Use the References to access important values if needed for this question. A buffer solution is made that is 0.379 M in HCN and 0.379 M in NaCN. If Ka for HCN is 4.00 x 10-¹0, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.090 mol HNO3 is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H+) + - +

A 76.0 mL sample of 0.0100 M HIO4 is titrated with 0.0200 M RbOH solution. Calculate the pH after the following volumes of base have been added. (a) 14.1 mL pH = (d) 39.9 mL pH = (b) 37.2 mL pH = (e) 69.5 mL pH = (c) 38.0 mL pH =

You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium chloride mixed well. Kb for ammonia =1.8 x 10^-5 (A) is this a buffer solution? Why or why not? (B)if it is a buffer solution, what is the pH of this buffer solution? (C)how many mL of 1.50 M HCl can be added to this solution before the buffer is exhausted (d) how many mL of 1.5 M NaOH can be added to this solution before the buffer is exhausted?

Determine the pH during the titration of 59.7 mL of 0.392 M hypochlorous acid (K₂ = 3.5×10-8) by 0.392 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 13.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 89.6 mL of KOH Submit Show Approach Show Tutor Steps