Calculate the pH of a 0.025 M solution of propanoic acid (K, = 1.3 x 10-5). 7.48 0.025 O 5.6 x 104 1.6

Acid-Base Equilibrium: 1. Find the pH of 0.0500M CH;CICOOH (a weak acid) where Ka=1.4 x 103 2. Ca(OH); is a strong base (meaning that nearly 100% ionizes). Find the pH for 5.0 x 103 M solution of Ca(OH)2.

Consider the following data on some weak acids and weak bases: acid base K, a name formula name formula hydrocyanic acid HCN -10 4.9 x 10 NH3 ammonia 1.8 x 10 nitrous acid HNO2 | 4.5 × 10 pyridine C5H5N 1.7 × 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M NaCN v choose one 1 (lowest) 0.1 М KСI 3 4 (highest) 0.1 M NH4BR 0.1 M KNO2 choose one ♥

Calculate the pH at 25 °C of a 0.63 M solution of sodium hypochlorite (NaC10). Note that hypochlorous acid (HC1O) is a weak acid with a pk of 7.50. Round your answer to 1 decimal place. pH -0 X S

The acid dissociation constant K, of carbonic acid (H,CO,) is 4.5 × 10 '. Calculate the pH of a 1.2M solution of carbonic acid. Round your answer to 1 decimal place. pH =

20)

The acid dissociation constant K of hydrocyanic acid (HCN) is 6.2 × 10 10 Calculate the pH of a 3.0M solution of hydrocyanic acid. Round your answer to 1 decimal place. pH = 0

The base protonation constant K, of ammonia (NH,) is 1.8 x 10. -5. Calculate the pH of a 1.2 M solution of ammonia at 25 °C. Round your answer to1 decimal place.