For H2SO4, Ka,1 is very large and pKa,2 = 1.96 at 25 °C.
For 0.00189 mol L−1 H2SO4(aq) at 25 °C, calculate:
(a) the equilibrium concentration of the singly-ionized form, HSO4−
(b) the fraction, α2, of H2SO4 that exists in the doubly-ionized form, S
(c) the pH
For H2SO4, Ka,1 is very large and pKa,2 = 1.96 at 25 °C. For 0.00189 mol...
Hydroselenic acid, H2Se, is a diprotic acid with pKa,1 = 3.89 and pKa,2 = 11.01 at 25 °C. For 0.147 mol L−1 H2Se(aq) at 25 °C, calculate: (a) the fraction, α1, of H2Se that exists in the singly-ionized form, HSe− α1 = (Enter a number between 0 and 1, accurate to 2 significant figures.) (b) the equilibrium concentration of the doubly-ionized form, Se2− [Se2− ]eq = mol L−1 (Enter a number accurate to 2 significant figures.) (c)...
Question 6: (1 point) Selenous acid, H2SO3, is a diprotic acid with pKa,1 = 2.64 and pKa,2 = 8.26 at 25 °C. For 0.169 mol L-1 H2SeO3(aq) at 25 °C, calculate: (a) the fraction, at, of H2SeO3 that exists in the singly-ionized form, HSEO3- ay = (Enter a number between 0 and 1, accurate to 2 significant figures.) (b) the equilibrium concentration of the doubly-ionized form, Se032- [SeO32-leq = _ (Enter a number accurate to 2 significant figures.) mol L-1...
Given that pKa = 3.74 at 25 °C for HCOOH, what is the pH of 0.113 mol L−1 HCOONa(aq) at 25 °C? What is the equilibrium concentration of HCOOH?
1- Calculating [H+] for Pure Water: In a certain acidic solution at 25 ∘C, [H+] is 100 times greater than [OH −]. What is the value for [OH −] for the solution? In a certain acidic solution at 25 , [] is 100 times greater than [ ]. What is the value for [ ] for the solution? 1.0×10−8 M 1.0×10−7 M 1.0×10−6 M 1.0×10−2 M 1.0×10−9 M 2. ± Acid-Base Relationships in Water: Water ionizes by the equation H2O(l)⇌H+(aq)+OH−(aq)The...
Need help on questions 1-3 Henderson-Hasselbalch: pH=pka + Log( [base]/(acid] ) 1. The value of Ka of nitrous acid (HNO2) is 4.6 x 104 M. Calculate the pH and the concentration of [H3O+] in a 0.02M aqueous solution of HNO2(aq). 2. Label conjugate acid-base pairs: HNO2(aq) + H2O → H30* + NO2 (aq) 3. What will happen to the reaction equilibrium if we increase the pressure in the reaction vessel? H2(g) + 12(e) → 2 HI(g)
1) Ammonia, NH3, is a monoprotic base with pKb = 4.74 at 25 °C. For 0.121 mol L−1 NH3(aq) at 25 °C, calculate (a) the percent ionization of NH3; and (b) the pH of the solution. 2) Hydrazoic acid, HN3, is a monoprotic acid with pKa = 4.72 at 25 °C. For 0.121 mol L−1 HN3(aq) at 25 °C, calculate (a) the percent ionization of HN3; and (b) the pH of the solution.
The pKa of NH4+ is 9.25 at 25°C. The rate constant at 25°C for the reaction of NH4+ and OH− to form aqueous NH3 is 4.0 ✕ 1010 dm3 mol−1 s−1. Calculate the rate constant for proton transfer to NH3. s−1 What relaxation time would be observed if a temperature jump were applied to a solution of 0.31 mol dm−3 NH3(aq) at 25°C?
The following equation represents the dissociation of propionic acid in water. HC3H502(aq) + H20(1) = H30+(aq) + C3H502 (aq) The value for the acid-dissociation constant for propionic acid (HC3H502) is 1.3x10-5 at 25°C. Calculate the hydronium ion concentration present in a propionic acid solution that has the following equilibrium concentrations. 3.24x10-2 mol/L HC3H502 3.06x10-4 mol/L for propionic acid's conjugate base, C3H5027 The general form of the acid-dissociation constant is Ka = [H30'A ], where Ka is the acid-dissociation constant, [HA]...
we consider an ammonium solution with a concentration of 0.05 mol / L 1) Write the equation of acidic basic equilibrium between NH4 + ammonium ions and water 2) Express literally the acidity constant KA of this equation. 3) Make the progress table showing the progress of the reaction x and give the expression of the acidity constant KA as a function of x. 4) Establish the second degree equation to determine the concentration of H3O + ions 5) Calculate...
Which one of the following species is amphiprotic? Select one: PO43–(aq) HCl(g) HSO4–(aq) Cl–(aq) For the system NH2OH + CH3NH3+⇌ CH3NH2 + NH3OH+ 95% 95 % 5 % 5 % the state of equilibrium in the system is described by the percentages given. Which of the species is the strongest base in the system? Select one: NH2OH CH3NH3+ CH3NH2 NH3OH+ An aqueous solution at 25.0 oC has an H3O+ concentration of 4.0 × 10–2 mol L–1. What is the OH–...