source : yahoo.com
Calculate the equilibrium concentration of H3O+ in a 0.20M solution of oxalic acid.?
H2C2O4 + H2O <—–> H3O+ + HC2O4-
5.9 x 10^-2 = x^2 / 0.20-x
0.0118 – 5.9 x 10^-2 x = x^2
x^2 + 5.9 x 10^-2 x – 0.0118=0
x = – 5.9 x 10^-2 + sq.rt ( 0.00348 + 0.0472)/2 = 0.083
HC2O4- + H2O <—–> H3O+ + C2O42-
6.4 x 10^-5 = ( 0.083+x)(x) / 0.083-x
solve for x by quadratic formula
[H3O+]= x + 0.083
PDF Microsoft Word – acid-base.htm | CHEMICAL EQUILIBRIA–ACID/BASE – The concentration of OH- in solution will be equal to the concentration of the strong base. Alkaline Buffers Suppose you have a alkaline buffer consisting of 0.20 M aqueous ammonia (NH3) The equilibrium constant will be calculated in a similar manner as for alkaline salts, using the Kw of…Note that the approximate concentration of the KMnO4 solution is already known to be about 0.01 M. In What should be the concentration of the oxalic acid for 25.00 mL of it to react completely with 25 mL of 0.01 M we can calculate the approximate number of moles of KMnO4 to use in the titration asMany household cleaning products contain oxalic acid, H2C2O4, a diprotic acid with the following dissociation constants: Ka1: 5.9×10-2, Ka1: 6.4×10-5 Calculate the equilibrium concentration of H3O+ in a 0.20M solution of oxalic acid.
Exp of Oxalic Acid | Molar Concentration | Titration – Solution Calculate the concentrations and substitute them into an expression and compute the "experimental concentration quotient" or "Q". 2. Assume that the analysis of another equilibrium mixture of the system from above shows that the equilibrium concentration of PCl5 is 0.012 mol/L…Secondly for this common type of equilibrium when concentrations are around the Ka you get a half-and-half situation. You can see from your equilibrium The total acid concentration instead is 0.2 M – in about the same ballpark. (I leave you to think qualitatively do you expect it to be more all less than…See below. If the concentration of the acid is 0.2 then we can find the H_3O^+ in total by using the two different K_a's. Also, I call Oxalic acid as Many household cleaning products contain oxalic acid, H2C2O4, a diprotic acid with the following dissociation constants: Ka1=5.9×10−2, Ka2=6.4×10−5.
Calculate the equilibrium concentration of H3O+… | Yahoo Answers – Oxalic acid (OA-H) is diprotic so to be absolutely accurate, you should consider both pKa1 and pKa2. However, usually the difference between pKa1 and We can easily fix this problem by acknowledging the existence of these ions in pure water, and calculating the true final concentration of H [math]…To calculate the pOH of a solution you need to know the concentration of the hydroxide ion in moles per liter (molarity). where "Ka" is the equilibrium constant for the ionization of the acid. The Kb for an acid is calculated from the pKb by performing the reverse of the mathematical operation used to…The concentration of a solution can be calculated using: the amount of dissolved solute in moles, mol. Calculate the concentration of the sodium hydroxide solution formed. 100 cm3 of dilute hydrochloric acid contains 0.02 mol of dissolved hydrogen chloride.