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Calculate the [OH (aq)] in limes which have a [H3O*(aq)] of 1.3 x 10 mol/L
Calculate the concentration of OH- in a solution that contains 3.9 × 10-4 mol L-1 H3O+ at 25 °C. Also identify the solution as acidic, basic, or neutral. Group of answer choices 2.7 × 10-2 mol L-1, acidic 2.7 × 10-2 mol L-1, basic 2.6 × 10-11 mol L-1, basic 2.6 × 10-11 mol L-1, acidic 3.9 × 10-4 mol L-1, neutral
Propionic acid has an acid-ionization constant of 1.3 × 10-5. C3H5O2H(aq) + H2O(l) ⇄ H3O+(aq) + C3H5O2-(aq) What is the pH of a 0.63-M solution of propionic acid? pH = What is the degree of ionization of propionic acid in this solution?
The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3 x 10 -13. H2S (aq) + H2O (l) <=> HS -(aq) + H3O +(aq) Ka = 1.0 x 10 -7 HS -(aq) + H2O (l) <=> S-2 (aq) + H3O +(aq) Ka = 1.3 x 10 -13 What is the equilibrium concentration of HS - in a 0.300 M solution of H2S?
Important Info: Ka reaction: HC2H3O2(aq) + H2O(l) <-->C2H3O2 (aq) +H3O+(aq) HC2H3O(aq) +OH-(aq) -> C2H3O2-(aq) + H2O (l) A 1.0 L buffer solution is 0.280 M in HC2H302 (acetic acid) and 0.320 M in NaC2H302 (sodium acetate). Calculate the pH of the budder and he Ka for HC2H3O2 IS 1.8 X 10-5 Calculate the pH of te solution above after the addition of 0.0400 moles of solid NaOH. Assume no volume change upon the addition of base.
6.What is the pH of a solution with [OH-] = 1.7 x 10-3M? 7.Calculate [H3O+] of a solution with a pH of 5.5 8. A 15.0 mL sample of H2SO4solution is titrated with 24.0 mL of 0.245 M NaOH solution. What is the molarity of the H2SO4solution?H2SO4(aq) + 2 NaOH (aq) →2 H2O (l) + Na2SO4(aq)
Complete the following table. [H3O+] [OH-] pH acidic, basic, or neutral? 1.3 x 10-'M 2.5 x 10-8 M 2.1
Calculate either [H3O+] or [OH-] for each of the solutions. Solution A: [OH-] = 1.29 x 10-7 M Solution A: [H3O+] = M Solution B: [H3O+] = = 9.97 x 10-9 M Solution B: [OH-] = M Solution C: [H3O+] = 6.69 x 10-4 M Solution C: [OH-] = M Which of these solutions are basic at 25 °C? A: [OH-] = 1.29 x 10-7 M
A 1.0 L solution of 0.30 M in H3O+(aq) containing Mn2+(aq), Cd2+(aq), and Fe2+(aq), all at 0.010 M, was saturated with H2S(g) at room temperature. Assume that the pH of the solution remains constant and that the [H2S]sat = 0.10 M. The Ksp for MnS9S) is 2.5 x 10-13 , Ksp for CdS(s) is 8.0 x 10 -27 and Ksp for FeS(s) is 6.3 x10-18 . For H2S:Ka1=1.3 x 10-7. Ka2=8.5 x 10-14. Calculate the equilibrium concentrations of Mn2+(aq),Cd2+(aq), and...
The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3 x 10 -13. H2S (aq) + H2O (l) <=> HS -(aq) + H3O +(aq) Ka = 1.0 x 10 -7 HS -(aq) + H2O (l) <=> S-2 (aq) + H3O +(aq) Ka = 1.3 x 10 -13 What is the equilibrium concentration of HS - in a 0.300 M solution of H2S?
Calculate either [H3O+] or [OH−] for each of the solutions. Solution A:[OH−]=2.59×10−7 M Solution A: [H3O+]= M Solution B:[H3O+]=8.91×10−9 M Solution B: [OH−]= M Solution C:[H3O+]=7.61×10−4 M Solution C: [OH−]= M Which of these solutions are basic at 25 °C? A:[OH−]=2.59×10−7 M B:[H3O+]=8.91×10−9 M