pH after 5 drops NaOH pH after 10 drops NaOH Initial pH pH change Buffer (Y or N Choose... H20 5.7 11.7 11.9 Choose... Choose... 0.1 M Nacl 6.9 13.1 13.4 Choose... - Choose... High pH buffer 9.9 10.1 10.3 Choose... Choose... Low pH buffer 3.8 4.1 4.4 Choose...

A buffer is prepared by adding 20.0g of sodium acetate to 500mL of a 0.150 M acetic acid solution.  Determine the pH of the buffer. a. 4.74 b. 6.32 c. 5.26 d. 4.23

1. Explain how a buffer made of hydrofluoric acid (0.20M) and fluoride ion (0.20M) adjusts to a small amount of added NaOH. 2. Calculate the amount of 0.1M NaOH that must be added to destroy the buffer solution from question 1.

Part A Review Constants | Periodic Table Learning Goal: To understand how buffers use reserves of conjugate acid and conjugate base to counteract the effects of acid or base addition on pH. A buffer is a mixture of a conjugate acid-base pair. In other words, it is a solution that contains a weak acid and its conjugate base, or a weak base and its conjugate acid. For example, an acetic acid buffer consists of acetic acid, CH3COOH, and its conjugate base, the acetate ion CH3COO. Because ions cannot simply be added to a solution, the conjugate base is added in a salt form (e.g., sodium acetate NaCH, COO). Buffers work because the conjugate acid-base pair work together to neutralize the addition of H+ or OH ions. Thus, for example, if H+ ions are added to the acetate buffer described above, they will be largely removed from solution by the reaction of H+ with the conjugate base: H++ CH3COO→CH3COOH Similarly, any added OH ions will be neutralized by a reaction with the conjugate acid: OH +…

[References] SIMULATION Buffer Solutions 7 7 0. 14 0- 14 0. 14 7.00 7.00 4.74 Reset All 1.0 M HCI 1.0 M NAOH 1.0 M HCI 1.0 M NAOH 1.0 M HCI 1.0 M NAOH Add Add Add Add Add Add 10. mL 10. mL 10. mL 10. mL 10. mL 10. mL Initial Solution 100 mL Initial Solution Initial Solution 100 mL 100 mL 1.0 M CH3CO,H(aq) 1.0 M NACH,CO,(aq) H,0 1.0 M NaCl What is the pH of water after the addition of 10 mL of 1.0 M HC1? Recheck (2 of 5) 7th attempt Incorrect The pH is given above the beaker.

5. Find the pH at the various points on the titration of 25.0 mL of 0.250 M carbonic acid with 0.100 M sodium hydroxide. a) Initial b) At the halfway point or midpoint c) At the equivalence point d) 10.0 mL past the equivalence point

Give detailed Solution..no need handwritten answer (don't use Ai for answering this)

Solve 16. 8

Find moles of NaOH added and equivalence point