19. Scientists have become concerned about the effects that increased carbon dioxide levels in the atmosphere will have on our oceans. Given the equilibrium equations below, what chemical changes would you expect to see in the ocean as atmospheric carbon dioxide levels rise? (4) CO2(g) + H2O(1) = H2CO3(aq) H2CO3(aq) = H+ + HCO3(aq) (aq) HCO3(aq) = H+ (aq) + CO2 (aq)

19. Scientists have become concerned about the effects that increased carbon dioxide levels in the atmosphere will have on our oceans. Given the equilibrium equations below, what chemical changes would you expect to see in the ocean as atmospheric carbon dioxide levels rise? (4) CO2(g) + H2O(1) = H2CO3(aq) H2CO3(aq) = H+ + HCO3(aq) (aq) HCO3(aq) = H+ (aq) + CO2 (aq)

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter13: Fundamental Equilibrium Concepts

Section: Chapter Questions

Problem 46E: Acetic acid is a weak acid that reacts with water according to this equation:...

See similar textbooks

Similar questions

Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.
1. Once a chemical equilibrium has been established, only the forward reaction occurs. only the reverse reaction occurs. the forward and reverse reactions occur at an equal rate. the forward and reverse reactions stop.
Complete each of these reactions by filling in the blanks. Predict whether each reaction is product-favored or reactant-favored, and explain your reasoning. (a) _________ (aq) + Br(aq) NH3(aq) + HBr(aq) (b) CH3COOH(aq) + CN(aq) ________ (aq) + HCN(aq) (c) ________ (aq)+H2O () NH3(aq) + OH(aq)
Complete each of these reactions by filling in the blanks. Predict whether each reaction is product-favored or reactant-favored, and explain your reasoning. (a) (aq)+HSO4(aq)HCN(aq)+SO42(aq) (b) H2S (aq) + H2O() H3O+(aq) + _____ (aq) (c) H(aq) + H2O() OH(aq) +_____ (g)
For an acid-base reaction, what is the reacting species (the ion or molecule that appears in the chemical equation) in the following bases? (a) barium hydroxide (b) trimethylamine (CH3)3N (c) aniline, C6H5NH2 (d) sodium hydroxide
Acetic acid is a weak acid that reacts with water according to this equation: CH3CO2H(aq)+H2O(aq)H3O+(aq)+CH3CO2(aq) Will any of the following increase the percent of acetic acid that reacts and produces CH3CO2 ion? (a) Addition of HCI (b) Addition of NaOH (c) Addition of NaCH3CO2
When a mixture of hydrogen and bromine is maintained at normal atmospheric pressure and heated above 200. °C in a closed container, the hydrogen and bromine react to form hydrogen bromide and a gas-phase equilibrium is established. Write a balanced chemical equation for the equilibrium reaction. Use bond enthalpies from Table 6.2 ( Sec. 6-6b) to estimate the enthalpy change for the reaction. Based on your answers to parts (a) and (b), which is more important in determining the position of this equilibrium, the entropy effect or the energy effect? In which direction will the equilibrium shift as the temperature increases above 200. °C? Explain. Suppose that the pressure were increased to triple its initial value. In which direction would the equilibrium shift? Why is the equilibrium not established at room temperature?
. Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
Equal amounts of two acidsHCl and HCO2H (formic acid)are placed in aqueous solution. When equilibrium has been achieved, the HCl solution has a much greater electrical conductivity than the HCO2H solution. Which reaction is more product-favored at equilibrium? HCl(aq)+H2O(l)H3O+(aq)+Cl-(aq) HCO2H(aq)+H2O(l)H3O+(aq)+HCO2-(aq)
What are the products of each of the following acid-base reactions? Indicate the acid and its conjugate base and the base and its conjugate acid. (a) HCIO4 + H2O (b) NH4 ++ H2O (c) HCO3 + OH