HA, a weak acid with a Ka of 4.0x10, also forms the ion HA,. The reaction is :- НА (aq) +A (aq) HA2 (aq) with an equilibrium constant of 4.0x102. Calculate the equilibrium concentrations of [HA], [H*], [A],[HA2] and calculate the pH of this solution if the initial concentration of HA (aq) is 1.0 M. [HA]= [H*]. [A].. [HA, ]=. pH

HA, a weak acid with a Ka of 4.0x10, also forms the ion HA,. The reaction is :- НА (aq) +A (aq) HA2 (aq) with an equilibrium constant of 4.0x102. Calculate the equilibrium concentrations of [HA], [H], [A],[HA2] and calculate the pH of this solution if the initial concentration of HA (aq) is 1.0 M. [HA]= [H]. [A].. [HA, ]=. pH

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 40QRT: Leucine is an amino acid with this Lewis structure: Write the Lewis structure for the zwitterion...

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Leucine is an amino acid with this Lewis structure: Write the Lewis structure for the zwitterion form of leucine.
Let's assume that there is 400 μatm of pCO2 in our atmosphere. Assumingthere is nothing else in the water coming from the atmosphere, what is the pH of rainwater in equilibrium with this atmospheric CO2?Assume KH = 5.4x10-2 mol kg-1 atm-1. KC1 = 3.47×10-7 mol2 kg-2 for freshwater rain.Hint: Because rainwater is acidic, it has little/no alkalinity, thus the (H+] = Alk = [HCO3-]
A laboratory technician wants to determine the aspirin content of a headache pill by acid-base titration. Aspirin has a Ka of 3.0 x 10−4. If the pill is dissolved in water to give a solution about 0.015 M, what is the pH of this solution? (Neglect dilution effects.) If the solution in the problem above is then titrated against KOH solution, what will be the pH at the stoichiometric point.
An organic acid(HA) has a molecular weight of 100. g mol^-1, a Kow=5.6 and a Ka=2.7x10^-2. If originally 2.0g of the acid is dissolved in 100mL of octanol (there is no dissociation in octanol), which is then placed in contact with 100mL of water, what will be the pH of the water? (consider the equilibrium processes to be sequential and unrelated chemically)
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Determine the pH of a 0.650 M solution of magnesium nitrite, Mg(NO2)2 at 25 °C. A solution containing 7.50 g of this salt is diluted with water until it reaches a pH of 8.18.What is its final volume? Give one example of a salt whose solution is expected to be acidic and briefly explain why. Give one example of a salt whose solution is expected to be basic and briefly explain why. You cannot reuse the compound in a) and b) to answer c) and d).
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8. (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 8.8 x 10−12. What is the pH of a 0.022 M solution of A−(aq)? The temperature is 25 ◦C. (b) For the reaction A(g) =A(l), the equilibrium constant is 0.666 at 25.0 ◦C and 0.222 at 75.0 ◦C. Making the approximation that the entropy and enthalpy changes of this reaction do not change with temperature, at what temperature will the equilibrium constant be equal to 0.777?

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