1.0L of aqueous solution in which [H2CO3]=[HCO3^-]=0.10M and has [H^+]=4.2E-7. What is the concentration of [H^+] ofter 0.005 mole of NaOH has been added? H2CO3 ==> H^+ + HCO3^- k1 = (H^+)(HCO3^-)/(H2CO3) I don't know if you are
Complete the following equilibrium reactions that are pertinent to an aqueous solution of Ag2CO3. Physical states, s, l, g, and aq, are optional. So far I worked it out to be: Ag2CO3(s) 2Ag^+ + CO3^(2-) H2CO3(aq) + H2O(l) H3O^(1+)
1. An aqueous solution contains 0.154 M ascorbic acid (H2C6H6O6) and 0.196 M hydrobromic acid. Calculate the ascorbate (C6H6O62-) ion concentration in this solution. Can you explain how to do this please? thank you. Also if you
I am having a bit of difficulty getting the net equation and the net ionic equation and the net ionic equation. I think I have the balance equation right. Thanks in advance for any help. For the acid base neutralization reaction
An aqueous solution of carbonic acid reacts to reach equilibrium as described below. H2CO3(aq) + H2O(l) HCO3^-(aq) + H3O^+(aq) The solution contains the following solute concentrations: Carbonic Acid: 3.3*10^-2 mol/L HCO3^-:
Calculate [CO32- ] in a 0.019 M solution of CO2 in water (H2CO3). If all the CO32- in this solution comes from the reaction shown below, what percentage of the H+ ions in the solution is a result of the dissociation of HCO3‾?
Calculate the pH of an aqueous solution of 0.15 M potassium carbonate. I know that pH = -log(H30+) but I am not sure how to start this problem. Chemistry(Please help) - DrBob222, Saturday, April 14, 2012 at 11:09pm Hydrolyze the