Question

1. A buffer solution contains 0.491 M KHCO₃ and 0.336 M Na₂CO₃. Determine the pH change when 0.073 mol HCl is added to 1.00 L of the buffer.

2.A buffer solution contains 0.386 M NH₄Br and 0.370 M NH₃ (ammonia). Determine the pH change when 0.100 mol NaOH is added to 1.00 L of the buffer.

pH after addition − pH before addition = pH change =

3. A buffer solution is made that is 0.349 M in H2CO3 and 0.349 M in KHCO3.

If Kal for H2CO3 is 4.20X10^-7, what is the pH of the buffer solution?

Write the net ionic equation for the reaction that occurs when 0.080 mol KOH is added to 1.00 L of the buffer solution.

4. A buffer solution is made that is 0.309 M in HClO and 0.309 M in KClO.

If Ka for HClO is 3.50x10^-8 , what is the pH of the buffer solution?

Write the net ionic equation for the reaction that occurs when 0.087 mol NaOH is added to 1.00 L of the buffer solution.

(Use the lowest possible coefficients. Omit states of matter.)

(Use the lowest possible coefficients. Omit states of matter.)

Answer 1