WebA 0.200 M solution of an acid has a pH = 1.00. What is the value of the ionization constant, Ka, for this acid? A 0.300 M solution of an acid, HZ, has a pH = 1.301. What is the value of the ionization constant, Ka, for this acid? A 0.200 M solution of a weak base in water has a pH = 10.40. Calculate the value of Kb for this base. WebA solution of 0.010 M sodium phenolate, NaC6H5O has a pH of 11.00. Calcuate the dissociation constant for the weak acid phenol, HC6H5O. Ans: 9.0 x 10^-11. Weak Base: A …
第六章 酸碱平衡及其在分析中的应用 - 百度文库
WebThe pH of 0.001N sodium hydroxide solution at 25 oC is: A 3 B 4 C 11 D 12 Medium Solution Verified by Toppr Correct option is C) pH=14−pOH pOH of 0.001 N NaOH=−log[1×10 −3]=3 pH=14−3=11 Was this answer helpful? 0 0 Similar questions Assertion The pH of an aqueous solution of acetic acid remains unchanged by the addition of sodium acetate. … WebScience Chemistry A buffer solution contains 0.89 mol of phenol (HC6H5O) and 0.86 mol of sodium phenoxide (NaC6H5O) in 8.80 L.The Ka of phenol (HC6H5O) is Ka = 1.3e-10.(a) … tryst dc menu
Fundementals J15 NaC6H5O is acid/base? - CHEMISTRY …
WebMar 1, 2024 · So, when NaC6H5O disassociates in water and releases the two ions, the Na+ won't be able to form NaOH, but the C6H5O- will form some C6H6O. This means that the anion has taken some H+ away from some water molecules in solution, meaning that H2O has had an H taken from it, leaving behind OH-. WebThe pH at 25 °C of an aqueous solution of the sodium salt of phenol (NaC6H5O) is 11.49. Calculate the concentration of C6H5O- in this solution, in moles per liter. Ka for HC6H5O … WebMar 19, 2024 · 1x10⁻¹⁰ = x²/0.393 Solving for x: x = √1x10⁻¹⁰ * 0.393 x = 6.27x10⁻⁶ M This would be the equilibrium concentration of the conjugate base, the weak acid would be practically the same. [C₆H₅OH] = 0.393 - 6.27x10⁻⁶ = 0.39399373 M Finally for the pH: pH = -log (6.27x10⁻⁶) pH = 5.2 Advertisement phillip ross bevan washington dc