In the laboratory, a general chemistry student measured the pH of a 0.392 M aqueous solution of methylamine, CH3NH2 to be 12.123. Use the information she obtained to determine the K₁ for this base. Kb (experiment) = =
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- Consider a 0.10 M solution of a weak polyprotic acid (H2A) with the possible values of Ka1 and Ka2 given here.a. Ka1 = 1.0 * 10-4; Ka2 = 5.0 * 10-5b. Ka1 = 1.0 * 10-4; Ka2 = 1.0 * 10-5c. Ka1 = 1.0 * 10-4; Ka2 = 1.0 * 10-6Calculate the contributions to [H3O+] from each ionization step. At what point can the contribution of the second step be neglected?Consider a mixture of 1.36 M HCIO and 1.65 M NaCIO. Given that the K, for HCIO = 2.9 x 10-8 determine the pH of this solution.A 23mL sample of HCl is titration to phenolphthalein end point with 26.43 mL of a 0.09181 M NaOH standard solution. Calculate the molar concentration of the HCl solution.
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- In the determination of the water hardness of a river water sample, the pH of the sample was adjusted to 12 instead of 10. Is there a positive error, negative error, no effect, or error could not be determined In terms of the ppm CaCO3 of sample?At −11.5 ∘C, a common temperature for household freezers, what is the maximum mass of sucralose (C12H19Cl3O8) you can add to 1.00 kg of pure water and still have the solution freeze? Assume that sucralose is a molecular solid and does not ionize when it dissolves in water. Consult the table of Kf values.This question is concerned with acid/base. The ionic product of water may be taken as 10-14 mol2dm-6. Aqueous solutions of a particular monobasic acid HX have the following pH values (see figure below). Concentration in moldm-3 PH Hydrogen ion concentration in moldm-3 Solution A 0.1 2.80 1.585 x 10-3 Solution B 0.001 3.85 For each solution, calculate the dissociation constant of the acid. Comment on the constancy of your values of Ka (the dissociation constant). Give the expression for the dissociation of the acid