A buffer is made by adding 0.300 mol CH3COOH and 0.300 mol CH3COONa to enough water to make 1.000 L of solution. The pH of the buffer is 4.74. Calculate the pH of this solution after 15.0 mL of 4.0 M NaOH(aq) solution is added.

If the equilibrium concentration (also known as the molar solubility) of CaF2 is 1.24 x 10-3M at 35 °C, what is Ksp at this temperature?

Which would be correct expression of the solubility product constant, Ksp, for Fe(OH)3?

If the pH of a solution is 6.27, which of the following statements is true?

Consider the following hypothetical aqueous reaction: A(aq) → B(aq). A flask is charged with 0.065 mol of A in a total volume of 100.0 mL. The following data are collected. Calculate the average rate of appearance for B in units of M/s between 20 and 40 seconds. Time (sec) 0 10 20 30 40 Moles of A 0.065 0.051 0.042 0.036 0.031

What is the pH of a 0.050M solution of benzoic acid, C6H5COOH, which has a Ka = 6.3 x 10-5?

What is the pH of a 0.075M solution of ethylamine, C2H5NH2, which has a Kb = 6.4 x 10-4?

From the following values for a calculated rate constant, which one would be for a second-order reaction?

What is the pH of a solution prepared by taking 10.0 mL of 0.45 M HClO4 and diluting it to a final volume of 250 mL?

With the polyprotic acid like H3PO4, the dissociation of which hydrogen atom gives the largest Ka value?