Answer to Question #140479 in General Chemistry for Ashley

Question

Calculate the pH of an aqueous solution of 0.571 M trimethylamine (a weak base with the formula (CH3)3N) . The value of Kb is 6.30×10-5.

pH =

A solution contains 0.428 M sodium fluoride and 0.284 M hydrofluoric acid.

Calculate the pH of this solution. The Ka of HF is 7.20×10-4.

pH =

A buffer solution contains 0.344 M hypochlorous acid (Ka = 3.50×10-8) and 0.291 M potassium hypochlorite.

If 0.0317 moles of potassium hydroxide are added to 150 mL of this buffer, what is the pH of the resulting solution?

(Assume that the volume does not change upon adding potassium hydroxide)

pH

How many grams of solid potassium cyanide should be added to 1.00 L of a 0.279 M hydrocyanic acid solution to prepare a buffer with a pH of 10.100? The Ka of hydrocyanic acid is 4.00×10-10.

Mass of potassium cyanide =

Answer 1

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