A solution of 0.2 M dehydroascorbate and 0.2 M ascorbate (E0+ = +0.06 V) was mixed...
412 tential of a Fe electrode in a solution of 0.05 M FeCh pH 2.0, E0-0.036 V at 25 °C. 412 tential of a Fe electrode in a solution of 0.05 M FeCh pH 2.0, E0-0.036 V at 25 °C.
A solution of 0.1 L of 0.3 M Ca(NO3)2 is mixed with 0.2 L of 0.06 M NaF. Calculate the reaction quotient Qsp. Does calcium fluoride precipitate? (Ksp (CaF2) = 3.2×10–11). (A) Qsp = 1.6×10–4; no precipitate. (B) Qsp = 1.6×10–4; a precipitate will form. (C) Qsp = 3.2×10–11; no precipitate. (D) Qsp = 3.2×10–11; a precipitate will form. (E) Qsp = 3.2×10–7; no precipitate.
. 100mL of a 0.2 M solution of NaOH is mixed with 150mL of a 0.3 M HCl solution. A neutralization reaction occurs: NaOH + HCl --> NaCl + H2O. What is the molarity of the molecules in the mixed solution after the reaction has reached completion?
Calculate pH of 0.2 M solution of Tartaric acid. Calculate the volume of 1 M solution of NaOH required to neutralize 20 mL of 0.2 M tartaric acid solution (final pH should be 7). (pKa's of Tartaric acid are 3.0 and 4.4). 3.
100 mL of a 0.2 M solution of NaOH is mixed with 150 mL of a 0.3 M HCl solution. A neutralization reaction occurs: NaOH + HCl —> NaCl + H2O. What is the molarity of the molecules in the mixed solution after the reaction has reached completion?
H aq H g anode An electrochemical cell consists of a H aq 1 .00 M H g) cat ode connected to a which e H concentration a ofa u er cons nu of a weak acid HA(0.116 M), mixed with its conjugate base, A (0.143 M). The measured cell voltage is E°ell 0.163 V at 25 °C, with PH2-1.00 atm at both electrodes. Calculate the pH in the buffer solution and the K of the weak acid. Ka H...
A 1.00 mL solution containing 0.400g BaCl2:2H2O is mixed with 50.00 mL of a solution containing 0.300 g NalO3. Determine the mass of Ba(103)2 formed. Ksp (Ba(103)2) = 1.6x10-9 Determine the saturation state of seawater (12) for calcite at pH 8.10 (current) and pH 7.80 (year 2100). The concentration of calcium is constant at 0.0103 M. The concentration of carbonate is 2.40x10-4M (pH 8.10) and 1.48x10-4M (pH 7.8). Ksp*(calcite) = 4.272x10-7 Calculate the activity coefficient of K+ in a 0.0500...
The titration of 50.00 mL solution of a 0.1 M OAc- with 0.2 M HCl. OAc- is a weak base. Ka for acetic acid = 1.75 * 10^-5. a) Calculate the pH of the 50.0 mL of 0.1 M OAc- solution before the addition of any HCl. b) Calculate the pH of the resulting solution after the addition of 5.0 mL of 0.2 M HCl to the 50.0 mL of 0.1 M OAc- solution. c) Calculate the pH of the resulting...
What is the pH of the solution when 0.2M HCl, 0.4M NaOH and 0.2 M HCN is mixed, assuming the volume is constant. (Ka(HCN)= 5x10-10)
A solution of 0.200 M KOH (17.6 mL) is mixed with 45.9 mL of 0.143 M HCl. Assuming that the final volume is the sum of the initial volumes, calculate: (a) the molarity of the K+ cation (b) the molarity of the Cl- anion (c) the pH of the final solution (d) the pOH of the final solution