A 18 M solution of an acid that ionizes only slightly in solution would be termed_

Aconcentrate and weake

b.strong and dilute

c.dilute and weak

Dconcentrated and strong (my guess)

Calculate the [H^+] for the aqueous solution in which [OH^-] is 1 x10^-9. Is this solution acidic, basic or neutral.

please help!!! show work!!

3.The volume of 3.50M HCl needed to make 275mL of 2.90M HCl is _

4.What are the products of the self-ionization of water ?

AH30^+ and H20
BOH^- and OH^+
COH^+ and H^-
DOH^- and H^+ (my guess)

The base dissociation constant is only found for____

Aconcentrated bases
Bdilute bases
Cstrong bases ***(my guess)
Dweak bases

What is an acid dissociation constant? When can it not be calculated and why? I got the first part of the question, just not the second part as to when it cannnot be calculated.

A 18 M solution of an acid that ionizes only slightly in solution would be termed
concentrated and weak. The concentration of the acid is high. The acid which dissociates partially in water is a weak acid.

Calculate the [H^+] for the aqueous solution in which [OH^-] is 1 x10^-9. Is this solution acidic, basic or neutral. To determine [H+] use:

1x10^-14 = [OH-][H+]
solve for [H+]
[H+] = 1x10^-14/1x10^-9
= 1x10^-5

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