(NO3)2(aq) + LIOH(aq) Question 4 Solid H,S is added to 280 ml of a 0.450M CaCl2 solution until no more Cas is formed (see reaction below). At the end of the experiment 5.50 g of CaS is formed. What is the percent yield for the reaction? Molar Masses: Ca (40.08), S (32.07), CI (35.45) CaCl2 (aq) + H,S(s) 2HC(aq)…