Part A Water ionizes by the equation H2O(1) =H (ag) + OH (ag) The extent of the reaction is small in pure water and dilute aqueous solutions. This reaction creates the following relationship between [H+] and [OH ]: What is the H+ concentration for an aqueous solution with pOH = 3.10 at 25 °C? Express your answer to two significant figures and include the appropriate units. Kw = [H*][OH ] • View Available Hint(s) Keep in mind that, like all equilibrium constants, the value of K, changes with temperature. HÀ ? [H*] = Value Units Submit Part B Arrange the following aqueous solutions, all at 25 °C, in order of decreasing acidity. Rank from most acidic to most basic. To rank items as equivalent, overlap them. • View Available Hint(s)

Part A Water ionizes by the equation H2O(1) =H (ag) + OH (ag) The extent of the reaction is small in pure water and dilute aqueous solutions. This reaction creates the following relationship between [H+] and [OH ]: What is the H+ concentration for an aqueous solution with pOH = 3.10 at 25 °C? Express your answer to two significant figures and include the appropriate units. Kw = [H][OH ] • View Available Hint(s) Keep in mind that, like all equilibrium constants, the value of K, changes with temperature. HÀ ? [H] = Value Units Submit Part B Arrange the following aqueous solutions, all at 25 °C, in order of decreasing acidity. Rank from most acidic to most basic. To rank items as equivalent, overlap them. • View Available Hint(s)

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

2. Consider the following ions: sulfate (SO, 2), acetate (C,H,O, '),hydrogen carbonate(HCO, '), which of these ions can be considered amphoteric? Write a series of equations to justify your answer. [3K]
Calculate the value of Δ?∘rxnΔGrxn∘ for the following reaction at 278 K. Ka = 2.9 × 10–8 and assume Ka does not change significantly with temperature. HClO(aq) + H2O(l) <--> ClO-(aq) + H3O+(aq)
At 25°C, Keq = 4.8 x 10-6 for the balanced decomposition reaction of 2 moles of ICI. 2ICI(g) = 1₂(g) + Cl₂(g) Calculate Keq at 25°C for the formation of 2 moles of ICI. Ⓒ 9.6 x 106 Ⓒ4.8x 10° 4.8 x 10° 2.1 x 105
NH4NO3 dissolves readily in water even though the dissolution is endothermic by 26.4 kJ/mol. Why is the process spontaneous? Increase in enthalpy upon dissolution of this strong electrolyte. Increase in disorder upon dissolution of this strong electrolyte. The vapor pressure of the water decreases upon addition of the solute. Decrease in enthalpy upon addition of the solute.
Provide all the related knowledge which can generates from the given information, please 2. Consider the following information: + H₂O (1) OH (aq) R = k[CH3COOH (aq)] loo Ka 1.8 x 10-5 Oe (aq) HO* (aq) ΔΗ < 0
Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq)+NaHCO3(aq)→NaCl(aq)+H2O(l)+CO2(g) The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 200.mL of a 0.089M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this much HCl? Be sure your answer has the correct number of significant digits.
What is AG° (in kJ/mol) for the autoionization of water at 25°C? R = 8.314462 J/K-mol IMPORTANT: When entering your answer: • Enter the number only (no units) • Do not leave any spaces • Include the sign if your answer is negative (not necessary for positive values) • Use a leading zero before the decimal when necessary Report your number to 1 decimal place (regardless of the significant figures) • Correctly round your answer to the 1st decimal place (margin of allowed error is only ± 0.1, so always use un-rounded numbers in your calculations). If the last digits are zeros they will not display once you click away, but the answer will still be marked correct. Examples: 12.3 or -0.4
Part b For the reaction given in Part A, how much heat is absorbed when 2.60 mol of A reacts? And part c said At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium?
Calculate ArH for the following reaction: CaO(s)+CO2(g)→CaCO3(s) Use the following reactions and given >ArH"s Ca(s)+CO2(g)+1/202(g) →CaCO3(s), ArH= -812.8 kJmol-1 2Ca(s)+02(g) →2CaO(s), ArH= -1269.8 kJmol-1 ArH=-177.9 kJ mol-1 ArH= 177.9 kJmol-1 ArH=327.9 kJmol-1 ArH=-327.9 kJmol-1
Given the thermodynamic properties below, determine the standard enthalpy change, ∆H˚, for the dissolution of calcium hydroxide. Give your answer to one decimal place in kJ/mol. 1 Ca(OH)2 (s) ⇌ Ca2+ (aq) + 2 OH– (aq)
The following reaction has a AG° value of +8.43 kJ/mol at 25 °C. HA(aq) + H20(1) =H;O*(aq) + A (aq) Calculate the KA for the acid HA.
The Gibbs energy for a reaction Mg(s) + H₂O(g) → MgO(s) + H₂(g) at a particular temperature is AG = -100.0 kJ/mol. At the same time under the sa conditions, A,G° = +341 kJ/mol. Which of the following statements is true? The reaction is at equilibrium and P(H₂O) = P(H₂). The reaction proceeds in the reverse direction to produce more H₂O(g). The reaction proceeds in the forward direction to produce more H₂(g). The reaction is at equilibrium and P(H₂O) > P(H₂). The reaction is at equilibrium and P(H₂O) < P(H2).