The reaction HCO3 CO2+ H is an important part of the carbonate system, and is governed by the equilibrium expression K [co¥ ][H*] HCO a) The average pH of surface seawater is predicted to decrease to 7.8 by the year 2100. Calculate the comesponding (H) for this pet (give your answer to 3 significant figures include appropriate units) b) If the bicarbonate ion concentration increases to 3.1 x 103 molkg by the same date, what would be the concentration of CO2 (to two significant figures), assuming that K2 is not changed? c) Briefly describe one adverse effect that a decrease in CO2 is likely to have (can be ecological or economic) ≈ 109

The reaction HCO3 CO2+ H is an important part of the carbonate system, and is governed by the equilibrium expression K [co¥ ][H*] HCO a) The average pH of surface seawater is predicted to decrease to 7.8 by the year 2100. Calculate the comesponding (H) for this pet (give your answer to 3 significant figures include appropriate units) b) If the bicarbonate ion concentration increases to 3.1 x 103 molkg by the same date, what would be the concentration of CO2 (to two significant figures), assuming that K2 is not changed? c) Briefly describe one adverse effect that a decrease in CO2 is likely to have (can be ecological or economic) ≈ 109

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 87SCQ: Most naturally occurring acids are weak acids. Lactic acid is one example....

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The pH scale for acidity is defined by pH – log10 H*| where |H*| is the concentration of hydrogen ions measured in moles per liter (M). (A) The pH of Drano is 13.3. Calculate the concentration of hydrogen ions in moles per liter (M). [H*] = M (B) The pH of rain water is 5.5. Calculate the concentration of hydrogen ions in moles per liter (M). [H*] = M
The pH scale for acidity is defined by pH log H| where H"| is the concentration of hydrogen ions measured in moles per liter (M). (A) The pH of Drano is 13.3. Calculate the concentration of hydrogen ions in moles per liter (M). Note: You may have to type in a lot of zeros. For example, an answer could be something like this 0.000000000000123. Or you can type your answer in scientific notation, such as 1.23*10-13 [H*] = (B) The pH of lemon juice is 2.0. Calculate the concentration of hydrogen ions in moles Niter (M). per [H*] =
Consider the following chemical equilibrium for the weak base CN in water: CN- (aq) + H₂O(1) = HCN (aq) + OH(aq). Which of the following statements is correct when more water is evaporated from system? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b C d pH will go up; [OH-] will go up; net amount of OH will go up pH will go down; [OH-]will go up; net amount of OH will go down pH will go down; [OH-]will go down; net amount of OH will go down pH will go up; [OH-] will go up; net amount of OH will go down
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.
COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…
Indicate how the concentration of each aqueous species in the chemical equation changes to reestablish equilibrium after changing the concentration of a reactant or product. Also indicate how the pH changes. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration. HC\(aq)+H,O()=CN (aq)+H,0*(aq) pH after the concentration of HCN is increased after the concentration of CN is decreased Answer Bank careers privacy poliy thelp 口 )
5) Find the concentration of H30*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka= 1.38 x 10*. 6) Write the equilibrium expression for the ionization of HOI, and calculate the concentration of HOI(aq) in solution if [H3O*]=2.3 x 10° M and pKa = 10.7 at 25°C.
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?
What is the equilibrium constant expression (Ka) for the acid dissociation of hypochlorous acid? HClO(aq)+H 2 O(l) H 3 O^ + (aq)+ClO-(aq) . a) Ka=[H 3 O^ + ]+[ClO-]-[HClO]; b) Ka=([HClOl[H 2 O]/([H 3 O^ + ][ClO-]); c) Ka=([H 3 O^ + ][ClO-])/([HClO][H 2 O]; d) Ka=(IH 3 O^ + ][ClO-])/[HClO]
The pH reading of a sample of each substance is given. Calculate the hydrogen ion concentration of the substance. (Give your answers in scientific notation, correct to one decimal place.) (a) Vinegar: pH = 3 %3D [H+] = x 10 M (b) Crackers: pH = 7.2 %3D [H+] = x 10 M (p ツ

3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.
6. (i) Define pH in words. The strong acid HClahas a pH value of 1, use the following equation for a strong acid: H+, + and convert the following expression to deduce the hydrogen ion concentration: pH = -log10 [H*] (ii) Use the above expression to deduce the pH of HCL (ag) given the concentration of the acid to be 4.5 mol/dm3 pH =