Webb17 maj 2016 · log10Kw = log10[H 3O+] +log10[H O−] = − 14 But by definition, −log10[H 3O+] = pH, and −log10[H O−] = pOH pKw = pH + pOH = 14 as required. Given that this is a bond-breaking reaction, how would you expect the equilibrium to evolve at temperatures greater than 298K? Would pH increase or decrease? Answer link WebbQuestion 2. Which one of the following is equal to the p Ka of a weak acid? a) Its relative molecular mass. b) The pKb of its conjugate base. c) The pH of a solution containing equal amounts of the acid and its conjugate base. d) The equilibrium concentration of its conjugate base.

What is the pOH of an aqueous solution that contains 5.3 x 10-13 …

Webb8 apr. 2024 · Given, the value of pOH of the solution containing hydroxide ions, pOH = 5.00. Substitute the value of the pOH in the equation (1): 5 = - log [OH⁻] log [OH⁻] = -5. [OH⁻] = 10⁻⁵ M. Therefore, the molarity of the hydroxide ions in an aqueous solution is equal to 10⁻⁵ M. Learn more about pOH, here: WebbA solution at standard conditions has {[H3O+] = 2.00 X 106 or [OH-] = 2.00 X 106). What is its {pH, POH}? A) ... Question 4 refers to a solution at standard conditions equal to [H3O+=2.00*10^-6 or ... where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak ... journal accounting term

Calculate the molarity of hydroxide ion in an aqueous solution that …

WebbSaturation defines an equilibrium condition: the rate of solute dissolution is equal to the rate of solute precipitation; alternatively, the rate of going up into solution is equal to the rate of coming out of solution. undissolved solute ⇌ dissolved solute. This saturation depends on temperature, the properties of the solvent, and the nature ... WebbQuestion: Use pH, pOH, [H3O+], and [OH–] relationships. (a) The hydroxide ion concentration in an aqueous solution of HCl is 3.4×10-13 M. Calculate [H3O+], pH, and pOH for this solution. [H3O+] = 2.9x10^-4 M pH = 1.54 pOH = 12.46 (b) The pOH of an aqueous solution of HNO3 is 9.30. Calculate [H3O+], [OH-], and pH for this solution. WebbThe pH of aqueous solutions can be measured with a glass electrode and a pH meter or a color-changing indicator. Measurements of pH are important in chemistry ... (HCl) is equal to 2 (pH = −log10(0.01)), while the pOH of a 0.01M solution of sodium hydroxide (NaOH) is equal to 2 (pOH = −log10(0.01)), which corresponds to a pH of ... journal adsb bouc bel air