The Pka of acrylic acid is 4.25.
What is the concentration of H3O+ in .190M, C3H3O2- in .190M, HC3H3O2 in .19M, OH- in .19M, and the % dissociation in .05M acrylic acid
The pH in .19M of acrylic acid is 2.49
Could someone please show me the steps to this? Thanks
The Pka of acrylic acid is 4.25. What is the concentration of H3O+ in .190M, C3H3O2-...
what is the hydronium ion concentration [H3O+] and the ph of a 0.5M acetic acid solution with Ka=1.8x10^-5? The equation for the dissociation of acetic acid is: CH3CO2H(aq) + H2O(l) = H3O + (aq) + CH3CO2-(aq)
Base/Acid Ratios in Buffers Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of Ka, pKa=?logKa The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: pH=pKa+log[base][acid] Notice that the pH of a buffer has a value close to the pKa of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. Part A Acetic acid has a Ka of 1.8
The pKa for acetic acid is 4.76. If the concentration of salt in 2mmol/L and that of acetic acid is 6mmol/L, what is the expected pH? Answer options: (A) 4.43 ; (B) 6.19 ; (C) 104 ; (D) 56 I keep getting pH=4.23 which is not one of the answer options. Can someone walk me through this Q?
In a solution of the weak acid DNP (pKa 4.11) in water, [H3O+] = 9.4 x 10^-4 M and DNX, the conjugate base, has a concentration of 0.00180 M. A.) What is the concentration of DNP in the above solution? B.) What is the pH of the solution?
4.13 Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of Ka, pKa=−logKa The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: pH=pKa+log[base][acid] Notice that the pH of a buffer has a value close to the pKa of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. Part B How many grams of dry NH4Cl need to be added to 2.10 L of a 0.400 M solution of ammonia,...
What is the pKa of a weak acid called dihydrogen arsenate H2AsO4-1 if a 0.001M aqueous solution has a pH of 5? This is for my BioChem class, the answer is supposed to be 7, can someone please very distinctly write out the steps? Also, I'm not allowed a calculator so please tell me how you know what the number would be when converting logs and exponents. Thank you!
could someone please show me step by step how to solve this? What is the [H3O*] if [OH-] is 5.0 x 10-8 M?
3) The pKa of chloroacetic acid is 2.9; the Ka is 1.4 x 103. Complete the following table for solutions of chloroacetic acid in water: H-O H CI H20 OH Concentration (M) [H3O*] pH 0.40 0.60 0.80 1.00 1.20
What is the pKa of a weak acid called dihydrogen arsenate H2AsO4-1 if a 0.001M aqueous solution has a pH of 5? This is for my BioChem class, the answer is supposed to be 7, can someone please very distinctly write out the steps? Also, I'm not allowed a calculator so please tell me how you know what the number would be when converting logs and exponents. Thank you!
For the solution of 0.020 moles of formic acid (HCOOH) and 0.010 moles of sodium formate (pka = 3.7545 at 25 C) obtain: a) the reactions involved in the process b) the derivation of the Henderson-Hasselbalch expression from equilibrium for the dissolution of the formic acid. c) the pH of the system and the pOH d) the concentration of H3O+ e) the concentration of OH- of the system