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Give the pH of 0.005 M C6H5O- (aq) at 298 K of the Ka for C6H5OH at the given T is 1.0 x 10-10
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- HF(g) + H,O(1) H,0*(aq)+ F"(aq) K = 1.1 x 10-3 F (aq) + HF(g) HF;(ag) K= 2.6 x 10- a. Is fluoride in pH 7.00 drinking water more likely to be present as F"(aq) or HF2 (aq)? O HF2 (aq) O F(aq) b. What is the equilibrium constant for this equilibrium? Number 2 HF(g) + H,0(1) H,0*(aq) + HF, (aq) c. What are the pH and equilibrium concentration of HF2" in a 0.150 M solution of HF? (HF, - Number Number pH = M Check Answer View SolutionFor H2SO4, Ka,1 is very large and pKa.2 = 1.96 at 25 °C. For 0.00105 mol L- H2SO4(aq) at 25 °C, calculate: (a) the equilibrium concentration of the singly-ionized form, HSO4 [HSO4 leq = Number mol L-1 (Enter a number accurate to 2 significant figures.) (b) the fraction, az, of H2SO4 that exists in the doubly-ionized form, SO22- a2= Number (Enter a number between 0 and 1, accurate to 2 significant figures.) (c) the pH pH = Number (Enter a number accurate to 2 decimal places.)hát is the équilibrium constant for the following reaction
- Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HCIO(aq) + H,O(1)=H;0*(aq) + CIO"(aq) K =Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. NH3 (aq) + H2O(1) =NH,* (aq) + OH(aq) K=-Consider the following aqueous chemical equilibrium of benzoic acid, a weak acid: C6H5COOH(aq) + H2O(l) is in equilibrium with H3O+(aq) + C6H5COO-(aq) a. The addition of H3O+(aq) to the chemical equilibrium will have what effect on the amount (moles) of C6H5COO-(aq) in the system? b. Addition of OH-(aq) to the chemical equilibrium will have what effect on the amount (moles) of C6H5COOH(aq) in the system? c. Removal of C6H5COO-(aq) from the chemical equilibrium will have what effect on the amount of (moles) H3O+(aq) in the system? d. Increasing the pH of the solution will have what effect on the amount (moles) of C6H5COOH(aq) in the system?
- An aqueous solution of acetic acid is found to have the following equilibrium concentrations at 25°C: [CH3COOH] = 1.65 x 10-2 M; [H+] = 5.44 x 10-4 M; and [CH3COO-] = 5.44x10-4 M. Calculate the equilibrium constant Kc for the ionization of acetic acid at 25°C. The reaction is CH3COOH(aq) ↔ H+(aq) + CH3COO-(aq)Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HCN (aq) + OH" (aq) CN" (aq) + H,0 (1) K =Given that K, for formic acid is, HCHO2 is 1.7 x10 and that for acetic acid, HC,H;0, is 1.8 x105, calculate K, for CHO,", and C,H3O2?
- The following equilibrium constants have been determined for hydrosulfuric acid at 25oC ; H2S(aq) ↔ H+(aq) + HS-(aq) Kc’ = 9.5x10-8 HS-(aq) ↔ H+(aq) + S2-(aq) Kc’’ = 1.0x10-19 Calculate the equilibrium constant Kc for the following reaction at the same temperature. H2S(aq) ↔ 2H+(aq) + S2-(aq) 8x10-18 5x10-27 4x10-16 8x10-25 9x10-24Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HNO,(aq) + H2O(1)=H;0*(aq) + NO,"(aq) K =formic acid (0.24mol) is placed in 2L of water and undergoes the following reaction:HCHO2(aq)+H2O(l) - H3O+(aq)+ CHO2-(aq) Kc= 2.1*10-4. (a) use your solver to calculate the equilibrium concentration of hydronim ion in this solution? (b) Approximate the answer to this problem by assuming x is small. show your work.