Self Check 6D.4A

Acidity $K_{a}$
Basicity $K_{b}$
The Conjugate Seesaw $K_{a}\times K_{b}=K_{w}$

Amy Luu 2G
Posts: 105
Joined: Wed Sep 18, 2019 12:19 am

Self Check 6D.4A

Use Tables 6D.1 and 6D.2 to decide whether aqueous solutions of the salts (a) Ba(NO2)2, (b) CrCl3, and (c) NH4NO3 are acidic, neutral, or basic.
I am confused on how to solve this problem. How do you know whether the solution of the salts will be acidic, neutral or basic? Thank you!

Ryan Chang 1C
Posts: 105
Joined: Sat Aug 24, 2019 12:17 am

Re: Self Check 6D.4A

In order to determine whether the solutions of the salts will be acidic, neutral, or basic, you must consider the cation and the anion of the salt. First check if the anion to see if it's acidic, neutral, or basic (Table 6D.2 gives a list of acidic, neutral, and basic anions). If the anion is acidic, the salt will produce an acidic solution, if the anion is neutral, look at the cation, and if the anion is basic, the salt will produce a basic solution. In the case of an anion being neutral, the solution will most likely be acidic because most cations produce acidic solutions (Table 6D.1 gives you a list of cations). However, watch out for cases where one ion is acidic and the other is basic, such as NH4F. In this case, compare the Ka, and Kb values or the acidic ion and basic ion. If the acidic ion has the largest K value, the solution will be acidic, and if the basic ion has the largest K value, the solution will be basic.