Question

Assuming that HCI and H2SO4 are a strong acids, and that NaOH and Ba(OH)2 are a strong bases, and that all four dissociate 100% in water as indicated below

Answer 1

Step-by-step explanation:

We start by writing the dissociation equation to yield hydrogen and hydroxide ion

We have that as:

`HCl\text{ + H}_2O\text{ }\rightleftarrows\text{ H}_3O^+\text{ + Cl}^-`

We have been told that the dissociation is 100% complete.

What this means is that the concentration of the acid is the concentration of the hydrogen ion

Thus, we have it that:

a)

`[H^+]\text{ = 0.00010 M}`

B) Mathematically:

`[H^+][OH^-]\text{ = 10}^(-14)`

We proceed to substitute for the concentration of the hydrogen ion:

`\begin{gathered} 0.0001\text{ }*\text{ \lbrack OH}^-]\text{ = 10}^(-14) \\ \\ [OH^-]\text{ = }(10^(-14))/(0.0001) \\ \\ [OH^-]\text{ = 1 }*\text{ 10}^(-10)\text{ M} \end{gathered}`

c) Mathematically:

`\begin{gathered} pH\text{ = -log\lbrack H}^+] \\ pH\text{ = -log\lparen0.0001\rparen} \\ pH\text{ = 4} \end{gathered}`

d) Mathematically:

`\begin{gathered} pH\text{ +}pOH\text{ = 14} \\ pOH\text{ = 14 - pH} \\ pOH\text{ = 14-4} \\ pOH\text{ = 10} \end{gathered}`